Answer:
4.0921 reflects the logarithm of the equilibrium constant.
Step-by-step explanation:
; E° = - 0.41 V
; E° = 0.80 V
Iron has a negative reduction potential, indicating its tendency to lose electrons and undergo oxidation, and thus it will be at the anode.
=Reduction potential of cathode - Reduction potential of anode
; E° = - 0.41 V
; E° = 0.80 V
Net reaction:
n = 2
To determine the equilibrium constant, we utilize the correlation with Gibbs free energy, as follows:
and,
Aligning these two equations yields:
where,
n = 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 = reaction temperature =
Substituting values into the equation, we arrive at:
4.0921 represents the logarithm of the equilibrium constant.
