A) AG becomes less negative and the reaction becomes less spontaneous. B) AG becomes more negative and the reaction becomes less spontaneous. AH = -201 kJ/mol C) AG becomes more negative and the reaction becomes more spontaneous. D) AG becomes less negative and the reaction becomes more spontaneous. AS = -189.2 J/mol•K E) AG becomes zero and the reaction reaches equilibrium.
A) AG becomes less negative and the reaction becomes less spontaneous. B) AG becomes more negative and the reaction becomes less spontaneous. AH = -201 kJ/mol C) AG becomes more negative and the reaction becomes more spontaneous. D) AG becomes less negative and the reaction becomes more spontaneous. AS = -189.2 J/mol•K E) AG becomes zero and the reaction reaches equilibrium.
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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Predict how ∆G changes with increasing temperature for the reaction A(g) + B(g) → C(g).
![**Thermodynamics and Spontaneity**
**Enthalpy and Entropy Values:**
- **ΔH = -201 kJ/mol**
- **ΔS = -189.2 J/mol·K**
These values are fundamental in determining the spontaneity of a chemical reaction through Gibbs Free Energy (ΔG).
**Multiple-Choice Question:**
Which of the following describes the effect on the Gibbs Free Energy (ΔG) and spontaneity of the reaction?
A) ΔG becomes less negative and the reaction becomes less spontaneous.
B) ΔG becomes more negative and the reaction becomes less spontaneous.
C) ΔG becomes more negative and the reaction becomes more spontaneous.
D) ΔG becomes less negative and the reaction becomes more spontaneous.
E) ΔG becomes zero and the reaction reaches equilibrium.
**Explanation:**
In the context of thermodynamics, the change in Gibbs Free Energy (ΔG) can be calculated using the equation:
\[ ΔG = ΔH - TΔS \]
Where \( ΔH \) is the change in enthalpy, \( T \) is the temperature in Kelvin, and \( ΔS \) is the change in entropy. For reactions to be spontaneous, \( ΔG \) must be negative. Depending on the conditions, particularly temperature, \( ΔG \) can vary, affecting the spontaneity of a reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2851f780-2f0c-4741-8c61-f17f4e74deaf%2F37973cad-ce71-45df-abcf-59df82c418bc%2Fnwosy6_processed.png&w=3840&q=75)
Transcribed Image Text:**Thermodynamics and Spontaneity**
**Enthalpy and Entropy Values:**
- **ΔH = -201 kJ/mol**
- **ΔS = -189.2 J/mol·K**
These values are fundamental in determining the spontaneity of a chemical reaction through Gibbs Free Energy (ΔG).
**Multiple-Choice Question:**
Which of the following describes the effect on the Gibbs Free Energy (ΔG) and spontaneity of the reaction?
A) ΔG becomes less negative and the reaction becomes less spontaneous.
B) ΔG becomes more negative and the reaction becomes less spontaneous.
C) ΔG becomes more negative and the reaction becomes more spontaneous.
D) ΔG becomes less negative and the reaction becomes more spontaneous.
E) ΔG becomes zero and the reaction reaches equilibrium.
**Explanation:**
In the context of thermodynamics, the change in Gibbs Free Energy (ΔG) can be calculated using the equation:
\[ ΔG = ΔH - TΔS \]
Where \( ΔH \) is the change in enthalpy, \( T \) is the temperature in Kelvin, and \( ΔS \) is the change in entropy. For reactions to be spontaneous, \( ΔG \) must be negative. Depending on the conditions, particularly temperature, \( ΔG \) can vary, affecting the spontaneity of a reaction.
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