3. Determine the reaction quotient and predict the direction that each of the following reactions will proceed to reach equilibrium: a. A 1.00 L flask containing 0.0500 mol NO (g), 0.0155 mol Cl₂ (g), and 0.500 mol NOCI(g): 2NO(g) + Cl₂(g) = 2NOCI(g) = 4.6 × 10¹ A: shift right Keq b. A 5.00 L flask containing 14 g N₂ (g), 12 g H₂ (g), and 17 g NH3(g): N₂(g) + 3H₂(g) = 2NH3(g) Keq = 0.060 (at 526 °C) c. A 2.00 L flask containing 230 g SO3 (8) 2SO3(8)2SO₂(g) + O₂(g) Keg = 0.230 A: shift left A: shift right
3. Determine the reaction quotient and predict the direction that each of the following reactions will proceed to reach equilibrium: a. A 1.00 L flask containing 0.0500 mol NO (g), 0.0155 mol Cl₂ (g), and 0.500 mol NOCI(g): 2NO(g) + Cl₂(g) = 2NOCI(g) = 4.6 × 10¹ A: shift right Keq b. A 5.00 L flask containing 14 g N₂ (g), 12 g H₂ (g), and 17 g NH3(g): N₂(g) + 3H₂(g) = 2NH3(g) Keq = 0.060 (at 526 °C) c. A 2.00 L flask containing 230 g SO3 (8) 2SO3(8)2SO₂(g) + O₂(g) Keg = 0.230 A: shift left A: shift right
Chemistry
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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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![# Reaction Equilibrium Analysis
**Objective:** Determine the reaction quotient and predict the direction that each of the following reactions will proceed to reach equilibrium.
### Reactions and Conditions:
**1. Reaction 1:**
- **Equation:** \( 2 \text{NO}(g) + \text{Cl}_2(g) \rightleftharpoons 2 \text{NOCl}(g) \)
- **Conditions:** A 1.00 L flask containing 0.1500 mol NO, 0.0155 mol Cl\(_2\), and 0.500 mol NOCl.
- **Equilibrium Constant (K\(_{\text{eq}}\)):** \( 4.16 \times 10^{-5} \)
- **Prediction:** Shift right.
**2. Reaction 2:**
- **Equation:** \( \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \)
- **Conditions:** A 500 L flask containing 14 g N\(_2\), 12 g H\(_2\), and 17 g NH\(_3\).
- **Equilibrium Constant (K\(_{\text{eq}}\)):** 0.060 (at 526°C)
- **Prediction:** Shift left.
**3. Reaction 3:**
- **Equation:** \( 2\text{SO}_2(g) \rightleftharpoons 2\text{SO}_3(g) + \text{O}_2(g) \)
- **Conditions:** A 200 L flask containing 230 g SO\(_3\).
- **Equilibrium Constant (K\(_{\text{eq}}\)):** 0.230
### Prediction:
**General Approach:**
1. **Calculate the Reaction Quotient (Q):** Compare Q to K\(_{\text{eq}}\) to predict the direction of the shift.
2. **Interpret the Shift:**
- If \( Q < K\), the reaction will shift right (toward products).
- If \( Q > K\), the reaction will shift left (toward reactants).
### Conclusion for Reaction 3:
- **Prediction:** The specific shift is not provided; calculate Q and compare with K\(_{\text{eq}}\) to predict the direction.
Use this analysis](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8e77b376-6a5c-4963-870c-f49a6e984799%2Fe2af2bf7-ea22-432e-9e31-0034b1675049%2Fgzkkvh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:# Reaction Equilibrium Analysis
**Objective:** Determine the reaction quotient and predict the direction that each of the following reactions will proceed to reach equilibrium.
### Reactions and Conditions:
**1. Reaction 1:**
- **Equation:** \( 2 \text{NO}(g) + \text{Cl}_2(g) \rightleftharpoons 2 \text{NOCl}(g) \)
- **Conditions:** A 1.00 L flask containing 0.1500 mol NO, 0.0155 mol Cl\(_2\), and 0.500 mol NOCl.
- **Equilibrium Constant (K\(_{\text{eq}}\)):** \( 4.16 \times 10^{-5} \)
- **Prediction:** Shift right.
**2. Reaction 2:**
- **Equation:** \( \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) \)
- **Conditions:** A 500 L flask containing 14 g N\(_2\), 12 g H\(_2\), and 17 g NH\(_3\).
- **Equilibrium Constant (K\(_{\text{eq}}\)):** 0.060 (at 526°C)
- **Prediction:** Shift left.
**3. Reaction 3:**
- **Equation:** \( 2\text{SO}_2(g) \rightleftharpoons 2\text{SO}_3(g) + \text{O}_2(g) \)
- **Conditions:** A 200 L flask containing 230 g SO\(_3\).
- **Equilibrium Constant (K\(_{\text{eq}}\)):** 0.230
### Prediction:
**General Approach:**
1. **Calculate the Reaction Quotient (Q):** Compare Q to K\(_{\text{eq}}\) to predict the direction of the shift.
2. **Interpret the Shift:**
- If \( Q < K\), the reaction will shift right (toward products).
- If \( Q > K\), the reaction will shift left (toward reactants).
### Conclusion for Reaction 3:
- **Prediction:** The specific shift is not provided; calculate Q and compare with K\(_{\text{eq}}\) to predict the direction.
Use this analysis
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