Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![### Writing Equilibrium Equations for Reactions
This section guides you through writing the equilibrium constant expression (\( K \)) for several chemical reactions.
#### Part A
**Reaction:**
\[ \text{S}_2(g) + 2\text{H}_2(g) \rightleftharpoons 2\text{H}_2\text{S}(g) \]
**Options for Equilibrium Constant (\( K \)):**
1. \( K = \frac{[\text{H}_2\text{S}]^2}{[\text{S}_2][\text{H}_2]^2} \)
2. \( K = \frac{[\text{H}_2\text{S}]}{[\text{S}_2][\text{H}_2]} \)
3. \( K = \frac{[\text{H}_2\text{S}]^2}{[\text{S}_2]^2} \)
4. \( K = \frac{[\text{H}_2\text{S}]}{[\text{S}_2][\text{H}_2]^2} \)
#### Part B
**Reaction:**
\[ \text{H}_2\text{S}(aq) + \text{Cl}_2(aq) \rightleftharpoons \text{S}(s) + 2\text{HCl}(aq) \]
**Options for Equilibrium Constant (\( K \)):**
1. \( K = \frac{[\text{HCl}]^2}{[\text{Cl}_2][\text{H}_2\text{S}]} \)
2. \( K = \frac{[\text{Cl}_2][\text{H}_2\text{S}]}{[\text{HCl}]} \)
3. \( K = \frac{[\text{HCl}]}{[\text{Cl}_2]^2[\text{H}_2\text{S}]} \)
#### Part C
**Reaction:**
\[ \text{Br}_2(g) + \text{Cl}_2(g) \rightleftharpoons 2\text{BrCl}(g) \]
**Options for Equilibrium Constant (\( K \)):**
1. \( K = \frac{[\text{BrCl}]^2}{[\text](https://content.bartleby.com/qna-images/question/7f185ec2-8c2e-4aee-a8f1-0a1f41f71cb3/38b72ee9-6ec5-412b-87dd-ae94add7754e/viw7au_processed.jpeg)
Transcribed Image Text:### Writing Equilibrium Equations for Reactions
This section guides you through writing the equilibrium constant expression (\( K \)) for several chemical reactions.
#### Part A
**Reaction:**
\[ \text{S}_2(g) + 2\text{H}_2(g) \rightleftharpoons 2\text{H}_2\text{S}(g) \]
**Options for Equilibrium Constant (\( K \)):**
1. \( K = \frac{[\text{H}_2\text{S}]^2}{[\text{S}_2][\text{H}_2]^2} \)
2. \( K = \frac{[\text{H}_2\text{S}]}{[\text{S}_2][\text{H}_2]} \)
3. \( K = \frac{[\text{H}_2\text{S}]^2}{[\text{S}_2]^2} \)
4. \( K = \frac{[\text{H}_2\text{S}]}{[\text{S}_2][\text{H}_2]^2} \)
#### Part B
**Reaction:**
\[ \text{H}_2\text{S}(aq) + \text{Cl}_2(aq) \rightleftharpoons \text{S}(s) + 2\text{HCl}(aq) \]
**Options for Equilibrium Constant (\( K \)):**
1. \( K = \frac{[\text{HCl}]^2}{[\text{Cl}_2][\text{H}_2\text{S}]} \)
2. \( K = \frac{[\text{Cl}_2][\text{H}_2\text{S}]}{[\text{HCl}]} \)
3. \( K = \frac{[\text{HCl}]}{[\text{Cl}_2]^2[\text{H}_2\text{S}]} \)
#### Part C
**Reaction:**
\[ \text{Br}_2(g) + \text{Cl}_2(g) \rightleftharpoons 2\text{BrCl}(g) \]
**Options for Equilibrium Constant (\( K \)):**
1. \( K = \frac{[\text{BrCl}]^2}{[\text
![**Write the equilibrium equations for the following reactions:**
