If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction Zn(s) + Cu2+ (aq) $\rightleftharpoons$ Zn2+(aq) + Cu(s) at 300 K is approximately, (R = 8 JK$-$1mol$-$1, F = 96000 C mol$-$1)

Question

If the standard electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction

Zn(s) + Cu²⁺ (aq) $\rightleftharpoons$ Zn²⁺(aq) + Cu(s)

at 300 K is approximately,

(R = 8 JK^$-$1mol^$-$1, F = 96000 C mol^$-$1)

e^$-$80