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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![### Understanding Electrode Polarity in a Zinc-Copper Cell
In a zinc-copper cell, represented as:
\[ \text{Zn}_{(s)} | \text{Zn}^{+2}_{(aq)} || \text{Cu}^{+2}_{(aq)} | \text{Cu}_{(s)} \]
Which electrode is positive?
#### Options:
- **A.** \( \text{Cu}^{+2} \)
- **B.** \( \text{Cu}_{(s)} \)
- **C.** \( \text{Zn}_{(s)} \)
- **D.** \( \text{Zn}^{+2} \)
### Explanation:
To understand which electrode is positive in this galvanic cell, we need to examine the standard cell notation and the principles of electrochemistry:
1. **Cell Notation:** The notation \( \text{Zn}_{(s)} | \text{Zn}^{+2}_{(aq)} || \text{Cu}^{+2}_{(aq)} | \text{Cu}_{(s)} \) represents a galvanic cell where zinc metal is oxidized to zinc ions \((\text{Zn}^{+2})\), and copper ions \((\text{Cu}^{+2})\) are reduced to copper metal.
2. **Oxidation and Reduction:**
- Oxidation occurs at the anode: \( \text{Zn}_{(s)} \rightarrow \text{Zn}^{+2}_{(aq)} + 2e^- \)
- Reduction occurs at the cathode: \( \text{Cu}^{+2}_{(aq)} + 2e^- \rightarrow \text{Cu}_{(s)} \)
3. **Electrode Polarity:**
- In a galvanic cell, the anode (where oxidation occurs) is negative.
- The cathode (where reduction occurs) is positive.
Therefore, in the given zinc-copper cell, \( \text{Cu}_{(s)} \) (the copper solid electrode) is the positive electrode, because it is where the copper ions \((\text{Cu}^{+2})\) gain electrons (reduction) to form solid copper.
### Correct Answer:
**B.** \( \text{Cu}_{(s)} \)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F76e38d3b-ade1-4412-8da2-a4b2bcd54116%2Fc9e27c7d-2be0-45f9-a308-152428cc4ca0%2Fq7l0gbh_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Understanding Electrode Polarity in a Zinc-Copper Cell
In a zinc-copper cell, represented as:
\[ \text{Zn}_{(s)} | \text{Zn}^{+2}_{(aq)} || \text{Cu}^{+2}_{(aq)} | \text{Cu}_{(s)} \]
Which electrode is positive?
#### Options:
- **A.** \( \text{Cu}^{+2} \)
- **B.** \( \text{Cu}_{(s)} \)
- **C.** \( \text{Zn}_{(s)} \)
- **D.** \( \text{Zn}^{+2} \)
### Explanation:
To understand which electrode is positive in this galvanic cell, we need to examine the standard cell notation and the principles of electrochemistry:
1. **Cell Notation:** The notation \( \text{Zn}_{(s)} | \text{Zn}^{+2}_{(aq)} || \text{Cu}^{+2}_{(aq)} | \text{Cu}_{(s)} \) represents a galvanic cell where zinc metal is oxidized to zinc ions \((\text{Zn}^{+2})\), and copper ions \((\text{Cu}^{+2})\) are reduced to copper metal.
2. **Oxidation and Reduction:**
- Oxidation occurs at the anode: \( \text{Zn}_{(s)} \rightarrow \text{Zn}^{+2}_{(aq)} + 2e^- \)
- Reduction occurs at the cathode: \( \text{Cu}^{+2}_{(aq)} + 2e^- \rightarrow \text{Cu}_{(s)} \)
3. **Electrode Polarity:**
- In a galvanic cell, the anode (where oxidation occurs) is negative.
- The cathode (where reduction occurs) is positive.
Therefore, in the given zinc-copper cell, \( \text{Cu}_{(s)} \) (the copper solid electrode) is the positive electrode, because it is where the copper ions \((\text{Cu}^{+2})\) gain electrons (reduction) to form solid copper.
### Correct Answer:
**B.** \( \text{Cu}_{(s)} \)
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