[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
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![## Thermodynamics and Solubility Problems
**Gibbs Free Energy and Reaction Equilibrium**
\[
\Delta G^\circ = -RT \ln K_{\text{eq}} \quad \text{and} \quad \ln K_{\text{eq}} = -\frac{\Delta G^\circ}{RT} \quad \text{or} \quad K_{\text{eq}} = e^{-\Delta G^\circ/RT}
\]
1. **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 \(+206.1\, \text{kJ/mol}\), while \( \Delta S^\circ \) is \(+215\, \text{J/K}\cdot\text{mol}\).\
Calculate \( \Delta G^\circ \) for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
2. **Reversible Reaction Analysis**
a. 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?\
\(\Delta G =\) _______\
c. Under what conditions of enthalpy and entropy change is a reaction always spontaneous?\
\(\Delta H =\) ______, \(\Delta S =\) ______\
d. Under what conditions of enthalpy and entropy change is a reaction never spontaneous?\
\(\Delta H =\) ______, \(\Delta S =\) ______\
e. If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low temperature be more likely to lead to a spontaneous reaction?
3. **Equilibrium Constant Calculation**
For the reaction \( \text{C}_2\text{H}_4(g) + 2\text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g) \), \(\Delta G^\circ(\text{C}_2\text{H}_2) = +209.2\, \text{kJ/mol}\) and \(](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F60cf892a-bc21-4928-b8d7-b5b696620db4%2F19c3c09d-e0ec-4a51-8156-6246296b0e9c%2F3zcy2fj_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Thermodynamics and Solubility Problems
**Gibbs Free Energy and Reaction Equilibrium**
\[
\Delta G^\circ = -RT \ln K_{\text{eq}} \quad \text{and} \quad \ln K_{\text{eq}} = -\frac{\Delta G^\circ}{RT} \quad \text{or} \quad K_{\text{eq}} = e^{-\Delta G^\circ/RT}
\]
1. **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 \(+206.1\, \text{kJ/mol}\), while \( \Delta S^\circ \) is \(+215\, \text{J/K}\cdot\text{mol}\).\
Calculate \( \Delta G^\circ \) for this reaction at 25.0°C and determine whether it is spontaneous at that temperature.
2. **Reversible Reaction Analysis**
a. 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?\
\(\Delta G =\) _______\
c. Under what conditions of enthalpy and entropy change is a reaction always spontaneous?\
\(\Delta H =\) ______, \(\Delta S =\) ______\
d. Under what conditions of enthalpy and entropy change is a reaction never spontaneous?\
\(\Delta H =\) ______, \(\Delta S =\) ______\
e. If the enthalpy change is unfavorable, but the entropy change is favorable, would a high temperature or a low temperature be more likely to lead to a spontaneous reaction?
3. **Equilibrium Constant Calculation**
For the reaction \( \text{C}_2\text{H}_4(g) + 2\text{H}_2(g) \rightarrow \text{C}_2\text{H}_6(g) \), \(\Delta G^\circ(\text{C}_2\text{H}_2) = +209.2\, \text{kJ/mol}\) and \(
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