Question

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

Answer 1

Answer:

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