The '''second law of thermodynamics''' states that the total [[entropy]] of an [[isolated system]] can never decrease over time, and is constant if and only if all processes are reversible.<ref>http://web.mit.edu/16.unified/www/FALL/thermodynamics/notes/node38.html#SECTION05224000000000000000</ref> Isolated systems spontaneously evolve towards [[thermodynamic equilibrium]], the state with maximum entropy.
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The second law of thermodynamics states that the total entropy of an isolated system can never decrease over time, and is constant if and only if all processes are reversible. Isolated systems spontaneously evolve towards thermodynamic equilibrium, the state with maximum entropy.
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<font color="#ff8000">'''热力学第二定律 Second Law Of Thermodynamics'''</font>指出,<font color="#ff8000">'''孤立系统Isolated System'''</font>的总熵永远不会随着时间而减少,且当且仅当所有过程都是可逆时,总熵才恒定。<ref>http://web.mit.edu/16.unified/www/FALL/thermodynamics/notes/node38.html#SECTION05224000000000000000</ref>孤立系统自发地到达到热力学平衡状态,此时为熵最大的状态。
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<font color="#ff8000">'''热力学第二定律 Second Law Of Thermodynamics'''</font>指出,<font color="#ff8000">'''孤立系统Isolated System'''</font>的总熵永远不会随着时间而减少,且当且仅当所有过程都是可逆时,总熵才恒定。孤立系统自发地到达到热力学平衡状态,此时为熵最大的状态。
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The total entropy of a system and its surroundings can remain constant in ideal cases where the system is in [[thermodynamic equilibrium]], or is undergoing a (fictive) [[Reversible process (thermodynamics)|reversible process]]. In all processes that occur, including [[spontaneous process]]es,<ref>Atkins and de Paula, p.78</ref> the total entropy of the system and its surroundings increases and the process is [[Irreversible process|irreversible in the thermodynamic sense]]. The increase in entropy accounts for the irreversibility of natural processes, and the [[Arrow of time|asymmetry between future and past]].<ref>{{cite book|last=Zohuri|first=Bahman|title=Dimensional Analysis Beyond the Pi Theorem|url=https://books.google.com/books?id=pRVuDQAAQBAJ|year=2016|publisher=Springer|isbn=978-3-319-45726-0|page=[https://books.google.com.ph/books?id=pRVuDQAAQBAJ&pg=PA111&dq=%22increase+in+entropy+accounts+for+the+irreversibility+of+natural+processes+and+the+asymmetry+between+future+and+past.%22&hl=en&sa=X&ved=0ahUKEwj6spb61tbaAhUFS7wKHfftDtIQ6AEIKDAA#v=onepage&q=%22increase%20in%20entropy%20accounts%20for%20the%20irreversibility%20of%20natural%20processes%20and%20the%20asymmetry%20between%20future%20and%20past.%22 111]}}</ref>
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The total entropy of a system and its surroundings can remain constant in ideal cases where the system is in thermodynamic equilibrium, or is undergoing a (fictive) reversible process. In all processes that occur, including spontaneous processes, the total entropy of the system and its surroundings increases and the process is irreversible in the thermodynamic sense. The increase in entropy accounts for the irreversibility of natural processes, and the asymmetry between future and past.
系统及其周围环境的总熵在理想情况下可以保持不变,在这种情况下,系统处于热力学平衡状态,或者正在经历一个假想的可逆过程。所有过程中,包括<font color="#ff8000">'''自发过程 Spontaneous Processes'''</font>,es,<ref>Atkins and de Paula, p.78</ref> 系统及其周围环境的总熵增加,这一过程在热力学意义上是不可逆的。熵的增加解释了自然过程的不可逆性,以及未来和过去之间的不对称性。<ref>{{cite book|last=Zohuri|first=Bahman|title=Dimensional Analysis Beyond the Pi Theorem|url=https://books.google.com/books?id=pRVuDQAAQBAJ|year=2016|publisher=Springer|isbn=978-3-319-45726-0|page=[https://books.google.com.ph/books?id=pRVuDQAAQBAJ&pg=PA111&dq=%22increase+in+entropy+accounts+for+the+irreversibility+of+natural+processes+and+the+asymmetry+between+future+and+past.%22&hl=en&sa=X&ved=0ahUKEwj6spb61tbaAhUFS7wKHfftDtIQ6AEIKDAA#v=onepage&q=%22increase%20in%20entropy%20accounts%20for%20the%20irreversibility%20of%20natural%20processes%20and%20the%20asymmetry%20between%20future%20and%20past.%22 111]}}</ref>
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Historically, the second law was an [[Empirical evidence|empirical finding]] that was accepted as an axiom of [[thermodynamics|thermodynamic theory]]. [[Statistical mechanics]], classical or [[quantum thermodynamics|quantum]], explains the microscopic origin of the law.
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Historically, the second law was an empirical finding that was accepted as an axiom of thermodynamic theory. Statistical mechanics, classical or quantum, explains the microscopic origin of the law.
The second law has been expressed in many ways. Its first formulation is credited to the French scientist [[Nicolas Léonard Sadi Carnot|Sadi Carnot]], who in 1824 showed that there is an upper limit to the efficiency of conversion of heat to work in a heat engine. This aspect of the second law is also known as [[Carnot's theorem (thermodynamics)|Carnot's rule]] or limit.<ref>Jaffe, R.L., Taylor, W. (2018). ''The Physics of Energy'', Cambridge University Press, Cambridge UK, pages 150, 151, 259, 772, 743.</ref>
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'''热力学第二定律'''可以使用多种方法表述。它的第一个公式归功于法国科学家'''卡诺Sadi Carnot'''</font>,卡诺在1824年证明了在热机中将热转化为功的效率有一个上限。第二定律的这个方面也被称为<font color="#ff8000">'''卡诺规则Carnot's Rule'''</font>或<font color="#ff8000">'''卡诺限制Carnot's Limit'''</font>。<ref>Jaffe, R.L., Taylor, W. (2018). ''The Physics of Energy'', Cambridge University Press, Cambridge UK, pages 150, 151, 259, 772, 743.</ref>
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The second law has been expressed in many ways. Its first formulation is credited to the French scientist Sadi Carnot, who in 1824 showed that there is an upper limit to the efficiency of conversion of heat to work in a heat engine. This aspect of the second law is also known as Carnot's rule or limit.
'''热力学第二定律 Second Law of Thermodynamics'''也是热力学的四条基本定律之一,它表述了热力学过程的不可逆性——孤立系统自发地朝着热力学平衡方向(即最大熵状态)演化,另一种表述为:第二类永动机永不可能实现。
'''热力学第二定律 Second Law of Thermodynamics'''也是热力学的四条基本定律之一,它表述了热力学过程的不可逆性——孤立系统自发地朝着热力学平衡方向(即最大熵状态)演化,另一种表述为:第二类永动机永不可能实现。
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The [[first law of thermodynamics]] provides the definition of the [[internal energy]] of a [[thermodynamic system]], and expresses the law of [[conservation of energy]].<ref>[[Max Planck|Planck, M.]] (1897/1903), pp. 40–41.</ref><ref>Munster A. (1970), pp. 8–9, 50–51.</ref> The second law is concerned with the direction of natural processes.<ref>{{harvnb|Mandl|1988}}</ref> It asserts that a natural process runs only in one sense, and is not reversible. For example, when a path for conduction and radiation is made available, heat always flows spontaneously from a hotter to a colder body. Such [[Phenomenon|phenomena]] are accounted for in terms of [[entropy]].<ref>[[Max Planck|Planck, M.]] (1897/1903), pp. 79–107.</ref><ref>Bailyn, M. (1994), Section 71, pp. 113–154.</ref> If an isolated system is held initially in internal thermodynamic equilibrium by internal partitioning impermeable walls, and then some operation makes the walls more permeable, then the system spontaneously evolves to reach a final new internal thermodynamic equilibrium, and its total entropy, {{math|''S''}}, increases.
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The first law of thermodynamics provides the definition of the internal energy of a thermodynamic system, and expresses the law of conservation of energy. The second law is concerned with the direction of natural processes. It asserts that a natural process runs only in one sense, and is not reversible. For example, when a path for conduction and radiation is made available, heat always flows spontaneously from a hotter to a colder body. Such phenomena are accounted for in terms of entropy. If an isolated system is held initially in internal thermodynamic equilibrium by internal partitioning impermeable walls, and then some operation makes the walls more permeable, then the system spontaneously evolves to reach a final new internal thermodynamic equilibrium, and its total entropy, S, increases.
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'''热力学第一定律 First Law Of Thermodynamics'''定义了热力学系统所涉及到的'''内能 Internal Energy''',并体现了能量守恒定律。热力学第二定律与'''自然过程Natural Processes'''的方向有关。它断言自然过程只在一种意义上进行,且不可逆 。例如,当有了传导和辐射的(传播)路径时,热总是自发地从一个较热的物体流向一个较冷的物体。这种现象可以用'''熵Entropy'''来解释。
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'''热力学第一定律 First Law Of Thermodynamics'''定义了热力学系统所涉及到的'''内能 Internal Energy''',<ref>[[Max Planck|Planck, M.]] (1897/1903), pp. 40–41.</ref><ref>Munster A. (1970), pp. 8–9, 50–51.</ref>并体现了能量守恒定律。热力学第二定律与'''自然过程Natural Processes'''<ref>{{harvnb|Mandl|1988}}</ref>的方向有关。它断言自然过程只在一种意义上进行,且不可逆 。例如,当有了传导和辐射的(传播)路径时,热总是自发地从一个较热的物体流向一个较冷的物体。 这种现象可以用<ref>[[Max Planck|Planck, M.]] (1897/1903), pp. 79–107.</ref><ref>Bailyn, M. (1994), Section 71, pp. 113–154.</ref> '''熵Entropy'''来解释。
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--[[用户:大白|大白]]([[用户讨论:大白|讨论]])这里是不是少了一段原文?
'''<font color="#32CD32">若一个'''孤立系统Isolated System'''最初在具有隔热内壁的系统内维持热力学平衡,通过一些操作使内壁透热,则该系统可自发地演变,最终达到一个新的内部热力学平衡,且其总熵{{math|''S''}}增加。If an isolated system is held initially in internal thermodynamic equilibrium by internal partitioning impermeable walls, and then some operation makes the walls more permeable, then the system spontaneously evolves to reach a final new internal thermodynamic equilibrium, and its total entropy, S, increases.</font>'''
'''<font color="#32CD32">若一个'''孤立系统Isolated System'''最初在具有隔热内壁的系统内维持热力学平衡,通过一些操作使内壁透热,则该系统可自发地演变,最终达到一个新的内部热力学平衡,且其总熵{{math|''S''}}增加。If an isolated system is held initially in internal thermodynamic equilibrium by internal partitioning impermeable walls, and then some operation makes the walls more permeable, then the system spontaneously evolves to reach a final new internal thermodynamic equilibrium, and its total entropy, S, increases.</font>'''
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In a fictive reversible process, an infinitesimal increment in the entropy ({{math|d''S''}}) of a system is defined to result from an infinitesimal transfer of heat ({{math|δ''Q''}}) to a [[closed system]] (which allows the entry or exit of energy – but not transfer of matter) divided by the common temperature ({{math|''T''}}) of the system in equilibrium and the surroundings which supply the heat:<ref>Bailyn, M. (1994), p. 120.</ref>
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In a fictive reversible process, an infinitesimal increment in the entropy () of a system is defined to result from an infinitesimal transfer of heat () to a closed system (which allows the entry or exit of energy – but not transfer of matter) divided by the common temperature () of the system in equilibrium and the surroundings which supply the heat:
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在假想的可逆过程中,系统的熵的无穷小增量<math>dS</math>被定义为由无穷小的热<math>δQ</math>传递到一个封闭系统(允许能量进入或出去,但不允许物质传递的系统)除以该平衡系统和提供热的环境的共同温度 <math>T</math>:<ref>Bailyn, M. (1994), p. 120.</ref>
Different notations are used for infinitesimal amounts of heat ({{mvar|δ}}) and infinitesimal amounts of entropy ({{mvar|d}}) because entropy is a [[function of state]], while heat, like work, is not. For an actually possible infinitesimal process without exchange of mass with the surroundings, the second law requires that the increment in system entropy fulfills the [[Clausius Theorem|inequality]] <ref name="MortimerBook"> Mortimer, R. G. ''Physical Chemistry''. 3rd ed., p. 120, Academic Press, 2008. </ref><ref name="FermiBook"> Fermi, E. ''Thermodynamics'', footnote on p. 48, Dover Publications,1956 (still in print). </ref>
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Different notations are used for infinitesimal amounts of heat () and infinitesimal amounts of entropy () because entropy is a function of state, while heat, like work, is not. For an actually possible infinitesimal process without exchange of mass with the surroundings, the second law requires that the increment in system entropy fulfills the inequality
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用不同的符号''δ''和''d''表示无穷小量的热和无穷小量的熵,因为熵是状态函数,而热和功一样,并不是状态函数。对于实际上可能存在的不与环境发生物质交换的无穷小过程,第二定律要求系统熵增量满足不等式: <ref name="MortimerBook"> Mortimer, R. G. ''Physical Chemistry''. 3rd ed., p. 120, Academic Press, 2008. </ref><ref name="FermiBook"> Fermi, E. ''Thermodynamics'', footnote on p. 48, Dover Publications,1956 (still in print). </ref>
This is because a general process for this case may include work being done on the system by its surroundings, which can have frictional or viscous effects inside the system, because a chemical reaction may be in progress, or because heat transfer actually occurs only irreversibly, driven by a finite difference between the system temperature ({{math|''T''}}) and the temperature of the surroundings ({{math|''T''}}<sub>''surr''</sub>).
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<ref name=":0">Adkins, C.J. (1968/1983), p. 75.</ref><ref name="Munster 45"/>
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Note that the equality still applies for pure heat flow,
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<ref name="Schmidt-Rohr 14"> Schmidt-Rohr, K. (2014). "Expansion Work without the External Pressure, and Thermodynamics in Terms of Quasistatic Irreversible Processes" ''J. Chem. Educ.'' '''91''': 402-409. https://dx.doi.org/10.1021/ed3008704 </ref>
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This is because a general process for this case may include work being done on the system by its surroundings, which can have frictional or viscous effects inside the system, because a chemical reaction may be in progress, or because heat transfer actually occurs only irreversibly, driven by a finite difference between the system temperature () and the temperature of the surroundings (<sub>surr</sub>).Note that the equality still applies for pure heat flow。
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这是因为在这种情况下的一般过程可能包括周围环境对系统所做的功,该功在系统内部会产生摩擦或粘滞效应,此时一个化学反应可能正在系统内部进行,或因为热传递实际上是不可逆地发生,系统温度<math>T</math>和周围环境温度<math>T_surr</math>之间的差异驱动了热传递的发生。<ref name=":0">Adkins, C.J. (1968/1983), p. 75.</ref><ref name="Munster 45"/> 注意该等式也适用于'''纯热流Pure Heat Flow'''<ref name="Schmidt-Rohr 14"> Schmidt-Rohr, K. (2014). "Expansion Work without the External Pressure, and Thermodynamics in Terms of Quasistatic Irreversible Processes" ''J. Chem. Educ.'' '''91''': 402-409. https://dx.doi.org/10.1021/ed3008704 </ref>
which is the basis of the accurate determination of the absolute entropy of pure substances from measured heat capacity curves and entropy changes at phase transitions, i.e. by calorimetry.<ref name="Oxtoby8th">Oxtoby, D. W; Gillis, H.P., [[Laurie Butler|Butler, L. J.]] (2015).''Principles of Modern Chemistry'', Brooks Cole. p. 617. {{ISBN|978-1305079113}}</ref> <ref name="MortimerBook"></ref> Introducing a set of internal variables <math>\xi</math> to describe the deviation of a thermodynamic system in physical equilibrium (with the required well-defined uniform pressure ''P'' and temperature ''T'')<ref name="Schmidt-Rohr 14"></ref> from the chemical equilibrium state, one can record the equality
which is the basis of the accurate determination of the absolute entropy of pure substances from measured heat capacity curves and entropy changes at phase transitions, i.e. by calorimetry.[16] [11] Introducing a set of internal variables {\displaystyle \xi }\xi to describe the deviation of a thermodynamic system in physical equilibrium (with the required well-defined uniform pressure P and temperature T)[15] from the chemical equilibrium state, one can record the equality
which is the basis of the accurate determination of the absolute entropy of pure substances from measured heat capacity curves and entropy changes at phase transitions, i.e. by calorimetry.[16] [11] Introducing a set of internal variables {\displaystyle \xi }\xi to describe the deviation of a thermodynamic system in physical equilibrium (with the required well-defined uniform pressure P and temperature T)[15] from the chemical equilibrium state, one can record the equality
这种方法是通过测量'''热容曲线 Heat Capacity Curves'''和相变中熵的变化,来准确测定纯物质的绝对熵的基础,<ref name="Oxtoby8th">Oxtoby, D. W; Gillis, H.P., [[Laurie Butler|Butler, L. J.]] (2015).''Principles of Modern Chemistry'', Brooks Cole. p. 617. {{ISBN|978-1305079113}}</ref> <ref name="MortimerBook"></ref>比如'''量热法calorimetry'''。
The second term represents work of internal variables that can be perturbed by external influences, but the system cannot perform any positive work via internal variables. This statement introduces the impossibility of the reversion of evolution of the thermodynamic system in time and can be considered as a formulation of ''the second principle of thermodynamics'' – the formulation, which is, of course, equivalent to the formulation of the principle in terms of entropy.<ref> Pokrovskii V.N. (2005) Extended thermodynamics in a discrete-system approach, Eur. J. Phys. vol. 26, 769–781.</ref><ref>{{Cite journal | doi=10.1155/2013/906136|title = A Derivation of the Main Relations of Nonequilibrium Thermodynamics| journal=ISRN Thermodynamics| volume=2013| pages=1–9|year = 2013|last1 = Pokrovskii|first1 = Vladimir N.|doi-access=free}}</ref>
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The second term represents work of internal variables that can be perturbed by external influences, but the system cannot perform any positive work via internal variables. This statement introduces the impossibility of the reversion of evolution of the thermodynamic system in time and can be considered as a formulation of the second principle of thermodynamics – the formulation, which is, of course, equivalent to the formulation of the principle in terms of entropy.
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第二项代表内部变量的功,这些内部变量可能受到外部影响的干扰,但是系统不能通过内部变量做任何正功。这种说法介绍了热力学系统在时间上演化不可能逆转的性质,并且可以被认为是热力学第二原理的另外一种相当于熵原理的表述。该公式可以被看作使用'''熵Entropy'''的热力学第二定律等价表述<ref> Pokrovskii V.N. (2005) Extended thermodynamics in a discrete-system approach, Eur. J. Phys. vol. 26, 769–781.</ref><ref>{{Cite journal | doi=10.1155/2013/906136|title = A Derivation of the Main Relations of Nonequilibrium Thermodynamics| journal=ISRN Thermodynamics| volume=2013| pages=1–9|year = 2013|last1 = Pokrovskii|first1 = Vladimir N.|doi-access=free}}</ref>
The [[zeroth law of thermodynamics]] in its usual short statement allows recognition that two bodies in a relation of thermal equilibrium have the same temperature, especially that a test body has the same temperature as a reference thermometric body.<ref name=dugdale>{{cite book|author=J. S. Dugdale|title=Entropy and its Physical Meaning|publisher=Taylor & Francis|year=1996|isbn=978-0-7484-0569-5|page=13|quote=This law is the basis of temperature.}}</ref> For a body in thermal equilibrium with another, there are indefinitely many empirical temperature scales, in general respectively depending on the properties of a particular reference thermometric body. The second law allows{{how?|date=August 2018}} a distinguished temperature scale, which defines an absolute, [[thermodynamic temperature]], independent of the properties of any particular reference thermometric body.<ref>[[Mark Zemansky|Zemansky, M.W.]] (1968), pp. 207–209.</ref><ref>Quinn, T.J. (1983), p. 8.</ref>
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The zeroth law of thermodynamics in its usual short statement allows recognition that two bodies in a relation of thermal equilibrium have the same temperature, especially that a test body has the same temperature as a reference thermometric body. For a body in thermal equilibrium with another, there are indefinitely many empirical temperature scales, in general respectively depending on the properties of a particular reference thermometric body. The second law allows a distinguished temperature scale, which defines an absolute, thermodynamic temperature, independent of the properties of any particular reference thermometric body.
热力学第零定律是指如果两个热力学系统都与第三个热力学系统处于热平衡(温度相同)状态,则它们彼此也必定处于热平衡状态。热力学第零定律在它这个简短叙述中让人们认识到热平衡关系中的两个物体具有相同的温度,特别是当一个被测物体与一个参考测温物体具有相同的温度时,对于两个处于热平衡状态的物体,有无限多的'''<font color = '#ff8000'>经验温标empirical temperature scales</font>''',这通常取决于特定参考温度体的性质。热力学第二定律允许区分'''<font color = '#ff8000'>温度标度temperature scale</font>''',它定义了一个绝对的热力学温度,与任何特定的参考温度体的性质无关。
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热力学第零定律是指如果两个热力学系统都与第三个热力学系统处于热平衡(温度相同)状态,则它们彼此也必定处于热平衡状态。热力学第零定律在它这个简短叙述中让人们认识到热平衡关系中的两个物体具有相同的温度,特别是当一个被测物体与一个参考测温物体具有相同的温度时,<ref name=dugdale>{{cite book|author=J. S. Dugdale|title=Entropy and its Physical Meaning|publisher=Taylor & Francis|year=1996|isbn=978-0-7484-0569-5|page=13|quote=This law is the basis of temperature.}}</ref>对于两个处于热平衡状态的物体,有无限多的'''<font color = '#ff8000'>经验温标empirical temperature scales</font>''',这通常取决于特定参考温度体的性质。热力学第二定律允许区分'''<font color = '#ff8000'>温度标度temperature scale</font>''',它定义了一个绝对的热力学温度,与任何特定的参考温度体的性质无关。<ref>[[Mark Zemansky|Zemansky, M.W.]] (1968), pp. 207–209.</ref><ref>Quinn, T.J. (1983), p. 8.</ref>
==Various statements of the law热力学第二定律的不同表述==
==Various statements of the law热力学第二定律的不同表述==
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The second law of thermodynamics may be expressed in many specific ways,<ref name=MIT>{{cite web|title=Concept and Statements of the Second Law|url=http://web.mit.edu/16.unified/www/FALL/thermodynamics/notes/node37.html|accessdate=2010-10-07 |publisher=web.mit.edu}}</ref> the most prominent classical statements{{sfnp|Lieb|Yngvason|1999}} being the statement by [[Rudolf Clausius]] (1854), the statement by [[William Thomson, 1st Baron Kelvin|Lord Kelvin]] (1851), and the statement in axiomatic thermodynamics by [[Constantin Carathéodory]] (1909). These statements cast the law in general physical terms citing the impossibility of certain processes. The Clausius and the Kelvin statements have been shown to be equivalent.{{sfnp|Rao|2004|p=213}}
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The second law of thermodynamics may be expressed in many specific ways, the most prominent classical statements being the statement by Rudolf Clausius (1854), the statement by Lord Kelvin (1851), and the statement in axiomatic thermodynamics by Constantin Carathéodory (1909). These statements cast the law in general physical terms citing the impossibility of certain processes. The Clausius and the Kelvin statements have been shown to be equivalent.
