19) 2 H2S(g) 2 H2(g) + S2(g) with Kc = 1.00x10-6 If the initial concentrations for the above reaction are 2 mole H2S, 1mole of H2, and 1mole of Sz in a 2L container, based on the reaction quotient what direction is the reaction going? c) at equilibrium d) not enough information to determine a) Forward b) Reverse
19) 2 H2S(g) 2 H2(g) + S2(g) with Kc = 1.00x10-6 If the initial concentrations for the above reaction are 2 mole H2S, 1mole of H2, and 1mole of Sz in a 2L container, based on the reaction quotient what direction is the reaction going? c) at equilibrium d) not enough information to determine a) Forward b) Reverse
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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![**Chemical Equilibrium Problem**
*Problem Statement:*
The chemical reaction is given as:
\[ 2 \text{H}_2\text{S}(g) \leftrightarrow 2 \text{H}_2(g) + \text{S}_2(g) \]
with \( K_c = 1.00 \times 10^{-6} \).
*Question:*
If the initial concentrations for the above reaction are 2 moles of \( \text{H}_2\text{S} \), 1 mole of \( \text{H}_2 \), and 1 mole of \( \text{S}_2 \) in a 2L container, based on the reaction quotient what direction is the reaction going?
a) Forward
b) Reverse
c) At equilibrium
d) Not enough information to determine
---
**Explanation:**
To determine the direction of the reaction, we compare the reaction quotient \( Q \) to the equilibrium constant \( K_c \).
1. **Calculate Initial Concentrations:**
Given the volume of the container is 2 liters:
- Initial concentration of \( \text{H}_2\text{S} \), \([ \text{H}_2\text{S} ]_i = \frac{2 \text{ moles}}{2 \text{ L}} = 1 \text{ M} \)
- Initial concentration of \( \text{H}_2 \), \([ \text{H}_2 ]_i = \frac{1 \text{ mole}}{2 \text{ L}} = 0.5 \text{ M} \)
- Initial concentration of \( \text{S}_2 \), \([ \text{S}_2 ]_i = \frac{1 \text{ mole}}{2 \text{ L}} = 0.5 \text{ M} \)
2. **Calculate the Reaction Quotient \( Q \):**
The reaction quotient \( Q \) is calculated using the initial concentrations:
\[ Q = \frac{[ \text{H}_2 ]^2 [ \text{S}_2 ]}{[ \text{H}_2\text{S} ]^2} \]
Substitute the values:
\[ Q = \frac{(0.5)^2 (0.5)}{(1)^2} = \frac{0.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd01c40b9-8944-4a44-8966-6ca7678f1a00%2Fe04d7d04-2886-41af-9fc1-1b9e48e9f787%2Fjydzoi_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium Problem**
*Problem Statement:*
The chemical reaction is given as:
\[ 2 \text{H}_2\text{S}(g) \leftrightarrow 2 \text{H}_2(g) + \text{S}_2(g) \]
with \( K_c = 1.00 \times 10^{-6} \).
*Question:*
If the initial concentrations for the above reaction are 2 moles of \( \text{H}_2\text{S} \), 1 mole of \( \text{H}_2 \), and 1 mole of \( \text{S}_2 \) in a 2L container, based on the reaction quotient what direction is the reaction going?
a) Forward
b) Reverse
c) At equilibrium
d) Not enough information to determine
---
**Explanation:**
To determine the direction of the reaction, we compare the reaction quotient \( Q \) to the equilibrium constant \( K_c \).
1. **Calculate Initial Concentrations:**
Given the volume of the container is 2 liters:
- Initial concentration of \( \text{H}_2\text{S} \), \([ \text{H}_2\text{S} ]_i = \frac{2 \text{ moles}}{2 \text{ L}} = 1 \text{ M} \)
- Initial concentration of \( \text{H}_2 \), \([ \text{H}_2 ]_i = \frac{1 \text{ mole}}{2 \text{ L}} = 0.5 \text{ M} \)
- Initial concentration of \( \text{S}_2 \), \([ \text{S}_2 ]_i = \frac{1 \text{ mole}}{2 \text{ L}} = 0.5 \text{ M} \)
2. **Calculate the Reaction Quotient \( Q \):**
The reaction quotient \( Q \) is calculated using the initial concentrations:
\[ Q = \frac{[ \text{H}_2 ]^2 [ \text{S}_2 ]}{[ \text{H}_2\text{S} ]^2} \]
Substitute the values:
\[ Q = \frac{(0.5)^2 (0.5)}{(1)^2} = \frac{0.
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