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=RTnFln K

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.

92% (394 ratings)
View Complete Written Solution
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

Frequently Asked Questions

What scientific concept do you need to know in order to solve this problem?

Our tutors have indicated that to solve this problem you will need to apply the The Nernst Equation concept. You can view video lessons to learn The Nernst Equation. Or if you need more The Nernst Equation practice, you can also practice The Nernst Equation practice problems.