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热力学第二定律可以用许多特定的方式来表达,最突出的经典陈述是 '''克劳修斯 Rudolf Clausius''' (1854)表述,'''开尔文 克劳修斯 Kelvin Clausius''' (1851)表述,以及康斯坦丁·卡拉西奥多里 Constantin Carathéodory(1909)在'''<font color = '#ff8000'>公理化热力学axiomatic thermodynamics</font>'''中的表述。这些表述用一般的物理术语来描述定律,引用某些过程的不可能性。克劳修斯和开尔文表述被证明是等价的。
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热力学第二定律可以用许多特定的方式来表达,<ref name=MIT>{{cite web|title=Concept and Statements of the Second Law|url=http://web.mit.edu/16.unified/www/FALL/thermodynamics/notes/node37.html|accessdate=2010-10-07 |publisher=web.mit.edu}}</ref> 最突出的经典陈述是 '''克劳修斯 Rudolf Clausius''' (1854)表述,'''开尔文 克劳修斯 Kelvin Clausius''' (1851)表述,以及康斯坦丁·卡拉西奥多里 Constantin Carathéodory(1909)在'''<font color = '#ff8000'>公理化热力学axiomatic thermodynamics</font>'''中的表述。这些表述用一般的物理术语来描述定律,引用某些过程的不可能性。克劳修斯和开尔文表述被证明是等价的。
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The historical origin<ref>[[Nicolas Léonard Sadi Carnot|Carnot, S.]] (1824/1986).</ref> of the second law of thermodynamics was in Carnot's principle. It refers to a cycle of a [[Carnot heat engine]], fictively operated in the limiting mode of extreme slowness known as quasi-static, so that the heat and work transfers are between subsystems that are always in their own internal states of thermodynamic equilibrium. The Carnot engine is an idealized device of special interest to engineers who are concerned with the efficiency of heat engines. Carnot's principle was recognized by Carnot at a time when the [[caloric theory]] of heat was seriously considered, before the recognition of the [[first law of thermodynamics]], and before the mathematical expression of the concept of entropy. Interpreted in the light of the first law, it is physically equivalent to the second law of thermodynamics, and remains valid today. Carnot's original arguments were made from the viewpoint of the caloric theory, before the discovery of the first law of thermodynamics. Some samples from his book are:
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The historical origin of the second law of thermodynamics was in Carnot's principle. It refers to a cycle of a Carnot heat engine, fictively operated in the limiting mode of extreme slowness known as quasi-static, so that the heat and work transfers are between subsystems that are always in their own internal states of thermodynamic equilibrium. The Carnot engine is an idealized device of special interest to engineers who are concerned with the efficiency of heat engines. Carnot's principle was recognized by Carnot at a time when the caloric theory of heat was seriously considered, before the recognition of the first law of thermodynamics, and before the mathematical expression of the concept of entropy. Interpreted in the light of the first law, it is physically equivalent to the second law of thermodynamics, and remains valid today. Carnot's original arguments were made from the viewpoint of the caloric theory, before the discovery of the first law of thermodynamics. Some samples from his book are:
它指的是'''<font color = '#ff8000'>卡诺热机Carnot heat engine</font>'''的一个循环,卡诺热机以'''<font color = '#ff8000'>准静态quasi-static</font>'''的极限慢速运转,因此热和功在子系统之间进行传递,子系统总是处于它们自己内部的热力学平衡状态。
它指的是'''<font color = '#ff8000'>卡诺热机Carnot heat engine</font>'''的一个循环,卡诺热机以'''<font color = '#ff8000'>准静态quasi-static</font>'''的极限慢速运转,因此热和功在子系统之间进行传递,子系统总是处于它们自己内部的热力学平衡状态。
卡诺热机是研究热机效率的工程师特别感兴趣的理想装置。
卡诺热机是研究热机效率的工程师特别感兴趣的理想装置。
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动力的产生不是由于蒸汽机实际消耗的热量,而是由于它从一个较热的物体转移到一个较冷的物体……。<ref>Carnot, S. (1824/1986), p. 46.</ref>
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::The production of motive power is then due in steam engines not to an actual consumption of caloric, but ''to its transportation from a warm body to a cold body ...''<ref>Carnot, S. (1824/1986), p. 46.</ref>
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The production of motive power is then due in steam engines not to an actual consumption of caloric, but to its transportation from a warm body to a cold body ...
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动力的产生不是由于蒸汽机实际消耗的热量,而是由于它从一个较热的物体转移到一个较冷的物体……。
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热的原动力与实现热的媒介无关,热的量完全取决于两个物体之间的温度,最后是热量的传递。<ref>Carnot, S. (1824/1986), p. 68.</ref>
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::''The motive power of heat is independent of the agents employed to realize it; its quantity is fixed solely by the temperatures of the bodies between which is effected, finally, the transfer of caloric.''<ref>Carnot, S. (1824/1986), p. 68.</ref>
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The motive power of heat is independent of the agents employed to realize it; its quantity is fixed solely by the temperatures of the bodies between which is effected, finally, the transfer of caloric.
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热的原动力与实现热的媒介无关,热的量完全取决于两个物体之间的温度,最后是热量的传递。
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In modern terms, Carnot's principle may be stated more precisely:
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In modern terms, Carnot's principle may be stated more precisely:
用现代术语,卡诺原理可能更为准确:
用现代术语,卡诺原理可能更为准确:
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::The efficiency of a quasi-static or reversible Carnot cycle depends only on the temperatures of the two heat reservoirs, and is the same, whatever the working substance. A Carnot engine operated in this way is the most efficient possible heat engine using those two temperatures.<ref>[[Clifford Truesdell|Truesdell, C.]] (1980), Chapter 5.</ref><ref>Adkins, C.J. (1968/1983), pp. 56–58.</ref><ref>Münster, A. (1970), p. 11.</ref><ref>Kondepudi, D., [[Ilya Prigogine|Prigogine, I.]] (1998), pp.67–75.</ref><ref>Lebon, G., Jou, D., Casas-Vázquez, J. (2008), p. 10.</ref><ref>Eu, B.C. (2002), pp. 32–35.</ref>
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The efficiency of a quasi-static or reversible Carnot cycle depends only on the temperatures of the two heat reservoirs, and is the same, whatever the working substance. A Carnot engine operated in this way is the most efficient possible heat engine using those two temperatures.
准静态卡诺循环或可逆卡诺循环的效率只取决于两种热源的温度,而且无论工作物质是什么,效率是相同的。使用两个热源与工作物质交换热源(一个高温热源温度<math>T_1</math>和一个低温热源温度<math>T_2</math>)的卡诺热机是最有效的热机。<ref>[[Clifford Truesdell|Truesdell, C.]] (1980), Chapter 5.</ref><ref>Adkins, C.J. (1968/1983), pp. 56–58.</ref><ref>Münster, A. (1970), p. 11.</ref><ref>Kondepudi, D., [[Ilya Prigogine|Prigogine, I.]] (1998), pp.67–75.</ref><ref>Lebon, G., Jou, D., Casas-Vázquez, J. (2008), p. 10.</ref><ref>Eu, B.C. (2002), pp. 32–35.</ref>
'''<font color="#32CD32">使用两个热源与工作物质交换热源(一个高温热源温度<math>T_1</math>和一个低温热源温度<math>T_2</math>)的卡诺热机是最有效的热机。 A Carnot engine operated in this way is the most efficient possible heat engine using those two temperatures.</font>'''
'''<font color="#32CD32">使用两个热源与工作物质交换热源(一个高温热源温度<math>T_1</math>和一个低温热源温度<math>T_2</math>)的卡诺热机是最有效的热机。 A Carnot engine operated in this way is the most efficient possible heat engine using those two temperatures.</font>'''
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The German scientist [[Rudolf Clausius]] laid the foundation for the second law of thermodynamics in 1850 by examining the relation between heat transfer and work.{{sfnp|Clausius|1850}} His formulation of the second law, which was published in German in 1854, is known as the ''Clausius statement'':
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The German scientist Rudolf Clausius laid the foundation for the second law of thermodynamics in 1850 by examining the relation between heat transfer and work. His formulation of the second law, which was published in German in 1854, is known as the Clausius statement:
1850年,德国科学家'''鲁道夫·克劳修斯 Rudolf Clausius''' 通过研究热传递和功之间的关系,为热力学第二定律奠定了基础。他在1854年用德语发表的论文中所提及的热力学第二定律定义被称为克劳修斯表述:
1850年,德国科学家'''鲁道夫·克劳修斯 Rudolf Clausius''' 通过研究热传递和功之间的关系,为热力学第二定律奠定了基础。他在1854年用德语发表的论文中所提及的热力学第二定律定义被称为克劳修斯表述:
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<blockquote>Heat can never pass from a colder to a warmer body without some other change, connected therewith, occurring at the same time.{{sfnp|Clausius|1854|p=86}}</blockquote>
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<blockquote>Heat can never pass from a colder to a warmer body without some other change, connected therewith, occurring at the same time.</blockquote>
不可能把热从低温物体传递到高温物体而不产生其他影响。
不可能把热从低温物体传递到高温物体而不产生其他影响。
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The statement by Clausius uses the concept of 'passage of heat'. As is usual in thermodynamic discussions, this means 'net transfer of energy as heat', and does not refer to contributory transfers one way and the other.
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The statement by Clausius uses the concept of 'passage of heat'. As is usual in thermodynamic discussions, this means 'net transfer of energy as heat', and does not refer to contributory transfers one way and the other.
克劳修斯的表述使用了“'''<font color = '#ff8000'>热通道Passage Of Heat</font>'''”的概念。
克劳修斯的表述使用了“'''<font color = '#ff8000'>热通道Passage Of Heat</font>'''”的概念。
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Heat cannot spontaneously flow from cold regions to hot regions without external work being performed on the system, which is evident from ordinary experience of [[refrigeration]], for example. In a refrigerator, heat flows from cold to hot, but only when forced by an external agent, the refrigeration system.
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Heat cannot spontaneously flow from cold regions to hot regions without external work being performed on the system, which is evident from ordinary experience of refrigeration, for example. In a refrigerator, heat flows from cold to hot, but only when forced by an external agent, the refrigeration system.
::It is impossible for a self-acting machine, unaided by any external agency, to convey heat from one body to another at a higher temperature.
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It is impossible for a self-acting machine, unaided by any external agency, to convey heat from one body to another at a higher temperature.
不可能从单一热源取热使之完全转换为有用的功而不产生其他影响。
不可能从单一热源取热使之完全转换为有用的功而不产生其他影响。
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::It is impossible, by means of inanimate material agency, to derive mechanical effect from any portion of matter by cooling it below the temperature of the coldest of the surrounding objects.{{sfnp|Thomson|1851}}
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It is impossible, by means of inanimate material agency, to derive mechanical effect from any portion of matter by cooling it below the temperature of the coldest of the surrounding objects.
不可能通过无生命物质的作用,将物质的任何部分冷却到低于周围物体最低的温度并产生'''<font color = '#ff8000'>机械效应 Mechanical Effect</font>'''。
不可能通过无生命物质的作用,将物质的任何部分冷却到低于周围物体最低的温度并产生'''<font color = '#ff8000'>机械效应 Mechanical Effect</font>'''。
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Suppose there is an engine violating the Kelvin statement: i.e., one that drains heat and converts it completely into work in a cyclic fashion without any other result. Now pair it with a reversed [[Carnot engine]] as shown by the figure. The [[Heat engine#Efficiency|efficiency]] of a normal heat engine is η and so the efficiency of the reversed heat engine is 1/η. The net and sole effect of the combined pair of engines is to transfer heat <math>\Delta Q=Q\left(\frac{1}{\eta}-1\right)</math> from the cooler reservoir to the hotter one, which violates the Clausius statement. (This is a consequence of the [[first law of thermodynamics]], as for the total system's energy to remain the same, <math> \text{Input}+\text{Output}=0 \implies Q-\frac{Q}{\eta} = -Q_c </math>, so therefore <math> Q_c=Q\left( \frac{1}{\eta}-1\right) </math> ). Thus a violation of the Kelvin statement implies a violation of the Clausius statement, i.e. the Clausius statement implies the Kelvin statement. We can prove in a similar manner that the Kelvin statement implies the Clausius statement, and hence the two are equivalent.
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Suppose there is an engine violating the Kelvin statement: i.e., one that drains heat and converts it completely into work in a cyclic fashion without any other result. Now pair it with a reversed Carnot engine as shown by the figure. The efficiency of a normal heat engine is η and so the efficiency of the reversed heat engine is 1/η. The net and sole effect of the combined pair of engines is to transfer heat from <math>\Delta Q=Q\left(\frac{1}{\eta}-1\right)</math> the cooler reservoir to the hotter one, which violates the Clausius statement. (This is a consequence of the first law of thermodynamics, as for the total system's energy to remain the same, <math> \text{Input}+\text{Output}=0 \implies Q-\frac{Q}{\eta} = -Q_c </math>, so therefore <math> Q_c=Q\left( \frac{1}{\eta}-1\right) </math> ). Thus a violation of the Kelvin statement implies a violation of the Clausius statement, i.e. the Clausius statement implies the Kelvin statement. We can prove in a similar manner that the Kelvin statement implies the Clausius statement, and hence the two are equivalent.
Planck offered the following proposition as derived directly from experience. This is sometimes regarded as his statement of the second law, but he regarded it as a starting point for the derivation of the second law.
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Planck offered the following proposition as derived directly from experience. This is sometimes regarded as his statement of the second law, but he regarded it as a starting point for the derivation of the second law.
::It is impossible to construct an engine which will work in a complete cycle, and produce no effect except the raising of a weight and cooling of a heat reservoir.<ref>[[Max Planck|Planck, M.]] (1897/1903), p. 86.</ref><ref>Roberts, J.K., Miller, A.R. (1928/1960), p. 319.</ref>
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不可能建造一台发动机,使其在一个完整的循环中工作,并且除了提高重量和冷却热储以外不会产生任何效果。<ref>[[Max Planck|Planck, M.]] (1897/1903), p. 86.</ref><ref>Roberts, J.K., Miller, A.R. (1928/1960), p. 319.</ref>
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It is impossible to construct an engine which will work in a complete cycle, and produce no effect except the raising of a weight and cooling of a heat reservoir.
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不可能建造一台发动机,使其在一个完整的循环中工作,并且除了提高重量和冷却热储以外不会产生任何效果。
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===Relation between Kelvin's statement and Planck's proposition 开尔文表述与普朗克命题的关系===
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===Relation between Kelvin's statement and Planck's proposition 开尔文表述与普朗克命题的关系===
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教科书中几乎总是用“'''<font color = '#ff8000'>开尔文-普朗克表述 Kelvin-Planck Statement</font>'''”来称呼该定律,例如'''<font color = '#ff8000'>德克·特哈尔 Diek ter Haar</font>''' 和'''<font color = '#ff8000'>哈拉尔德·沃格兰 Harald Wergeland</font>''' 就是这样表述的。<ref>[[Dirk ter Haar|ter Haar, D.]], [[Harald Wergeland|Wergeland, H.]] (1966), p. 17.</ref>
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It is almost customary in textbooks to speak of the "[[Kelvin-Planck statement]]" of the law, as for example in the text by [[Dirk ter Haar|ter Haar]] and [[Harald Wergeland|Wergeland]].<ref>[[Dirk ter Haar|ter Haar, D.]], [[Harald Wergeland|Wergeland, H.]] (1966), p. 17.</ref>
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It is almost customary in textbooks to speak of the "Kelvin-Planck statement" of the law, as for example in the text by ter Haar and Wergeland.
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教科书中几乎总是用“'''<font color = '#ff8000'>开尔文-普朗克表述 Kelvin-Planck Statement</font>'''”来称呼该定律,例如'''<font color = '#ff8000'>德克·特哈尔 Diek ter Haar</font>''' 和'''<font color = '#ff8000'>哈拉尔德·沃格兰 Harald Wergeland</font>''' 就是这样表述的。
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热力学第二定律的开尔文-普朗克表述(或称“'''<font color = '#ff8000'>热机表述 Heat Engine Statement</font>'''”)指出
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The '''Kelvin–Planck statement''' (or the ''heat engine statement'') of the second law of thermodynamics states that
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设计一种唯一效果是从单一热源吸收热并提供等量的功的循环运行装置是不可能的。<ref name="Rao">{{cite book|last=Rao|first=Y. V. C.|title=Chemical Engineering Thermodynamics|publisher=Universities Press|isbn=978-81-7371-048-3|page=158|year=1997}}</ref>
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The Kelvin–Planck statement (or the heat engine statement) of the second law of thermodynamics states that
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===Planck's statement 普朗克表述===
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热力学第二定律的开尔文-普朗克表述(或称“'''<font color = '#ff8000'>热机表述 Heat Engine Statement</font>'''”)指出
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::It is impossible to devise a [[thermodynamic cycle|cyclically]] operating device, the sole effect of which is to absorb energy in the form of heat from a single [[heat reservoir|thermal reservoir]] and to deliver an equivalent amount of [[Work (physics)|work]].<ref name="Rao">{{cite book|last=Rao|first=Y. V. C.|title=Chemical Engineering Thermodynamics|publisher=Universities Press|isbn=978-81-7371-048-3|page=158|year=1997}}</ref>
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It is impossible to devise a cyclically operating device, the sole effect of which is to absorb energy in the form of heat from a single thermal reservoir and to deliver an equivalent amount of work.
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普朗克表述第二定律如下。
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设计一种唯一效果是从单一热源吸收热并提供等量的功的循环运行装置是不可能的。
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===Planck's statement 普朗克表述===
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自然界中发生的任一过程都是沿参与其中的所有物体的熵之和增加的方向进行的。在极限情况中,即对于可逆过程,熵的总和保持不变。<ref name="Planck 100">[[Max Planck|Planck, M.]] (1897/1903), p. 100.</ref><ref name="Planck 463">[[Max Planck|Planck, M.]] (1926), p. 463, translation by Uffink, J. (2003), p. 131.</ref><ref name="Roberts & Miller 382">Roberts, J.K., Miller, A.R. (1928/1960), p. 382. This source is partly verbatim from Planck's statement, but does not cite Planck. This source calls the statement the principle of the increase of entropy.</ref>
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Planck stated the second law as follows.
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Planck stated the second law as follows.
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普朗克表述第二定律如下。
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::Every process occurring in nature proceeds in the sense in which the sum of the entropies of all bodies taking part in the process is increased. In the limit, i.e. for reversible processes, the sum of the entropies remains unchanged.<ref name="Planck 100">[[Max Planck|Planck, M.]] (1897/1903), p. 100.</ref><ref name="Planck 463">[[Max Planck|Planck, M.]] (1926), p. 463, translation by Uffink, J. (2003), p. 131.</ref><ref name="Roberts & Miller 382">Roberts, J.K., Miller, A.R. (1928/1960), p. 382. This source is partly verbatim from Planck's statement, but does not cite Planck. This source calls the statement the principle of the increase of entropy.</ref>
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Every process occurring in nature proceeds in the sense in which the sum of the entropies of all bodies taking part in the process is increased. In the limit, i.e. for reversible processes, the sum of the entropies remains unchanged.
与普朗克表述非常相似的是'''<font color = '#ff8000'>乌伦贝克 Uhlenbeck</font>'''和'''<font color = '#ff8000'>福特 Ford</font>'''关于不可逆现象的表述。
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Rather like Planck's statement is that of Uhlenbeck and Ford for ''irreversible phenomena''.
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Rather like Planck's statement is that of Uhlenbeck and Ford for irreversible phenomena.
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与普朗克表述非常相似的是'''<font color = '#ff8000'>乌伦贝克 Uhlenbeck</font>'''和'''<font color = '#ff8000'>福特 Ford</font>'''关于不可逆现象的表述。
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……在从一个平衡态到另一个平衡态的不可逆或自发的变化中(例如,当两个物体 A 和 B 接触时的温度平衡过程),熵总是增加。<ref>[[George Uhlenbeck|Uhlenbeck, G.E.]], Ford, G.W. (1963), p. 16.</ref>
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::... in an irreversible or spontaneous change from one equilibrium state to another (as for example the equalization of temperature of two bodies A and B, when brought in contact) the entropy always increases.<ref>[[George Uhlenbeck|Uhlenbeck, G.E.]], Ford, G.W. (1963), p. 16.</ref>
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... in an irreversible or spontaneous change from one equilibrium state to another (as for example the equalization of temperature of two bodies A and B, when brought in contact) the entropy always increases.