### Part B
**Reaction:**
\[ \text{H}_2\text{S(aq)} + \text{Cl}_2\text{(aq)} \rightleftharpoons \text{S(s)} + 2\text{HCl(aq)} \]
**Equilibrium Expressions:**
- \( K = \frac{[\text{HCl}]^2}{[\text{Cl}_2][\text{H}_2\text{S}]} \)
- \( K = \frac{[\text{S}][\text{H}_2\text{S}]^2}{[\text{HCl}]^2} \)
- \( K = \frac{[\text{Cl}_2][\text{H}_2\text{S}]}{[\text{HCl}]} \)
- \( K = \frac{[\text{HCl}]}{[\text{Cl}_2][\text{H}_2\text{S}]} \)
**Options to select from are formatted as bulleted lists with different equilibrium constant (K) expressions.**
---
### Part C
**Reaction:**
\[ \text{Br}_2\text{(g)} + \text{Cl}_2\text{(g)} \rightleftharpoons 2\text{BrCl(g)} \]
**Equilibrium Expressions:**
- \( K = \frac{[\text{BrCl}]^2}{[\text{Br}_2][\text{Cl}_2]} \)
- \( K = \frac{[\text{BrCl}]}{[\text{Br}_2][\text{Cl}_2]^2} \)
- \( K = \frac{[\text{BrCl}]}{[\text{Br}_2]\left[\text{Cl}_2\right]^{2}} \)
- \( K = \frac{[\text{BrCl}]^2}{[\text{Br}_2][\text{Cl}_2]} \)
**The options are demonstrated with different ways of expressing the equilibrium constant (K) calculations.**
---
### Part D
**Reaction:**
\[ \text{C(s)} + \text{H}_2\text{O(g)} \rightleftharpoons \text{CO(g)} + \text](https://content.bartleby.com/qna-images/question/7f185ec2-8c2e-4aee-a8f1-0a1f41f71cb3/38b72ee9-6ec5-412b-87dd-ae94add7754e/evhlvs_processed.jpeg)
Transcribed Image Text:**Write the equilibrium equations for the following reactions:**
### Part B
**Reaction:**
\[ \text{H}_2\text{S(aq)} + \text{Cl}_2\text{(aq)} \rightleftharpoons \text{S(s)} + 2\text{HCl(aq)} \]
**Equilibrium Expressions:**
- \( K = \frac{[\text{HCl}]^2}{[\text{Cl}_2][\text{H}_2\text{S}]} \)
- \( K = \frac{[\text{S}][\text{H}_2\text{S}]^2}{[\text{HCl}]^2} \)
- \( K = \frac{[\text{Cl}_2][\text{H}_2\text{S}]}{[\text{HCl}]} \)
- \( K = \frac{[\text{HCl}]}{[\text{Cl}_2][\text{H}_2\text{S}]} \)
**Options to select from are formatted as bulleted lists with different equilibrium constant (K) expressions.**
---
### Part C
**Reaction:**
\[ \text{Br}_2\text{(g)} + \text{Cl}_2\text{(g)} \rightleftharpoons 2\text{BrCl(g)} \]
**Equilibrium Expressions:**
- \( K = \frac{[\text{BrCl}]^2}{[\text{Br}_2][\text{Cl}_2]} \)
- \( K = \frac{[\text{BrCl}]}{[\text{Br}_2][\text{Cl}_2]^2} \)
- \( K = \frac{[\text{BrCl}]}{[\text{Br}_2]\left[\text{Cl}_2\right]^{2}} \)
- \( K = \frac{[\text{BrCl}]^2}{[\text{Br}_2][\text{Cl}_2]} \)
**The options are demonstrated with different ways of expressing the equilibrium constant (K) calculations.**
---
### Part D
**Reaction:**
\[ \text{C(s)} + \text{H}_2\text{O(g)} \rightleftharpoons \text{CO(g)} + \text
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