8 Show why reaction is spontaneous only hure, while reaction (a) is always at low tempre non spontaneous a) CH4 (g) + 20₂(g) → 2 H₂O (l) + CO₂ (g) (endothermic) b) 2C₂H6 (g) +702(g) → 6 H₂0 (e) + 4 (0₂ (g) (@xothermic)
8 Show why reaction is spontaneous only hure, while reaction (a) is always at low tempre non spontaneous a) CH4 (g) + 20₂(g) → 2 H₂O (l) + CO₂ (g) (endothermic) b) 2C₂H6 (g) +702(g) → 6 H₂0 (e) + 4 (0₂ (g) (@xothermic)
Principles of Modern Chemistry
8th Edition
ISBN:9781305079113
Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler
Chapter13: Spontaneous Processes And Thermodynamic Equilibrium
Section: Chapter Questions
Problem 34P
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![**Understanding Reaction Spontaneity Based on Temperature: An Explanation with Examples**
**Objective:**
To demonstrate why certain chemical reactions are spontaneous at low temperatures while others are non-spontaneous regardless of temperature.
**Reactions:**
(a) \( \text{CH}_4 (\text{g}) + 2\text{O}_2 (\text{g}) \rightarrow 2\text{H}_2\text{O} (\text{l}) + \text{CO}_2 (\text{g}) \)
(b) \( 2\text{C}_2\text{H}_6 (\text{g}) + 7\text{O}_2 (\text{g}) \rightarrow 6\text{H}_2\text{O} (\text{l}) + 4\text{CO}_2 (\text{g}) \) (exothermic)
**Problem:**
Show why reaction (b) is spontaneous only at low temperatures, while reaction (a) is always non-spontaneous.
### Explanation:
**1. Reaction Equations:**
- **Reaction (a):**
\[
\text{CH}_4 (\text{g}) + 2\text{O}_2 (\text{g}) \rightarrow 2\text{H}_2\text{O} (\text{l}) + \text{CO}_2 (\text{g})
\]
- **Reaction (b):**
\[
2\text{C}_2\text{H}_6 (\text{g}) + 7\text{O}_2 (\text{g}) \rightarrow 6\text{H}_2\text{O} (\text{l}) + 4\text{CO}_2 (\text{g}) \, (\text{{exothermic}})
\]
**2. Enthalpy (ΔH) and Entropy (ΔS) considerations:**
- **Exothermic Reactions:** These reactions release heat, denoted by a negative ΔH.
- **Endothermic Reactions:** These reactions absorb heat, denoted by a positive ΔH.
For spontaneity:
- Spontaneous at all temperatures: ΔG = ΔH - TΔS < 0 when ΔH is negative and ΔS positive.
- Spontaneous at low temperatures: When](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2704aedc-cd59-4651-b157-0d8c71ae74f0%2F3d3edc44-f509-49bb-85cc-d36ac81f6b8d%2Fq6nw29n_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Understanding Reaction Spontaneity Based on Temperature: An Explanation with Examples**
**Objective:**
To demonstrate why certain chemical reactions are spontaneous at low temperatures while others are non-spontaneous regardless of temperature.
**Reactions:**
(a) \( \text{CH}_4 (\text{g}) + 2\text{O}_2 (\text{g}) \rightarrow 2\text{H}_2\text{O} (\text{l}) + \text{CO}_2 (\text{g}) \)
(b) \( 2\text{C}_2\text{H}_6 (\text{g}) + 7\text{O}_2 (\text{g}) \rightarrow 6\text{H}_2\text{O} (\text{l}) + 4\text{CO}_2 (\text{g}) \) (exothermic)
**Problem:**
Show why reaction (b) is spontaneous only at low temperatures, while reaction (a) is always non-spontaneous.
### Explanation:
**1. Reaction Equations:**
- **Reaction (a):**
\[
\text{CH}_4 (\text{g}) + 2\text{O}_2 (\text{g}) \rightarrow 2\text{H}_2\text{O} (\text{l}) + \text{CO}_2 (\text{g})
\]
- **Reaction (b):**
\[
2\text{C}_2\text{H}_6 (\text{g}) + 7\text{O}_2 (\text{g}) \rightarrow 6\text{H}_2\text{O} (\text{l}) + 4\text{CO}_2 (\text{g}) \, (\text{{exothermic}})
\]
**2. Enthalpy (ΔH) and Entropy (ΔS) considerations:**
- **Exothermic Reactions:** These reactions release heat, denoted by a negative ΔH.
- **Endothermic Reactions:** These reactions absorb heat, denoted by a positive ΔH.
For spontaneity:
- Spontaneous at all temperatures: ΔG = ΔH - TΔS < 0 when ΔH is negative and ΔS positive.
- Spontaneous at low temperatures: When
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