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
![The image contains four equations related to electrochemistry and thermodynamics. Each equation is accompanied by a checkbox to the left, suggesting a multiple-choice question format. Below is the transcription of each equation:
1. **Equation 1:**
\[
E = E^\circ - \frac{RT}{nF}
\]
2. **Equation 2:**
\[
E^\circ = \frac{RT}{nF}
\]
3. **Equation 3:**
\[
E^\circ = -nF
\]
4. **Equation 4:**
\[
E^\circ = -\frac{RT}{nF}
\]
Each equation seems to be derived from or related to the Nernst equation, which describes the electrochemical cell potential. Here, \(E\) is the cell potential, \(E^\circ\) is the standard cell potential, \(R\) is the universal gas constant, \(T\) is the temperature in Kelvin, \(n\) is the number of moles of electrons exchanged, and \(F\) is Faraday's constant.
There are no graphs or diagrams in this image.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2ceb2d65-29b4-49d4-9830-4ba06589987b%2F891107a7-8d25-44b3-8d08-744f5218d3d1%2F6xzt76l_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The image contains four equations related to electrochemistry and thermodynamics. Each equation is accompanied by a checkbox to the left, suggesting a multiple-choice question format. Below is the transcription of each equation:
1. **Equation 1:**
\[
E = E^\circ - \frac{RT}{nF}
\]
2. **Equation 2:**
\[
E^\circ = \frac{RT}{nF}
\]
3. **Equation 3:**
\[
E^\circ = -nF
\]
4. **Equation 4:**
\[
E^\circ = -\frac{RT}{nF}
\]
Each equation seems to be derived from or related to the Nernst equation, which describes the electrochemical cell potential. Here, \(E\) is the cell potential, \(E^\circ\) is the standard cell potential, \(R\) is the universal gas constant, \(T\) is the temperature in Kelvin, \(n\) is the number of moles of electrons exchanged, and \(F\) is Faraday's constant.
There are no graphs or diagrams in this image.
![### Question: Which is the Nernst equation?
#### Multiple Choice
- (Option 1)
- None of these statements is correct.
- (Option 2)
- \( E = E^o - \frac{RT}{nF} \cdot \ln{2} \)
- (Option 3)
- \( E^o = \frac{RT}{nF} \cdot \ln{ \frac{1}{}} \)
---
### Explanation:
The Nernst equation is used to calculate the electrochemical potential across a cell membrane based on ion concentration. The correct form of the Nernst equation is:
\[ E = E^o - \frac{RT}{nF} \cdot \ln Q \]
where:
- \( E \) is the cell potential.
- \( E^o \) is the standard cell potential.
- \( R \) is the universal gas constant.
- \( T \) is the temperature in Kelvin.
- \( n \) is the number of moles of electrons transferred.
- \( F \) is Faraday's constant.
- \( Q \) is the reaction quotient.
In the given options, part of the equation is presented incorrectly. The correct application involves using the terms appropriately to calculate the potential based on accurate values and conditions.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2ceb2d65-29b4-49d4-9830-4ba06589987b%2F891107a7-8d25-44b3-8d08-744f5218d3d1%2Fjotkprd_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Question: Which is the Nernst equation?
#### Multiple Choice
- (Option 1)
- None of these statements is correct.
- (Option 2)
- \( E = E^o - \frac{RT}{nF} \cdot \ln{2} \)
- (Option 3)
- \( E^o = \frac{RT}{nF} \cdot \ln{ \frac{1}{}} \)
---
### Explanation:
The Nernst equation is used to calculate the electrochemical potential across a cell membrane based on ion concentration. The correct form of the Nernst equation is:
\[ E = E^o - \frac{RT}{nF} \cdot \ln Q \]
where:
- \( E \) is the cell potential.
- \( E^o \) is the standard cell potential.
- \( R \) is the universal gas constant.
- \( T \) is the temperature in Kelvin.
- \( n \) is the number of moles of electrons transferred.
- \( F \) is Faraday's constant.
- \( Q \) is the reaction quotient.
In the given options, part of the equation is presented incorrectly. The correct application involves using the terms appropriately to calculate the potential based on accurate values and conditions.
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