# Problem: What is the equilibrium constant for the reaction taking place at room temperature (T = 25°C) in the battery Zn(s) I Zn2+(aq) II Ce4+(aq) I Ce3+(aq) ? Assume that the number of electrons transferred in the reaction is n = 2.Zn2+ + 2 e- → Zn                 E°red = -0.76 VCe4+ + e- → Ce3+                 E°red = +1.61 V1. 1:33 x 10802. 2.373. 6:52 x 10794. 1:84 x 1025. 1:44 x 102

###### FREE Expert Solution

We are asked to calculate for the equilibrium constant for the reaction

Recall that the Nernst Equation relates the concentrations of compounds and cell potential.

E°cell = cell potential, V
R = gas constant = 8.314 J/(mol
·K)
T = temperature, K
n = mole e- transferred
F = Faraday’s constant, 96485 C/mol e-
K = equilibrium constant

We're going to calculate for the equilibrium constant using the following steps:

Step 1: Identify the anode and the cathode in the reaction.
Step 2:
Calculate the cell potential of the reaction.
Step 3:
Calculate the equilibrium constant (K) using the Nernst Equation.

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###### Problem Details

What is the equilibrium constant for the reaction taking place at room temperature (T = 25°C) in the battery Zn(s) I Zn2+(aq) II Ce4+(aq) I Ce3+(aq) ? Assume that the number of electrons transferred in the reaction is n = 2.
Zn2+ + 2 e- → Zn                 E°red = -0.76 V
Ce4+ + e- → Ce3+                 E°red = +1.61 V

1. 1:33 x 1080

2. 2.37

3. 6:52 x 1079

4. 1:84 x 102

5. 1:44 x 102