Let the reaction achieve equilibrium, and the, according to Le Chatlier's Principle, the concentration o NH3 (at equilibrium) will a. increase if the concentration of N2 is decreased b. increase if the concentration of H2 is decreased c. increase if the temperature is increased d. decrease if the pressure of the reaction is decreased
Let the reaction achieve equilibrium, and the, according to Le Chatlier's Principle, the concentration o NH3 (at equilibrium) will a. increase if the concentration of N2 is decreased b. increase if the concentration of H2 is decreased c. increase if the temperature is increased d. decrease if the pressure of the reaction is decreased
Chemistry
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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
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![### Equilibrium in Chemical Reactions
**For the following endothermic reaction:**
\[ \text{N}_2 (g) + 3\text{ H}_2 (g) \leftrightarrow 2\text{ NH}_3 (g), \quad K_c = 112 \text{ (at 450 K)} \quad \Delta H^0 = + 29 \text{ kJ/mol} \]
#### Question 1:
In this reaction at equilibrium, the concentration of \(\text{N}_2\) is found to be 0.040 M, and that of \(\text{NH}_3\) is 0.251 M. What is the concentration of \(\text{H}_2\)?
Options:
a. 0.211 M
b. 0.242 M
c. 0.120 M
d. 0.065 M
e. 0.291 M
**Correct Answer:** a. 0.211 M
_A detailed explanation for students on how to solve this problem typically follows, demonstrating the use of the equilibrium constant expression._
#### Question 2:
Let the reaction achieve equilibrium, and then, according to Le Chatelier’s Principle, the concentration of \(\text{NH}_3\) (at equilibrium) will:
a. increase if the concentration of \(\text{N}_2\) is decreased
b. increase if the concentration of \(\text{H}_2\) is decreased
c. increase if the temperature is increased
d. decrease if the pressure of the reaction is decreased
**Explore the Options:**
- **Option a**: Decreasing the concentration of \(\text{N}_2\) will shift the equilibrium to the left, producing more \(\text{N}_2\) and \(\text{H}_2\), thus decreasing \(\text{NH}_3\).
- **Option b**: Decreasing the concentration of \(\text{H}_2\) will also shift the equilibrium to the left, decreasing \(\text{NH}_3\).
- **Option c**: Increasing the temperature for an endothermic reaction shifts the equilibrium to the right, thus increasing \(\text{NH}_3\).
- **Option d**: Decreasing the pressure of the reaction shifts the equilibrium towards the side with more moles of gas, which in](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F48deb947-3d41-43de-ac43-bef03e01cc59%2Fda4b267c-dc98-4d79-b7d8-db8612bf1556%2Fbb8bofv.png&w=3840&q=75)
Transcribed Image Text:### Equilibrium in Chemical Reactions
**For the following endothermic reaction:**
\[ \text{N}_2 (g) + 3\text{ H}_2 (g) \leftrightarrow 2\text{ NH}_3 (g), \quad K_c = 112 \text{ (at 450 K)} \quad \Delta H^0 = + 29 \text{ kJ/mol} \]
#### Question 1:
In this reaction at equilibrium, the concentration of \(\text{N}_2\) is found to be 0.040 M, and that of \(\text{NH}_3\) is 0.251 M. What is the concentration of \(\text{H}_2\)?
Options:
a. 0.211 M
b. 0.242 M
c. 0.120 M
d. 0.065 M
e. 0.291 M
**Correct Answer:** a. 0.211 M
_A detailed explanation for students on how to solve this problem typically follows, demonstrating the use of the equilibrium constant expression._
#### Question 2:
Let the reaction achieve equilibrium, and then, according to Le Chatelier’s Principle, the concentration of \(\text{NH}_3\) (at equilibrium) will:
a. increase if the concentration of \(\text{N}_2\) is decreased
b. increase if the concentration of \(\text{H}_2\) is decreased
c. increase if the temperature is increased
d. decrease if the pressure of the reaction is decreased
**Explore the Options:**
- **Option a**: Decreasing the concentration of \(\text{N}_2\) will shift the equilibrium to the left, producing more \(\text{N}_2\) and \(\text{H}_2\), thus decreasing \(\text{NH}_3\).
- **Option b**: Decreasing the concentration of \(\text{H}_2\) will also shift the equilibrium to the left, decreasing \(\text{NH}_3\).
- **Option c**: Increasing the temperature for an endothermic reaction shifts the equilibrium to the right, thus increasing \(\text{NH}_3\).
- **Option d**: Decreasing the pressure of the reaction shifts the equilibrium towards the side with more moles of gas, which in
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