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……在从一个平衡态到另一个平衡态的不可逆或自发的变化中(例如,当两个物体 A 和 B 接触时的温度平衡过程),熵总是增加。
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—— caratheodory 的原理在这里重新定向——
—— caratheodory 的原理在这里重新定向——
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[[Constantin Carathéodory]] formulated thermodynamics on a purely mathematical axiomatic foundation. His statement of the second law is known as the Principle of Carathéodory, which may be formulated as follows:<ref>[[Constantin Carathéodory|Carathéodory, C.]] (1909).</ref>
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Constantin Carathéodory formulated thermodynamics on a purely mathematical axiomatic foundation. His statement of the second law is known as the Principle of Carathéodory, which may be formulated as follows:
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'''<font color = '#ff8000'>康斯坦丁·卡拉西奥多里 Constantin Carathéodory</font>'''在纯数学公理的基础上进行了热力学'''<font color = '#ff8000'>公理化formulated</font>'''阐明。他对第二定律的陈述被称为'''<font color = '#ff8000'>卡拉西奥多里原理 Principle of Carathéodory</font>''',可以这样表述:<ref>[[Constantin Carathéodory|Carathéodory, C.]] (1909).</ref>
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'''<font color = '#ff8000'>康斯坦丁·卡拉西奥多里 Constantin Carathéodory</font>'''在纯数学公理的基础上进行了热力学'''<font color = '#ff8000'>公理化formulated</font>'''阐明。他对第二定律的陈述被称为'''<font color = '#ff8000'>卡拉西奥多里原理 Principle of Carathéodory</font>''',可以这样表述:
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<blockquote>In every neighborhood of any state S of an adiabatically enclosed system there are states inaccessible from S.<ref>Buchdahl, H.A. (1966), p. 68.</ref></blockquote>
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在绝热封闭系统的任意状态 S 附近,总有从 S 出发不可达的状态。<ref>Buchdahl, H.A. (1966), p. 68.</ref>
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<blockquote>In every neighborhood of any state S of an adiabatically enclosed system there are states inaccessible from S.</blockquote>
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在绝热封闭系统的任意状态 S 附近,总有从 S 出发不可达的状态。
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通过这个阐明,他首次描述了'''<font color = '#ff8000'>绝热可达性 Adiabatic Accessibility</font>'''的概念,并为经典热力学的一个新的子领域,即通常所说的'''<font color = '#ff8000'>几何热力学 Geometrical Thermodynamics</font>'''奠定了基础。由卡拉西奥多里原理可以推出,作为热的能量的准静态转移是一个'''<font color="#ff8000"> 完整的过程函数holonomic process function</font>'''即<math>\delta Q=TdS</math>。<ref name="Sychev1991">{{cite book |last=Sychev |first=V. V. |title=The Differential Equations of Thermodynamics |year=1991 |publisher=Taylor & Francis |isbn=978-1-56032-121-7}}</ref>
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With this formulation, he described the concept of [[adiabatic accessibility]] for the first time and provided the foundation for a new subfield of classical thermodynamics, often called [[Ruppeiner geometry|geometrical thermodynamics]]. It follows from Carathéodory's principle that quantity of energy quasi-statically transferred as heat is a holonomic [[process function]], in other words, <math>\delta Q=TdS</math>.<ref name="Sychev1991">{{cite book |last=Sychev |first=V. V. |title=The Differential Equations of Thermodynamics |year=1991 |publisher=Taylor & Francis |isbn=978-1-56032-121-7}}</ref> {{clarify|date=February 2014}}
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With this formulation, he described the concept of adiabatic accessibility for the first time and provided the foundation for a new subfield of classical thermodynamics, often called geometrical thermodynamics. It follows from Carathéodory's principle that quantity of energy quasi-statically transferred as heat is a holonomic process function, in other words, <math>\delta Q=TdS</math>.
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通过这个阐明,他首次描述了'''<font color = '#ff8000'>绝热可达性 Adiabatic Accessibility</font>'''的概念,并为经典热力学的一个新的子领域,即通常所说的'''<font color = '#ff8000'>几何热力学 Geometrical Thermodynamics</font>'''奠定了基础。由卡拉西奥多里原理可以推出,作为热的能量的准静态转移是一个'''<font color="#ff8000"> 完整的过程函数holonomic process function</font>'''即<math>\delta Q=TdS</math>。
Though it is almost customary in textbooks to say that Carathéodory's principle expresses the second law and to treat it as equivalent to the Clausius or to the Kelvin-Planck statements, such is not the case. To get all the content of the second law, Carathéodory's principle needs to be supplemented by Planck's principle, that isochoric work always increases the internal energy of a closed system that was initially in its own internal thermodynamic equilibrium.<ref name="Munster 45">Münster, A. (1970), p. 45.</ref>{{sfnp|Lieb|Yngvason|1999|p=49}}<ref name="Planck 1926">[[Max Planck|Planck, M.]] (1926).</ref><ref>Buchdahl, H.A. (1966), p. 69.</ref> {{clarify|date=February 2014}}
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Though it is almost customary in textbooks to say that Carathéodory's principle expresses the second law and to treat it as equivalent to the Clausius or to the Kelvin-Planck statements, such is not the case. To get all the content of the second law, Carathéodory's principle needs to be supplemented by Planck's principle, that isochoric work always increases the internal energy of a closed system that was initially in its own internal thermodynamic equilibrium.
尽管在教科书几乎惯称卡拉西奥多里原理也是第二定律的一种表述,并认为其与克劳修斯表述或开尔文-普朗克表述等价,但事实并非如此。为了得到第二定律的所有内容,需要对卡拉西奥多里原理补充普朗克表述,即等量功总是增加一个最初处于自身内部热力学平衡的封闭系统的内部能量。<ref name="Munster 45">Münster, A. (1970), p. 45.</ref>{{sfnp|Lieb|Yngvason|1999|p=49}}<ref name="Planck 1926">[[Max Planck|Planck, M.]] (1926).</ref><ref>Buchdahl, H.A. (1966), p. 69.</ref>
===Planck's principle 普朗克原理===
===Planck's principle 普朗克原理===
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In 1926, [[Max Planck]] wrote an important paper on the basics of thermodynamics.<ref name="Planck 1926"/><ref>Uffink, J. (2003), pp. 129–132.</ref> He indicated the principle
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In 1926, Max Planck wrote an important paper on the basics of thermodynamics. He indicated the principle
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1926年,'''<font color = '#ff8000'>马克斯·普朗克 Max Planck</font>'''写了一篇关于热力学基础的重要论文。他指出了以下原理
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1926年,'''<font color = '#ff8000'>马克斯·普朗克 Max Planck</font>'''写了一篇关于热力学基础的重要论文。<ref name="Planck 1926"/><ref>Uffink, J. (2003), pp. 129–132.</ref> 他指出了以下原理
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::The internal energy of a closed system is increased by an adiabatic process, throughout the duration of which, the volume of the system remains constant.<ref name="Munster 45"/>{{sfnp |Lieb|Yngvason|1999|p=49}}
The internal energy of a closed system is increased by an adiabatic process, throughout the duration of which, the volume of the system remains constant.
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一个封闭系统的内部能量因绝热过程增加,在整个过程中,系统的体积保持不变。
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这个公式没有提到热,没有提到温度,甚至没有提到熵,也不一定隐含地依赖于这些概念,但它暗示了第二定律的内容。一个密切相关的表述为,“摩擦力从来不做正功。”<ref>[[Clifford Truesdell|Truesdell, C.]], Muncaster, R.G. (1980). ''Fundamentals of Maxwell's Kinetic Theory of a Simple Monatomic Gas, Treated as a Branch of Rational Mechanics'', Academic Press, New York, {{ISBN|0-12-701350-4}}, p. 15.</ref>普朗克写道: “摩擦生热是不可逆的。”<ref>[[Max Planck|Planck, M.]] (1897/1903), p. 81.</ref><ref>[[Max Planck|Planck, M.]] (1926), p. 457, Wikipedia editor's translation.</ref>
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This formulation does not mention heat and does not mention temperature, nor even entropy, and does not necessarily implicitly rely on those concepts, but it implies the content of the second law. A closely related statement is that "Frictional pressure never does positive work."<ref>[[Clifford Truesdell|Truesdell, C.]], Muncaster, R.G. (1980). ''Fundamentals of Maxwell's Kinetic Theory of a Simple Monatomic Gas, Treated as a Branch of Rational Mechanics'', Academic Press, New York, {{ISBN|0-12-701350-4}}, p. 15.</ref> Planck wrote: "The production of heat by friction is irreversible."<ref>[[Max Planck|Planck, M.]] (1897/1903), p. 81.</ref><ref>[[Max Planck|Planck, M.]] (1926), p. 457, Wikipedia editor's translation.</ref>
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This formulation does not mention heat and does not mention temperature, nor even entropy, and does not necessarily implicitly rely on those concepts, but it implies the content of the second law. A closely related statement is that "Frictional pressure never does positive work." Planck wrote: "The production of heat by friction is irreversible."
这个普朗克定理没有提到熵,是用物理术语来表述的。它与上面给出的开尔文表述密切相关。<ref>Lieb, E.H., Yngvason, J. (2003), p. 149.</ref>相关的是,对于恒定体积和摩尔数的系统,熵是内能的单调函数。然而,普朗克的这个原理实际上并不是普朗克对第二定律的首选表述(见前面小节),而是依赖于熵的概念。
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Not mentioning entropy, this principle of Planck is stated in physical terms. It is very closely related to the Kelvin statement given just above.<ref>Lieb, E.H., Yngvason, J. (2003), p. 149.</ref> It is relevant that for a system at constant volume and [[Mole (unit)|mole numbers]], the entropy is a monotonic function of the internal energy. Nevertheless, this principle of Planck is not actually Planck's preferred statement of the second law, which is quoted above, in a previous sub-section of the present section of this present article, and relies on the concept of entropy.
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Not mentioning entropy, this principle of Planck is stated in physical terms. It is very closely related to the Kelvin statement given just above. It is relevant that for a system at constant volume and mole numbers, the entropy is a monotonic function of the internal energy. Nevertheless, this principle of Planck is not actually Planck's preferred statement of the second law, which is quoted above, in a previous sub-section of the present section of this present article, and relies on the concept of entropy.
A statement that in a sense is complementary to Planck's principle is made by Borgnakke and Sonntag. They do not offer it as a full statement of the second law:
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A statement that in a sense is complementary to Planck's principle is made by Borgnakke and Sonntag. They do not offer it as a full statement of the second law:
::... there is only one way in which the entropy of a [closed] system can be decreased, and that is to transfer heat from the system.<ref>Borgnakke, C., Sonntag., R.E. (2009), p. 304.</ref>
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... there is only one way in which the entropy of a [closed] system can be decreased, and that is to transfer heat from the system.
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……只有一种方法可以减少(封闭)系统的熵,将热从系统中转移出去。
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……只有一种方法可以减少(封闭)系统的熵,将热从系统中转移出去。<ref>Borgnakke, C., Sonntag., R.E. (2009), p. 304.</ref>
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Differing from Planck's just foregoing principle, this one is explicitly in terms of entropy change. Removal of matter from a system can also decrease its entropy.
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Differing from Planck's just foregoing principle, this one is explicitly in terms of entropy change. Removal of matter from a system can also decrease its entropy.
与普朗克之前提出的原理不同,这一原理明确地用熵的变化来表示。从系统中去除物质也可以减少系统的熵。
与普朗克之前提出的原理不同,这一原理明确地用熵的变化来表示。从系统中去除物质也可以减少系统的熵。
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The second law has been shown to be equivalent to the [[internal energy]] ''U'' being a weakly [[convex function]], when written as a function of extensive properties (mass, volume, entropy, ...).<ref>{{cite book |last1=van Gool |first1=W. |last2=Bruggink |first2=J.J.C. (Eds) |url= |title=Energy and time in the economic and physical sciences |publisher=North-Holland |year=1985 |pages=41–56 |quote= |isbn=978-0-444-87748-2}}</ref><ref>{{Cite journal | last1 = Grubbström | first1 = Robert W. | doi = 10.1016/j.apenergy.2007.01.003 | title = An Attempt to Introduce Dynamics Into Generalised Exergy Considerations| journal = Applied Energy| volume = 84| issue = 7–8 | pages = 701–718 | year = 2007}}</ref> {{clarify|date=February 2014}}
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The second law has been shown to be equivalent to the internal energy U being a weakly convex function, when written as a function of extensive properties (mass, volume, entropy, ...).
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'''<font color="#32CD32">写成广泛性质(质量,体积,熵……)的函数时,第二定律被证明等价于弱凸函数内能 U。The second law has been shown to be equivalent to the internal energy U being a weakly convex function, when written as a function of extensive properties (mass, volume, entropy, ...).</font>'''
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'''<font color="#32CD32">写成广泛性质(质量,体积,熵……)的函数时,第二定律被证明等价于弱凸函数内能 U。The second law has been shown to be equivalent to the internal energy U being a weakly convex function, when written as a function of extensive properties (mass, volume, entropy, ...).</font>'''<ref>{{cite book |last1=van Gool |first1=W. |last2=Bruggink |first2=J.J.C. (Eds) |url= |title=Energy and time in the economic and physical sciences |publisher=North-Holland |year=1985 |pages=41–56 |quote= |isbn=978-0-444-87748-2}}</ref><ref>{{Cite journal | last1 = Grubbström | first1 = Robert W. | doi = 10.1016/j.apenergy.2007.01.003 | title = An Attempt to Introduce Dynamics Into Generalised Exergy Considerations| journal = Applied Energy| volume = 84| issue = 7–8 | pages = 701–718 | year = 2007}}</ref>
Before the establishment of the second law, many people who were interested in inventing a perpetual motion machine had tried to circumvent the restrictions of [[first law of thermodynamics]] by extracting the massive internal energy of the environment as the power of the machine. Such a machine is called a "perpetual motion machine of the second kind". The second law declared the impossibility of such machines.
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* 所有<font color = 'blue'>在两个热源之间工作的</font>不可逆热机的效率低于在<font color = 'red'><s>两相同</s></font><font color = 'blue'>同一个</font>热源之间工作的'''<font color = '#ff8000'>卡诺热机 Carnot Engine</font>'''。
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* 所有<font color = 'blue'>在两个热源之间工作的</font>可逆热机的效率与在<font color = 'red'><s>两相同</s></font><font color = 'blue'>同一个</font>热源之间工作的卡诺机相等。
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Before the establishment of the second law, many people who were interested in inventing a perpetual motion machine had tried to circumvent the restrictions of first law of thermodynamics by extracting the massive internal energy of the environment as the power of the machine. Such a machine is called a "perpetual motion machine of the second kind". The second law declared the impossibility of such machines.
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'''<font color="#32CD32">所有在两个热源之间工作的可逆热机的效率与在两相同热源之间工作的卡诺机相等。All irreversible heat engines between two heat reservoirs are less efficient than a [[Carnot engine]] operating between the same reservoirs.</font>'''
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在第二定律建立之前,许多志在发明永动机的人试图通过提取环境的巨大内能作为机器动力,以突破'''热力学第一定律 First Law of Thermodynamics''' 的限制。这种机器被称为“'''第二类永动机 Perpetual Motion Machine of the Second Kind'''”。热力学第二定律表明这种机器是不可能的。
--[[用户:嘉树|嘉树]]([[用户讨论:嘉树|讨论]])我不太理解什么叫between the same reservoirs。我的理解是效率不取决于热源这个实体,而取决于温差,所以就按照两个热源和一个相同的热源相对应地翻译了。但是这一句我仍然有疑问,因为两个热源之间工作和两相同热源之间工作,似乎还不构成相互比较的关系。已经标绿
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===Carnot theorem 卡诺定理===
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[[Carnot theorem (thermodynamics)|Carnot's theorem]] (1824) is a principle that limits the maximum efficiency for any possible engine. The efficiency solely depends on the temperature difference between the hot and cold thermal reservoirs. Carnot's theorem states:
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Carnot's theorem (1824) is a principle that limits the maximum efficiency for any possible engine. The efficiency solely depends on the temperature difference between the hot and cold thermal reservoirs. Carnot's theorem states:
*All irreversible heat engines between two heat reservoirs are less efficient than a [[Carnot engine]] operating between the same reservoirs.
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*All reversible heat engines between two heat reservoirs are equally efficient with a Carnot engine operating between the same reservoirs.
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* 所有<font color = 'blue'>在两个热源之间工作的</font>不可逆热机的效率低于在<font color = 'red'><s>两相同</s></font><font color = 'blue'>同一个</font>热源之间工作的'''<font color = '#ff8000'>卡诺热机 Carnot Engine</font>'''。
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* 所有<font color = 'blue'>在两个热源之间工作的</font>可逆热机的效率与在<font color = 'red'><s>两相同</s></font><font color = 'blue'>同一个</font>热源之间工作的卡诺机相等。
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'''<font color="#32CD32">所有在两个热源之间工作的可逆热机的效率与在两相同热源之间工作的卡诺机相等。All irreversible heat engines between two heat reservoirs are less efficient than a [[Carnot engine]] operating between the same reservoirs.</font>'''
--[[用户:嘉树|嘉树]]([[用户讨论:嘉树|讨论]])我不太理解什么叫between the same reservoirs。我的理解是效率不取决于热源这个实体,而取决于温差,所以就按照两个热源和一个相同的热源相对应地翻译了。但是这一句我仍然有疑问,因为两个热源之间工作和两相同热源之间工作,似乎还不构成相互比较的关系。已经标绿
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In his ideal model, the heat of caloric converted into work could be reinstated by reversing the motion of the cycle, a concept subsequently known as [[thermodynamic reversibility]]. Carnot, however, further postulated that some caloric is lost, not being converted to mechanical work. Hence, no real heat engine could realise the [[Carnot cycle]]'s reversibility and was condemned to be less efficient.
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In his ideal model, the heat of caloric converted into work could be reinstated by reversing the motion of the cycle, a concept subsequently known as thermodynamic reversibility. Carnot, however, further postulated that some caloric is lost, not being converted to mechanical work. Hence, no real heat engine could realise the Carnot cycle's reversibility and was condemned to be less efficient.
在他的理想模型中,热转化为功的过程可以通过逆转循环的运动而恢复,这个概念后来被称为'''<font color = '#ff8000'>热力学可逆性 Thermodynamic Reversibility</font>'''。然而,卡诺进一步假定,一些热<s>量</s>损失了,并没有转化为机械功。因此,没有一个真实的热机能够实现'''<font color = '#ff8000'>卡诺循环 Carnot Cycle</font>'''的可逆性,并且被认为效率较低。
在他的理想模型中,热转化为功的过程可以通过逆转循环的运动而恢复,这个概念后来被称为'''<font color = '#ff8000'>热力学可逆性 Thermodynamic Reversibility</font>'''。然而,卡诺进一步假定,一些热<s>量</s>损失了,并没有转化为机械功。因此,没有一个真实的热机能够实现'''<font color = '#ff8000'>卡诺循环 Carnot Cycle</font>'''的可逆性,并且被认为效率较低。
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Though formulated in terms of caloric (see the obsolete [[caloric theory]]), rather than [[entropy]], this was an early insight into the second law.
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Though formulated in terms of caloric (see the obsolete caloric theory), rather than entropy, this was an early insight into the second law.
该理论尽管是用热<s>量</s>表述的(见被取代的'''<font color = '#ff8000'>热质说</font>'''),而不是熵,但是它是对第二定律的早期认识。
该理论尽管是用热<s>量</s>表述的(见被取代的'''<font color = '#ff8000'>热质说</font>'''),而不是熵,但是它是对第二定律的早期认识。
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The [[Clausius theorem]] (1854) states that in a cyclic process
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The Clausius theorem (1854) states that in a cyclic process
'''<font color = '#ff8000'>克劳修斯定理 Clausius Theorem</font>'''(1854)指出,在一个循环的过程中
'''<font color = '#ff8000'>克劳修斯定理 Clausius Theorem</font>'''(1854)指出,在一个循环的过程中
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The equality holds in the reversible case<ref>[http://scienceworld.wolfram.com/physics/ClausiusTheorem.html ''Clausius theorem''] at [[Wolfram Research]]</ref> and the strict inequality holds in the irreversible case. The reversible case is used to introduce the state function [[entropy]]. This is because in cyclic processes the variation of a state function is zero from state functionality.
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The equality holds in the reversible case and the strict inequality holds in the irreversible case. The reversible case is used to introduce the state function entropy. This is because in cyclic processes the variation of a state function is zero from state functionality.
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等号在可逆情况下成立,严格不等号在不可逆情况下成立。可逆情况下引入状态函数熵。'''<font color="#32CD32">这是因为在循环过程中,状态功能的变化相对于状态功能为零。This is because in cyclic processes the variation of a state function is zero from state functionality.</font>'''
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等号在可逆情况下成立,<ref>[http://scienceworld.wolfram.com/physics/ClausiusTheorem.html ''Clausius theorem''] at [[Wolfram Research]]</ref>严格不等号在不可逆情况下成立。可逆情况下引入状态函数熵。'''<font color="#32CD32">这是因为在循环过程中,状态功能的变化相对于状态功能为零。This is because in cyclic processes the variation of a state function is zero from state functionality.</font>'''
[[Carnot theorem (thermodynamics)|Carnot's theorem]] states that all reversible engines operating between the same heat reservoirs are equally efficient.
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Carnot's theorem states that all reversible engines operating between the same heat reservoirs are equally efficient.
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卡诺定理指出,所有在相同热源间运行的可逆热机的效率是相同的。
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Thus, any reversible heat engine operating between temperatures ''T''<sub>1</sub> and ''T''<sub>2</sub> must have the same efficiency, that is to say, the efficiency is the function of temperatures only:
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Thus, any reversible heat engine operating between temperatures T<sub>1</sub> and T<sub>2</sub> must have the same efficiency, that is to say, the efficiency is the function of temperatures only:
In addition, a reversible heat engine operating between temperatures ''T''<sub>1</sub> and ''T''<sub>3</sub> must have the same efficiency as one consisting of two cycles, one between ''T''<sub>1</sub> and another (intermediate) temperature ''T''<sub>2</sub>, and the second between ''T''<sub>2</sub> and''T''<sub>3</sub>. This can only be the case if
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In addition, a reversible heat engine operating between temperatures T<sub>1</sub> and T<sub>3</sub> must have the same efficiency as one consisting of two cycles, one between T<sub>1</sub> and another (intermediate) temperature T<sub>2</sub>, and the second between T<sub>2</sub> andT<sub>3</sub>. This can only be the case if
Now consider the case where <math>T_1</math> is a fixed reference temperature: the temperature of the [[triple point]] of water. Then for any ''T''<sub>2</sub> and ''T''<sub>3</sub>,
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Now consider the case where <math>T_1</math> is a fixed reference temperature: the temperature of the triple point of water. Then for any T<sub>2</sub> and T<sub>3</sub>,
Therefore, if thermodynamic temperature is defined by
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Therefore, if thermodynamic temperature is defined by
因此,如果热力学温度被定义为
因此,如果热力学温度被定义为
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then the function ''f'', viewed as a function of thermodynamic temperature, is simply
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then the function f, viewed as a function of thermodynamic temperature, is simply
那么函数 ''f'' 作为热力学温度的函数,为
那么函数 ''f'' 作为热力学温度的函数,为
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and the reference temperature ''T''<sub>1</sub> will have the value 273.16. (Any reference temperature and any positive numerical value could be used{{snd}}the choice here corresponds to the [[Kelvin]] scale.)
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and the reference temperature T<sub>1</sub> will have the value 273.16. (Any reference temperature and any positive numerical value could be used the choice here corresponds to the Kelvin scale.)
