What is the change in Gibb's Free Energy for a reaction that has an enthalpy change of 229.6 kJ/mol and a entropy change of 87.5 J/(mol K) at 62.6 °C? Your Answer:
What is the change in Gibb's Free Energy for a reaction that has an enthalpy change of 229.6 kJ/mol and a entropy change of 87.5 J/(mol K) at 62.6 °C? Your Answer:
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:**
What is the change in Gibbs Free Energy for a reaction that has an enthalpy change of 229.6 kJ/mol and an entropy change of 87.5 J/(mol K) at 62.6 °C?
**Your Answer:**
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| **Answer** | |
| **Units** | |
*Note: This section contains an input area designed for entering numerical and unit responses.*
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To solve this problem, use the Gibbs Free Energy equation:
\[ \Delta G = \Delta H - T \Delta S \]
Where:
- \(\Delta G\) is the change in Gibbs Free Energy.
- \(\Delta H\) is the change in enthalpy.
- \(T\) is the temperature in Kelvin.
- \(\Delta S\) is the change in entropy.
*Convert the temperature to Kelvin by adding 273.15 to the Celsius temperature:*
\[ T = 62.6 + 273.15 = 335.75 \, \text{K} \]
*Ensure units are consistent: Convert \(\Delta S\) from J/(mol K) to kJ/(mol K) by dividing by 1000:*
\[ \Delta S = 87.5 \, \text{J/(mol K)} = 0.0875 \, \text{kJ/(mol K)} \]
*Substitute the values into the Gibbs Free Energy equation:*
\[ \Delta G = 229.6 \, \text{kJ/mol} - 335.75 \, \text{K} \times 0.0875 \, \text{kJ/(mol K)} \]
*Calculate the change in Gibbs Free Energy.*](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fb5cb748f-b247-416f-8df5-751d92c52687%2F8ca940c5-88c8-4bb8-b547-80675983d154%2Fnnmqpa_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
What is the change in Gibbs Free Energy for a reaction that has an enthalpy change of 229.6 kJ/mol and an entropy change of 87.5 J/(mol K) at 62.6 °C?
**Your Answer:**
| | |
|-------------------|------------|
| **Answer** | |
| **Units** | |
*Note: This section contains an input area designed for entering numerical and unit responses.*
---
To solve this problem, use the Gibbs Free Energy equation:
\[ \Delta G = \Delta H - T \Delta S \]
Where:
- \(\Delta G\) is the change in Gibbs Free Energy.
- \(\Delta H\) is the change in enthalpy.
- \(T\) is the temperature in Kelvin.
- \(\Delta S\) is the change in entropy.
*Convert the temperature to Kelvin by adding 273.15 to the Celsius temperature:*
\[ T = 62.6 + 273.15 = 335.75 \, \text{K} \]
*Ensure units are consistent: Convert \(\Delta S\) from J/(mol K) to kJ/(mol K) by dividing by 1000:*
\[ \Delta S = 87.5 \, \text{J/(mol K)} = 0.0875 \, \text{kJ/(mol K)} \]
*Substitute the values into the Gibbs Free Energy equation:*
\[ \Delta G = 229.6 \, \text{kJ/mol} - 335.75 \, \text{K} \times 0.0875 \, \text{kJ/(mol K)} \]
*Calculate the change in Gibbs Free Energy.*
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