A mixture of isobutylene ((CH:)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH:):CCI) is 3.45 at 500.0 K. (CH:).CCI(g) = (CH:).CCH:(g) + HCl(g) %3D Based on your ICE table, set up the expression for K for the decomposition of (CH:):CCI. (CH:).CCI(g) = (CH:).CCH:(g) + HCl(g) 1 Do not combine or simplify terms. K = 3.45 %3D
A mixture of isobutylene ((CH:)2CCH2, 0.400 bar partial pressure) and HCI (0.600 bar partial pressure) is heated at 500.0 K. The equilibrium constant K for the gas-phase thermal decomposition of tert-butyl chloride ((CH:):CCI) is 3.45 at 500.0 K. (CH:).CCI(g) = (CH:).CCH:(g) + HCl(g) %3D Based on your ICE table, set up the expression for K for the decomposition of (CH:):CCI. (CH:).CCI(g) = (CH:).CCH:(g) + HCl(g) 1 Do not combine or simplify terms. K = 3.45 %3D
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
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![### Equilibrium Constant for Gas-Phase Thermal Decomposition
A mixture of isobutylene \((\text{(CH}_3)_2\text{CCH}_2, 0.400 \,\text{bar partial pressure})\) and HCl \((0.600 \,\text{bar partial pressure})\) is heated to \(500.0 \,\text{K}\). The equilibrium constant \(K\) for the gas-phase thermal decomposition of tert-butyl chloride \((\text{(CH}_3)_3\text{CCl})\) is \(3.45\) at \(500.0 \,\text{K}\).
\[
(\text{CH}_3)_3\text{CCl(g)} \rightleftharpoons (\text{CH}_3)_2\text{CCH}_2\text{(g)} + \text{HCl(g)}
\]
Based on your ICE table, set up the expression for \(K\) for the decomposition of \((\text{CH}_3)_3\text{CCl}\).
\[
(\text{CH}_3)_3\text{CCl(g)} \rightleftharpoons (\text{CH}_3)_2\text{CCH}_2\text{(g)} + \text{HCl(g)}
\]
**Graphical Representation:**
The image contains a horizontal equilibrium bar showing the balance between the reactants and products. The bar is divided into a dark segment and a light segment, each representing different parts of the equilibrium reaction.
**Expression for the Equilibrium Constant \(K\):**
\[
K = \frac{\text{[Products]}}{\text{[Reactants]}} = 3.45
\]
*Note: Do not combine or simplify terms.*
### Key Facts:
- **Initial Conditions:**
- Isobutylene: 0.400 bar
- HCl: 0.600 bar
- **Temperature:**
- Heated at 500.0 K
- **Equilibrium Reaction:**
\[
(\text{CH}_3)_3\text{CCl(g)} \rightleftharpoons (\text{CH}_3)_2\text{CCH}_2\text{(g)} + \text{HCl(g)}
\]
Ensure that the expression derived from your](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1243504b-5612-4510-ba6c-7b5ec7c70d6e%2F92c2c0c9-ef66-43fd-8439-bcc63a6178b5%2F8ql16ad_processed.png&w=3840&q=75)
Transcribed Image Text:### Equilibrium Constant for Gas-Phase Thermal Decomposition
A mixture of isobutylene \((\text{(CH}_3)_2\text{CCH}_2, 0.400 \,\text{bar partial pressure})\) and HCl \((0.600 \,\text{bar partial pressure})\) is heated to \(500.0 \,\text{K}\). The equilibrium constant \(K\) for the gas-phase thermal decomposition of tert-butyl chloride \((\text{(CH}_3)_3\text{CCl})\) is \(3.45\) at \(500.0 \,\text{K}\).
\[
(\text{CH}_3)_3\text{CCl(g)} \rightleftharpoons (\text{CH}_3)_2\text{CCH}_2\text{(g)} + \text{HCl(g)}
\]
Based on your ICE table, set up the expression for \(K\) for the decomposition of \((\text{CH}_3)_3\text{CCl}\).
\[
(\text{CH}_3)_3\text{CCl(g)} \rightleftharpoons (\text{CH}_3)_2\text{CCH}_2\text{(g)} + \text{HCl(g)}
\]
**Graphical Representation:**
The image contains a horizontal equilibrium bar showing the balance between the reactants and products. The bar is divided into a dark segment and a light segment, each representing different parts of the equilibrium reaction.
**Expression for the Equilibrium Constant \(K\):**
\[
K = \frac{\text{[Products]}}{\text{[Reactants]}} = 3.45
\]
*Note: Do not combine or simplify terms.*
### Key Facts:
- **Initial Conditions:**
- Isobutylene: 0.400 bar
- HCl: 0.600 bar
- **Temperature:**
- Heated at 500.0 K
- **Equilibrium Reaction:**
\[
(\text{CH}_3)_3\text{CCl(g)} \rightleftharpoons (\text{CH}_3)_2\text{CCH}_2\text{(g)} + \text{HCl(g)}
\]
Ensure that the expression derived from your
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