So we can define a state function S called entropy, which for a reversible process or for pure heat transfer<ref name="Schmidt-Rohr 14" /> satisfies
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So we can define a state function S called entropy, which for a reversible process or for pure heat transfer satisfies
所以我们可以定义一个叫做熵的状态函数 S,对于可逆过程或者纯热传递满足
所以我们可以定义一个叫做熵的状态函数 S,对于可逆过程或者纯热传递满足
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With this we can only obtain the difference of entropy by integrating the above formula. To obtain the absolute value, we need the [[third law of thermodynamics]], which states that ''S'' = 0 at [[absolute zero]] for perfect crystals.
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With this we can only obtain the difference of entropy by integrating the above formula. To obtain the absolute value, we need the third law of thermodynamics, which states that S = 0 at absolute zero for perfect crystals.
据此,只有对上述公式进行积分,才能得到熵的差值。为了获得绝对值,我们需要<font color="#ff8000">'''热力学第三定律 Third Law of Thermodynamics'''</font>,它指出<font color="#ff8000">'''绝对零度 Absolute Zero'''</font>下完美晶体的 ''S'' = 0。
据此,只有对上述公式进行积分,才能得到熵的差值。为了获得绝对值,我们需要<font color="#ff8000">'''热力学第三定律 Third Law of Thermodynamics'''</font>,它指出<font color="#ff8000">'''绝对零度 Absolute Zero'''</font>下完美晶体的 ''S'' = 0。
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For any irreversible process, since entropy is a state function, we can always connect the initial and terminal states with an imaginary reversible process and integrating on that path to calculate the difference in entropy.
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For any irreversible process, since entropy is a state function, we can always connect the initial and terminal states with an imaginary reversible process and integrating on that path to calculate the difference in entropy.
An important and revealing idealized special case is to consider applying the Second Law to the scenario of an isolated system (called the total system or universe), made up of two parts: a sub-system of interest, and the sub-system's surroundings. These surroundings are imagined to be so large that they can be considered as an ''unlimited'' heat reservoir at temperature ''T<sub>R</sub>'' and pressure ''P<sub>R</sub>'' {{snd}}so that no matter how much heat is transferred to (or from) the sub-system, the temperature of the surroundings will remain ''T<sub>R</sub>''; and no matter how much the volume of the sub-system expands (or contracts), the pressure of the surroundings will remain ''P<sub>R</sub>''.
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An important and revealing idealized special case is to consider applying the Second Law to the scenario of an isolated system (called the total system or universe), made up of two parts: a sub-system of interest, and the sub-system's surroundings. These surroundings are imagined to be so large that they can be considered as an unlimited heat reservoir at temperature T<sub>R</sub> and pressure P<sub>R</sub> so that no matter how much heat is transferred to (or from) the sub-system, the temperature of the surroundings will remain T<sub>R</sub>; and no matter how much the volume of the sub-system expands (or contracts), the pressure of the surroundings will remain P<sub>R</sub>.
Whatever changes to ''dS'' and ''dS<sub>R</sub>'' occur in the entropies of the sub-system and the surroundings individually, according to the Second Law the entropy ''S<sub>tot</sub>'' of the isolated total system must not decrease:
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Whatever changes to dS and dS<sub>R</sub> occur in the entropies of the sub-system and the surroundings individually, according to the Second Law the entropy S<sub>tot</sub> of the isolated total system must not decrease:
According to the [[first law of thermodynamics]], the change ''dU'' in the internal energy of the sub-system is the sum of the heat ''δq'' added to the sub-system, ''less'' any work ''δw'' done ''by'' the sub-system, ''plus'' any net chemical energy entering the sub-system ''d ∑μ<sub>iR</sub>N<sub>i</sub>'', so that:
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According to the first law of thermodynamics, the change dU in the internal energy of the sub-system is the sum of the heat δq added to the sub-system, less any work δw done by the sub-system, plus any net chemical energy entering the sub-system d ∑μ<sub>iR</sub>N<sub>i</sub>, so that:
根据热力学第一定律,子系统内能的变化 dU 是加在子系统上的热δq的和<font color = 'blue'></font>,减去子系统所做的任何功w,再加上进入子系统的任何净化学能 d ∑μ<sub>iR</sub>N<sub>i</sub>,因此
根据热力学第一定律,子系统内能的变化 dU 是加在子系统上的热δq的和<font color = 'blue'></font>,减去子系统所做的任何功w,再加上进入子系统的任何净化学能 d ∑μ<sub>iR</sub>N<sub>i</sub>,因此
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where μ<sub>iR</sub> are the [[chemical potential]]s of chemical species in the external surroundings.
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where μ<sub>iR</sub> are the chemical potentials of chemical species in the external surroundings.
其中μ<sub>iR</sub>是外部环境中'''<font color = '#ff8000'>化学形态 chemical species</font>'''的化学势。
其中μ<sub>iR</sub>是外部环境中'''<font color = '#ff8000'>化学形态 chemical species</font>'''的化学势。
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Now the heat leaving the reservoir and entering the sub-system is
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Now the heat leaving the reservoir and entering the sub-system is
where we have first used the definition of entropy in classical thermodynamics (alternatively, in statistical thermodynamics, the relation between entropy change, temperature and absorbed heat can be derived); and then the Second Law inequality from above.
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where we have first used the definition of entropy in classical thermodynamics (alternatively, in statistical thermodynamics, the relation between entropy change, temperature and absorbed heat can be derived); and then the Second Law inequality from above.
在这个过程中,首先使用了经典热力学中熵的定义(在统计热力学中,熵变、温度和吸收热量之间的关系'''<font color = '#32CD32'>可以将其推导出来 can be derived</font>''') ,然后从上面的公式可以推导出第二定律的不等式。
在这个过程中,首先使用了经典热力学中熵的定义(在统计热力学中,熵变、温度和吸收热量之间的关系'''<font color = '#32CD32'>可以将其推导出来 can be derived</font>''') ,然后从上面的公式可以推导出第二定律的不等式。
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It therefore follows that any net work ''δw'' done by the sub-system must obey
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It therefore follows that any net work δw done by the sub-system must obey
因此,子系统所做的任何净功δw必须服从
因此,子系统所做的任何净功δw必须服从
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: <math> \delta w \le - dU + T_R dS + \sum \mu_{iR} dN_i \,</math>
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<math> \delta w \le - dU + T_R dS + \sum \mu_{iR} dN_i \,</math>
数学增量 w le-dU + tds + sum mu { iR } dN i,/ math
数学增量 w le-dU + tds + sum mu { iR } dN i,/ math
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It is useful to separate the work ''δw'' done by the subsystem into the ''useful'' work ''δw<sub>u</sub>'' that can be done ''by'' the sub-system, over and beyond the work ''p<sub>R</sub> dV'' done merely by the sub-system expanding against the surrounding external pressure, giving the following relation for the useful work (exergy) that can be done:
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It is useful to separate the work δw done by the subsystem into the useful work δw<sub>u</sub> that can be done by the sub-system, over and beyond the work p<sub>R</sub> dV done merely by the sub-system expanding against the surrounding external pressure, giving the following relation for the useful work (exergy) that can be done:
将子系统所做的功δw划分为子系统可以完成的有用功δw<sub>u</sub> ,除了子系统在周围外部压力下膨胀所做的功p<sub>R</sub> dV外,给出以下可用功('''<font color = 'ff8000'>有用能 exergy</font>''')关系式:
将子系统所做的功δw划分为子系统可以完成的有用功δw<sub>u</sub> ,除了子系统在周围外部压力下膨胀所做的功p<sub>R</sub> dV外,给出以下可用功('''<font color = 'ff8000'>有用能 exergy</font>''')关系式:
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It is convenient to define the right-hand-side as the exact derivative of a thermodynamic potential, called the ''availability'' or ''[[exergy]]'' ''E'' of the subsystem,
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It is convenient to define the right-hand-side as the exact derivative of a thermodynamic potential, called the availability or exergy E of the subsystem,
为方便起见,可以把右边定义为热力学势的精确导数,称为子系统的'''<font color = 'ff8000'>可用性 Availability </font>'''或'''<font color = 'ff8000'>有用能 exergy</font>'''
为方便起见,可以把右边定义为热力学势的精确导数,称为子系统的'''<font color = 'ff8000'>可用性 Availability </font>'''或'''<font color = 'ff8000'>有用能 exergy</font>'''
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The Second Law therefore implies that for any process which can be considered as divided simply into a subsystem, and an unlimited temperature and pressure reservoir with which it is in contact,
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The Second Law therefore implies that for any process which can be considered as divided simply into a subsystem, and an unlimited temperature and pressure reservoir with which it is in contact,
<font color="#32CD32">因此,第二定律意味着,对于任何可以简单地被视为分为一个子系统和一个与之接触的无限温度和压力'''<font color="#ff8000">热源 Reservoir</font>''' 的过程,The Second Law therefore implies that for any process which can be considered as divided simply into a subsystem, and an unlimited temperature and pressure reservoir with which it is in contact,</font>
<font color="#32CD32">因此,第二定律意味着,对于任何可以简单地被视为分为一个子系统和一个与之接触的无限温度和压力'''<font color="#ff8000">热源 Reservoir</font>''' 的过程,The Second Law therefore implies that for any process which can be considered as divided simply into a subsystem, and an unlimited temperature and pressure reservoir with which it is in contact,</font>
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i.e. the change in the subsystem's exergy plus the useful work done ''by'' the subsystem (or, the change in the subsystem's exergy less any work, additional to that done by the pressure reservoir, done ''on'' the system) must be less than or equal to zero.
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i.e. the change in the subsystem's exergy plus the useful work done by the subsystem (or, the change in the subsystem's exergy less any work, additional to that done by the pressure reservoir, done on the system) must be less than or equal to zero.
也就是。子系统有用能的变化加上子系统所做的有用功(或者,子系统有用能的变化减去除了'''<font color = '#ff8000'>压力热源</font>'''外任何对系统做的功</font>)必须小于或等于零。
也就是。子系统有用能的变化加上子系统所做的有用功(或者,子系统有用能的变化减去除了'''<font color = '#ff8000'>压力热源</font>'''外任何对系统做的功</font>)必须小于或等于零。
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In sum, if a proper ''infinite-reservoir-like'' reference state is chosen as the system surroundings in the real world, then the Second Law predicts a decrease in ''E'' for an irreversible process and no change for a reversible process.
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In sum, if a proper infinite-reservoir-like reference state is chosen as the system surroundings in the real world, then the Second Law predicts a decrease in E for an irreversible process and no change for a reversible process.
总之,如果选择一个合适的类似于无限库的参考状态作为现实世界中的系统环境,
总之,如果选择一个合适的类似于无限库的参考状态作为现实世界中的系统环境,
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This expression together with the associated reference state permits a [[design engineer]] working at the macroscopic scale (above the [[thermodynamic limit]]) to utilize the Second Law without directly measuring or considering entropy change in a total isolated system. (''Also, see [[process engineer]]''). Those changes have already been considered by the assumption that the system under consideration can reach equilibrium with the reference state without altering the reference state. An efficiency for a process or collection of processes that compares it to the reversible ideal may also be found (''See [[Exergy efficiency|second law efficiency]]''.)
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This expression together with the associated reference state permits a design engineer working at the macroscopic scale (above the thermodynamic limit) to utilize the Second Law without directly measuring or considering entropy change in a total isolated system. (Also, see process engineer). Those changes have already been considered by the assumption that the system under consideration can reach equilibrium with the reference state without altering the reference state. An efficiency for a process or collection of processes that compares it to the reversible ideal may also be found (See second law efficiency.)
这个表达式和相关的参考状态允许设计工程师在宏观尺度(高于热力学极限)下使用第二定律,而无需直接测量或考虑整个孤立系统中的熵变。(另见'''<font color = '#ff8000'>工艺工程师process engineer</font>''')。这些变化已经在假设中被考虑到,该假设认为所考虑的系统可以在不改变参考状态的情况下与参考状态达到平衡。将其与可逆理想<font color = 'blue'>状态</font>进行比较,还可以找到一个过程或过程集合的效率(见'''<font color = '#ff8000'>第二定律效率second law efficiency</font>''')
这个表达式和相关的参考状态允许设计工程师在宏观尺度(高于热力学极限)下使用第二定律,而无需直接测量或考虑整个孤立系统中的熵变。(另见'''<font color = '#ff8000'>工艺工程师process engineer</font>''')。这些变化已经在假设中被考虑到,该假设认为所考虑的系统可以在不改变参考状态的情况下与参考状态达到平衡。将其与可逆理想<font color = 'blue'>状态</font>进行比较,还可以找到一个过程或过程集合的效率(见'''<font color = '#ff8000'>第二定律效率second law efficiency</font>''')
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This approach to the Second Law is widely utilized in [[engineering]] practice, [[environmental accounting]], [[systems ecology]], and other disciplines.
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This approach to the Second Law is widely utilized in engineering practice, environmental accounting, systems ecology, and other disciplines.
第二定律的这种方法被广泛应用于'''<font color = '#ff8000'>工程实践engineering practice</font>'''、'''<font color = '#ff8000'>环境会计environmental accounting</font>'''、'''<font color = '#ff8000'>系统生态学systems ecology</font>'''等其他学科。
第二定律的这种方法被广泛应用于'''<font color = '#ff8000'>工程实践engineering practice</font>'''、'''<font color = '#ff8000'>环境会计environmental accounting</font>'''、'''<font color = '#ff8000'>系统生态学systems ecology</font>'''等其他学科。
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For a [[spontaneous process|spontaneous chemical process]] in a closed system at constant temperature and pressure without non-''PV'' work, the Clausius inequality Δ''S > Q/T<sub>surr</sub>'' transforms into a condition for the change in [[Gibbs free energy]]
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For a spontaneous chemical process in a closed system at constant temperature and pressure without non-PV work, the Clausius inequality ΔS > Q/T<sub>surr</sub> transforms into a condition for the change in Gibbs free energy
对于一个恒温恒压封闭系统中的自发化学过程,在没有 non-PV 功的情况下,克劳修斯不等式Δ''S > Q/T<sub>surr</sub>''由于'''<font color = '#ff8000'>吉布斯自由能Gibbs free energy</font>'''的变化而转化为:</font>
对于一个恒温恒压封闭系统中的自发化学过程,在没有 non-PV 功的情况下,克劳修斯不等式Δ''S > Q/T<sub>surr</sub>''由于'''<font color = '#ff8000'>吉布斯自由能Gibbs free energy</font>'''的变化而转化为:</font>
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or d''G'' < 0. For a similar process at constant temperature and volume, the change in [[Helmholtz free energy]] must be negative, <math>\Delta A < 0 </math>. Thus, a negative value of the change in free energy (G or A) is a necessary condition for a process to be spontaneous. This is the most useful form of the second law of thermodynamics in chemistry, where free-energy changes can be calculated from tabulated enthalpies of formation and standard molar entropies of reactants and products.<ref name="Oxtoby8th"/> <ref name="MortimerBook"></ref> The chemical equilibrium condition at constant ''T'' and ''p'' without electrical work is d''G'' = 0.
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or dG < 0. For a similar process at constant temperature and volume, the change in Helmholtz free energy must be negative, <math>\Delta A < 0 </math>. Thus, a negative value of the change in free energy (G or A) is a necessary condition for a process to be spontaneous. This is the most useful form of the second law of thermodynamics in chemistry, where free-energy changes can be calculated from tabulated enthalpies of formation and standard molar entropies of reactants and products. The chemical equilibrium condition at constant T and p without electrical work is dG = 0.
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或者 dG < 0。对于一个相似的恒温恒压过程,'''<font color = '#ff8000'>亥姆霍兹自由能 Helmholtz free energy </font>'''的变化一定是负的, <math>\Delta A < 0 </math>。因此,一个负的自由能(G 或 A)变化是过程自发的必要条件。这是热力学第二定律在化学中最有用的形式,其中自由能的变化可以通过'''<font color = '#ff8000'>表列生成焓 Tabulated Enthalpies of Formation</font>'''和反应物及产物的标准摩尔熵来计算。在温度和压力</font>不变的情况下,化学平衡条件是 dG = 0。
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或者 dG < 0。对于一个相似的恒温恒压过程,'''<font color = '#ff8000'>亥姆霍兹自由能 Helmholtz free energy </font>'''的变化一定是负的, <math>\Delta A < 0 </math>。因此,一个负的自由能(G 或 A)变化是过程自发的必要条件。这是热力学第二定律在化学中最有用的形式,其中自由能的变化可以通过'''<font color = '#ff8000'>表列生成焓 Tabulated Enthalpies of Formation</font>'''和反应物及产物的标准摩尔熵来计算。<ref name="MortimerBook"></ref> 在温度和压力</font>不变的情况下,化学平衡条件是 dG = 0。
==History历史==
==History历史==
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[[File:Sadi Carnot.jpeg|thumb|upright|Nicolas Léonard Sadi Carnot in the traditional uniform of a student of the [[École Polytechnique]].]]
Nicolas Léonard Sadi Carnot in the traditional uniform of a student of the [[École Polytechnique.]]
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尼古拉·莱昂纳尔·萨迪·卡诺穿着传统的巴黎综合理工学院制服
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The first theory of the conversion of heat into mechanical work is due to [[Nicolas Léonard Sadi Carnot]] in 1824. He was the first to realize correctly that the efficiency of this conversion depends on the difference of temperature between an engine and its environment.
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The first theory of the conversion of heat into mechanical work is due to Nicolas Léonard Sadi Carnot in 1824. He was the first to realize correctly that the efficiency of this conversion depends on the difference of temperature between an engine and its environment.
Recognizing the significance of [[James Prescott Joule]]'s work on the conservation of energy, [[Rudolf Clausius]] was the first to formulate the second law during 1850, in this form: heat does not flow ''spontaneously'' from cold to hot bodies. While common knowledge now, this was contrary to the [[caloric theory]] of heat popular at the time, which considered heat as a fluid. From there he was able to infer the principle of Sadi Carnot and the definition of entropy (1865).
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Recognizing the significance of James Prescott Joule's work on the conservation of energy, Rudolf Clausius was the first to formulate the second law during 1850, in this form: heat does not flow spontaneously from cold to hot bodies. While common knowledge now, this was contrary to the caloric theory of heat popular at the time, which considered heat as a fluid. From there he was able to infer the principle of Sadi Carnot and the definition of entropy (1865).
Established during the 19th century, the [[Kelvin-Planck statement|Kelvin-Planck statement of the Second Law]] says, "It is impossible for any device that operates on a [[cyclic process|cycle]] to receive heat from a single [[heat reservoir|reservoir]] and produce a net amount of work." This was shown to be equivalent to the statement of Clausius.
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Established during the 19th century, the Kelvin-Planck statement of the Second Law says, "It is impossible for any device that operates on a cycle to receive heat from a single reservoir and produce a net amount of work." This was shown to be equivalent to the statement of Clausius.
The [[ergodic hypothesis]] is also important for the [[Boltzmann]] approach. It says that, over long periods of time, the time spent in some region of the phase space of microstates with the same energy is proportional to the volume of this region, i.e. that all accessible microstates are equally probable over a long period of time. Equivalently, it says that time average and average over the statistical ensemble are the same.
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The ergodic hypothesis is also important for the Boltzmann approach. It says that, over long periods of time, the time spent in some region of the phase space of microstates with the same energy is proportional to the volume of this region, i.e. that all accessible microstates are equally probable over a long period of time. Equivalently, it says that time average and average over the statistical ensemble are the same.
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克劳修斯还提出了一种传统的学说,他认为熵可以被理解为宏观系统中的'''<font color = '#ff8000'>分子“无序”molecular 'disorder'</font>''',但这种学说已经过时了。<ref>Denbigh, K.G., Denbigh, J.S. (1985). ''Entropy in Relation to Incomplete Knowledge'', Cambridge University Press, Cambridge UK, {{ISBN|0-521-25677-1}}, pp. 43–44.</ref><ref>Grandy, W.T., Jr (2008). ''Entropy and the Time Evolution of Macroscopic Systems'', Oxford University Press, Oxford, {{ISBN|978-0-19-954617-6}}, pp. 55–58.</ref><ref name=Lambert>[http://entropysite.oxy.edu Entropy Sites — A Guide] Content selected by [[Frank L. Lambert]]</ref>
There is a traditional doctrine, starting with Clausius, that entropy can be understood in terms of molecular 'disorder' within a [[Macroscopic bodies|macroscopic system]]. This doctrine is obsolescent.<ref>Denbigh, K.G., Denbigh, J.S. (1985). ''Entropy in Relation to Incomplete Knowledge'', Cambridge University Press, Cambridge UK, {{ISBN|0-521-25677-1}}, pp. 43–44.</ref><ref>Grandy, W.T., Jr (2008). ''Entropy and the Time Evolution of Macroscopic Systems'', Oxford University Press, Oxford, {{ISBN|978-0-19-954617-6}}, pp. 55–58.</ref><ref name=Lambert>[http://entropysite.oxy.edu Entropy Sites — A Guide] Content selected by [[Frank L. Lambert]]</ref>
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There is a traditional doctrine, starting with Clausius, that entropy can be understood in terms of molecular 'disorder' within a macroscopic system. This doctrine is obsolescent.
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克劳修斯还提出了一种传统的学说,他认为熵可以被理解为宏观系统中的'''<font color = '#ff8000'>分子“无序”molecular 'disorder'</font>''',但这种学说已经过时了。
In 1856, the German physicist [[Rudolf Clausius]] stated what he called the "second fundamental theorem in the [[mechanical theory of heat]]" in the following form:{{sfnp|Clausius|1867}}
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In 1856, the German physicist Rudolf Clausius stated what he called the "second fundamental theorem in the mechanical theory of heat" in the following form:
1856年,德国物理学家'''<font color = '#ff8000'>鲁道夫 • 克劳修斯Rudolf Clausius </font>'''阐述了他所谓的“热力学理论中的第二个基本定理second fundamental theorem in the mechanical theory of heat” ,其形式如下:
1856年,德国物理学家'''<font color = '#ff8000'>鲁道夫 • 克劳修斯Rudolf Clausius </font>'''阐述了他所谓的“热力学理论中的第二个基本定理second fundamental theorem in the mechanical theory of heat” ,其形式如下:
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where ''Q'' is heat, ''T'' is temperature and ''N'' is the "equivalence-value" of all uncompensated transformations involved in a cyclical process. Later, in 1865, Clausius would come to define "equivalence-value" as entropy. On the heels of this definition, that same year, the most famous version of the second law was read in a presentation at the Philosophical Society of Zurich on April 24, in which, in the end of his presentation, Clausius concludes:
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where Q is heat, T is temperature and N is the "equivalence-value" of all uncompensated transformations involved in a cyclical process. Later, in 1865, Clausius would come to define "equivalence-value" as entropy. On the heels of this definition, that same year, the most famous version of the second law was read in a presentation at the Philosophical Society of Zurich on April 24, in which, in the end of his presentation, Clausius concludes:
<blockquote>The entropy of the universe tends to a maximum.</blockquote>
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<blockquote>The entropy of the universe tends to a maximum.</blockquote>
宇宙的熵趋于最大
宇宙的熵趋于最大
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This statement is the best-known phrasing of the second law. Because of the looseness of its language, e.g. [[universe]], as well as lack of specific conditions, e.g. open, closed, or isolated, many people take this simple statement to mean that the second law of thermodynamics applies virtually to every subject imaginable. This is not true; this statement is only a simplified version of a more extended and precise description.
