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.
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
3. 6:52 x 1079
4. 1:84 x 102
5. 1:44 x 102
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