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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![## Electrolytic Cell Question
**Question 3:**
*Explain the transformation when an electrolytic cell is in operation. Discuss why Cu is positive in this reaction:*
\[ \text{Zn(s) | Zn}^{2+} || \text{Cu}^{2+} | \text{Cu} \]
---
### Explanation:
An electrolytic cell is a device that uses electrical energy to drive a non-spontaneous chemical reaction. When an electrolytic cell is in operation, the external electrical energy forces electrons to move towards the cathode and away from the anode, causing oxidation-reduction reactions to occur.
In this specific reaction:
\[ \text{Zn(s) | Zn}^{2+} || \text{Cu}^{2+} | \text{Cu} \]
- **Anode Reaction (Oxidation):** Zinc (Zn) loses electrons to form zinc ions \( \text{Zn}^{2+} \):
\[
\text{Zn} \rightarrow \text{Zn}^{2+} + 2\text{e}^-
\]
- **Cathode Reaction (Reduction):** Copper ions \( \text{Cu}^{2+} \) gain electrons to form copper (Cu):
\[
\text{Cu}^{2+} + 2\text{e}^- \rightarrow \text{Cu}
\]
In an electrolytic cell, the anode is the positive electrode, and the cathode is the negative electrode. However, the specifics provided in the question suggest a galvanic cell notation where zinc is initially oxidized and copper is reduced.
### Why Cu is Positive
Copper (Cu) is referenced as positive in this reaction because it is involved in the reduction half-reaction, gaining electrons. In the traditional sense of an electrolytic cell setup:
- The **anode** (where oxidation occurs) is positively charged.
- The **cathode** (where reduction occurs) is negatively charged.
However, based on the cell notation provided (which typically represents a galvanic cell structure), Zn is the anode that gets oxidized, and Cu is the cathode that gets reduced. Hence, the question might imply that copper ions (Cu²⁺) are initially present on the positive side of the galvanic cell setup, showing they get reduced during the operation.
### Conclusion
Understanding the transformation in an electrolytic setup requires knowing the specific reactions and](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F5106b7d5-4699-43ee-ae46-0af4e3f0b206%2Ff95016db-53f0-4765-be34-6e35929b4623%2Fgove4hp_processed.jpeg&w=3840&q=75)
Transcribed Image Text:## Electrolytic Cell Question
**Question 3:**
*Explain the transformation when an electrolytic cell is in operation. Discuss why Cu is positive in this reaction:*
\[ \text{Zn(s) | Zn}^{2+} || \text{Cu}^{2+} | \text{Cu} \]
---
### Explanation:
An electrolytic cell is a device that uses electrical energy to drive a non-spontaneous chemical reaction. When an electrolytic cell is in operation, the external electrical energy forces electrons to move towards the cathode and away from the anode, causing oxidation-reduction reactions to occur.
In this specific reaction:
\[ \text{Zn(s) | Zn}^{2+} || \text{Cu}^{2+} | \text{Cu} \]
- **Anode Reaction (Oxidation):** Zinc (Zn) loses electrons to form zinc ions \( \text{Zn}^{2+} \):
\[
\text{Zn} \rightarrow \text{Zn}^{2+} + 2\text{e}^-
\]
- **Cathode Reaction (Reduction):** Copper ions \( \text{Cu}^{2+} \) gain electrons to form copper (Cu):
\[
\text{Cu}^{2+} + 2\text{e}^- \rightarrow \text{Cu}
\]
In an electrolytic cell, the anode is the positive electrode, and the cathode is the negative electrode. However, the specifics provided in the question suggest a galvanic cell notation where zinc is initially oxidized and copper is reduced.
### Why Cu is Positive
Copper (Cu) is referenced as positive in this reaction because it is involved in the reduction half-reaction, gaining electrons. In the traditional sense of an electrolytic cell setup:
- The **anode** (where oxidation occurs) is positively charged.
- The **cathode** (where reduction occurs) is negatively charged.
However, based on the cell notation provided (which typically represents a galvanic cell structure), Zn is the anode that gets oxidized, and Cu is the cathode that gets reduced. Hence, the question might imply that copper ions (Cu²⁺) are initially present on the positive side of the galvanic cell setup, showing they get reduced during the operation.
### Conclusion
Understanding the transformation in an electrolytic setup requires knowing the specific reactions and
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