A 2.50 L container with 6.0 moles each of carbon monoxide and water vapor is allowed to come to equilibrium with carbon dioxide and hydrogen. If the equilibrium constant K is 23.2 at this temperature, what are the concentrations of carbon monoxide, water, carbon dioxide and hydrogen (in that order and in molarity) at equilibrium? 2.4, 2.4, 2.0, 2.0 0.41, 0.41, 2.0, 2.0 O 0.20, 0.20, 2.4, 2.4 ○ 1.0, 1.0, 5.0, 5.0 6.0, 6.0, 5.0, 5.0
A 2.50 L container with 6.0 moles each of carbon monoxide and water vapor is allowed to come to equilibrium with carbon dioxide and hydrogen. If the equilibrium constant K is 23.2 at this temperature, what are the concentrations of carbon monoxide, water, carbon dioxide and hydrogen (in that order and in molarity) at equilibrium? 2.4, 2.4, 2.0, 2.0 0.41, 0.41, 2.0, 2.0 O 0.20, 0.20, 2.4, 2.4 ○ 1.0, 1.0, 5.0, 5.0 6.0, 6.0, 5.0, 5.0
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 Quiz**
**Problem:**
A 2.50 L container with 6.0 moles each of carbon monoxide (CO) and water vapor (H₂O) is allowed to come to equilibrium with carbon dioxide (CO₂) and hydrogen (H₂). If the equilibrium constant Kc is 23.2 at this temperature, what are the concentrations of carbon monoxide, water, carbon dioxide, and hydrogen (in that order and in molarity) at equilibrium?
**Options:**
- 2.4, 2.4, 2.0, 2.0
- 0.41, 0.41, 2.0, 2.0
- 0.20, 0.20, 2.4, 2.4
- 1.0, 1.0, 5.0, 5.0
- 6.0, 6.0, 5.0, 5.0
**Explanation:**
Given:
- Volume of container, V = 2.50 L
- Initial moles of CO = 6.0 moles
- Initial moles of H₂O = 6.0 moles
- Equilibrium constant, Kc = 23.2
We are to determine the molar concentrations (in M) of CO, H₂O, CO₂, and H₂ at equilibrium.
**Equilibrium Reaction:**
\[ \text{CO(g)} + \text{H₂O(g)} \leftrightarrow \text{CO₂(g)} + \text{H₂(g)} \]
Use the ICE (Initial, Change, Equilibrium) table to determine the equilibrium concentrations.
Calculate the initial concentrations in mol/L:
\[ [\text{CO}]_{\text{initial}} = \frac{6.0 \, \text{moles}}{2.50 \, \text{L}} = 2.4 \, \text{M} \]
\[ [\text{H₂O}]_{\text{initial}} = \frac{6.0 \, \text{moles}}{2.50 \, \text{L}} = 2.4 \, \text{M} \]
Let's denote the change in concentration by \( x \). At equilibrium:
\[ [\text{CO}] = 2.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2cfc3a1d-71f5-4849-9f61-cac9f1c46434%2Fb3330b23-86ec-41e1-a774-afa9a988d721%2Frv6jvoa_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Chemical Equilibrium Quiz**
**Problem:**
A 2.50 L container with 6.0 moles each of carbon monoxide (CO) and water vapor (H₂O) is allowed to come to equilibrium with carbon dioxide (CO₂) and hydrogen (H₂). If the equilibrium constant Kc is 23.2 at this temperature, what are the concentrations of carbon monoxide, water, carbon dioxide, and hydrogen (in that order and in molarity) at equilibrium?
**Options:**
- 2.4, 2.4, 2.0, 2.0
- 0.41, 0.41, 2.0, 2.0
- 0.20, 0.20, 2.4, 2.4
- 1.0, 1.0, 5.0, 5.0
- 6.0, 6.0, 5.0, 5.0
**Explanation:**
Given:
- Volume of container, V = 2.50 L
- Initial moles of CO = 6.0 moles
- Initial moles of H₂O = 6.0 moles
- Equilibrium constant, Kc = 23.2
We are to determine the molar concentrations (in M) of CO, H₂O, CO₂, and H₂ at equilibrium.
**Equilibrium Reaction:**
\[ \text{CO(g)} + \text{H₂O(g)} \leftrightarrow \text{CO₂(g)} + \text{H₂(g)} \]
Use the ICE (Initial, Change, Equilibrium) table to determine the equilibrium concentrations.
Calculate the initial concentrations in mol/L:
\[ [\text{CO}]_{\text{initial}} = \frac{6.0 \, \text{moles}}{2.50 \, \text{L}} = 2.4 \, \text{M} \]
\[ [\text{H₂O}]_{\text{initial}} = \frac{6.0 \, \text{moles}}{2.50 \, \text{L}} = 2.4 \, \text{M} \]
Let's denote the change in concentration by \( x \). At equilibrium:
\[ [\text{CO}] = 2.
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