Using the standard reduction potentials below, what is the cell potential for a fuel operating under standard conditions:1 Man H₂ EP=OV +4H¹ (aq) + 4e¯¯ →→→ V 2H* +2e 0₂(g) + 1.229 Part 2 → 2H₂O(1) Fº=1.229 V If the cell is operated at 200.0°C, 9.06 bar H₂, 8.2 bar O₂, and a pH of 1.00, what is the resulting cell potential? V
Using the standard reduction potentials below, what is the cell potential for a fuel operating under standard conditions:1 Man H₂ EP=OV +4H¹ (aq) + 4e¯¯ →→→ V 2H* +2e 0₂(g) + 1.229 Part 2 → 2H₂O(1) Fº=1.229 V If the cell is operated at 200.0°C, 9.06 bar H₂, 8.2 bar O₂, and a pH of 1.00, what is the resulting cell potential? V
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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![### Fuel Cells and Redox Reactions
**Overview:**
The particulate model depicted illustrates the redox reactions involved in the production of energy from fuel cells. This model provides a basis for answering subsequent questions regarding fuel cell operations.
---
**Diagram Explanation:**
The diagram consists of three molecular representations:
1. **Hydrogen Molecule (H₂):** Two white spheres connected, representing diatomic hydrogen.
2. **Oxygen Molecule (O₂):** Two red spheres connected, representing diatomic oxygen.
3. **Water Molecule (H₂O):** A bent shape with two smaller white spheres (hydrogen) and a larger red sphere (oxygen), representing water, the product.
Arrows indicate the flow of electrons from hydrogen to oxygen, illustrating the electron transfer during the reaction.
---
**6th Attempt:**
#### Part 1
**Objective:** Determine the cell potential for a fuel cell under standard conditions (1 M concentration, 1 atm pressure, 25°C).
**Standard Reduction Potentials:**
- \(2H^+ + 2e^- \rightarrow H_2\) with \(E^\circ = 0 \, \text{V}\)
- \(O_2(g) + 4H^+(aq) + 4e^- \rightarrow 2H_2O(l)\) with \(E^\circ = 1.229 \, \text{V}\)
**Cell Potential Calculation:**
\[ E^\circ_{\text{cell}} = 1.229 \, \text{V} \]
---
#### Part 2
**Objective:** Calculate the resulting cell potential when the cell operates at non-standard conditions: 200.0°C, 9.06 bar H₂, 8.2 bar O₂, and a pH of 1.00.
**Answer Box:**
- Resulting cell potential: _____ V
---
This structured approach allows students to engage with chemical concepts related to fuel cells and practice applying redox reaction principles and Nernst equation applications for calculating cell potentials.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F9beb5ab6-4fd3-4e9c-8c6c-c4109f4c868c%2F405d640e-adb2-4acd-b1ab-d027d9296677%2F0kp2bio_processed.png&w=3840&q=75)
Transcribed Image Text:### Fuel Cells and Redox Reactions
**Overview:**
The particulate model depicted illustrates the redox reactions involved in the production of energy from fuel cells. This model provides a basis for answering subsequent questions regarding fuel cell operations.
---
**Diagram Explanation:**
The diagram consists of three molecular representations:
1. **Hydrogen Molecule (H₂):** Two white spheres connected, representing diatomic hydrogen.
2. **Oxygen Molecule (O₂):** Two red spheres connected, representing diatomic oxygen.
3. **Water Molecule (H₂O):** A bent shape with two smaller white spheres (hydrogen) and a larger red sphere (oxygen), representing water, the product.
Arrows indicate the flow of electrons from hydrogen to oxygen, illustrating the electron transfer during the reaction.
---
**6th Attempt:**
#### Part 1
**Objective:** Determine the cell potential for a fuel cell under standard conditions (1 M concentration, 1 atm pressure, 25°C).
**Standard Reduction Potentials:**
- \(2H^+ + 2e^- \rightarrow H_2\) with \(E^\circ = 0 \, \text{V}\)
- \(O_2(g) + 4H^+(aq) + 4e^- \rightarrow 2H_2O(l)\) with \(E^\circ = 1.229 \, \text{V}\)
**Cell Potential Calculation:**
\[ E^\circ_{\text{cell}} = 1.229 \, \text{V} \]
---
#### Part 2
**Objective:** Calculate the resulting cell potential when the cell operates at non-standard conditions: 200.0°C, 9.06 bar H₂, 8.2 bar O₂, and a pH of 1.00.
**Answer Box:**
- Resulting cell potential: _____ V
---
This structured approach allows students to engage with chemical concepts related to fuel cells and practice applying redox reaction principles and Nernst equation applications for calculating cell potentials.
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