Question

Consider the two gaseous equilibria: so2(g) 1/2o2(g) ↔ so3(g) k1 2so3(g) ↔ 2so2(g) o2(g) k2 the values of the equilibrium constants k1 and k2 are related by

a) k2 = 1/k12
b) k2 = 1/k1
c) k2 = k12
d) none of the above.
e) k22 = k1

Answer 1

The equilibrium constant K2 for the reverse reaction is the inverse of K1, so the relationship between the two equilibrium constants is K2 = 1/K1. So, the correct option is B.

Step-by-step explanation:

The equilibrium constants for the given reactions SO2(g) + 1/2O2(g) ↔ SO3(g) with K1 and 2SO3(g) ↔ 2SO2(g) + O2(g) with K2 are related in such a way due to the principle of microscopic reversibility. Essentially, the reverse reaction's equilibrium constant is the inverse of the forward reaction when coefficients are considered. Since the second reaction is directly the reverse of the first, with coefficients doubled, the relationship between K1 and K2 is K2 = 1/K1.