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This statement is the best-known phrasing of the second law. Because of the looseness of its language, e.g. universe, as well as lack of specific conditions, e.g. open, closed, or isolated, many people take this simple statement to mean that the second law of thermodynamics applies virtually to every subject imaginable. This is not true; this statement is only a simplified version of a more extended and precise description.
In terms of time variation, the mathematical statement of the second law for an [[isolated system]] undergoing an arbitrary transformation is:
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In terms of time variation, the mathematical statement of the second law for an isolated system undergoing an arbitrary transformation is:
就时间变化而言,<font color = 'blue'>一个</font>经历任意变换的孤立系统<font color = 'blue'>的</font>第二定律的数学表述是:
就时间变化而言,<font color = 'blue'>一个</font>经历任意变换的孤立系统<font color = 'blue'>的</font>第二定律的数学表述是:
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<!-- A reversible process requires equilibrium with the surroundings. This is not possible for an isolated system. Therefore, the discussion about the reversible process has been shifted to the analysis of closed systems -->
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<!-- A reversible process requires equilibrium with the surroundings. This is not possible for an isolated system. Therefore, the discussion about the reversible process has been shifted to the analysis of closed systems -->
The equality sign applies after equilibration. An alternative way of formulating of the second law for isolated systems is:
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The equality sign applies after equilibration. An alternative way of formulating of the second law for isolated systems is:
平衡后用等号。另一种表述孤立系统第二定律的方法是:
平衡后用等号。另一种表述孤立系统第二定律的方法是:
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with <math> \dot S_{i}</math> the sum of the rate of [[entropy production]] by all processes inside the system. The advantage of this formulation is that it shows the effect of the entropy production. The rate of entropy production is a very important concept since it determines (limits) the efficiency of thermal machines. Multiplied with ambient temperature <math>T_{a}</math> it gives the so-called dissipated energy <math> P_{diss}=T_{a}\dot S_{i}</math>.
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with <math> \dot S_{i}</math> the sum of the rate of entropy production by all processes inside the system. The advantage of this formulation is that it shows the effect of the entropy production. The rate of entropy production is a very important concept since it determines (limits) the efficiency of thermal machines. Multiplied with ambient temperature <math>T_{a}</math> it gives the so-called dissipated energy <math> P_{diss}=T_{a}\dot S_{i}</math>.
用<math> \dot S_{i}</math>表示系统内所有进程'''<font color = '#ff8000'>熵产生Entropy Production</font>'''的速率之和。这个公式的优点是它显示了熵产生的效果。熵产生率是一个非常重要的概念,因为它决定(或限制)热机的效率。乘以环境温度<math>T_{a}</math>,它给出所谓的耗散能<math> P_{diss}=T_{a}\dot S_{i}</math>。
用<math> \dot S_{i}</math>表示系统内所有进程'''<font color = '#ff8000'>熵产生Entropy Production</font>'''的速率之和。这个公式的优点是它显示了熵产生的效果。熵产生率是一个非常重要的概念,因为它决定(或限制)热机的效率。乘以环境温度<math>T_{a}</math>,它给出所谓的耗散能<math> P_{diss}=T_{a}\dot S_{i}</math>。
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The expression of the second law for closed systems (so, allowing heat exchange and moving boundaries, but not exchange of matter) is:
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The expression of the second law for closed systems (so, allowing heat exchange and moving boundaries, but not exchange of matter) is:
封闭系统的第二定律(允许热<s>量</s>交换和移动边界,但不允许物质交换)的表达式是:
封闭系统的第二定律(允许热<s>量</s>交换和移动边界,但不允许物质交换)的表达式是:
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The equality sign holds in the case that only reversible processes take place inside the system. If irreversible processes take place (which is the case in real systems in operation) the >-sign holds. If heat is supplied to the system at several places we have to take the algebraic sum of the corresponding terms.
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The equality sign holds in the case that only reversible processes take place inside the system. If irreversible processes take place (which is the case in real systems in operation) the >-sign holds. If heat is supplied to the system at several places we have to take the algebraic sum of the corresponding terms.
For open systems (also allowing exchange of matter):
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For open systems (also allowing exchange of matter):
对于开放系统(也允许物质交换) :
对于开放系统(也允许物质交换) :
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Here <math>\dot S</math> is the flow of entropy into the system associated with the flow of matter entering the system. It should not be confused with the time derivative of the entropy. If matter is supplied at several places we have to take the algebraic sum of these contributions.
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Here <math>\dot S</math> is the flow of entropy into the system associated with the flow of matter entering the system. It should not be confused with the time derivative of the entropy. If matter is supplied at several places we have to take the algebraic sum of these contributions.
[[Statistical mechanics]] gives an explanation for the second law by postulating that a material is composed of atoms and molecules which are in constant motion. A particular set of positions and velocities for each particle in the system is called a [[microstate (statistical mechanics)|microstate]] of the system and because of the constant motion, the system is constantly changing its microstate. Statistical mechanics postulates that, in equilibrium, each microstate that the system might be in is equally likely to occur, and when this assumption is made, it leads directly to the conclusion that the second law must hold in a statistical sense. That is, the second law will hold on average, with a statistical variation on the order of 1/{{radic|''N''}} where ''N'' is the number of particles in the system. For everyday (macroscopic) situations, the probability that the second law will be violated is practically zero. However, for systems with a small number of particles, thermodynamic parameters, including the entropy, may show significant statistical deviations from that predicted by the second law. Classical thermodynamic theory does not deal with these statistical variations.
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Statistical mechanics gives an explanation for the second law by postulating that a material is composed of atoms and molecules which are in constant motion. A particular set of positions and velocities for each particle in the system is called a microstate of the system and because of the constant motion, the system is constantly changing its microstate. Statistical mechanics postulates that, in equilibrium, each microstate that the system might be in is equally likely to occur, and when this assumption is made, it leads directly to the conclusion that the second law must hold in a statistical sense. That is, the second law will hold on average, with a statistical variation on the order of 1/{{radic|''N''}} where N is the number of particles in the system. For everyday (macroscopic) situations, the probability that the second law will be violated is practically zero. However, for systems with a small number of particles, thermodynamic parameters, including the entropy, may show significant statistical deviations from that predicted by the second law. Classical thermodynamic theory does not deal with these statistical variations.
统计力学通过假设物质是由不断运动的原子和分子组成的,来对第二定律给出了解释。系统中每个粒子的一组特定的位置和速度称为系统的微观状态,由于系统的不断运动,系统不断地改变其微观状态。统计力学假设,在平衡状态下,系统处于<s>的</s>每个微观状态的可能性是相等的。这个假设的提出直接导致第二定律必须在统计学意义上成立,也就是说,第二定律在平均意义上成立,其中统计学变异取决于数量级1/{{radic|''N''}},其中 N 是系统中粒子数。在日常(宏观)情况下,违反第二定律的概率几乎为零。然而,对于粒子数量很少的系统,热力学参数,包括熵,可能显示出与第二定律预测结果的显著的统计偏差。经典热力学理论不处理这些统计变量。
统计力学通过假设物质是由不断运动的原子和分子组成的,来对第二定律给出了解释。系统中每个粒子的一组特定的位置和速度称为系统的微观状态,由于系统的不断运动,系统不断地改变其微观状态。统计力学假设,在平衡状态下,系统处于<s>的</s>每个微观状态的可能性是相等的。这个假设的提出直接导致第二定律必须在统计学意义上成立,也就是说,第二定律在平均意义上成立,其中统计学变异取决于数量级1/{{radic|''N''}},其中 N 是系统中粒子数。在日常(宏观)情况下,违反第二定律的概率几乎为零。然而,对于粒子数量很少的系统,热力学参数,包括熵,可能显示出与第二定律预测结果的显著的统计偏差。经典热力学理论不处理这些统计变量。
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The first mechanical argument of the [[Kinetic theory of gases]] that molecular collisions entail an equalization of temperatures and hence a tendency towards equilibrium was due to [[James Clerk Maxwell]] in 1860;<ref>{{Cite journal | last1 = Gyenis | first1 = Balazs | doi = 10.1016/j.shpsb.2017.01.001 | title = Maxwell and the normal distribution: A colored story of probability, independence, and tendency towards equilibrium | journal = Studies in History and Philosophy of Modern Physics | volume = 57 | pages = 53–65 | year = 2017| arxiv = 1702.01411 | bibcode = 2017SHPMP..57...53G }}</ref> [[Ludwig Boltzmann]] with his [[H-theorem]] of 1872 also argued that due to collisions gases should over time tend toward the [[Maxwell–Boltzmann distribution]].
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The first mechanical argument of the Kinetic theory of gases that molecular collisions entail an equalization of temperatures and hence a tendency towards equilibrium was due to James Clerk Maxwell in 1860; Ludwig Boltzmann with his H-theorem of 1872 also argued that due to collisions gases should over time tend toward the Maxwell–Boltzmann distribution.
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'''<font color="#ff8000">气体动力学Kinetic theory of gases</font>'''理论的第一个力学论证由'''<font color="#ff8000">麦克斯韦James Clerk Maxwell</font>'''在1860年给出,指出分子碰撞引起温度均衡化,因此整体趋向于'''<font color="#ff8000">平衡 Equilibrium </font>'''; '''<font color="#ff8000">玻尔兹曼Ludwig Boltzmann</font>'''在1872年提出的'''<font color="#ff8000"> H 定理H-theorem</font>'''也认为,气体由于碰撞应该随着时间的推移趋向于'''<font color="#ff8000">麦克斯韦-波兹曼分布Maxwell–Boltzmann distribution</font>'''。
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'''<font color="#ff8000">气体动力学Kinetic theory of gases</font>'''理论的第一个力学论证由'''<font color="#ff8000">麦克斯韦James Clerk Maxwell</font>'''在1860年给出,指出分子碰撞引起温度均衡化,因此整体趋向于'''<font color="#ff8000">平衡 Equilibrium </font>'''; '''<font color="#ff8000">玻尔兹曼Ludwig Boltzmann</font>'''<ref>{{Cite journal | last1 = Gyenis | first1 = Balazs | doi = 10.1016/j.shpsb.2017.01.001 | title = Maxwell and the normal distribution: A colored story of probability, independence, and tendency towards equilibrium | journal = Studies in History and Philosophy of Modern Physics | volume = 57 | pages = 53–65 | year = 2017| arxiv = 1702.01411 | bibcode = 2017SHPMP..57...53G }}</ref>在1872年提出的'''<font color="#ff8000"> H 定理H-theorem</font>'''也认为,气体由于碰撞应该随着时间的推移趋向于'''<font color="#ff8000">麦克斯韦-波兹曼分布Maxwell–Boltzmann distribution</font>'''。
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Due to [[Loschmidt's paradox]], derivations of the Second Law have to make an assumption regarding the past, namely that the system is [[Correlation and dependence|uncorrelated]] at some time in the past; this allows for simple probabilistic treatment. This assumption is usually thought as a [[boundary condition]], and thus the second Law is ultimately a consequence of the initial conditions somewhere in the past, probably at the beginning of the universe (the [[Big Bang]]), though [[Boltzmann brain|other scenarios]] have also been suggested.<ref name="Hawking AOT">{{cite journal|last=Hawking|first=SW|title=Arrow of time in cosmology|journal=Phys. Rev. D|year=1985|volume=32|issue=10|pages=2489–2495|doi=10.1103/PhysRevD.32.2489|pmid=9956019|bibcode = 1985PhRvD..32.2489H }}</ref><ref>{{cite book | last = Greene | first = Brian | authorlink = Brian Greene | title = The Fabric of the Cosmos | url = https://archive.org/details/fabricofcosmossp00gree | url-access = registration | publisher = Alfred A. Knopf | year = 2004 | page = [https://archive.org/details/fabricofcosmossp00gree/page/171 171] | isbn = 978-0-375-41288-2}}</ref><ref name=Lebowitz>{{cite journal|last=Lebowitz|first=Joel L.|title= Boltzmann's Entropy and Time's Arrow|journal=Physics Today|date=September 1993|volume=46|issue=9|pages=32–38|url=http://users.df.uba.ar/ariel/materias/FT3_2008_1C/papers_pdf/lebowitz_370.pdf|accessdate=2013-02-22|doi=10.1063/1.881363|bibcode = 1993PhT....46i..32L }}</ref>
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Due to Loschmidt's paradox, derivations of the Second Law have to make an assumption regarding the past, namely that the system is uncorrelated at some time in the past; this allows for simple probabilistic treatment. This assumption is usually thought as a boundary condition, and thus the second Law is ultimately a consequence of the initial conditions somewhere in the past, probably at the beginning of the universe (the Big Bang), though other scenarios have also been suggested.
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由于'''<font color="#ff8000">洛施密特悖论Loschmidt's paradox</font>''',第二定律的导出必须对过去做出一个假设,即系统在过去的某个时刻是不相关的;这样的假设允许进行简单的概率处理。这个假设通常被认为是一个'''<font color="#ff8000">边界条件boundary condition</font>''',因此热力学第二定律最终是过去某个地方的初始条件的结果,可能是在宇宙的开始('''<font color="#ff8000">大爆炸 the Big Bang</font>''') ,尽管也有人提出了其他场景。
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由于'''<font color="#ff8000">洛施密特悖论Loschmidt's paradox</font>''',第二定律的导出必须对过去做出一个假设,即系统在过去的某个时刻是不相关的;这样的假设允许进行简单的概率处理。这个假设通常被认为是一个'''<font color="#ff8000">边界条件boundary condition</font>''',因此热力学第二定律最终是过去某个地方的初始条件的结果,可能是在宇宙的开始('''<font color="#ff8000">大爆炸 the Big Bang</font>''') ,尽管也有人提出了其他场景。.<ref name="Hawking AOT">{{cite journal|last=Hawking|first=SW|title=Arrow of time in cosmology|journal=Phys. Rev. D|year=1985|volume=32|issue=10|pages=2489–2495|doi=10.1103/PhysRevD.32.2489|pmid=9956019|bibcode = 1985PhRvD..32.2489H }}</ref><ref>{{cite book | last = Greene | first = Brian | authorlink = Brian Greene | title = The Fabric of the Cosmos | url = https://archive.org/details/fabricofcosmossp00gree | url-access = registration | publisher = Alfred A. Knopf | year = 2004 | page = [https://archive.org/details/fabricofcosmossp00gree/page/171 171] | isbn = 978-0-375-41288-2}}</ref><ref name=Lebowitz>{{cite journal|last=Lebowitz|first=Joel L.|title= Boltzmann's Entropy and Time's Arrow|journal=Physics Today|date=September 1993|volume=46|issue=9|pages=32–38|url=http://users.df.uba.ar/ariel/materias/FT3_2008_1C/papers_pdf/lebowitz_370.pdf|accessdate=2013-02-22|doi=10.1063/1.881363|bibcode = 1993PhT....46i..32L }}</ref>
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Given these assumptions, in statistical mechanics, the Second Law is not a postulate, rather it is a consequence of the [[Statistical mechanics#Fundamental postulate|fundamental postulate]], also known as the equal prior probability postulate, so long as one is clear that simple probability arguments are applied only to the future, while for the past there are auxiliary sources of information which tell us that it was low entropy.{{citation needed|date=August 2012}} The first part of the second law, which states that the entropy of a thermally isolated system can only increase, is a trivial consequence of the equal prior probability postulate, if we restrict the notion of the entropy to systems in thermal equilibrium. The entropy of an isolated system in thermal equilibrium containing an amount of energy of <math>E</math> is:
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Given these assumptions, in statistical mechanics, the Second Law is not a postulate, rather it is a consequence of the fundamental postulate, also known as the equal prior probability postulate, so long as one is clear that simple probability arguments are applied only to the future, while for the past there are auxiliary sources of information which tell us that it was low entropy. The first part of the second law, which states that the entropy of a thermally isolated system can only increase, is a trivial consequence of the equal prior probability postulate, if we restrict the notion of the entropy to systems in thermal equilibrium. The entropy of an isolated system in thermal equilibrium containing an amount of energy of <math>E</math> is:
基于这些假设,在统计力学中,第二定律不是一个假设,而是'''统计力学基本假设Statistical mechanics#Fundamental postulate|fundamental postulate'''的一个结果,也被称为'''<font color="#ff8000">等先验概率假设 equal prior probability postulate</font>'''。这个基本假设表明,只要一个人清楚地知道,简单的概率论证只适用于未来,而对于过去,有辅助的信息来源告诉我们,它是低熵的。如果我们把熵的概念限制在热平衡系统中,那么热力学第二定律的第一部分即热孤立系统的熵只能增加,是等先验概率假设的一个显然结果。处于热平衡状态的孤立系统且具有能量<math>E</math>的熵表示为:
基于这些假设,在统计力学中,第二定律不是一个假设,而是'''统计力学基本假设Statistical mechanics#Fundamental postulate|fundamental postulate'''的一个结果,也被称为'''<font color="#ff8000">等先验概率假设 equal prior probability postulate</font>'''。这个基本假设表明,只要一个人清楚地知道,简单的概率论证只适用于未来,而对于过去,有辅助的信息来源告诉我们,它是低熵的。如果我们把熵的概念限制在热平衡系统中,那么热力学第二定律的第一部分即热孤立系统的熵只能增加,是等先验概率假设的一个显然结果。处于热平衡状态的孤立系统且具有能量<math>E</math>的熵表示为:
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where <math>\Omega\left(E\right)</math> is the number of quantum states in a small interval between <math>E</math> and <math>E +\delta E</math>. Here <math>\delta E</math> is a macroscopically small energy interval that is kept fixed. Strictly speaking this means that the entropy depends on the choice of <math>\delta E</math>. However, in the thermodynamic limit (i.e. in the limit of infinitely large system size), the specific entropy (entropy per unit volume or per unit mass) does not depend on <math>\delta E</math>.
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where <math>\Omega\left(E\right)</math> is the number of quantum states in a small interval between <math>E</math> and <math>E +\delta E</math>. Here <math>\delta E</math> is a macroscopically small energy interval that is kept fixed. Strictly speaking this means that the entropy depends on the choice of <math>\delta E</math>. However, in the thermodynamic limit (i.e. in the limit of infinitely large system size), the specific entropy (entropy per unit volume or per unit mass) does not depend on <math>\delta E</math>.
Suppose we have an isolated system whose macroscopic state is specified by a number of variables. These macroscopic variables can, e.g., refer to the total volume, the positions of pistons in the system, etc. Then <math>\Omega</math> will depend on the values of these variables. If a variable is not fixed, (e.g. we do not clamp a piston in a certain position), then because all the accessible states are equally likely in equilibrium, the free variable in equilibrium will be such that <math>\Omega</math> is maximized as that is the most probable situation in equilibrium.
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Suppose we have an isolated system whose macroscopic state is specified by a number of variables. These macroscopic variables can, e.g., refer to the total volume, the positions of pistons in the system, etc. Then <math>\Omega</math> will depend on the values of these variables. If a variable is not fixed, (e.g. we do not clamp a piston in a certain position), then because all the accessible states are equally likely in equilibrium, the free variable in equilibrium will be such that <math>\Omega</math> is maximized as that is the most probable situation in equilibrium.
If the variable was initially fixed to some value then upon release and when the new equilibrium has been reached, the fact the variable will adjust itself so that <math>\Omega</math> is maximized, implies that the entropy will have increased or it will have stayed the same (if the value at which the variable was fixed happened to be the equilibrium value).
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If the variable was initially fixed to some value then upon release and when the new equilibrium has been reached, the fact the variable will adjust itself so that <math>\Omega</math> is maximized, implies that the entropy will have increased or it will have stayed the same (if the value at which the variable was fixed happened to be the equilibrium value).
Suppose we start from an equilibrium situation and we suddenly remove a constraint on a variable. Then right after we do this, there are a number <math>\Omega</math> of accessible microstates, but equilibrium has not yet been reached, so the actual probabilities of the system being in some accessible state are not yet equal to the prior probability of <math>1/\Omega</math>. We have already seen that in the final equilibrium state, the entropy will have increased or have stayed the same relative to the previous equilibrium state. Boltzmann's [[H-theorem]], however, proves that the quantity {{math|''H''}} increases monotonically as a function of time during the intermediate out of equilibrium state.
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Suppose we start from an equilibrium situation and we suddenly remove a constraint on a variable. Then right after we do this, there are a number <math>\Omega</math> of accessible microstates, but equilibrium has not yet been reached, so the actual probabilities of the system being in some accessible state are not yet equal to the prior probability of <math>1/\Omega</math>. We have already seen that in the final equilibrium state, the entropy will have increased or have stayed the same relative to the previous equilibrium state. Boltzmann's H-theorem, however, proves that the quantity increases monotonically as a function of time during the intermediate out of equilibrium state.
The second part of the Second Law states that the entropy change of a system undergoing a reversible process is given by:
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The second part of the Second Law states that the entropy change of a system undergoing a reversible process is given by:
热力学第二定律的第二部分指出,经历可逆过程的系统的熵变为:
热力学第二定律的第二部分指出,经历可逆过程的系统的熵变为:
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where the temperature is defined as:
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where the temperature is defined as:
其中温度定义为:
其中温度定义为:
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See [[Microcanonical ensemble|here]] for the justification for this definition. Suppose that the system has some external parameter, x, that can be changed. In general, the energy eigenstates of the system will depend on x. According to the [[adiabatic theorem]] of quantum mechanics, in the limit of an infinitely slow change of the system's Hamiltonian, the system will stay in the same energy eigenstate and thus change its energy according to the change in energy of the energy eigenstate it is in.
