1 minus (0.15 M)|Mn²+ (2.69 M)|O H 1 minus X(s)|X¹+ (8.07 M) || Mn 04 The reduction potential for X¹+ is 0.81 V. What is the potential of this non standard cell (in Volts)? (8.98 M)
1 minus (0.15 M)|Mn²+ (2.69 M)|O H 1 minus X(s)|X¹+ (8.07 M) || Mn 04 The reduction potential for X¹+ is 0.81 V. What is the potential of this non standard cell (in Volts)? (8.98 M)
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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Transcribed Image Text:**Cell Notation:**
X(s) | X¹⁺ (8.07 M) || MnO₄⁻ (0.15 M) | Mn²⁺ (2.69 M) | OH⁻ (8.98 M)
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**Details:**
- The reduction potential for X¹⁺ is 0.81 V.
**Problem Statement:**
What is the potential of this non-standard cell (in Volts)?
---
**Explanation of Notation:**
The cell notation represents an electrochemical cell:
- **X(s) | X¹⁺ (8.07 M)**: The anode half-cell with solid X and its ion X¹⁺ at 8.07 M.
- **MnO₄⁻ (0.15 M) | Mn²⁺ (2.69 M) | OH⁻ (8.98 M)**: The cathode half-cell with MnO₄⁻ at 0.15 M, Mn²⁺ at 2.69 M, and OH⁻ at 8.98 M.
- The double vertical lines "||" indicate a salt bridge or a porous barrier separating the two half-cells.
![# Non-Standard Cells and the Nernst Equation
### Reactions and Standard Electrode Potentials
1. \( \text{MnO}_4^- + 4 \, \text{H}^+ + 3 \, \text{e}^- \rightarrow \text{MnO}_2 + 2 \, \text{H}_2\text{O} \) \((E^0 = 1.70 \, \text{V})\)
2. \( \text{MnO}_4^- + 8 \, \text{H}^+ + 5 \, \text{e}^- \rightarrow \text{Mn}^{2+} + 4 \, \text{H}_2\text{O} \) \((E^0 = 1.51 \, \text{V})\)
3. \( \text{MnO}_4^- + 4 \, \text{H}_2\text{O} + 5 \, \text{e}^- \rightarrow \text{Mn}^{2+} + 8 \, \text{OH}^- \) \((E^0 = 0.90 \, \text{V})\)
4. \( \text{MnO}_4^- + 2 \, \text{H}_2\text{O} + 3 \, \text{e}^- \rightarrow \text{MnO}_2 + 4 \, \text{OH}^- \) \((E^0 = 0.60 \, \text{V})\)
### Nernst Equation
\[ E_{\text{cell}} = E^0_{\text{cell}} - \left( \frac{0.0592 \, \text{V}}{n} \right) \log Q \]
This equation is used to calculate the potential of a cell under non-standard conditions, where \( E_{\text{cell}} \) is the cell potential, \( E^0_{\text{cell}} \) is the standard cell potential, \( n \) is the number of moles of electrons transferred in the reaction, and \( Q \) is the reaction quotient.
### Alternative Representations
- OR \( \text{MnO}_4^{1-} + 4 \, \text{H}^+ +](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6ae95cc5-a0cd-43b0-8331-9678c9dacca0%2F64955817-4f91-4455-bb7d-64e0f15c8069%2Fur2ugl8_processed.png&w=3840&q=75)
Transcribed Image Text:# Non-Standard Cells and the Nernst Equation
### Reactions and Standard Electrode Potentials
1. \( \text{MnO}_4^- + 4 \, \text{H}^+ + 3 \, \text{e}^- \rightarrow \text{MnO}_2 + 2 \, \text{H}_2\text{O} \) \((E^0 = 1.70 \, \text{V})\)
2. \( \text{MnO}_4^- + 8 \, \text{H}^+ + 5 \, \text{e}^- \rightarrow \text{Mn}^{2+} + 4 \, \text{H}_2\text{O} \) \((E^0 = 1.51 \, \text{V})\)
3. \( \text{MnO}_4^- + 4 \, \text{H}_2\text{O} + 5 \, \text{e}^- \rightarrow \text{Mn}^{2+} + 8 \, \text{OH}^- \) \((E^0 = 0.90 \, \text{V})\)
4. \( \text{MnO}_4^- + 2 \, \text{H}_2\text{O} + 3 \, \text{e}^- \rightarrow \text{MnO}_2 + 4 \, \text{OH}^- \) \((E^0 = 0.60 \, \text{V})\)
### Nernst Equation
\[ E_{\text{cell}} = E^0_{\text{cell}} - \left( \frac{0.0592 \, \text{V}}{n} \right) \log Q \]
This equation is used to calculate the potential of a cell under non-standard conditions, where \( E_{\text{cell}} \) is the cell potential, \( E^0_{\text{cell}} \) is the standard cell potential, \( n \) is the number of moles of electrons transferred in the reaction, and \( Q \) is the reaction quotient.
### Alternative Representations
- OR \( \text{MnO}_4^{1-} + 4 \, \text{H}^+ +
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