What is the equilibrium constant for the following reaction at 25°C?

Mg (s) + Zn2 + (aq) = Mg2 + (aq) + Zn (s)

2.45*10^54

Explanation:

Mg (s) + Zn2 + (aq) = Mg2 + (aq) + Zn (s)

From the equation;

n = 2 moles of electrons

E°anode = - 2.37 V

E°cathode = - 0.76 V

From E°Cell = E°cathode - E°anode

E°Cell = - 0.76 - (-2.37) = 1.61 V

Recall that E°cell = 0.0592/n log K

1.61 = 0.0592/2 log K

log K = 1.61/0.0296

K = Antilog (54.39)

K = 2.45*10^54