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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![**Question 1: What is the correct cell notation for the reaction below?**
\[ \text{Cd}^{2+}(aq) + \text{Ni}(s) \rightarrow \text{Cd}(s) + \text{Ni}^{2+}(aq) \]
**Explanation:**
The given chemical reaction represents a redox process where cadmium ions (\(\text{Cd}^{2+}\)) in aqueous solution react with solid nickel (\(\text{Ni}\)) to produce solid cadmium (\(\text{Cd}\)) and nickel ions (\(\text{Ni}^{2+}\)) in aqueous solution.
In electrochemistry, the cell notation is used to describe the components of a galvanic (voltaic) cell in a standardized way. The notation is written as:
\[ \text{Anode} \ | \ \text{Anode Solution} \ || \ \text{Cathode Solution} \ | \ \text{Cathode} \]
For the reaction given:
- **Anode (oxidation occurs):** \(\text{Ni}(s) \rightarrow \text{Ni}^{2+}(aq) + 2e^-\)
- **Cathode (reduction occurs):** \(\text{Cd}^{2+}(aq) + 2e^- \rightarrow \text{Cd}(s)\)
Using this information, the cell notation for the reaction is:
\[ \text{Ni}(s) | \text{Ni}^{2+}(aq) || \text{Cd}^{2+}(aq) | \text{Cd}(s) \]
This notation indicates that nickel is the anode where oxidation occurs, and cadmium is the cathode where reduction happens. The double vertical lines represent the salt bridge or membrane separating the two half-cells.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F816b840c-3165-49ec-880b-7eda3f3e03a8%2Fe3d4c2b9-c3da-4c55-a63e-f9763180c0e2%2Fnlctcxd_processed.png&w=3840&q=75)
Transcribed Image Text:**Question 1: What is the correct cell notation for the reaction below?**
\[ \text{Cd}^{2+}(aq) + \text{Ni}(s) \rightarrow \text{Cd}(s) + \text{Ni}^{2+}(aq) \]
**Explanation:**
The given chemical reaction represents a redox process where cadmium ions (\(\text{Cd}^{2+}\)) in aqueous solution react with solid nickel (\(\text{Ni}\)) to produce solid cadmium (\(\text{Cd}\)) and nickel ions (\(\text{Ni}^{2+}\)) in aqueous solution.
In electrochemistry, the cell notation is used to describe the components of a galvanic (voltaic) cell in a standardized way. The notation is written as:
\[ \text{Anode} \ | \ \text{Anode Solution} \ || \ \text{Cathode Solution} \ | \ \text{Cathode} \]
For the reaction given:
- **Anode (oxidation occurs):** \(\text{Ni}(s) \rightarrow \text{Ni}^{2+}(aq) + 2e^-\)
- **Cathode (reduction occurs):** \(\text{Cd}^{2+}(aq) + 2e^- \rightarrow \text{Cd}(s)\)
Using this information, the cell notation for the reaction is:
\[ \text{Ni}(s) | \text{Ni}^{2+}(aq) || \text{Cd}^{2+}(aq) | \text{Cd}(s) \]
This notation indicates that nickel is the anode where oxidation occurs, and cadmium is the cathode where reduction happens. The double vertical lines represent the salt bridge or membrane separating the two half-cells.
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