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See here for the justification for this definition. Suppose that the system has some external parameter, x, that can be changed. In general, the energy eigenstates of the system will depend on x. According to the adiabatic theorem of quantum mechanics, in the limit of an infinitely slow change of the system's Hamiltonian, the system will stay in the same energy eigenstate and thus change its energy according to the change in energy of the energy eigenstate it is in.
请参阅'''此处Microcanonical ensemble|here'''查看该定义的正当性。假设系统有一些可以改变的外部参数 x。一般来说,系统的能量本征态将依赖于 x。根据量子力学的'''<font color="#ff8000">绝热定理adiabatic theorem</font>''',在系统哈密顿量无限缓慢变化的极限下,系统将保持在相同的'''<font color = '#ff8000'>能量本征态 energy eigenstate</font>''',因此系统的能量会随着其所在能量本征态的能量变化而变化。
请参阅'''此处Microcanonical ensemble|here'''查看该定义的正当性。假设系统有一些可以改变的外部参数 x。一般来说,系统的能量本征态将依赖于 x。根据量子力学的'''<font color="#ff8000">绝热定理adiabatic theorem</font>''',在系统哈密顿量无限缓慢变化的极限下,系统将保持在相同的'''<font color = '#ff8000'>能量本征态 energy eigenstate</font>''',因此系统的能量会随着其所在能量本征态的能量变化而变化。
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The generalized force, X, corresponding to the external variable x is defined such that <math>X dx</math> is the work performed by the system if x is increased by an amount dx. E.g., if x is the volume, then X is the pressure. The generalized force for a system known to be in energy eigenstate <math>E_{r}</math> is given by:
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The generalized force, X, corresponding to the external variable x is defined such that <math>X dx</math> is the work performed by the system if x is increased by an amount dx. E.g., if x is the volume, then X is the pressure. The generalized force for a system known to be in energy eigenstate <math>E_{r}</math> is given by:
对于外部变量 x 可以定义'''<font color="#ff8000">广义力generalized force</font>''' X ,因此如果 x 增加 dx,那么<math>X dx</math> 就是系统所做的功。例如,如果 x 是体积,那么 X 就是压强。一个已知处于能量本征态<math>E_{r}</math>的系统的广义力为:
对于外部变量 x 可以定义'''<font color="#ff8000">广义力generalized force</font>''' X ,因此如果 x 增加 dx,那么<math>X dx</math> 就是系统所做的功。例如,如果 x 是体积,那么 X 就是压强。一个已知处于能量本征态<math>E_{r}</math>的系统的广义力为:
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Since the system can be in any energy eigenstate within an interval of <math>\delta E</math>, we define the generalized force for the system as the expectation value of the above expression:
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Since the system can be in any energy eigenstate within an interval of <math>\delta E</math>, we define the generalized force for the system as the expectation value of the above expression:
To evaluate the average, we partition the <math>\Omega\left(E\right)</math> energy eigenstates by counting how many of them have a value for <math>\frac{dE_{r}}{dx}</math> within a range between <math>Y</math> and <math>Y + \delta Y</math>. Calling this number <math>\Omega_{Y}\left(E\right)</math>, we have:
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To evaluate the average, we partition the <math>\Omega\left(E\right)</math> energy eigenstates by counting how many of them have a value for <math>\frac{dE_{r}}{dx}</math> within a range between <math>Y</math> and <math>Y + \delta Y</math>. Calling this number <math>\Omega_{Y}\left(E\right)</math>, we have:
We can relate this to the derivative of the entropy with respect to x at constant energy E as follows. Suppose we change x to x + dx. Then <math>\Omega\left(E\right)</math> will change because the energy eigenstates depend on x, causing energy eigenstates to move into or out of the range between <math>E</math> and <math>E+\delta E</math>. Let's focus again on the energy eigenstates for which <math>\frac{dE_{r}}{dx}</math> lies within the range between <math>Y</math> and <math>Y + \delta Y</math>. Since these energy eigenstates increase in energy by Y dx, all such energy eigenstates that are in the interval ranging from E – Y dx to E move from below E to above E. There are
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We can relate this to the derivative of the entropy with respect to x at constant energy E as follows. Suppose we change x to x + dx. Then <math>\Omega\left(E\right)</math> will change because the energy eigenstates depend on x, causing energy eigenstates to move into or out of the range between <math>E</math> and <math>E+\delta E</math>. Let's focus again on the energy eigenstates for which <math>\frac{dE_{r}}{dx}</math> lies within the range between <math>Y</math> and <math>Y + \delta Y</math>. Since these energy eigenstates increase in energy by Y dx, all such energy eigenstates that are in the interval ranging from E – Y dx to E move from below E to above E. There are
我们可以把它和由恒定能量 E 下的 x 导出来的熵联系起来。假定我们把 x 改变至 x + dx。然后因为能量本征态依赖于 x, <math>\Omega\left(E\right)</math> 将会改变,这导致能量本征态进入或超出<math>E</math> 和<math>E+\delta E</math> 之间的范围。让我们再次关注<math>\frac{dE_{r}}{dx}</math> 处于 <math>Y</math> 和 <math>Y + \delta Y</math> 之间的能量本征态。由于这些能量本征态的能量增加了 Y dx,所有这些在 E-Y dx 到 E 之间能量本征态都从 E 以下移动到 E 以上。 因此有
我们可以把它和由恒定能量 E 下的 x 导出来的熵联系起来。假定我们把 x 改变至 x + dx。然后因为能量本征态依赖于 x, <math>\Omega\left(E\right)</math> 将会改变,这导致能量本征态进入或超出<math>E</math> 和<math>E+\delta E</math> 之间的范围。让我们再次关注<math>\frac{dE_{r}}{dx}</math> 处于 <math>Y</math> 和 <math>Y + \delta Y</math> 之间的能量本征态。由于这些能量本征态的能量增加了 Y dx,所有这些在 E-Y dx 到 E 之间能量本征态都从 E 以下移动到 E 以上。 因此有
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such energy eigenstates. If <math>Y dx\leq\delta E</math>, all these energy eigenstates will move into the range between <math>E</math> and <math>E+\delta E</math> and contribute to an increase in <math>\Omega</math>. The number of energy eigenstates that move from below <math>E+\delta E</math> to above <math>E+\delta E</math> is given by <math>N_{Y}\left(E+\delta E\right)</math>. The difference
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such energy eigenstates. If <math>Y dx\leq\delta E</math>, all these energy eigenstates will move into the range between <math>E</math> and <math>E+\delta E</math> and contribute to an increase in <math>\Omega</math>. The number of energy eigenstates that move from below <math>E+\delta E</math> to above <math>E+\delta E</math> is given by <math>N_{Y}\left(E+\delta E\right)</math>. The difference
is thus the net contribution to the increase in <math>\Omega</math>. Note that if Y dx is larger than <math>\delta E</math> there will be the energy eigenstates that move from below E to above <math>E+\delta E</math>. They are counted in both <math>N_{Y}\left(E\right)</math> and <math>N_{Y}\left(E+\delta E\right)</math>, therefore the above expression is also valid in that case.
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is thus the net contribution to the increase in <math>\Omega</math>. Note that if Y dx is larger than <math>\delta E</math> there will be the energy eigenstates that move from below E to above <math>E+\delta E</math>. They are counted in both <math>N_{Y}\left(E\right)</math> and <math>N_{Y}\left(E+\delta E\right)</math>, therefore the above expression is also valid in that case.
因此是 <math>\Omega</math>增长的净贡献。请注意如果 Y dx 大于 <math>\delta E</math>,那么将会有能量本征态从 E 以下移动到<math>E+\delta E</math>以上。它们在<math>N_{Y}\left(E\right)</math> 和 <math>N_{Y}\left(E+\delta E\right)</math>中都有计数,因此上述表达式在这种情况下也是有效的。
因此是 <math>\Omega</math>增长的净贡献。请注意如果 Y dx 大于 <math>\delta E</math>,那么将会有能量本征态从 E 以下移动到<math>E+\delta E</math>以上。它们在<math>N_{Y}\left(E\right)</math> 和 <math>N_{Y}\left(E+\delta E\right)</math>中都有计数,因此上述表达式在这种情况下也是有效的。
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Expressing the above expression as a derivative with respect to E and summing over Y yields the expression:
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Expressing the above expression as a derivative with respect to E and summing over Y yields the expression:
将上面的表达式表示为对 E 的导数,并且对 Y 求和得到表达式:
将上面的表达式表示为对 E 的导数,并且对 Y 求和得到表达式:
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The logarithmic derivative of <math>\Omega</math> with respect to x is thus given by:
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The logarithmic derivative of <math>\Omega</math> with respect to x is thus given by:
<math>\Omega</math>的对数关于x的导数由以下方式给出:
<math>\Omega</math>的对数关于x的导数由以下方式给出:
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The first term is intensive, i.e. it does not scale with system size. In contrast, the last term scales as the inverse system size and will thus vanishes in the thermodynamic limit. We have thus found that:
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The first term is intensive, i.e. it does not scale with system size. In contrast, the last term scales as the inverse system size and will thus vanishes in the thermodynamic limit. We have thus found that:
If a system is in thermal contact with a heat bath at some temperature T then, in equilibrium, the probability distribution over the energy eigenvalues are given by the [[canonical ensemble]]:
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If a system is in thermal contact with a heat bath at some temperature T then, in equilibrium, the probability distribution over the energy eigenvalues are given by the canonical ensemble:
如果一个系统与某个温度为T的热浴热接触,那么在平衡状态下,关于能量本征值的概率分布值由'''<font color = '#ff8000'>正则系综canonical ensemble</font>'''给出:
如果一个系统与某个温度为T的热浴热接触,那么在平衡状态下,关于能量本征值的概率分布值由'''<font color = '#ff8000'>正则系综canonical ensemble</font>'''给出:
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Here Z is a factor that normalizes the sum of all the probabilities to 1, this function is known as the [[Partition function (statistical mechanics)|partition function]]. We now consider an infinitesimal reversible change in the temperature and in the external parameters on which the energy levels depend. It follows from the general formula for the entropy:
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Here Z is a factor that normalizes the sum of all the probabilities to 1, this function is known as the partition function. <font color = 'red'>We now consider an infinitesimal reversible change in the temperature and in the external parameters on which the energy levels depend. </font>It follows from the general formula for the entropy:
这里 Z 是一个使所有概率之和归一化到 1 的因子,这个函数被称为'''<font color = '#ff8000'>配分函数Partition function (statistical mechanics)|partition function</font>'''。现在我们考虑对温度和能级所依赖的外部参数的无限小的可逆改变。它遵循熵的一般公式:
这里 Z 是一个使所有概率之和归一化到 1 的因子,这个函数被称为'''<font color = '#ff8000'>配分函数Partition function (statistical mechanics)|partition function</font>'''。现在我们考虑对温度和能级所依赖的外部参数的无限小的可逆改变。它遵循熵的一般公式:
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Inserting the formula for <math>P_{j}</math> for the canonical ensemble in here gives:
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Inserting the formula for <math>P_{j}</math> for the canonical ensemble in here gives:
There are two principal ways of formulating thermodynamics, (a) through passages from one state of thermodynamic equilibrium to another, and (b) through cyclic processes, by which the system is left unchanged, while the total entropy of the surroundings is increased. These two ways help to understand the processes of life. This topic is mostly beyond the scope of this present article, but has been considered by several authors, such as [[What is Life?|Erwin Schrödinger]], [[Léon Brillouin]]<ref>Léon Brillouin [https://books.google.com/books?hl=en&lr=&id=tPXVbiw_1P0C ''Science and Information Theory''] (Academic Press, 1962) (Dover, 2004)</ref> and [[Life and Energy|Isaac Asimov]]. It is also the topic of current{{When|date=July 2019}} research.{{Citation needed|date=July 2019}}
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表述热力学主要有两种方式:(a)描述从一种热力学平衡状态到另一种状态的路径,(b)通过系统保持不变但周围环境的总熵增加的循环过程。这两种方法有助于理解生命过程。这个话题大大超出了本文的范围,但是已经有一些研究者考虑过这个问题,比如'''<font color = '#ff8000'>薛定谔Erwin Schrödinger</font>'''、'''<font color = '#ff8000'>布里渊Léon Brillouin</font>'''<ref>Léon Brillouin [https://books.google.com/books?hl=en&lr=&id=tPXVbiw_1P0C ''Science and Information Theory''] (Academic Press, 1962) (Dover, 2004)</ref>和'''<font color = '#ff8000'>阿西莫夫Isaac Asimov</font>'''。这也是当前研究的主题。
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There are two principal ways of formulating thermodynamics, (a) through passages from one state of thermodynamic equilibrium to another, and (b) through cyclic processes, by which the system is left unchanged, while the total entropy of the surroundings is increased. These two ways help to understand the processes of life. This topic is mostly beyond the scope of this present article, but has been considered by several authors, such as Erwin Schrödinger, Léon Brillouin and Isaac Asimov. It is also the topic of current research.
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表述热力学主要有两种方式:(a)描述从一种热力学平衡状态到另一种状态的路径,(b)通过系统保持不变但周围环境的总熵增加的循环过程。这两种方法有助于理解生命过程。这个话题大大超出了本文的范围,但是已经有一些研究者考虑过这个问题,比如'''<font color = '#ff8000'>薛定谔Erwin Schrödinger</font>'''、'''<font color = '#ff8000'>布里渊Léon Brillouin</font>'''和'''<font color = '#ff8000'>阿西莫夫Isaac Asimov</font>'''。这也是当前研究的主题。
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To a fair approximation, living organisms may be considered as examples of (b). Approximately, an animal's physical state cycles by the day, leaving the animal nearly unchanged. Animals take in food, water, and oxygen, and, as a result of [[metabolism]], give out breakdown products and heat. Plants [[Photosynthesis|take in radiative energy]] from the sun, which may be regarded as heat, and carbon dioxide and water. They give out oxygen. In this way they grow. Eventually they die, and their remains rot away, turning mostly back into carbon dioxide and water. This can be regarded as a cyclic process. Overall, the sunlight is from a high temperature source, the sun, and its energy is passed to a lower temperature sink, i.e. radiated into space. This is an increase of entropy of the surroundings of the plant. Thus animals and plants obey the second law of thermodynamics, considered in terms of cyclic processes. Simple concepts of efficiency of heat engines are hardly applicable to this problem because they assume closed systems.
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To a fair approximation, living organisms may be considered as examples of (b). Approximately, an animal's physical state cycles by the day, leaving the animal nearly unchanged. Animals take in food, water, and oxygen, and, as a result of metabolism, give out breakdown products and heat. Plants take in radiative energy from the sun, which may be regarded as heat, and carbon dioxide and water. They give out oxygen. In this way they grow. Eventually they die, and their remains rot away, turning mostly back into carbon dioxide and water. This can be regarded as a cyclic process. Overall, the sunlight is from a high temperature source, the sun, and its energy is passed to a lower temperature sink, i.e. radiated into space. This is an increase of entropy of the surroundings of the plant. Thus animals and plants obey the second law of thermodynamics, considered in terms of cyclic processes. Simple concepts of efficiency of heat engines are hardly applicable to this problem because they assume closed systems.
从近似的角度来看,生命体可以被认为是(b)的一个例子。近似地,一只动物的身体状态每天循环,使得它几乎没有什么变化。动物吸收食物、水和氧气,经过'''<font color = '#ff8000'>新陈代谢metabolism</font>''',输出分解的产物和热<s>量</s>。植物吸收来自太阳的辐射能量,这可以认为是热<s>量</s>,以及二氧化碳和水,然后它们释放氧气。它们就是这样生长的。<font color = 'blue'>它们</font>最终会死亡,尸体腐烂,大部分重新变成二氧化碳和水。这可以看作是一个循环过程。总的来说,阳光来自一个高温的源——太阳,它的能量被传递到一个较低的温度源,即向太空辐射。这个过程使得植物周围环境的熵增加。因此从循环过程的角度来看,动物和植物服从热力学第二定律。简单的热机效率概念很难适用于这个问题,因为它们假定系统是封闭的。
从近似的角度来看,生命体可以被认为是(b)的一个例子。近似地,一只动物的身体状态每天循环,使得它几乎没有什么变化。动物吸收食物、水和氧气,经过'''<font color = '#ff8000'>新陈代谢metabolism</font>''',输出分解的产物和热<s>量</s>。植物吸收来自太阳的辐射能量,这可以认为是热<s>量</s>,以及二氧化碳和水,然后它们释放氧气。它们就是这样生长的。<font color = 'blue'>它们</font>最终会死亡,尸体腐烂,大部分重新变成二氧化碳和水。这可以看作是一个循环过程。总的来说,阳光来自一个高温的源——太阳,它的能量被传递到一个较低的温度源,即向太空辐射。这个过程使得植物周围环境的熵增加。因此从循环过程的角度来看,动物和植物服从热力学第二定律。简单的热机效率概念很难适用于这个问题,因为它们假定系统是封闭的。
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From the thermodynamic viewpoint that considers (a), passages from one equilibrium state to another, only a roughly approximate picture appears, because living organisms are never in states of thermodynamic equilibrium. Living organisms must often be considered as open systems, because they take in nutrients and give out waste products. Thermodynamics of open systems is currently often considered in terms of passages from one state of thermodynamic equilibrium to another, or in terms of flows in the approximation of local thermodynamic equilibrium. The problem for living organisms may be further simplified by the approximation of assuming a steady state with unchanging flows. General principles of entropy production for such approximations are subject to [[Non-equilibrium thermodynamics|unsettled current debate or research]]. Nevertheless, ideas derived from this viewpoint on the second law of thermodynamics are enlightening about living creatures.
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From the thermodynamic viewpoint that considers (a), passages from one equilibrium state to another, only a roughly approximate picture appears, because living organisms are never in states of thermodynamic equilibrium. Living organisms must often be considered as open systems, because they take in nutrients and give out waste products. Thermodynamics of open systems is currently often considered in terms of passages from one state of thermodynamic equilibrium to another, or in terms of flows in the approximation of local thermodynamic equilibrium. The problem for living organisms may be further simplified by the approximation of assuming a steady state with unchanging flows. General principles of entropy production for such approximations are subject to unsettled current debate or research. Nevertheless, ideas derived from this viewpoint on the second law of thermodynamics are enlightening about living creatures.
In systems that do not require for their descriptions the general theory of relativity, bodies always have positive [[heat capacity]], meaning that the temperature rises with energy. Therefore, when energy flows from a high-temperature object to a low-temperature object, the source temperature is decreased while the sink temperature is increased; hence temperature differences tend to diminish over time. This is not always the case for systems in which the gravitational force is important and the general theory of relativity is required. Such systems can spontaneously change towards uneven spread of mass and energy. This applies to the universe in large scale, and consequently it may be difficult or impossible to apply the second law to it.<ref name="Grandy 151">Grandy, W.T. (Jr) (2008), p. 151.</ref> Beyond this, the thermodynamics of systems described by the general theory of relativity is beyond the scope of the present article.
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In systems that do not require for their descriptions the general theory of relativity, bodies always have positive heat capacity, meaning that the temperature rises with energy. Therefore, when energy flows from a high-temperature object to a low-temperature object, the source temperature is decreased while the sink temperature is increased; hence temperature differences tend to diminish over time. This is not always the case for systems in which the gravitational force is important and the general theory of relativity is required. Such systems can spontaneously change towards uneven spread of mass and energy. This applies to the universe in large scale, and consequently it may be difficult or impossible to apply the second law to it. Beyond this, the thermodynamics of systems described by the general theory of relativity is beyond the scope of the present article.
在不需要对其广义相对论解释的系统中,物体始终具有正热容,这意味着温度随能量而升高。因此,当能量从高温物体流向低温物体时,发射源温度降低而冷源温度升高;因此,温差会随着时间的流逝而减小。对于引力很重要并且需要广义相对论的系统而言,情况并非总是如此。这样的系统可以自发地向质量和能量不均匀的分布转变。这适用于大规模的宇宙,因此可能很难或不可能对它应用第二定律。<ref name="Grandy 151">Grandy, W.T. (Jr) (2008), p. 151.</ref>除此之外,广义相对论描述的系统的热力学超出了本文的范围。
==Non-equilibrium states==
==Non-equilibrium states==
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== Non-equilibrium states 非平衡状态 ==
== Non-equilibrium states 非平衡状态 ==
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The theory of classical or [[thermodynamic equilibrium|equilibrium thermodynamics]] is idealized. A main postulate or assumption, often not even explicitly stated, is the existence of systems in their own internal states of thermodynamic equilibrium. In general, a region of space containing a physical system at a given time, that may be found in nature, is not in thermodynamic equilibrium, read in the most stringent terms. In looser terms, nothing in the entire universe is or has ever been truly in exact thermodynamic equilibrium.<ref name="Grandy 151"/><ref>Callen, H.B. (1960/1985), p. 15.</ref>
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The theory of classical or equilibrium thermodynamics is idealized. A main postulate or assumption, often not even explicitly stated, is the existence of systems in their own internal states of thermodynamic equilibrium. In general, a region of space containing a physical system at a given time, that may be found in nature, is not in thermodynamic equilibrium, read in the most stringent terms. In looser terms, nothing in the entire universe is or has ever been truly in exact thermodynamic equilibrium.
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经典热力学或平衡热力学理论是理想化的。其主要假定或假设(通常甚至没有明确地陈述),是基于系统处在自身内部的热力学平衡状态。通常,在自然界可能发现的,在给定时间包含物理系统的空间区域,其热力学平衡状态并不是能用最严格的术语来表示。用较宽泛的术语来说,整个宇宙中没有任何东西是或曾经是真正处于精确的热力学平衡状态中。<ref>Callen, H.B. (1960/1985), p. 15.</ref>
For purposes of physical analysis, it is often enough convenient to make an assumption of [[thermodynamic equilibrium]]. Such an assumption may rely on trial and error for its justification. If the assumption is justified, it can often be very valuable and useful because it makes available the theory of thermodynamics. Elements of the equilibrium assumption are that a system is observed to be unchanging over an indefinitely long time, and that there are so many particles in a system, that its particulate nature can be entirely ignored. Under such an equilibrium assumption, in general, there are no macroscopically detectable [[thermal fluctuations|fluctuations]]. There is an exception, the case of [[critical point (thermodynamics)|critical states]], which exhibit to the naked eye the phenomenon of [[critical opalescence]]. For laboratory studies of critical states, exceptionally long observation times are needed.
