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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.<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

: <math>\mathrm dS = \frac{\delta Q}{T} - \frac{1}{T} \sum_{j} \, \Xi_{j} \,\delta \xi_j \,\, \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, \text {(closed system, actually possible quasistatic irreversible process).}</math>

: <math>\mathrm dS = \frac{\delta Q}{T} - \frac{1}{T} \sum_{j} \, \Xi_{j} \,\delta \xi_j \,\, \,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\,\, \text {(closed system, actually possible quasistatic irreversible process 封闭系统，实际可能的准静态不可逆过程).}</math>

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.

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.

 

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.

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——如果两个热力学系统中的每一个都与第三个热力学系统处于热平衡(温度相同)，则它们彼此也必定处于热平衡。热力学第零定律在它通常的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，对于一个与另一个处于热平衡的物体，有无限多的经验温标，这通常取决于特定参考温度标度的性质。热力学第二定律允许区分温度标度，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。

热力学第零定律是指如果两个热力学系统<font color='red'><s>中的每一个</s></font>都与第三个热力学系统处于热平衡(温度相同)<font color= 'blue'>状态</font>，则它们彼此也必定处于热平衡<font color= 'blue'>状态</font>。热力学第零定律在<font color='red'><s>它</s></font>这个<font color= 'blue'></font><font color='red'><s>通常的</s></font>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<font color='red'><s>一个与另一个</s></font>两个<font color= 'blue'></font>处于热平衡<font color= 'blue'>状态</font>的物体，有无限多的'''经验温标empirical temperature scales'''，这通常<font color= 'blue'>分别</font>取决于特定参考温度<font color='red'><s>标度</s></font><font color= 'blue'>体</font>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。

   --[[用户:趣木木|趣木木]]（[[用户讨论:趣木木|讨论]]）补充热力学第零定律

   --[[用户:趣木木|趣木木]]（[[用户讨论:趣木木|讨论]]）补充热力学第零定律