Chemistry
10th Edition
ISBN: 9781305957404
Author: Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher: Cengage Learning
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Please answer A:
![### Using the Voltaic Cell
#### A) Write the equation for this cell.
---
#### B) Calculate standard cell potential (E°).
---
#### C) Calculate the voltage for this cell.
---
#### D) Diagram Analysis
**In the above diagram, label the anode, cathode, and draw an arrow showing the flow of electrons in the cell.**
The diagram depicts a voltaic cell with two half-cells connected by a porous barrier. The left half-cell contains an aluminum (Al) electrode submerged in a 0.435 M Al³⁺ solution. The right half-cell contains a tin (Sn) electrode submerged in a 0.00212 M Sn²⁺ solution.
At the top of the diagram, a voltmeter (V) is shown connecting the aluminum and tin electrodes.
---
#### E) Write the cell diagram.
---
### Diagram Analysis:
1. **Voltmeter (V)**: Positioned at the top, indicating measurement of potential difference between the two electrodes.
2. **Porous Barrier**: Positioned in the center, it separates the two half-cells while allowing the flow of ions to maintain electrical neutrality.
3. **Aluminum Electrode (Al)**: Located on the left, submerged in a solution of 0.435 M Al³⁺ indicating it likely functions as the anode (site of oxidation).
4. **Tin Electrode (Sn)**: Positioned on the right, submerged in 0.00212 M Sn²⁺ solution, indicating it functions as the cathode (site of reduction).
5. **Concentrations**:
- For Al³⁺: 0.435 M
- For Sn²⁺: 0.00212 M
---
### Notation:
- **Anode (Oxidation Site)**: Al is typically here, as it will lose electrons.
- **Cathode (Reduction Site)**: Sn often gains the electrons.
*Flow of Electrons*: Electrons will flow from the anode (Al) to the cathode (Sn).
---
### Cell Diagram:
\[ \text{Anode} | \text{Anode Solution} (concentration) || \text{Cathode Solution} (concentration) | \text{Cathode} \]
\[ \text{Al} | \text{Al}^{3+} (0.435 \text{ M}) || \text{](https://content.bartleby.com/qna-images/question/43ef5448-495e-49e8-9cec-405cabc5c22f/157e62ab-777d-415f-a996-6b379d44cf27/78gkej.jpeg)
Transcribed Image Text:### Using the Voltaic Cell
#### A) Write the equation for this cell.
---
#### B) Calculate standard cell potential (E°).
---
#### C) Calculate the voltage for this cell.
---
#### D) Diagram Analysis
**In the above diagram, label the anode, cathode, and draw an arrow showing the flow of electrons in the cell.**
The diagram depicts a voltaic cell with two half-cells connected by a porous barrier. The left half-cell contains an aluminum (Al) electrode submerged in a 0.435 M Al³⁺ solution. The right half-cell contains a tin (Sn) electrode submerged in a 0.00212 M Sn²⁺ solution.
At the top of the diagram, a voltmeter (V) is shown connecting the aluminum and tin electrodes.
---
#### E) Write the cell diagram.
---
### Diagram Analysis:
1. **Voltmeter (V)**: Positioned at the top, indicating measurement of potential difference between the two electrodes.
2. **Porous Barrier**: Positioned in the center, it separates the two half-cells while allowing the flow of ions to maintain electrical neutrality.
3. **Aluminum Electrode (Al)**: Located on the left, submerged in a solution of 0.435 M Al³⁺ indicating it likely functions as the anode (site of oxidation).
4. **Tin Electrode (Sn)**: Positioned on the right, submerged in 0.00212 M Sn²⁺ solution, indicating it functions as the cathode (site of reduction).
5. **Concentrations**:
- For Al³⁺: 0.435 M
- For Sn²⁺: 0.00212 M
---
### Notation:
- **Anode (Oxidation Site)**: Al is typically here, as it will lose electrons.
- **Cathode (Reduction Site)**: Sn often gains the electrons.
*Flow of Electrons*: Electrons will flow from the anode (Al) to the cathode (Sn).
---
### Cell Diagram:
\[ \text{Anode} | \text{Anode Solution} (concentration) || \text{Cathode Solution} (concentration) | \text{Cathode} \]
\[ \text{Al} | \text{Al}^{3+} (0.435 \text{ M}) || \text{
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