Chemical Principles in the Laboratory
11th Edition
ISBN:9781305264434
Author:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Publisher:Emil Slowinski, Wayne C. Wolsey, Robert Rossi
Chapter32: Voltaic Cell Measurements
Section: Chapter Questions
Problem 1ASA
Related questions
Question
Explain the process of electrolysis using the diagram below.
![### Understanding the Process of Electrolysis: An Educational Overview
#### Explain the process of electrolysis using the diagram below.
- **Where does oxidation occur?**
- **Where does reduction occur?**
- **Describe the direction of the flow of electrons.**
- **How is this electrolytic cell different from a voltaic cell?**
**Note:** The symbol Me stands for a metal.
**Answer in complete sentences:**
#### Diagram Explanation:
The diagram below illustrates an electrolytic cell setup. In this diagram:
- The **cathode** is labeled as "Me," indicating a generic metal.
- The **anode** is labeled as "Cu," indicating copper.
- The solution contains \( \text{Cu}^{2+} \) (copper ions) and \( \text{SO}_4^{2-} \) (sulfate ions).
**Key Components:**
- **Cathode (Me):** This is the electrode where reduction takes place. Electrons are supplied from an external power source and enter this electrode.
- **Anode (Cu):** This is the electrode where oxidation occurs. Electrons are removed from this electrode and flow out to the external circuit.
**Electron Flow:**
- Electrons move from the anode (copper) to the cathode (metal). This is depicted by arrows indicating the direction of electron movement.
**Electrolytic Process:**
- At the **cathode**, \( \text{Cu}^{2+} \) ions in the solution gain electrons (reduce) to form solid copper, which deposits on the cathode.
\[ \text{Cu}^{2+} + 2\text{e}^- \rightarrow \text{Cu (s)} \]
- At the **anode**, copper metal loses electrons (oxidizes) to form \( \text{Cu}^{2+} \) ions, which enter the solution.
\[ \text{Cu (s)} \rightarrow \text{Cu}^{2+} + 2\text{e}^- \]
**Electrolytic Cell vs. Voltaic Cell:**
- In an **electrolytic cell**, electrical energy is used to drive a non-spontaneous chemical reaction.
- In a **voltaic cell**, a spontaneous chemical reaction produces electrical energy.
#### Diagram
1. **Cathode](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F77bec1a3-8760-4cef-a7d6-db82a48756ea%2Ff70538b1-0c3d-42f4-ad3a-32a254ac3f63%2Fuwumw9s_processed.jpeg&w=3840&q=75)
Transcribed Image Text:### Understanding the Process of Electrolysis: An Educational Overview
#### Explain the process of electrolysis using the diagram below.
- **Where does oxidation occur?**
- **Where does reduction occur?**
- **Describe the direction of the flow of electrons.**
- **How is this electrolytic cell different from a voltaic cell?**
**Note:** The symbol Me stands for a metal.
**Answer in complete sentences:**
#### Diagram Explanation:
The diagram below illustrates an electrolytic cell setup. In this diagram:
- The **cathode** is labeled as "Me," indicating a generic metal.
- The **anode** is labeled as "Cu," indicating copper.
- The solution contains \( \text{Cu}^{2+} \) (copper ions) and \( \text{SO}_4^{2-} \) (sulfate ions).
**Key Components:**
- **Cathode (Me):** This is the electrode where reduction takes place. Electrons are supplied from an external power source and enter this electrode.
- **Anode (Cu):** This is the electrode where oxidation occurs. Electrons are removed from this electrode and flow out to the external circuit.
**Electron Flow:**
- Electrons move from the anode (copper) to the cathode (metal). This is depicted by arrows indicating the direction of electron movement.
**Electrolytic Process:**
- At the **cathode**, \( \text{Cu}^{2+} \) ions in the solution gain electrons (reduce) to form solid copper, which deposits on the cathode.
\[ \text{Cu}^{2+} + 2\text{e}^- \rightarrow \text{Cu (s)} \]
- At the **anode**, copper metal loses electrons (oxidizes) to form \( \text{Cu}^{2+} \) ions, which enter the solution.
\[ \text{Cu (s)} \rightarrow \text{Cu}^{2+} + 2\text{e}^- \]
**Electrolytic Cell vs. Voltaic Cell:**
- In an **electrolytic cell**, electrical energy is used to drive a non-spontaneous chemical reaction.
- In a **voltaic cell**, a spontaneous chemical reaction produces electrical energy.
#### Diagram
1. **Cathode
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