Enter your answer in the provided box. What is the potential of a cell made up of Zn / Zn2+ and Cu / Cu²+ half-cells at 25°C if [Zn²*] = 0.31 M and [Cu2*] = 0.41 M ? V
Enter your answer in the provided box. What is the potential of a cell made up of Zn / Zn2+ and Cu / Cu²+ half-cells at 25°C if [Zn²*] = 0.31 M and [Cu2*] = 0.41 M ? V
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:**
Enter your answer in the provided box.
What is the potential of a cell made up of Zn/Zn²⁺ and Cu/Cu²⁺ half-cells at 25°C if \([Zn^{2+}] = 0.31 \, M\) and \([Cu^{2+}] = 0.41 \, M\)?
[Input Box] V
**Instructions for Solving:**
To find the potential of the cell, use the Nernst equation:
\[
E = E^\circ - \frac{0.0592}{n} \log \frac{[Zn^{2+}]}{[Cu^{2+}]}
\]
**Given:**
- Standard reduction potentials (\(E^\circ\)):
- \(E^\circ_{Zn^{2+}/Zn} = -0.76 \, V\)
- \(E^\circ_{Cu^{2+}/Cu} = +0.34 \, V\)
- Concentrations:
- \([Zn^{2+}] = 0.31 \, M\)
- \([Cu^{2+}] = 0.41 \, M\)
- Temperature: \(25^\circ C\)
- Number of electrons (\(n\)): 2
Collect these values and substitute them into the Nernst equation to calculate the cell potential.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F6b9a5e3a-13c3-426b-8948-52c1d49e3a86%2Ff2c88d4f-fadb-47c1-ab03-4d2b1edcf633%2Fz66ugxp_processed.png&w=3840&q=75)
Transcribed Image Text:**Question:**
Enter your answer in the provided box.
What is the potential of a cell made up of Zn/Zn²⁺ and Cu/Cu²⁺ half-cells at 25°C if \([Zn^{2+}] = 0.31 \, M\) and \([Cu^{2+}] = 0.41 \, M\)?
[Input Box] V
**Instructions for Solving:**
To find the potential of the cell, use the Nernst equation:
\[
E = E^\circ - \frac{0.0592}{n} \log \frac{[Zn^{2+}]}{[Cu^{2+}]}
\]
**Given:**
- Standard reduction potentials (\(E^\circ\)):
- \(E^\circ_{Zn^{2+}/Zn} = -0.76 \, V\)
- \(E^\circ_{Cu^{2+}/Cu} = +0.34 \, V\)
- Concentrations:
- \([Zn^{2+}] = 0.31 \, M\)
- \([Cu^{2+}] = 0.41 \, M\)
- Temperature: \(25^\circ C\)
- Number of electrons (\(n\)): 2
Collect these values and substitute them into the Nernst equation to calculate the cell potential.
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