AH KJ/mol S°, J/mol AG, KJ/mol CH3OH -201.2 237.6 -161.9 H2 130.58 -32.89 C2H6 H20 -84.68 229.5 -241.82 188.83 -228.57 2CH;OH(g) + H2(g) C,H5(g) + 2H,0(g) AH° = -165.92 kJ/mol AS° = 1.18 J/mol AG° = -166.23 kJ/mol Is the reaction exothermic or endothermic? Explain your answer. Is the reaction endergonic or exergonic? Explain your answer.
AH KJ/mol S°, J/mol AG, KJ/mol CH3OH -201.2 237.6 -161.9 H2 130.58 -32.89 C2H6 H20 -84.68 229.5 -241.82 188.83 -228.57 2CH;OH(g) + H2(g) C,H5(g) + 2H,0(g) AH° = -165.92 kJ/mol AS° = 1.18 J/mol AG° = -166.23 kJ/mol Is the reaction exothermic or endothermic? Explain your answer. Is the reaction endergonic or exergonic? Explain your answer.
Chemistry
10th Edition
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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![**Transcription and Explanation for an Educational Website**
**Thermochemical Data Table:**
- **Standard Enthalpy Change (\(ΔH^\circ\) KJ/mol):**
- CH\(_3\)OH: -201.2
- H\(_2\): 0
- C\(_2\)H\(_6\): -84.68
- H\(_2\)O: -241.82
- **Standard Entropy (\(S^\circ\) J/mol):**
- CH\(_3\)OH: 237.6
- H\(_2\): 130.58
- C\(_2\)H\(_6\): 229.5
- H\(_2\)O: 188.83
- **Standard Gibbs Free Energy Change (\(ΔG^\circ\) KJ/mol):**
- CH\(_3\)OH: -161.9
- H\(_2\): 0
- C\(_2\)H\(_6\): -32.89
- H\(_2\)O: -228.57
**Chemical Reaction:**
\[ 2\text{CH}_3\text{OH(g)} + \text{H}_2\text{(g)} \rightleftharpoons \text{C}_2\text{H}_6\text{(g)} + 2\text{H}_2\text{O(g)} \]
**Calculated Thermochemical Values for the Reaction:**
- \(ΔH^\circ = -165.92 \text{ kJ/mol}\)
- \(ΔS^\circ = 1.18 \text{ J/mol}\)
- \(ΔG^\circ = -166.23 \text{ kJ/mol}\)
**Discussion Questions:**
1. **Is the reaction exothermic or endothermic? Explain your answer.**
2. **Is the reaction endergonic or exergonic? Explain your answer.**
3. **Is the reaction spontaneous in the forward direction? Explain your answer.**
4. **Draw Lewis structures for the system under study in this experiment.**
5. **Is the reaction in question 8 isodesmic? Explain how you know.**
**Graphical Explanation:**
No graphs](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc6455b61-2b88-4fed-b7af-14c7804cb924%2F846a1bbf-2cdf-48d5-8ecd-1bb24a70df0b%2Fukqnb49_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Transcription and Explanation for an Educational Website**
**Thermochemical Data Table:**
- **Standard Enthalpy Change (\(ΔH^\circ\) KJ/mol):**
- CH\(_3\)OH: -201.2
- H\(_2\): 0
- C\(_2\)H\(_6\): -84.68
- H\(_2\)O: -241.82
- **Standard Entropy (\(S^\circ\) J/mol):**
- CH\(_3\)OH: 237.6
- H\(_2\): 130.58
- C\(_2\)H\(_6\): 229.5
- H\(_2\)O: 188.83
- **Standard Gibbs Free Energy Change (\(ΔG^\circ\) KJ/mol):**
- CH\(_3\)OH: -161.9
- H\(_2\): 0
- C\(_2\)H\(_6\): -32.89
- H\(_2\)O: -228.57
**Chemical Reaction:**
\[ 2\text{CH}_3\text{OH(g)} + \text{H}_2\text{(g)} \rightleftharpoons \text{C}_2\text{H}_6\text{(g)} + 2\text{H}_2\text{O(g)} \]
**Calculated Thermochemical Values for the Reaction:**
- \(ΔH^\circ = -165.92 \text{ kJ/mol}\)
- \(ΔS^\circ = 1.18 \text{ J/mol}\)
- \(ΔG^\circ = -166.23 \text{ kJ/mol}\)
**Discussion Questions:**
1. **Is the reaction exothermic or endothermic? Explain your answer.**
2. **Is the reaction endergonic or exergonic? Explain your answer.**
3. **Is the reaction spontaneous in the forward direction? Explain your answer.**
4. **Draw Lewis structures for the system under study in this experiment.**
5. **Is the reaction in question 8 isodesmic? Explain how you know.**
**Graphical Explanation:**
No graphs
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