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
![### Understanding Equilibrium Constant in Endothermic Reactions
#### Question:
As the temperature increases for an endothermic reaction, what happens to the equilibrium constant?
#### Answer Choices:
- **A) stays the same**
- **B) increases**
- **C) decreases**
- **D) increases only if ΔS is negative**
- **E) decreases only if ΔS is positive**
For endothermic reactions, the equilibrium constant increases with an increase in temperature. This is due to the fact that increasing temperature favors the forward reaction, which absorbs heat. This follows Le Chatelier's principle, which states that the system will adjust to counteract the change (in this case, the temperature increase).
To understand deeper, consider the Van't Hoff equation which shows the relationship between the equilibrium constant (K) and temperature (T):
\[ \ln K = -\frac{\Delta H}{RT} + \frac{\Delta S}{R} \]
Where:
- \( \Delta H \) is the enthalpy change (positive for endothermic reactions).
- \( R \) is the universal gas constant.
- \( \Delta S \) is the entropy change.
For an endothermic reaction (\(\Delta H > 0\)), an increase in \( T \) will increase \( K \) because \(\Delta H / RT\) decreases with increasing \( T \), leading to a larger value of \( K \). This aligns with option **B) increases**.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fad75d3c3-f925-415c-aa85-2c90219f0688%2F18775b4e-b49a-430e-9386-2565829a48e5%2Fs3udva_processed.png&w=3840&q=75)
Transcribed Image Text:### Understanding Equilibrium Constant in Endothermic Reactions
#### Question:
As the temperature increases for an endothermic reaction, what happens to the equilibrium constant?
#### Answer Choices:
- **A) stays the same**
- **B) increases**
- **C) decreases**
- **D) increases only if ΔS is negative**
- **E) decreases only if ΔS is positive**
For endothermic reactions, the equilibrium constant increases with an increase in temperature. This is due to the fact that increasing temperature favors the forward reaction, which absorbs heat. This follows Le Chatelier's principle, which states that the system will adjust to counteract the change (in this case, the temperature increase).
To understand deeper, consider the Van't Hoff equation which shows the relationship between the equilibrium constant (K) and temperature (T):
\[ \ln K = -\frac{\Delta H}{RT} + \frac{\Delta S}{R} \]
Where:
- \( \Delta H \) is the enthalpy change (positive for endothermic reactions).
- \( R \) is the universal gas constant.
- \( \Delta S \) is the entropy change.
For an endothermic reaction (\(\Delta H > 0\)), an increase in \( T \) will increase \( K \) because \(\Delta H / RT\) decreases with increasing \( T \), leading to a larger value of \( K \). This aligns with option **B) increases**.
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