. The cell in which the following reaction occurs
2Fe3+ (aq) + 2I- (aq) → 2Fe3+ (aq) + I2 (s) has Ecell = 0.236 V at 298 K.
Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction.
Best Answer
Explanation:
Eº= 0.236 V
T = 293 k
We know that G =- nFEº
F = 96500
n = 2 (no. of electron)
ΔG = -2965000.236 = -45.548kJ
From nernst equation
Ecell = Eº- 0.591/n logk
Ecell = 0 (at equilibrium)
Logk = nEº/0.591= 2×0.236/0.591
Logk = 7.98
K = 107.98= 9.616 ×107
Final Answer:
Hence standard Gibbs energy = -45.548kJ & equilibrium constant of the cell reaction K = 9.616 107.
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