A chemist designs a galvanic cell that uses these two half-reactions: half-reaction N₂(g)+4H₂O(1)+4e → N₂H₂(aq)+4OH¯ (aq) Cu²+ (aq) + Cut (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. standard reduction potential E = -1.16 V "red E "red = +0.153 V ローロ 10₁ % 0.²
A chemist designs a galvanic cell that uses these two half-reactions: half-reaction N₂(g)+4H₂O(1)+4e → N₂H₂(aq)+4OH¯ (aq) Cu²+ (aq) + Cut (aq) Answer the following questions about this cell. Write a balanced equation for the half-reaction that happens at the cathode. standard reduction potential E = -1.16 V "red E "red = +0.153 V ローロ 10₁ % 0.²
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Chapter1: Chemical Foundations
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![### Galvanic Cell Design and Analysis
#### A chemist designs a galvanic cell that uses these two half-reactions:
| half-reaction | standard reduction potential |
|-----------------------------------------|-----------------------------------|
| N₂(g) + 4H₂O(l) + 4e⁻ → N₂H₄(aq) + 4OH⁻(aq) | E₀_{red} = -1.16 V |
| Cu²⁺(aq) + e⁻ → Cu⁺(aq) | E₀_{red} = +0.153 V |
---
### Answer the following questions about this cell.
1. **Write a balanced equation for the half-reaction that happens at the cathode.**
\[ \boxed{} \]
2. **Write a balanced equation for the half-reaction that happens at the anode.**
\[ \boxed{} \]
3. **Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.**
\[ \boxed{} \]
4. **Do you have enough information to calculate the cell voltage under standard conditions?**
- [ ] Yes
- [ ] No
5. **If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits.**
\[ \boxed{} \, \text{V} \]
### Explanation of Components:
- **Cathode Half-Reaction:** This is where the reduction occurs (gain of electrons).
- **Anode Half-Reaction:** This is where the oxidation occurs (loss of electrons).
- **Overall Cell Reaction:** The sum of the anode and cathode half-reactions, ensuring spontaneity based on standard reduction potentials.
- **Cell Voltage:** The potential difference between the cathode and anode, calculated using standard reduction potentials.
---
In the table above, standard reduction potentials (E₀_{red}) are provided for the given half-reactions. Use these values to determine the overall cell voltage and the spontaneity of the galvanic cell reaction.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F12c0a0e9-4d98-45bb-8c42-bb6fd08d9097%2Fbead0d7f-a75d-4209-b294-7134a2e2c519%2Fmaxl8u1j_processed.png&w=3840&q=75)
Transcribed Image Text:### Galvanic Cell Design and Analysis
#### A chemist designs a galvanic cell that uses these two half-reactions:
| half-reaction | standard reduction potential |
|-----------------------------------------|-----------------------------------|
| N₂(g) + 4H₂O(l) + 4e⁻ → N₂H₄(aq) + 4OH⁻(aq) | E₀_{red} = -1.16 V |
| Cu²⁺(aq) + e⁻ → Cu⁺(aq) | E₀_{red} = +0.153 V |
---
### Answer the following questions about this cell.
1. **Write a balanced equation for the half-reaction that happens at the cathode.**
\[ \boxed{} \]
2. **Write a balanced equation for the half-reaction that happens at the anode.**
\[ \boxed{} \]
3. **Write a balanced equation for the overall reaction that powers the cell. Be sure the reaction is spontaneous as written.**
\[ \boxed{} \]
4. **Do you have enough information to calculate the cell voltage under standard conditions?**
- [ ] Yes
- [ ] No
5. **If you said it was possible to calculate the cell voltage, do so and enter your answer here. Be sure your answer has the correct number of significant digits.**
\[ \boxed{} \, \text{V} \]
### Explanation of Components:
- **Cathode Half-Reaction:** This is where the reduction occurs (gain of electrons).
- **Anode Half-Reaction:** This is where the oxidation occurs (loss of electrons).
- **Overall Cell Reaction:** The sum of the anode and cathode half-reactions, ensuring spontaneity based on standard reduction potentials.
- **Cell Voltage:** The potential difference between the cathode and anode, calculated using standard reduction potentials.
---
In the table above, standard reduction potentials (E₀_{red}) are provided for the given half-reactions. Use these values to determine the overall cell voltage and the spontaneity of the galvanic cell reaction.
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