Consider the following reaction: CO2 (g) + C(s) = 2 CO(g) AH = -588 kJ A 1.0-L container at 1200 K contains CO2 and CO at equilibrium pressures of 2.00 atm and 3.40 atm, respectively. What will happen to the value of equilibrium constant if the temperature is increased? What will happen to the value of equilibrium constant if the volume of the container is reduced to 0.5 L ? increases b) no change a) increases b) increases a) decreases b) no change
Consider the following reaction: CO2 (g) + C(s) = 2 CO(g) AH = -588 kJ A 1.0-L container at 1200 K contains CO2 and CO at equilibrium pressures of 2.00 atm and 3.40 atm, respectively. What will happen to the value of equilibrium constant if the temperature is increased? What will happen to the value of equilibrium constant if the volume of the container is reduced to 0.5 L ? increases b) no change a) increases b) increases a) decreases b) no change
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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![**Equilibrium Constant and Reaction Conditions**
Consider the following reaction:
\[ \text{CO}_2 (g) + \text{C}(s) \rightleftharpoons 2 \text{CO}(g) \quad \Delta H = -588 \, \text{kJ} \]
A 1.0-L container at 1200 K contains \( \text{CO}_2 \) and \( \text{CO} \) at equilibrium pressures of 2.00 atm and 3.40 atm, respectively.
**Questions:**
1. What will happen to the value of the equilibrium constant if the temperature is increased?
2. What will happen to the value of the equilibrium constant if the volume of the container is reduced to 0.5 L?
**Options:**
- a) increases
- b) no change
1.
- a) increases
- b) increases
2.
- a) decreases
- b) no change
3.
- a) no change
- b) no change](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F52e1156a-f288-4965-9230-d44d38f3b407%2F275a3565-d24a-45e4-ae27-62ef43a6b8f7%2Fgvel01l_processed.jpeg&w=3840&q=75)
Transcribed Image Text:**Equilibrium Constant and Reaction Conditions**
Consider the following reaction:
\[ \text{CO}_2 (g) + \text{C}(s) \rightleftharpoons 2 \text{CO}(g) \quad \Delta H = -588 \, \text{kJ} \]
A 1.0-L container at 1200 K contains \( \text{CO}_2 \) and \( \text{CO} \) at equilibrium pressures of 2.00 atm and 3.40 atm, respectively.
**Questions:**
1. What will happen to the value of the equilibrium constant if the temperature is increased?
2. What will happen to the value of the equilibrium constant if the volume of the container is reduced to 0.5 L?
**Options:**
- a) increases
- b) no change
1.
- a) increases
- b) increases
2.
- a) decreases
- b) no change
3.
- a) no change
- b) no change
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