📚 Gibbs Free Energy | 吉布斯自由能考点精讲
Gibbs free energy is a central concept in chemical thermodynamics that combines enthalpy and entropy to predict the feasibility of a reaction at constant temperature and pressure. It answers one of the most fundamental questions in chemistry: will a reaction happen on its own? At A‑Level, a clear grasp of ΔG, its link to entropy change in the universe, and its quantitative relationship with the equilibrium constant is essential for tackling exam questions with confidence.
吉布斯自由能是化学热力学的核心概念，它结合了焓与熵，用于判断在恒温恒压下反应的自发性。它回答了一个化学中最基本的问题：一个反应能自发进行吗？在A‑Level阶段，清晰理解ΔG、它与宇宙熵变的关系，以及与平衡常数的定量联系，是自信应对考试的关键。
1. The Definition of Gibbs Free Energy | 吉布斯自由能的定义
Gibbs free energy, G, is defined as G = H – opy. Because absolute values of G cannot be measured, we always work with changes: ΔG = ΔH – t temperature and pressure, which are the standard conditions for most chemical reactions.
吉布斯自由能G定义为 G = H – TS，其中H是焓，T是热力学温度（开尔文），S是熵。由于无法测定G的绝对值，我们总是使用其变化量：ΔG = ΔH – TΔS。该方程适用于恒温恒压条件，这也是大多数化学反应的标准条件。
2. Spontaneity and the Sign of ΔG | 自发性与ΔG的符号
hough the reverse reaction would be spontaneous. When ΔG = 0, the system is at equilibrium — there is no net tendency to change in either direction.
当ΔG < 0时，反应在热力学上是自发的（可行的）。如果ΔG > 0，反应在给定条件下不自发，但其逆反应是自发的。当ΔG = 0时，系统处于平衡状态——没有向任一方向发生净变化的趋势。
3. The Link to Total Entropy Change | 与总熵变的关系
ous process. ΔG is directly proportional to the negative of the total entropy change: ΔG = –TΔStotal. Thus a negative ΔG corresponds to a positive ΔStotal, which aligns with the second law of thermodynamics. This connection helps explain why exothermic reactions with a decrease in entropy can still be spontaneous if the temperature is low enough.
吉布斯从自发过程必须使宇宙总熵增加这一要求出发，推导出他的方程。ΔG与总熵变的负值成正比：ΔG = –TΔStotal。因此，ΔG为负对应ΔStotal为正，这符合热力学第二定律。这一联系有助于解释为何熵减小的放热反应在足够低的温度下仍可自发进行。
4. Standard Gibbs Free Energy Change, ΔG° | 标准吉布斯自由能变 ΔG°
ids or liquids). ΔG° can be calculated from standard free energies of formation: ΔG° = ΣΔGf°(products) – ΣΔGf°(reactants). It can also be determined from ΔH° and ΔS° using ΔG° = ΔH° – TΔS°.
标准吉布斯自由能变ΔG°是指所有反应物和产物都处于标准状态（气体分压1 bar，溶液浓度1 mol dm⁻³，纯固体或液体）时的变化量。ΔG°可由标准生成自由能计算：ΔG° = ΣΔGf°(产物) – ΣΔGf°(反应物)。也可由ΔH°和ΔS°通过ΔG° = ΔH° – TΔS°求得。
5. Temperature Dependence and the Enthalpy–Entropy Interplay | 温度依赖性与焓-熵权衡
The term –TΔS makes ΔG temperature‑dependent. This means a reaction can be made spontaneous or non‑spontaneous by changing T. Four combinations are possible: (i) ΔH < 0, ΔS > 0 ⇒ ΔG always < 0; (ii) ΔH > 0, ΔS < 0 ⇒ ΔG always > 0; (iii) ΔH < 0, ΔS < 0 ⇒ spontaneous only below a certain temperature; (iv) ΔH > 0, ΔS > 0 ⇒ ove a certain temperature. The transition temperature is given by T = ΔH/ΔS (when ΔG = 0).
–TΔS这一项使ΔG依赖于温度。这意味着可以通过改变温度使反应变为自发或非自发。共有四种可能组合：(i) ΔH < 0，ΔS > 0 ⇒ ΔG始终为负；(ii) ΔH > 0，ΔS < 0 ⇒ ΔG始终为正；(iii) ΔH < 0，ΔS < 0 ⇒ 仅在低于某一温度时自发；(iv) ΔH > 0，ΔS > 0 ⇒ 仅在高于某一温度时自发。转变温度可由T = ΔH/ΔS（当ΔG = 0时）求得。
6. Calculation of Transition Temperature | 转变温度的计算
. It is crucial to use consistent units: ΔH in J mol⁻¹ and ΔS in J K⁻¹ mol⁻¹, or ΔH in kJ mol⁻¹ and convert accordingly. Examiners expect careful attention to unit conversion.
