[1] Given: CH,(g) + H2O(g) CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol. Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
[1] Given: CH,(g) + H2O(g) CO(g) + 3H2(g). AH° for the reaction is +206.1 kJ/mol, while AS° is +215 J/K•mol. Calculate AG° for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![**Thermodynamics and Reaction Spontaneity**
### Key Equations
\[ \Delta G^\circ = -RT \ln K_{eq} \]
\[ \ln K_{eq} = \frac{-\Delta G^\circ}{RT} \]
\[ K_{eq} = e^{-\Delta G^\circ/RT} \]
---
### Problems and Questions
1. **Given Reaction:**
\[\text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + 3\text{H}_2(g)\]
- \(\Delta H^\circ\) for the reaction is \(+206.1 \text{ kJ/mol}\)
- \(\Delta S^\circ\) is \(+215 \text{ J/K·mol}\)
**Task**: Calculate \(\Delta G^\circ\) for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
2. **Concept Questions:**
- [a] If the forward reaction is spontaneous for a particular reversible reaction, what can you conclude about the reverse reaction?
- [b] What does the sign of the free energy have to be such that a reaction is spontaneous?
\[\Delta G = \underline{\hspace{1cm}}\]
- [c] Under what conditions of enthalpy and entropy change is a reaction always spontaneous?
\[
\Delta H = \underline{\hspace{2cm}} \quad \Delta S = \underline{\hspace{2cm}}
\]
- [d] If the entropy change is unfavorable for a certain reaction, is the reaction more likely to be spontaneous at a high temperature or a low temperature?
- [e] If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low temperature lead to a spontaneous reaction?
3. **Reaction and Equilibrium:**
- For the reaction:
\[\text{C}_2\text{H}_2(g) + 2\text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)\]
- \(\Delta G^\circ(\text{C}_2\text{H}_2) = +209.2 \text{ kJ](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60cf892a-bc21-4928-b8d7-b5b696620db4%2F7e342af8-1ee4-4a5e-b7f3-e2ca5887f413%2Fy9rl6pe_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Thermodynamics and Reaction Spontaneity**
### Key Equations
\[ \Delta G^\circ = -RT \ln K_{eq} \]
\[ \ln K_{eq} = \frac{-\Delta G^\circ}{RT} \]
\[ K_{eq} = e^{-\Delta G^\circ/RT} \]
---
### Problems and Questions
1. **Given Reaction:**
\[\text{CH}_4(g) + \text{H}_2\text{O}(g) \rightarrow \text{CO}(g) + 3\text{H}_2(g)\]
- \(\Delta H^\circ\) for the reaction is \(+206.1 \text{ kJ/mol}\)
- \(\Delta S^\circ\) is \(+215 \text{ J/K·mol}\)
**Task**: Calculate \(\Delta G^\circ\) for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
2. **Concept Questions:**
- [a] If the forward reaction is spontaneous for a particular reversible reaction, what can you conclude about the reverse reaction?
- [b] What does the sign of the free energy have to be such that a reaction is spontaneous?
\[\Delta G = \underline{\hspace{1cm}}\]
- [c] Under what conditions of enthalpy and entropy change is a reaction always spontaneous?
\[
\Delta H = \underline{\hspace{2cm}} \quad \Delta S = \underline{\hspace{2cm}}
\]
- [d] If the entropy change is unfavorable for a certain reaction, is the reaction more likely to be spontaneous at a high temperature or a low temperature?
- [e] If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low temperature lead to a spontaneous reaction?
3. **Reaction and Equilibrium:**
- For the reaction:
\[\text{C}_2\text{H}_2(g) + 2\text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g)\]
- \(\Delta G^\circ(\text{C}_2\text{H}_2) = +209.2 \text{ kJ
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