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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![### Reaction Equilibrium Analysis
Consider the following reaction where \( K_c = 7.00 \times 10^{-5} \) at 673 K:
\[ \text{NH}_4\text{I}(s) \rightleftharpoons \text{NH}_3(g) + \text{HI}(g) \]
A reaction mixture was found to contain \( 5.96 \times 10^{-2} \) moles of \(\text{NH}_4\text{I}(s)\), \( 5.51 \times 10^{-3} \) moles of \(\text{NH}_3(g)\), and \( 8.37 \times 10^{-3} \) moles of \(\text{HI}(g)\), in a 1.00 liter container.
#### Questions:
Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium?
- The reaction quotient, \( Q_c \), equals [input box].
- The reaction [selection box]:
- A. must run in the forward direction to reach equilibrium.
- B. must run in the reverse direction to reach equilibrium.
- C. is at equilibrium.
### Explanation:
To determine whether the reaction is at equilibrium, calculate the reaction quotient \( Q_c \) and compare it to \( K_c \). If \( Q_c < K_c \), the reaction will proceed in the forward direction to reach equilibrium. If \( Q_c > K_c \), the reaction needs to go in the reverse direction. If \( Q_c = K_c \), the reaction is at equilibrium.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa59a73bf-87c2-48f6-829d-0178c9223cc0%2Ff61bfdbe-18ea-45f9-9140-584a99f45238%2Fgz91ckd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Reaction Equilibrium Analysis
Consider the following reaction where \( K_c = 7.00 \times 10^{-5} \) at 673 K:
\[ \text{NH}_4\text{I}(s) \rightleftharpoons \text{NH}_3(g) + \text{HI}(g) \]
A reaction mixture was found to contain \( 5.96 \times 10^{-2} \) moles of \(\text{NH}_4\text{I}(s)\), \( 5.51 \times 10^{-3} \) moles of \(\text{NH}_3(g)\), and \( 8.37 \times 10^{-3} \) moles of \(\text{HI}(g)\), in a 1.00 liter container.
#### Questions:
Is the reaction at equilibrium? If not, what direction must it run in order to reach equilibrium?
- The reaction quotient, \( Q_c \), equals [input box].
- The reaction [selection box]:
- A. must run in the forward direction to reach equilibrium.
- B. must run in the reverse direction to reach equilibrium.
- C. is at equilibrium.
### Explanation:
To determine whether the reaction is at equilibrium, calculate the reaction quotient \( Q_c \) and compare it to \( K_c \). If \( Q_c < K_c \), the reaction will proceed in the forward direction to reach equilibrium. If \( Q_c > K_c \), the reaction needs to go in the reverse direction. If \( Q_c = K_c \), the reaction is at equilibrium.
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