ons for the following Part A S₂(g) + 2H₂(g) → 2H₂S(g) = Okeele = Ok=ame Ok= Ok= Submit ▾ Part B P K= Okle= H₂S(aq) + Cl₂(aq) = S(s) + 2HCl(aq) OK= Submit = Part C OK SH₂S2 [HC1² OK= Oke= [H₂S² [S₂][H₂)² OK= [H₂S] [S₂][H₂] OK= Submit [H₂S² [S₂] H₂] [H₂S] [S₂][H₂2 Request Answer [HCT2 C1₂H₂S Br₂(g) + Cl₂(g) = 2BrCl(g) [C1₂]²[H₂S] HC1 [HC] [C1₂]²[H₂S] Request Answer [BrC1]² [Br₂]²[C1₂]² [BrC1] [Br₂][C1₂] [BrCl] [Br₂]²[C1₂² Review | Constants | Periodic Table [BrC1² [Br₂][Cl₂] Request Answer
ons for the following Part A S₂(g) + 2H₂(g) → 2H₂S(g) = Okeele = Ok=ame Ok= Ok= Submit ▾ Part B P K= Okle= H₂S(aq) + Cl₂(aq) = S(s) + 2HCl(aq) OK= Submit = Part C OK SH₂S2 [HC1² OK= Oke= [H₂S² [S₂][H₂)² OK= [H₂S] [S₂][H₂] OK= Submit [H₂S² [S₂] H₂] [H₂S] [S₂][H₂2 Request Answer [HCT2 C1₂H₂S Br₂(g) + Cl₂(g) = 2BrCl(g) [C1₂]²[H₂S] HC1 [HC] [C1₂]²[H₂S] Request Answer [BrC1]² [Br₂]²[C1₂]² [BrC1] [Br₂][C1₂] [BrCl] [Br₂]²[C1₂² Review | Constants | Periodic Table [BrC1² [Br₂][Cl₂] Request 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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![### 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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f185ec2-8c2e-4aee-a8f1-0a1f41f71cb3%2F38b72ee9-6ec5-412b-87dd-ae94add7754e%2Fviw7au_processed.jpeg&w=3840&q=75)
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](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F7f185ec2-8c2e-4aee-a8f1-0a1f41f71cb3%2F38b72ee9-6ec5-412b-87dd-ae94add7754e%2Fevhlvs_processed.jpeg&w=3840&q=75)
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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