**Electrochemical Cell Problem**For the electrochemical cell:\[ 2 \text{Al}(s) + 3 \text{Mn}^{2+}(aq) \rightarrow 2 \text{Al}^{3+}(aq) + 3 \text{Mn}(s) \]- Given: - Standard cell potential (\(E^\circ\)) = 0.48 V - Concentration of \([\text{Al}^{3+}]\) = 1.0 M - Concentration of \([\text{Mn}^{2+}]\) = 0.068 M - Temperature (T) = 298 K**Objective:** Calculate the cell potential (E) under these conditions.**Note:** No graphs or diagrams are included. The problem is textual and involves electrochemical calculations using the Nernst Equation.

Nernst equation for the given reaction is : Ecell = E°cell -…

For the electrochemical cell 2 AI(s) + 3 Mn²*(aq) → 2 Al*(aq) + 3 Mn(s) (E° = 0.48 V, [AI**] = 1.0 M), what is the value of E when [ Mn2*] = 0.068 M? Assume T is 298 K

For the electrochemical cell 2 AI(s) + 3 Mn²(aq) → 2 Al(aq) + 3 Mn(s) (E° = 0.48 V, [AI**] = 1.0 M), what is the value of E when [ Mn2*] = 0.068 M? Assume T is 298 K

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

**Electrochemical Cell Problem**

For the electrochemical cell:

\[ 2 \text{Al}(s) + 3 \text{Mn}^{2+}(aq) \rightarrow 2 \text{Al}^{3+}(aq) + 3 \text{Mn}(s) \]

- Given:
- Standard cell potential (\(E^\circ\)) = 0.48 V
- Concentration of \([\text{Al}^{3+}]\) = 1.0 M
- Concentration of \([\text{Mn}^{2+}]\) = 0.068 M
- Temperature (T) = 298 K

**Objective:**

Calculate the cell potential (E) under these conditions.

**Note:** No graphs or diagrams are included. The problem is textual and involves electrochemical calculations using the Nernst Equation.

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