. 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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