Consider the following system at equilibrium and its corresponding concentration equilibrium constant:
3 O₂(g) 2 O₃(g) K c = 1.8*10^{- 56} at 570 K What is the value of K p for this reaction at 570 K?

Question

Consider the following system at equilibrium and its corresponding concentration equilibrium constant:
3 O₂(g)

2 O₃(g) K c = 1.8*10^{- 56} at 570 K What is the value of K p for this reaction at 570 K?

Quizplus · Accepted Answer

The relationship between Kp and Kc for the reaction: 
aA(g) + bB(g) ⇌ cC(g) + dD(g)
is
Kp = Kc(RT)Δn
where Δn = (c + d) - (a + b) is the difference in the number of moles of gas between the products and the reactants, and R is the gas constant.
In this case, the balanced equation is:
3 O₂(g) ⇌ 2 O₃(g)
so
Δn = (2) - (3) = -1
Substituting into the equation gives:
Kp = Kc(RT)^(-1) = 1.8×10^(-56)(570 K)^(-1) = 3.85×10^(-58)
Thus, the best choice is B.

Consider the Following System at Equilibrium and Its Corresponding Concentration