Following reaction occurs in the given electrochemical system: [tex] Fe^{2+} + Zn [/tex] → Fe + [tex] Zn^{2+} [/tex] Thus, under standard conditions E(0) = E(0) Fe2+/Fe - E(0) Zn2+/Zn where, [tex] E^{0}Fe2+/Fe[/tex] = standard reduction potential of Fe2+/Fe = -0.44 v [tex] E^{0}Zn2+/Zn[/tex] = standard reduction potential of Zn2+/Zn = -0.763 v
E(0) = 0.323 v now, we know that, ΔG(0) =-nFE(0) ............... (1) Also, Δ[tex] G^{0} = -RTln(K) ............ (2)[/tex]
On equating and rearranging equation 1 and 2, we get K = exp( [tex] \frac{nFE(0)}{RT} [/tex] )= exp ([tex] \frac{2X96500X0.323}{8.314X298} [/tex]) = 8.46 x [tex] 10^{10} [/tex]
