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第1,093行：
第1,093行： − + + − 化学热力学的第二定律 第1,101行：
第1,101行： − 对于一个<font color = 'blue'>恒温恒压</font>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>+ 第1,120行：
第1,120行： − +
→The second law in chemical thermodynamics
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。
===The second law in chemical thermodynamics===
===The second law in chemical thermodynamics 化学热力学的第二定律===
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]]
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]]
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
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>
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.
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.
或者 dG < 0。对于一个相似的<font color = 'blue'>恒温恒压</font>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。
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。
-- [[用户:嘉树|嘉树]]（[[用户讨论:嘉树|讨论]]） tabulated enthalpies of formation 表列生成焓？？
-- [[用户:嘉树|嘉树]]（[[用户讨论:嘉树|讨论]]） tabulated enthalpies of formation 表列生成焓？？