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For purposes of physical analysis, it is often enough convenient to make an assumption of thermodynamic equilibrium. Such an assumption may rely on trial and error for its justification. If the assumption is justified, it can often be very valuable and useful because it makes available the theory of thermodynamics. Elements of the equilibrium assumption are that a system is observed to be unchanging over an indefinitely long time, and that there are so many particles in a system, that its particulate nature can be entirely ignored. Under such an equilibrium assumption, in general, there are no macroscopically detectable fluctuations. There is an exception, the case of critical states, which exhibit to the naked eye the phenomenon of critical opalescence. For laboratory studies of critical states, exceptionally long observation times are needed.
为了进行物理分析,通常做一个热力学平衡的假设就足够方便可行。 这样的假设可能依赖于反复试验和试错来证明其合理性。如果假设是合理的,那么它通常会非常有价值,因为它使热力学理论成为可能。平衡假设的要素是,观察到的系统会无限期地保持不变,并且因为系统中有很多粒子,以至于完全可以忽略其微粒的本质。通常在这种平衡假设下,不存在一个宏观上可检测到的波动。临界状态是一个例外,肉眼可以观察到临界'''<font color = '#ff8000'>乳光现象opalescence</font>'''。对于临界状态的实验室研究,需要非常长的观察时间。
为了进行物理分析,通常做一个热力学平衡的假设就足够方便可行。 这样的假设可能依赖于反复试验和试错来证明其合理性。如果假设是合理的,那么它通常会非常有价值,因为它使热力学理论成为可能。平衡假设的要素是,观察到的系统会无限期地保持不变,并且因为系统中有很多粒子,以至于完全可以忽略其微粒的本质。通常在这种平衡假设下,不存在一个宏观上可检测到的波动。临界状态是一个例外,肉眼可以观察到临界'''<font color = '#ff8000'>乳光现象opalescence</font>'''。对于临界状态的实验室研究,需要非常长的观察时间。
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In all cases, the assumption of [[thermodynamic equilibrium]], once made, implies as a consequence that no putative candidate "fluctuation" alters the entropy of the system.
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In all cases, the assumption of thermodynamic equilibrium, once made, implies as a consequence that no putative candidate "fluctuation" alters the entropy of the system.
It can easily happen that a physical system exhibits internal macroscopic changes that are fast enough to invalidate the assumption of the constancy of the entropy. Or that a physical system has so few particles that the particulate nature is manifest in observable fluctuations. Then the assumption of thermodynamic equilibrium is to be abandoned. There is no unqualified general definition of entropy for non-equilibrium states.<ref>Lieb, E.H., Yngvason, J. (2003), p. 190.</ref>
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It can easily happen that a physical system exhibits internal macroscopic changes that are fast enough to invalidate the assumption of the constancy of the entropy. Or that a physical system has so few particles that the particulate nature is manifest in observable fluctuations. Then the assumption of thermodynamic equilibrium is to be abandoned. There is no unqualified general definition of entropy for non-equilibrium states.
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物理系统很容易发生内部宏观变化,其速度之快足以使熵的恒定性假设失效。或物理系统中的粒子太少,以至于微粒的本质在可观测的波动中显而易见。那么热力学平衡的假设就会被放弃。对于非平衡态,熵没有绝对的通俗定义。<ref>Lieb, E.H., Yngvason, J. (2003), p. 190.</ref>
There are intermediate cases, in which the assumption of local [[thermodynamic equilibrium]] is a very good approximation,<ref>Gyarmati, I. (1967/1970), pp. 4-14.</ref><ref>Glansdorff, P., Prigogine, I. (1971).</ref><ref>[[Gottfried Wilhelm Leibniz Prize|Müller, I.]] (1985).</ref><ref>[[Gottfried Wilhelm Leibniz Prize|Müller, I.]] (2003).</ref> but strictly speaking it is still an approximation, not theoretically ideal.
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There are intermediate cases, in which the assumption of local thermodynamic equilibrium is a very good approximation, but strictly speaking it is still an approximation, not theoretically ideal.
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还有一些中间情况,其中局部热力学平衡的假设是一个非常好的近似,</ref><ref>Glansdorff, P., Prigogine, I. (1971).</ref><ref>[[Gottfried Wilhelm Leibniz Prize|Müller, I.]] (1985).</ref><ref>[[Gottfried Wilhelm Leibniz Prize|Müller, I.]] (2003).</ref>但严格地说它仍然是一个近似值,不是理论上的理想值。
For non-equilibrium situations in general, it may be useful to consider statistical mechanical definitions of other quantities that may be conveniently called 'entropy', but they should not be confused or conflated with thermodynamic entropy properly defined for the second law. These other quantities indeed belong to statistical mechanics, not to thermodynamics, the primary realm of the second law.
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For non-equilibrium situations in general, it may be useful to consider statistical mechanical definitions of other quantities that may be conveniently called 'entropy', but they should not be confused or conflated with thermodynamic entropy properly defined for the second law. These other quantities indeed belong to statistical mechanics, not to thermodynamics, the primary realm of the second law.
The physics of macroscopically observable fluctuations is beyond the scope of this article.
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The physics of macroscopically observable fluctuations is beyond the scope of this article.
宏观上可观察到的波动的物理学超出了本文的范围。
宏观上可观察到的波动的物理学超出了本文的范围。
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==Arrow of time==
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== Arrow of time 时间之箭 ==
时间之箭
时间之箭
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{{Further information|Entropy (arrow of time)}}Thermodynamic Asymmetry in Time
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Thermodynamic Asymmetry in Time
时间中的热力学不对称性
时间中的热力学不对称性
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The second law of thermodynamics is a physical law that is not symmetric to reversal of the time direction. This does not conflict with notions that have been observed of the fundamental laws of physics, namely [[CPT symmetry]], since the second law applies statistically, it is hypothesized, on time-asymmetric ''boundary conditions''.<ref>{{cite web|first=Craig|last=Callender|url=https://plato.stanford.edu/archives/fall2011/entries/time-thermo/|title=Thermodynamic Asymmetry in Time|encyclopedia=Stanford Encyclopedia of Philosophy|date=29 July 2011}}</ref>
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The second law of thermodynamics is a physical law that is not symmetric to reversal of the time direction. This does not conflict with symmetries observed in the fundamental laws of physics (particularly CPT symmetry) since the second law applies statistically on time-asymmetric boundary conditions.[78] The second law has been related to the difference between moving forwards and backwards in time, or to the principle that cause precedes effect (the causal arrow of time, or causality).[79]
热力学第二定律是在时间方向上不对称的物理定律。这与在物理学基本定律中观察到的对称性概念(特别是CPT对称性)<s>并</s>没有冲突,因为第二定律在统计上适用于时间非对称边界条件。第二定律与时间向前和向后移动之间的差异有关,或者与原因先于结果的原理(时间的因果关系或因果关系)有关。<ref>{{cite web|first=Craig|last=Callender|url=https://plato.stanford.edu/archives/fall2011/entries/time-thermo/|title=Thermodynamic Asymmetry in Time|encyclopedia=Stanford Encyclopedia of Philosophy|date=29 July 2011}}</ref>
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The second law has been proposed to supply a partial explanation of the difference between moving forward and backwards in time, such as why the cause precedes the effect ([[Arrow of time#The causal arrow of time|the causal arrow of time]]).<ref>{{cite book | first = J.J.| last = Halliwell | title = Physical Origins of Time Asymmetry| publisher = Cambridge | year = 1994| isbn = 978-0-521-56837-1|display-authors=etal}} chapter 6</ref>
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The second law has been proposed to supply a partial explanation of the difference between moving forward and backwards in time, such as why the cause precedes the effect (the causal arrow of time).
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第二定律被提出来侧面解释时间向前和向后移动的区别,例如为什么原因先于结果(因果关系的时间箭头)。.<ref>{{cite book | first = J.J.| last = Halliwell | title = Physical Origins of Time Asymmetry| publisher = Cambridge | year = 1994| isbn = 978-0-521-56837-1|display-authors=etal}} chapter 6</ref>
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第二定律被提出来侧面解释时间向前和向后移动的区别,例如为什么原因先于结果(因果关系的时间箭头)。
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==Irreversibility==
== Irreversibility 不可逆性 ==
== Irreversibility 不可逆性 ==
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Irreversibility in [[thermodynamic process]]es is a consequence of the asymmetric character of thermodynamic operations, and not of any internally irreversible microscopic properties of the bodies. Thermodynamic operations are macroscopic external interventions imposed on the participating bodies, not derived from their internal properties. There are reputed "paradoxes" that arise from failure to recognize this.
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Irreversibility in thermodynamic processes is a consequence of the asymmetric character of thermodynamic operations, and not of any internally irreversible microscopic properties of the bodies. Thermodynamic operations are macroscopic external interventions imposed on the participating bodies, not derived from their internal properties. There are reputed "paradoxes" that arise from failure to recognize this.
[[Loschmidt's paradox]], also known as the reversibility paradox, is the objection that it should not be possible to deduce an irreversible process from the time-symmetric dynamics that describe the microscopic evolution of a macroscopic system.
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Loschmidt's paradox, also known as the reversibility paradox, is the objection that it should not be possible to deduce an irreversible process from the time-symmetric dynamics that describe the microscopic evolution of a macroscopic system.
In the opinion of [[Erwin Schrödinger|Schrödinger]], "It is now quite obvious in what manner you have to reformulate the law of entropy{{snd}}or for that matter, all other irreversible statements{{snd}}so that they be capable of being derived from reversible models. You must not speak of one isolated system but at least of two, which you may for the moment consider isolated from the rest of the world, but not always from each other."<ref>[[Erwin Schrödinger|Schrödinger, E.]] (1950), p. 192.</ref> The two systems are isolated from each other by the wall, until it is removed by the thermodynamic operation, as envisaged by the law. The thermodynamic operation is externally imposed, not subject to the reversible microscopic dynamical laws that govern the constituents of the systems. It is the cause of the irreversibility. The statement of the law in this present article complies with Schrödinger's advice. The cause–effect relation is logically prior to the second law, not derived from it.
In the opinion of Schrödinger, "It is now quite obvious in what manner you have to reformulate the law of entropyor for that matter, all other irreversible statementsso that they be capable of being derived from reversible models. You must not speak of one isolated system but at least of two, which you may for the moment consider isolated from the rest of the world, but not always from each other." The two systems are isolated from each other by the wall, until it is removed by the thermodynamic operation, as envisaged by the law. The thermodynamic operation is externally imposed, not subject to the reversible microscopic dynamical laws that govern the constituents of the systems. It is the cause of the irreversibility. The statement of the law in this present article complies with Schrödinger's advice. The cause–effect relation is logically prior to the second law, not derived from it.
The [[Poincaré recurrence theorem]] considers a theoretical microscopic description of an isolated physical system. This may be considered as a model of a thermodynamic system after a thermodynamic operation has removed an internal wall. The system will, after a sufficiently long time, return to a microscopically defined state very close to the initial one. The Poincaré recurrence time is the length of time elapsed until the return. It is exceedingly long, likely longer than the life of the universe, and depends sensitively on the geometry of the wall that was removed by the thermodynamic operation. The recurrence theorem may be perceived as apparently contradicting the second law of thermodynamics. More obviously, however, it is simply a microscopic model of thermodynamic equilibrium in an isolated system formed by removal of a wall between two systems. For a typical thermodynamical system, the recurrence time is so large (many many times longer than the lifetime of the universe) that, for all practical purposes, one cannot observe the recurrence. One might wish, nevertheless, to imagine that one could wait for the Poincaré recurrence, and then re-insert the wall that was removed by the thermodynamic operation. It is then evident that the appearance of irreversibility is due to the utter unpredictability of the Poincaré recurrence given only that the initial state was one of thermodynamic equilibrium, as is the case in macroscopic thermodynamics. Even if one could wait for it, one has no practical possibility of picking the right instant at which to re-insert the wall. The Poincaré recurrence theorem provides a solution to Loschmidt's paradox. If an isolated thermodynamic system could be monitored over increasingly many multiples of the average Poincaré recurrence time, the thermodynamic behavior of the system would become invariant under time reversal.
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The Poincaré recurrence theorem considers a theoretical microscopic description of an isolated physical system. This may be considered as a model of a thermodynamic system after a thermodynamic operation has removed an internal wall. The system will, after a sufficiently long time, return to a microscopically defined state very close to the initial one. The Poincaré recurrence time is the length of time elapsed until the return. It is exceedingly long, likely longer than the life of the universe, and depends sensitively on the geometry of the wall that was removed by the thermodynamic operation. The recurrence theorem may be perceived as apparently contradicting the second law of thermodynamics. More obviously, however, it is simply a microscopic model of thermodynamic equilibrium in an isolated system formed by removal of a wall between two systems. For a typical thermodynamical system, the recurrence time is so large (many many times longer than the lifetime of the universe) that, for all practical purposes, one cannot observe the recurrence. One might wish, nevertheless, to imagine that one could wait for the Poincaré recurrence, and then re-insert the wall that was removed by the thermodynamic operation. It is then evident that the appearance of irreversibility is due to the utter unpredictability of the Poincaré recurrence given only that the initial state was one of thermodynamic equilibrium, as is the case in macroscopic thermodynamics.Even if one could wait for it, one has no practical possibility of picking the right instant at which to re-insert the wall. The Poincaré recurrence theorem provides a solution to Loschmidt's paradox. If an isolated thermodynamic system could be monitored over increasingly many multiples of the average Poincaré recurrence time, the thermodynamic behavior of the system would become invariant under time reversal.
庞加莱始态复现定理考虑了孤立物理系统的理论微观描述。
庞加莱始态复现定理考虑了孤立物理系统的理论微观描述。
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{{main article|Maxwell's demon}}
{{main article|Maxwell's demon}}
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[[James Clerk Maxwell]] imagined one container divided into two parts, ''A'' and ''B''. Both parts are filled with the same [[gas]] at equal temperatures and placed next to each other, separated by a wall. Observing the [[molecule]]s on both sides, an imaginary [[demon]] guards a microscopic trapdoor in the wall. When a faster-than-average molecule from ''A'' flies towards the trapdoor, the demon opens it, and the molecule will fly from ''A'' to ''B''. The average [[speed]] of the molecules in ''B'' will have increased while in ''A'' they will have slowed down on average. Since average molecular speed corresponds to temperature, the temperature decreases in ''A'' and increases in ''B'', contrary to the second law of thermodynamics.
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James Clerk Maxwell imagined one container divided into two parts, A and B. Both parts are filled with the same gas at equal temperatures and placed next to each other, separated by a wall. Observing the molecules on both sides, an imaginary demon guards a microscopic trapdoor in the wall. When a faster-than-average molecule from A flies towards the trapdoor, the demon opens it, and the molecule will fly from A to B. The average speed of the molecules in B will have increased while in A they will have slowed down on average. Since average molecular speed corresponds to temperature, the temperature decreases in A and increases in B, contrary to the second law of thermodynamics.
'''麦克斯韦 James Clerk Maxwell'''设想一个容器分为A和B两部分。两部分均在相同温度下充满相同的气体,并彼此相邻由内壁隔开。一个虚构的妖精看守着一个内壁上的微型陷门,并观察者内壁两边的分子。当来自A的速度快于平均水平的分子飞向门时,妖精将门打开,该分子将从A飞向B。B中分子的平均速度将增加,而A中分子的平均速度将降低。由于平均分子速度与温度相对应,因此与热力学第二定律相反,温度在A中降低,在B中升高。
'''麦克斯韦 James Clerk Maxwell'''设想一个容器分为A和B两部分。两部分均在相同温度下充满相同的气体,并彼此相邻由内壁隔开。一个虚构的妖精看守着一个内壁上的微型陷门,并观察者内壁两边的分子。当来自A的速度快于平均水平的分子飞向门时,妖精将门打开,该分子将从A飞向B。B中分子的平均速度将增加,而A中分子的平均速度将降低。由于平均分子速度与温度相对应,因此与热力学第二定律相反,温度在A中降低,在B中升高。
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One response to this question was suggested in 1929 by [[Leó Szilárd]] and later by [[Léon Brillouin]]. Szilárd pointed out that a real-life Maxwell's demon would need to have some means of measuring molecular speed, and that the act of acquiring information would require an expenditure of energy.
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One response to this question was suggested in 1929 by Leó Szilárd and later by Léon Brillouin. Szilárd pointed out that a real-life Maxwell's demon would need to have some means of measuring molecular speed, and that the act of acquiring information would require an expenditure of energy.
Maxwell's 'demon' repeatedly alters the permeability of the wall between ''A'' and ''B''. It is therefore performing [[thermodynamic operation]]s on a microscopic scale, not just observing ordinary spontaneous or natural macroscopic thermodynamic processes.
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Maxwell's 'demon' repeatedly alters the permeability of the wall between A and B. It is therefore performing thermodynamic operations on a microscopic scale, not just observing ordinary spontaneous or natural macroscopic thermodynamic processes.
麦克斯韦的“妖”重复地改变 A 和 B 之间壁的热透性。因此,它是在微观尺度上执行热力学操作,而不仅仅是观察普通的自发或自然的宏观热力学过程。
麦克斯韦的“妖”重复地改变 A 和 B 之间壁的热透性。因此,它是在微观尺度上执行热力学操作,而不仅仅是观察普通的自发或自然的宏观热力学过程。
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==Quotations==
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==Quotations==
语录
语录
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{{quote|The law that entropy always increases holds, I think, the supreme position among the [[Laws of science|laws of Nature]]. If someone points out to you that your pet theory of the [[universe]] is in disagreement with [[Maxwell's equations]] – then so much the worse for Maxwell's equations. If it is found to be contradicted by observation – well, these experimentalists do bungle things sometimes. But if your theory is found to be against the second law of thermodynamics I can give you no hope; there is nothing for it but to collapse in deepest humiliation.|Sir [[Arthur Stanley Eddington]], ''The Nature of the Physical World'' (1927)}}
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The law that entropy always increases holds, I think, the supreme position among the laws of Nature. If someone points out to you that your pet theory of the universe is in disagreement with Maxwell's equations – then so much the worse for Maxwell's equations. If it is found to be contradicted by observation – well, these experimentalists do bungle things sometimes. But if your theory is found to be against the second law of thermodynamics I can give you no hope; there is nothing for it but to collapse in deepest humiliation.
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— Sir Arthur Stanley Eddington, The Nature of the Physical World (1927)
{{quote|There have been nearly as many formulations of the second law as there have been discussions of it.|Philosopher / Physicist [[Percy Williams Bridgman|P.W. Bridgman]], (1941)}}
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There have been nearly as many formulations of the second law as there have been discussions of it.
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— Philosopher / Physicist P.W. Bridgman, (1941)
关于第二定律的公式几乎与关于第二定律的讨论一样多。
关于第二定律的公式几乎与关于第二定律的讨论一样多。
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{{quote|Clausius is the author of the sibyllic utterance, "The energy of the universe is constant; the entropy of the universe tends to a maximum." The objectives of continuum thermomechanics stop far short of explaining the "universe", but within that theory we may easily derive an explicit statement in some ways reminiscent of Clausius, but referring only to a modest object: an isolated body of finite size.|[[Clifford Truesdell|Truesdell, C.]], Muncaster, R. G. (1980). ''Fundamentals of Maxwell's Kinetic Theory of a Simple Monatomic Gas, Treated as a Branch of Rational Mechanics'', Academic Press, New York, {{ISBN|0-12-701350-4}}, p. 17.}}
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Clausius is the author of the sibyllic utterance, "The energy of the universe is constant; the entropy of the universe tends to a maximum." The objectives of continuum thermomechanics stop far short of explaining the "universe", but within that theory we may easily derive an explicit statement in some ways reminiscent of Clausius, but referring only to a modest object: an isolated body of finite size.
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— Truesdell, C., Muncaster, R. G. (1980). Fundamentals of Maxwell's Kinetic Theory of a Simple Monatomic Gas, Treated as a Branch of Rational Mechanics, Academic Press, New York, ISBN 0-12-701350-4, p. 17.
--趣木木(讨论)The second law has been expressed in many ways. Its first formulation is credited to the French scientist Sadi Carnot, who in 1824 showed that there is an upper limit to the efficiency of conversion of heat to work in a heat engine. This aspect of the second law is often named after Carnot.[4] 这个是对应的原文 可能是百科进行了迭代
Heat flow from hot water to cold water. 热总是从热水流向冷水
热力学第一定律 First Law Of Thermodynamics定义了热力学系统所涉及到的内能 Internal Energy,[5][6]并体现了能量守恒定律。热力学第二定律与自然过程Natural Processes[7]的方向有关。它断言自然过程只在一种意义上进行,且不可逆 。例如,当有了传导和辐射的(传播)路径时,热总是自发地从一个较热的物体流向一个较冷的物体。 这种现象可以用[8][9]熵Entropy来解释。
--大白(讨论)这里是不是少了一段原文?
若一个孤立系统Isolated System最初在具有隔热内壁的系统内维持热力学平衡,通过一些操作使内壁透热,则该系统可自发地演变,最终达到一个新的内部热力学平衡,且其总熵S增加。If an isolated system is held initially in internal thermodynamic equilibrium by internal partitioning impermeable walls, and then some operation makes the walls more permeable, then the system spontaneously evolves to reach a final new internal thermodynamic equilibrium, and its total entropy, S, increases.
