You discover a cell that uses Cu² as the final electron acceptor in mitochondrial electron transpo (MET) instead of O. Cu* + 2e e → Cu° E°=+0.337 V A. How much free energy can be gained by oxidation of NADH in this novel MET system? Show calculations.
You discover a cell that uses Cu² as the final electron acceptor in mitochondrial electron transpo (MET) instead of O. Cu* + 2e e → Cu° E°=+0.337 V A. How much free energy can be gained by oxidation of NADH in this novel MET system? Show calculations.
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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![### Mitochondrial Electron Transport Adaptation
2. **Unique Electron Acceptor in Mitochondrial Electron Transport**:
- **Observation**: A cell is discovered to use Cu²⁺ as the final electron acceptor in mitochondrial electron transport (MET) instead of O₂.
- **Reaction**:
\[ \text{Cu}^{2+} + 2e^- \leftrightarrow \text{Cu}^0 \]
\[ \text{E}^\circ = +0.337 \, \text{V} \]
- **Problem Statement**:
**A. Calculation of Free Energy**:
Determine how much free energy can be gained by the oxidation of NADH in this novel MET system. Show calculations.
### Detailed Explanation
The reduction potential (Eº) for the half-reaction provided is +0.337 V for Cu²⁺/Cu⁰. To determine the free energy change (ΔG) from the oxidation of NADH, we need to use the Nernst equation and the known standard reduction potential for NADH/NAD⁺.
Key Steps for Calculation:
1. **Identify the standard reduction potentials**:
- For Cu²⁺ + 2e⁻ → Cu⁰:
Eº = +0.337 V
- For NAD⁺ + H⁺ + 2e⁻ → NADH:
Eº = -0.320 V
2. **Calculate the overall cell potential (Eºcell)**:
\[
\text{Eº} = \text{Eº (electron acceptor) - Eº (electron donor)}
\]
\[
\text{Eºcell} = 0.337 \, \text{V} - (-0.320 \, \text{V}) = 0.657 \, \text{V}
\]
3. **Use the Gibbs free energy equation**:
\[
\Delta G = -nFEºcell
\]
where:
- \( n \) = number of moles of electrons exchanged (n = 2 for NADH oxidation reaction)
- \( F \) = Faraday constant (approximately 96485 C/mol)
- \( Eºcell \) = total cell potential (0.657 V)
4. **](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fc0f85ff8-2ea0-4d43-a0c0-84de96cc63b8%2Ff980d60f-e705-40ef-8540-086527366a83%2Fyz0o13c_processed.png&w=3840&q=75)
Transcribed Image Text:### Mitochondrial Electron Transport Adaptation
2. **Unique Electron Acceptor in Mitochondrial Electron Transport**:
- **Observation**: A cell is discovered to use Cu²⁺ as the final electron acceptor in mitochondrial electron transport (MET) instead of O₂.
- **Reaction**:
\[ \text{Cu}^{2+} + 2e^- \leftrightarrow \text{Cu}^0 \]
\[ \text{E}^\circ = +0.337 \, \text{V} \]
- **Problem Statement**:
**A. Calculation of Free Energy**:
Determine how much free energy can be gained by the oxidation of NADH in this novel MET system. Show calculations.
### Detailed Explanation
The reduction potential (Eº) for the half-reaction provided is +0.337 V for Cu²⁺/Cu⁰. To determine the free energy change (ΔG) from the oxidation of NADH, we need to use the Nernst equation and the known standard reduction potential for NADH/NAD⁺.
Key Steps for Calculation:
1. **Identify the standard reduction potentials**:
- For Cu²⁺ + 2e⁻ → Cu⁰:
Eº = +0.337 V
- For NAD⁺ + H⁺ + 2e⁻ → NADH:
Eº = -0.320 V
2. **Calculate the overall cell potential (Eºcell)**:
\[
\text{Eº} = \text{Eº (electron acceptor) - Eº (electron donor)}
\]
\[
\text{Eºcell} = 0.337 \, \text{V} - (-0.320 \, \text{V}) = 0.657 \, \text{V}
\]
3. **Use the Gibbs free energy equation**:
\[
\Delta G = -nFEºcell
\]
where:
- \( n \) = number of moles of electrons exchanged (n = 2 for NADH oxidation reaction)
- \( F \) = Faraday constant (approximately 96485 C/mol)
- \( Eºcell \) = total cell potential (0.657 V)
4. **
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