Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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![#### Chemical Equilibrium
**Question 15:**
For the reaction:
\[ \text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g) \]
\[ K_c = 0.15 \text{ at } 25 °C \]
We initially mixed 3 M (Molar) of \( \text{N}_2\text{O}_4 \) gas with 1 M of \( \text{NO}_2 \) gas in a 1.0 L sealed flask and allowed the reaction to reach equilibrium. Before equilibrium is reached, in which direction will the reaction be shifted to reach equilibrium?
a. Reaction will shift **L --> R**
b. Reaction will shift **L <-- R**
c. **Reaction is at equilibrium, no shift**
d. **None of the above**
### Equilibrium Constant and Reaction Direction:
The equilibrium constant \( K_c \) is given as 0.15 at 25 °C. The initial concentrations are:
- \( \text{N}_2\text{O}_4 \): 3 M
- \( \text{NO}_2 \): 1 M
**Reaction Quotient (\( Q \)):**
To determine the direction in which the reaction will proceed, we calculate the reaction quotient \( Q \):
\[ Q = \frac{[\text{NO}_2]^2}{[\text{N}_2\text{O}_4]} \]
\[ Q = \frac{(1)^2}{3} = \frac{1}{3} = 0.33 \]
**Comparison with \( K_c \):**
- If \( Q < K_c \), the reaction shifts right (towards the products).
- If \( Q > K_c \), the reaction shifts left (towards the reactants).
- If \( Q = K_c \), the reaction is at equilibrium.
In this case:
\[ Q < K_c \quad \text{(0.33 < 0.15)} \]
Therefore, the reaction will shift to the **right** to reach equilibrium.
**Answer:**
a. Reaction will shift **L --> R**](https://content.bartleby.com/qna-images/question/50ac3af8-ea03-460e-925c-2b4d70dad9f3/425d8728-6f3d-433c-821b-5845e390db29/xdwdmll.png)
Transcribed Image Text:#### Chemical Equilibrium
**Question 15:**
For the reaction:
\[ \text{N}_2\text{O}_4(g) \rightleftharpoons 2\text{NO}_2(g) \]
\[ K_c = 0.15 \text{ at } 25 °C \]
We initially mixed 3 M (Molar) of \( \text{N}_2\text{O}_4 \) gas with 1 M of \( \text{NO}_2 \) gas in a 1.0 L sealed flask and allowed the reaction to reach equilibrium. Before equilibrium is reached, in which direction will the reaction be shifted to reach equilibrium?
a. Reaction will shift **L --> R**
b. Reaction will shift **L <-- R**
c. **Reaction is at equilibrium, no shift**
d. **None of the above**
### Equilibrium Constant and Reaction Direction:
The equilibrium constant \( K_c \) is given as 0.15 at 25 °C. The initial concentrations are:
- \( \text{N}_2\text{O}_4 \): 3 M
- \( \text{NO}_2 \): 1 M
**Reaction Quotient (\( Q \)):**
To determine the direction in which the reaction will proceed, we calculate the reaction quotient \( Q \):
\[ Q = \frac{[\text{NO}_2]^2}{[\text{N}_2\text{O}_4]} \]
\[ Q = \frac{(1)^2}{3} = \frac{1}{3} = 0.33 \]
**Comparison with \( K_c \):**
- If \( Q < K_c \), the reaction shifts right (towards the products).
- If \( Q > K_c \), the reaction shifts left (towards the reactants).
- If \( Q = K_c \), the reaction is at equilibrium.
In this case:
\[ Q < K_c \quad \text{(0.33 < 0.15)} \]
Therefore, the reaction will shift to the **right** to reach equilibrium.
**Answer:**
a. Reaction will shift **L --> R**
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