在假想的可逆过程中,系统的熵的无穷小增量[math]\displaystyle{ dS }[/math]被定义为由无穷小的热[math]\displaystyle{ δQ }[/math]传递到一个封闭系统(允许能量进入或出去,但不允许物质传递的系统)除以该平衡系统和提供热的环境的共同温度 [math]\displaystyle{ T }[/math]:[10]
这是因为在这种情况下的一般过程可能包括周围环境对系统所做的功,该功在系统内部会产生摩擦或粘滞效应,此时一个化学反应可能正在系统内部进行,或因为热传递实际上是不可逆地发生,系统温度[math]\displaystyle{ T }[/math]和周围环境温度[math]\displaystyle{ T_surr }[/math]之间的差异驱动了热传递的发生。[13][14] 注意该等式也适用于纯热流Pure Heat Flow[15]
[math]\displaystyle{ \mathrm dS = \frac{\delta Q}{T} \,\, \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, \text {(actually possible quasistatic irreversible process without composition change 实际上可能的,不改变成分的准静态不可逆性).} }[/math]
which is the basis of the accurate determination of the absolute entropy of pure substances from measured heat capacity curves and entropy changes at phase transitions, i.e. by calorimetry.[16] [11] Introducing a set of internal variables {\displaystyle \xi }\xi to describe the deviation of a thermodynamic system in physical equilibrium (with the required well-defined uniform pressure P and temperature T)[15] from the chemical equilibrium state, one can record the equality
热力学第零定律是指如果两个热力学系统都与第三个热力学系统处于热平衡(温度相同)状态,则它们彼此也必定处于热平衡状态。热力学第零定律在它这个简短叙述中让人们认识到热平衡关系中的两个物体具有相同的温度,特别是当一个被测物体与一个参考测温物体具有相同的温度时,[19]对于两个处于热平衡状态的物体,有无限多的经验温标empirical temperature scales,这通常取决于特定参考温度体的性质。热力学第二定律允许区分温度标度temperature scale,它定义了一个绝对的热力学温度,与任何特定的参考温度体的性质无关。[20][21]
Various statements of the law热力学第二定律的不同表述
热力学第二定律可以用许多特定的方式来表达,[22] 最突出的经典陈述是 克劳修斯 Rudolf Clausius (1854)表述,开尔文 克劳修斯 Kelvin Clausius (1851)表述,以及康斯坦丁·卡拉西奥多里 Constantin Carathéodory(1909)在公理化热力学axiomatic thermodynamics中的表述。这些表述用一般的物理术语来描述定律,引用某些过程的不可能性。克劳修斯和开尔文表述被证明是等价的。
Carnot's principle卡诺原理
热力学第二定律的历史起源[23]是卡诺原理Carnot's principle。
它指的是卡诺热机Carnot heat engine的一个循环,卡诺热机以准静态quasi-static的极限慢速运转,因此热和功在子系统之间进行传递,子系统总是处于它们自己内部的热力学平衡状态。
卡诺热机是研究热机效率的工程师特别感兴趣的理想装置。
当卡诺发现卡诺原理时,热量理论caloric theory of heat还没有得到重视,热力学第一定律还没有得到承认,熵的概念还没有数学表达。
根据第一定律的解释,它在物理上等同于热力学第二定律,并沿用至今。
在热力学第一定律被发现之前,卡诺最初的论点是从热量理论的观点出发的。
下面是他书中的一些例子:
...wherever there exists a difference of temperature, motive power can be produced.[24]
...wherever there exists a difference of temperature, motive power can be produced.
使用两个热源与工作物质交换热源(一个高温热源温度[math]\displaystyle{ T_1 }[/math]和一个低温热源温度[math]\displaystyle{ T_2 }[/math])的卡诺热机是最有效的热机。 A Carnot engine operated in this way is the most efficient possible heat engine using those two temperatures.
Clausius statement克劳修斯表述
1850年,德国科学家鲁道夫·克劳修斯 Rudolf Clausius 通过研究热传递和功之间的关系,为热力学第二定律奠定了基础。他在1854年用德语发表的论文中所提及的热力学第二定律定义被称为克劳修斯表述:
不可能把热从低温物体传递到高温物体而不产生其他影响。
克劳修斯的表述使用了“热通道Passage Of Heat”的概念。
在热力学的讨论中,通常这意味着“能量作为热的形式的净转移” ,而不是指其他方式的转移。
--Dorr(讨论)准静态转移的热量值是一个可积过程函数 存疑
--嘉树(讨论)本句的修改供讨论。可积函数的英文应该是Integrable function。但是什么是完整的函数存疑,是连续的函数?
--小头盔(讨论)这里建议标注一下 完整的过程函数 holonomic process function
Statement for a system that has a known expression of its internal energy as a function of its extensive state variables 一个其内能有已知表达式(其扩展状态变量的函数)的系统的表述
写成广泛性质(质量,体积,熵……)的函数时,第二定律被证明等价于弱凸函数内能 U。The second law has been shown to be equivalent to the internal energy U being a weakly convex function, when written as a function of extensive properties (mass, volume, entropy, ...).[52][53]
所有在两个热源之间工作的可逆热机的效率与在两相同热源之间工作的卡诺机相等。All irreversible heat engines between two heat reservoirs are less efficient than a Carnot engine operating between the same reservoirs.
--Dorr(讨论)改成同一个正确吗??????????????????????????
--嘉树(讨论)我不太理解什么叫between the same reservoirs。我的理解是效率不取决于热源这个实体,而取决于温差,所以就按照两个热源和一个相同的热源相对应地翻译了。但是这一句我仍然有疑问,因为两个热源之间工作和两相同热源之间工作,似乎还不构成相互比较的关系。已经标绿
等号在可逆情况下成立,[54]严格不等号在不可逆情况下成立。可逆情况下引入状态函数熵。这是因为在循环过程中,状态功能的变化相对于状态功能为零。This is because in cyclic processes the variation of a state function is zero from state functionality.
--Dorr(讨论)末句存疑
--嘉树(讨论) 我也没看懂,按照字面意思修改了一下
--小头盔(讨论)感觉修改后的句子还是怪怪的,这里标成疑难句吧 这是因为在循环过程中,状态功能的变化相对于状态功能为零。This is because in cyclic processes the variation of a state function is zero from state functionality.
[math]\displaystyle{ E = U - T_R S + p_R V - \sum \mu_{iR} N_i }[/math]
[math]\displaystyle{ E = U - T_R S + p_R V - \sum \mu_{iR} N_i }[/math]
[math]\displaystyle{ E = U - T_R S + p_R V - \sum \mu_{iR} N_i }[/math]
因此,第二定律意味着,对于任何可以简单地被视为分为一个子系统和一个与之接触的无限温度和压力热源 Reservoir 的过程,The Second Law therefore implies that for any process which can be considered as divided simply into a subsystem, and an unlimited temperature and pressure reservoir with which it is in contact,
[math]\displaystyle{ dE + \delta w_u \le 0 \, }[/math]
[math]\displaystyle{ dE + \delta w_u \le 0 \, }[/math]
[math]\displaystyle{ dE + \delta w_u \le 0 \, }[/math]
[math]\displaystyle{ dS_{tot} \ge 0 }[/math] Is equivalent to [math]\displaystyle{ dE + \delta w_u \le 0 }[/math]
[math]\displaystyle{ dS_{tot} \ge 0 }[/math] Is equivalent to [math]\displaystyle{ dE + \delta w_u \le 0 }[/math]
[math]\displaystyle{ dS_{tot} \ge 0 }[/math] Is equivalent to [math]\displaystyle{ dE + \delta w_u \le 0 }[/math]
这个表达式和相关的参考状态允许设计工程师在宏观尺度(高于热力学极限)下使用第二定律,而无需直接测量或考虑整个孤立系统中的熵变。(另见工艺工程师process engineer)。这些变化已经在假设中被考虑到,该假设认为所考虑的系统可以在不改变参考状态的情况下与参考状态达到平衡。将其与可逆理想状态进行比较,还可以找到一个过程或过程集合的效率(见第二定律效率second law efficiency)
这里[math]\displaystyle{ \dot S }[/math] 是进入系统的熵流,与进入系统的物质流有关。它不应该与熵的时间导数混淆。如果物质在几个地方被供给,需要取这些贡献的代数和。
Statistical mechanics
统计力学
统计力学通过假设物质是由不断运动的原子和分子组成的,来对第二定律给出了解释。系统中每个粒子的一组特定的位置和速度称为系统的微观状态,由于系统的不断运动,系统不断地改变其微观状态。统计力学假设,在平衡状态下,系统处于的每个微观状态的可能性是相等的。这个假设的提出直接导致第二定律必须在统计学意义上成立,也就是说,第二定律在平均意义上成立,其中统计学变异取决于数量级1/模板:Radic,其中 N 是系统中粒子数。在日常(宏观)情况下,违反第二定律的概率几乎为零。然而,对于粒子数量很少的系统,热力学参数,包括熵,可能显示出与第二定律预测结果的显著的统计偏差。经典热力学理论不处理这些统计变量。
(by Jie XIANG) 在通过假定一种物质由不断运动的原子和分子组成的前提下,统计力学对热力学第二定律进行了解释。系统中每个粒子其特定的位置和速度组成为系统的微观状态,由于(原子和分子的)不断运动,系统也持续改变其微观状态。统计力学假设,在系统力平衡的情况下,其微观状态其实是等可能发生的,进而能够得出结论:热力学第二定律必须在统计学意义上成立。也就是说,第二定律将保持均值不变, 其统计变化为1 /√N,N为系统中的粒子数。在日常(宏观)情况下,违反热力学第二定律的概率几乎为零,但是,对于粒子数量非常少的系统,其热力学参数(包括熵)可能会显示出与第二定律所预测的明显统计偏差。然而经典热力学理论并不处理这些统计变量。
气体动力学Kinetic theory of gases理论的第一个力学论证由麦克斯韦James Clerk Maxwell在1860年给出,指出分子碰撞引起温度均衡化,因此整体趋向于平衡 Equilibrium ; 玻尔兹曼Ludwig Boltzmann[58]在1872年提出的 H 定理H-theorem也认为,气体由于碰撞应该随着时间的推移趋向于麦克斯韦-波兹曼分布Maxwell–Boltzmann distribution。
由于洛施密特悖论Loschmidt's paradox,第二定律的导出必须对过去做出一个假设,即系统在过去的某个时刻是不相关的;这样的假设允许进行简单的概率处理。这个假设通常被认为是一个边界条件boundary condition,因此热力学第二定律最终是过去某个地方的初始条件的结果,可能是在宇宙的开始(大爆炸 the Big Bang) ,尽管也有人提出了其他场景。.[59][60][61]
基于这些假设,在统计力学中,第二定律不是一个假设,而是统计力学基本假设Statistical mechanics#Fundamental postulate|fundamental postulate的一个结果,也被称为等先验概率假设 equal prior probability postulate。这个基本假设表明,只要一个人清楚地知道,简单的概率论证只适用于未来,而对于过去,有辅助的信息来源告诉我们,它是低熵的。如果我们把熵的概念限制在热平衡系统中,那么热力学第二定律的第一部分即热孤立系统的熵只能增加,是等先验概率假设的一个显然结果。处于热平衡状态的孤立系统且具有能量[math]\displaystyle{ E }[/math]的熵表示为:
[math]\displaystyle{ S = k_{\mathrm B} \ln\left[\Omega\left(E\right)\right]\, }[/math]
[math]\displaystyle{ S = k_{\mathrm B} \ln\left[\Omega\left(E\right)\right]\, }[/math]
其中[math]\displaystyle{ \Omega\left(E\right) }[/math] 是处于 [math]\displaystyle{ E }[/math]和[math]\displaystyle{ E +\delta E\lt /math这个小区间内的量子态数目。这里的 \lt math\gt \delta E }[/math] 是一个宏观上很小的固定能量区间。严格地说,这意味着熵取决于对[math]\displaystyle{ \delta E }[/math]的选择。然而在热力学极限下(例如无穷大系统的极限),狭义的熵(单位体积或单位质量的熵)不依赖于 [math]\displaystyle{ \delta E }[/math]。
对于外部变量 x 可以定义广义力generalized force X ,因此如果 x 增加 dx,那么[math]\displaystyle{ X dx }[/math] 就是系统所做的功。例如,如果 x 是体积,那么 X 就是压强。一个已知处于能量本征态[math]\displaystyle{ E_{r} }[/math]的系统的广义力为:
[math]\displaystyle{ X = -\frac{dE_{r}}{dx} }[/math]
[math]\displaystyle{ X = -\frac{dE_{r}}{dx} }[/math]
由于系统可以在[math]\displaystyle{ \delta E }[/math] 区间内的任意能量本征态内,我们将系统的广义力定义为上述表达式的期望值:
[math]\displaystyle{ X = -\left\langle\frac{dE_{r}}{dx}\right\rangle\, }[/math]
[math]\displaystyle{ X = -\left\langle\frac{dE_{r}}{dx}\right\rangle\, }[/math]
为了计算平均值,我们按照能量本征态来划分[math]\displaystyle{ \Omega\left(E\right) }[/math],通过计算有多少能量本征态的[math]\displaystyle{ \frac{dE_{r}}{dx} }[/math]值在区间在[math]\displaystyle{ Y }[/math] 到 [math]\displaystyle{ Y + \delta Y }[/math]之间。把这个数字叫做为 [math]\displaystyle{ \Omega_{Y}\left(E\right) }[/math],我们有:
我们可以把它和由恒定能量 E 下的 x 导出来的熵联系起来。假定我们把 x 改变至 x + dx。然后因为能量本征态依赖于 x, [math]\displaystyle{ \Omega\left(E\right) }[/math] 将会改变,这导致能量本征态进入或超出[math]\displaystyle{ E }[/math] 和[math]\displaystyle{ E+\delta E }[/math] 之间的范围。让我们再次关注[math]\displaystyle{ \frac{dE_{r}}{dx} }[/math] 处于 [math]\displaystyle{ Y }[/math] 和 [math]\displaystyle{ Y + \delta Y }[/math] 之间的能量本征态。由于这些能量本征态的能量增加了 Y dx,所有这些在 E-Y dx 到 E 之间能量本征态都从 E 以下移动到 E 以上。 因此有
[math]\displaystyle{ N_{Y}\left(E\right)=\frac{\Omega_{Y}\left(E\right)}{\delta E} Y dx\, }[/math]
[math]\displaystyle{ N_{Y}\left(E\right)=\frac{\Omega_{Y}\left(E\right)}{\delta E} Y dx\, }[/math]
这些的能量本征态。如果[math]\displaystyle{ Y dx\leq\delta E }[/math],则所有这些能量本征态将移动到 [math]\displaystyle{ E }[/math] 到 [math]\displaystyle{ E+\delta E }[/math]的范围内,使得[math]\displaystyle{ \Omega }[/math]增加。从[math]\displaystyle{ E+\delta E }[/math]以下移动到[math]\displaystyle{ E+\delta E }[/math]以上的能量本征态数目为 [math]\displaystyle{ N_{Y}\left(E+\delta E\right) }[/math]。它们的差
这里 Z 是一个使所有概率之和归一化到 1 的因子,这个函数被称为配分函数Partition function (statistical mechanics)|partition function。现在我们考虑对温度和能级所依赖的外部参数的无限小的可逆改变。它遵循熵的一般公式:
--嘉树(讨论) 能级依赖温度吗?即“现在我们考虑……的可逆改变”当中,“on which the energy levels depend”修饰(1)in the external parameters,还是(2)in the temperature and in the external parameters
--小头盔(讨论)修饰in the external parameters
[math]\displaystyle{ S = -k_{\mathrm B}\sum_{j}P_{j}\ln\left(P_{j}\right) }[/math]
[math]\displaystyle{ S = -k_{\mathrm B}\sum_{j}P_{j}\ln\left(P_{j}\right) }[/math]
麦克斯韦 James Clerk Maxwell设想一个容器分为A和B两部分。两部分均在相同温度下充满相同的气体,并彼此相邻由内壁隔开。一个虚构的妖精看守着一个内壁上的微型陷门,并观察者内壁两边的分子。当来自A的速度快于平均水平的分子飞向门时,妖精将门打开,该分子将从A飞向B。B中分子的平均速度将增加,而A中分子的平均速度将降低。由于平均分子速度与温度相对应,因此与热力学第二定律相反,温度在A中降低,在B中升高。
— Truesdell, C., Muncaster, R. G. (1980). Fundamentals of Maxwell's Kinetic Theory of a Simple Monatomic Gas, Treated as a Branch of Rational Mechanics, Academic Press, New York, ISBN 0-12-701350-4, p. 17. 特雷斯德尔,C.,蒙卡斯特,R.G.(1980)。麦克斯韦的单原子气体动力学理论的基本原理,被作为“理性力学”的一个分支,纽约学术出版社,ISBN 0-12-701350-4,第1页. 17。
↑ 15.015.1 Schmidt-Rohr, K. (2014). "Expansion Work without the External Pressure, and Thermodynamics in Terms of Quasistatic Irreversible Processes" J. Chem. Educ.91: 402-409. https://dx.doi.org/10.1021/ed3008704
↑Oxtoby, D. W; Gillis, H.P., Butler, L. J. (2015).Principles of Modern Chemistry, Brooks Cole. p. 617.
↑Planck, M. (1926), p. 463, translation by Uffink, J. (2003), p. 131.
↑Roberts, J.K., Miller, A.R. (1928/1960), p. 382. This source is partly verbatim from Planck's statement, but does not cite Planck. This source calls the statement the principle of the increase of entropy.
↑Truesdell, C., Muncaster, R.G. (1980). Fundamentals of Maxwell's Kinetic Theory of a Simple Monatomic Gas, Treated as a Branch of Rational Mechanics, Academic Press, New York,
↑van Gool, W.; Bruggink, J.J.C. (Eds) (1985). Energy and time in the economic and physical sciences. North-Holland. pp. 41–56. ISBN978-0-444-87748-2.
↑Grubbström, Robert W. (2007). "An Attempt to Introduce Dynamics Into Generalised Exergy Considerations". Applied Energy. 84 (7–8): 701–718. doi:10.1016/j.apenergy.2007.01.003.
2010年3月15日 "Untersuchungen über die Grundlagen der Thermodynamik"]. Mathematische Annalen. 67 (3): 355–386. doi:10.1007/bf01450409. Axiom II: In jeder beliebigen Umgebung eines willkürlich vorgeschriebenen Anfangszustandes gibt es Zustände, die durch adiabatische Zustandsänderungen nicht beliebig approximiert werden können. (p.363){{cite journal}}: Check |url= value (help); Text "第355-386页" ignored (help); line feed character in |url= at position 93 (help). A translation may be found here. Also a mostly reliable translation is to be found at Kestin, J. (1976). The Second Law of Thermodynamics, Dowden, Hutchinson & Ross, Stroudsburg PA.
|quote=Axiom II: In jeder beliebigen Umgebung eines willkürlich vorgeschriebenen Anfangszustandes gibt es Zustände, die durch adiabatische Zustandsänderungen nicht beliebig approximiert werden können. (p.363)|doi=10.1007/bf01450409}}. A translation may be found here. Also a mostly reliable translation is to be found at Kestin, J. (1976). The Second Law of Thermodynamics, Dowden, Hutchinson & Ross, Stroudsburg PA.
|quote=Axiom II: In jeder beliebigen Umgebung eines willkürlich vorgeschriebenen Anfangszustandes gibt es Zustände, die durch adiabatische Zustandsänderungen nicht beliebig approximiert werden können.(p. 363) | doi 10.1007 / bf01450409}.译文可以在这里找到[ http://neo-classical-physics.info/uploads/3/0/6/5/3065888/caratheodory_-_thermodynamics.pdf ]。同时,在 Kestin,j。(1976).热力学第二定律,Dowden,Hutchinson & Ross,Stroudsburg PA. 。
Chapman, S., Cowling, T.G. (1939/1970). The Mathematical Theory of Non-uniform gases. An Account of the Kinetic Theory of Viscosity, Thermal Conduction and Diffusion in Gases, third edition 1970, Cambridge University Press, London.
Denbigh, K. (1954/1981). The Principles of Chemical Equilibrium. With Applications in Chemistry and Chemical Engineering, fourth edition, Cambridge University Press, Cambridge UK,
Gibbs, J.W. (1876/1878). On the equilibrium of heterogeneous substances, Trans. Conn. Acad., 3: 108-248, 343-524, reprinted in The Collected Works of J. Willard Gibbs, Ph.D, LL. D., edited by W.R. Longley, R.G. Van Name, Longmans, Green & Co., New York, 1928, volume 1, pp. 55–353.
Griem, H.R. (2005). Principles of Plasma Spectroscopy (Cambridge Monographs on Plasma Physics), Cambridge University Press, New York
Guggenheim, E.A. (1949). 'Statistical basis of thermodynamics', Research, 2: 450–454.
Guggenheim, E.A. (1967). Thermodynamics. An Advanced Treatment for Chemists and Physicists, fifth revised edition, North Holland, Amsterdam.
Gyarmati, I. (1967/1970) Non-equilibrium Thermodynamics. Field Theory and Variational Principles, translated by E. Gyarmati and W.F. Heinz, Springer, New York.
Kittel, C., Kroemer, H. (1969/1980). Thermal Physics, second edition, Freeman, San Francisco CA,
Lieb, E.H., Yngvason, J. (2003). The Entropy of Classical Thermodynamics, pp. 147–195, Chapter 8 of Entropy, Greven, A., Keller, G., Warnecke (editors) (2003).
Pippard, A.B. (1957/1966). Elements of Classical Thermodynamics for Advanced Students of Physics, original publication 1957, reprint 1966, Cambridge University Press, Cambridge UK.
Planck, M. (1926). Über die Begründung des zweiten Hauptsatzes der Thermodynamik, Sitzungsberichte der Preussischen Akademie der Wissenschaften: Physikalisch-mathematische Klasse: 453–463.
Pokrovskii V.N. (2005) Extended thermodynamics in a discrete-system approach, Eur. J. Phys. vol. 26, 769-781.
Uffink, J. (2001). Bluff your way in the second law of thermodynamics, Stud. Hist. Phil. Mod. Phys., 32(3): 305–394.
Uffink, J. (2003). Irreversibility and the Second Law of Thermodynamics, Chapter 7 of Entropy, Greven, A., Keller, G., Warnecke (editors) (2003), Princeton University Press, Princeton NJ,
Uhlenbeck, G.E., Ford, G.W. (1963). Lectures in Statistical Mechanics, American Mathematical Society, Providence RI.
Zemansky, M.W. (1968). Heat and Thermodynamics. An Intermediate Textbook, fifth edition, McGraw-Hill Book Company, New York.
Further reading
Further reading
进一步阅读
Goldstein, Martin, and Inge F., 1993. The Refrigerator and the Universe. Harvard Univ. Press. Chpts. 4–9 contain an introduction to the Second Law, one a bit less technical than this entry.
Leff, Harvey S., and Rex, Andrew F. (eds.) 2003. Maxwell's Demon 2 : Entropy, classical and quantum information, computing. Bristol UK; Philadelphia PA: Institute of Physics.
Halliwell, J.J. (1994). Physical Origins of Time Asymmetry. Cambridge. ISBN978-0-521-56837-1.(technical).
Carnot, Sadi (1890). Thurston, Robert Henry. ed. Reflections on the Motive Power of Heat and on Machines Fitted to Develop That Power. New York: J. Wiley & Sons. (full text of 1897 ed.) (html)
Stephen Jay Kline (1999). The Low-Down on Entropy and Interpretive Thermodynamics, La Cañada, CA: DCW Industries.
Kostic, M (2011). Revisiting The Second Law of Energy Degradation and Entropy Generation: From Sadi Carnot's Ingenious Reasoning to Holistic Generalization. AIP Conference Proceedings. 1411. pp. 327–350. Bibcode2011AIPC.1411..327K. doi:10.1063/1.3665247. ISBN978-0-7354-0985-9. also at [1].