当反应的ΔH和ΔS同号时，反应刚好变为自发（ΔG = 0）的温度用 T = ΔH / ΔS 计算。关键是要使用一致的单位：ΔH的单位为J mol⁻¹，ΔS的单位为J K⁻¹ mol⁻¹；或者ΔH用kJ mol⁻¹并进行相应换算。阅卷人期望考生仔细进行单位换算。
7. ΔG and the Equilibrium Constant, K | ΔG与平衡常数K
librium, ΔG = 0. However, ΔG° is related to the equilibrium constant by the equation ΔG° = – m favours products. Conversely, ΔG° > 0 gives K < 1. It allows the calculation of K from thermodynamic data, and vice versa.
对于处于平衡的反应，ΔG = 0。然而，ΔG°与平衡常数K之间通过方程 ΔG° = –RT ln K 相关联，其中R = 8.314 J K⁻¹ mol⁻¹，T为热力学温度。这一关系非常强大：若ΔG° < 0，则ln K > 0且K > 1，意味着平衡有利于产物。反之，ΔG° > 0时K < 1。它使得我们可以从热力学数据计算K，反之亦然。
8. Using ΔG° to Predict Reaction Direction | 利用ΔG°预测反应方向
While ΔG° gives the position of equilibrium, ΔG under non‑ ion quotient. If ΔG < 0 the forward reaction is spontaneous; if ΔG > 0 the reverse reaction is spontaneous. This distinction is a favourite in exam questions testing deeper understanding.
虽然ΔG°给出平衡的位置，但非标准条件下的ΔG决定了实际方向。其关系式为 ΔG = ΔG° + RT ln Q，其中Q是反应商。如果ΔG < 0，正向反应自发；如果ΔG > 0，逆向反应自发。这一区分常常出现在考试中，考查更深层次的理解。
9. Coupled Reactions: Making the Impossible Possible | 耦合反应：变不可能为可能
sum of the individual ΔG values. Biological systems frequently use ATP hydrolysis (ΔG°′ ≈ –30.5 kJ mol⁻¹) to drive otherwise non‑spontaneous processes such as protein synthesis or active transport.
热力学不利的反应（ΔG > 0）可以通过与一个高度自发的反应（ΔG << 0）相耦合而被驱动，前提是二者共享一个共同的中间体。总ΔG为各步ΔG的代数和。生物系统中常利用ATP水解（ΔG°′ ≈ –30.5 kJ mol⁻¹）来驱动原本不能自发的过程，如蛋白质合成或主动运输。
10. Common Pitfalls and Key Takeaways | 常见误区与关键总结
equilibrium; ΔG° is a constant at a given temperature. Also, spontaneity does not mean the reaction will occur quickly — ation energy, making it imperceptibly slow like the conversion of diamond to graphite at room temperature.
混淆ΔG和ΔG°可能是最常见的错误。请记住：平衡时ΔG = 0；ΔG°在给定温度下是常数。同时，自发性并不意味着反应会快速进行——动力学是另一个问题。一个反应可能ΔG < 0，但活化能很高，因此在室温下几乎察觉不到，比如金刚石转变为石墨。
11. Worked Example: Calculating ΔG and K | 示例：计算ΔG与K
Consider the reaction N₂(g) + 3H₂(g) ⇌ 2NH₃(g) at 298 K, with ΔH° = –92.4 kJ mol⁻¹ and ΔS° = –3 J K⁻¹ mol⁻¹. Calculate ΔG° and the equilibrium constant K. First, convert kJ to J: ΔH° = –92400 J mol⁻¹. Then ΔG° = ΔH° – TΔS° = –92400 – 298×(–198.3) = –92400 + 59093.4 = –33306.6 J mol⁻¹ ≈ –33.3 kJ mol⁻¹. Then use ΔG° = –RT ln K: ln K = –ΔG° / (RT) = 33306.6 / (8.314 × 298) ≈ 13.44. Therefore K = e¹³·⁴⁴ ≈ 6.8×10⁵.
考虑反应 N₂(g) + 3H₂(g) ⇌ 2NH₃(g) 在298 K下，ΔH° = –92.4 kJ mol⁻¹，ΔS° = –198.3 J K⁻¹ mol⁻¹。计算ΔG°和平衡常数K。首先将kJ转换为J：ΔH° = –92400 J mol⁻¹。则ΔG° = ΔH° – TΔS° = –92400 – 298×(–198.3) = –92400 + 59093.4 = –33306.6 J mol⁻¹ ≈ –33.3 kJ mol⁻¹。然后利用ΔG° = –RT ln K：ln K = –ΔG° / (RT) = 33306.6 / (8.314 × 298) ≈ 13.44。因此K = e¹³·⁴⁴ ≈ 6.8×10⁵。
12. Exam Tips for Gibbs Free Energy Questions | 吉布斯自由能应考技巧
ergy dimension, usually joules. Know how to interpret a graph of ΔG versus T; the slope is –ΔS. Be prepared to rearrange ΔG° = – ation. Practice linking thermodynamic feasibility with the kinetic stability of compounds.
始终检查单位。ΔH和ΔS必须使用相同的能量量纲，通常为焦耳。学会解读ΔG对T的图；斜率为–ΔS。要能灵活变形ΔG° = –RT ln K。如果题目给出K和T，可求出ΔG°，再结合ΔH°或ΔS°运用吉布斯方程。多练习将热力学可行性与化合物的动力学稳定性联系起来。
Published by TutorHao | Chemistry Revision Series | aleveler.com
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