The exothermic process CH,O) + 60(9) -- 6CO() + 6H,00) is initially at equilibrium. Which of the following statements isare true? (Select all that apply) O Adding HyO) wil increase Q and cause the reaction to shift left to re-achieve equilbrium. O creasing the volume of the reaction container will cause the system to shift right to re-achieve equilibrium O xp K O Decreasing the temperature causes K to increase in magnitude. O Adaing Helgi causes the total pressure in the system to increase but does not change the value of Q.
The exothermic process CH,O) + 60(9) -- 6CO() + 6H,00) is initially at equilibrium. Which of the following statements isare true? (Select all that apply) O Adding HyO) wil increase Q and cause the reaction to shift left to re-achieve equilbrium. O creasing the volume of the reaction container will cause the system to shift right to re-achieve equilibrium O xp K O Decreasing the temperature causes K to increase in magnitude. O Adaing Helgi causes the total pressure in the system to increase but does not change the value of Q.
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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![**Question: Understanding the Effects on Equilibrium**
The exothermic process C\(_6\)H\(_{12}\)(g) + 9O\(_2\)(g) ⇌ 6CO\(_2\)(g) + 6H\(_2\)O(g) is initially at equilibrium. Which of the following statements are true? (Select all that apply.)
- [ ] Adding H\(_2\)O(g) will increase Q and cause the reaction to shift left to re-achieve equilibrium.
- [ ] Increasing the volume of the reaction container will cause the system to shift right to re-achieve equilibrium.
- [ ] Kp = Kc.
- [ ] Decreasing the temperature causes K to increase in magnitude.
- [ ] Adding He(g) causes the total pressure in the system to increase but does not change the value of Q.
**Explanation (for use on educational website):**
This question pertains to the principles of Le Chatelier’s Principle and equilibrium constants for a chemical reaction. Given the balanced chemical equation, C\(_6\)H\(_{12}\)(g) + 9O\(_2\)(g) ⇌ 6CO\(_2\)(g) + 6H\(_2\)O(g), various factors can influence the direction in which the reaction shifts to maintain equilibrium.
1. **Effect of Adding H\(_2\)O(g)**:
- If H\(_2\)O(g) is added to the system, the quotient Q (reaction quotient) will momentarily increase because the concentration of one of the products increases. To re-achieve equilibrium, the system will shift towards the reactants (left side of the equation) to balance the increased concentration of the product.
2. **Effect of Increasing Reaction Volume**:
- When the volume of the reaction container is increased, the system will respond by shifting the equilibrium to the side with more gas molecules. In this case, there are 6 moles of gas on the product side and 10 moles of gas on the reactant side. Thus, the reaction will shift to the right, towards the products, to re-achieve equilibrium.
3. **Equating Kp and Kc**:
- The equilibrium constant Kp (in terms of partial pressures) and Kc (in terms of concentrations) are not necessarily equal. The relationship between](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc60fc3dd-1ac3-4d9e-b80d-dba4849839ee%2F2441acbd-409c-4617-a3be-4b535ae71551%2Fsrspelj_processed.png&w=3840&q=75)
Transcribed Image Text:**Question: Understanding the Effects on Equilibrium**
The exothermic process C\(_6\)H\(_{12}\)(g) + 9O\(_2\)(g) ⇌ 6CO\(_2\)(g) + 6H\(_2\)O(g) is initially at equilibrium. Which of the following statements are true? (Select all that apply.)
- [ ] Adding H\(_2\)O(g) will increase Q and cause the reaction to shift left to re-achieve equilibrium.
- [ ] Increasing the volume of the reaction container will cause the system to shift right to re-achieve equilibrium.
- [ ] Kp = Kc.
- [ ] Decreasing the temperature causes K to increase in magnitude.
- [ ] Adding He(g) causes the total pressure in the system to increase but does not change the value of Q.
**Explanation (for use on educational website):**
This question pertains to the principles of Le Chatelier’s Principle and equilibrium constants for a chemical reaction. Given the balanced chemical equation, C\(_6\)H\(_{12}\)(g) + 9O\(_2\)(g) ⇌ 6CO\(_2\)(g) + 6H\(_2\)O(g), various factors can influence the direction in which the reaction shifts to maintain equilibrium.
1. **Effect of Adding H\(_2\)O(g)**:
- If H\(_2\)O(g) is added to the system, the quotient Q (reaction quotient) will momentarily increase because the concentration of one of the products increases. To re-achieve equilibrium, the system will shift towards the reactants (left side of the equation) to balance the increased concentration of the product.
2. **Effect of Increasing Reaction Volume**:
- When the volume of the reaction container is increased, the system will respond by shifting the equilibrium to the side with more gas molecules. In this case, there are 6 moles of gas on the product side and 10 moles of gas on the reactant side. Thus, the reaction will shift to the right, towards the products, to re-achieve equilibrium.
3. **Equating Kp and Kc**:
- The equilibrium constant Kp (in terms of partial pressures) and Kc (in terms of concentrations) are not necessarily equal. The relationship between
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