Answer:
4.0921 is the logarithm of the equilibrium constant.
Step-by-step explanation:
; E° = - 0.41 V
; E° = 0.80 V
Iron having negative value of reduction potential .So ,that means that it will loose electron easily and get oxidized.Hence, will be at anode.
=Reduction potential of cathode - Reduction potential of anode
; E° = - 0.41 V
; E° = 0.80 V
Net reaction:
n = 2
To calculate equilibrium constant, we use the relation between Gibbs free energy, which is:
and,
Equating these two equations, we get:
where,
n = number of electrons transferred = 2
F = Faraday's constant = 96500 C
= standard electrode potential of the cell = 1.21 V
R = Gas constant = 8.314 J/K.mol
T = temperature of the reaction =
Putting values in above equation, we get:
4.0921 is the logarithm of the equilibrium constant.
