What will happen to the ratio of partial pressure of PCl5 to partial pressure of Cl2 as the temperature is raised?

Question

Consider the following system at equilibrium at 25°C: PCl₃(g) + Cl₂(g) <=> PCl₅(g) for which ∆G° = -92.50 kJ. 

The answer is decreases, but I would like to know why?

Answer 1

PCl₃(g) + Cl₂(g) <==> PCl₅(g)

K = (PCl₅) / (PCl₃)(Cl₂)

∆G = ∆Gº + RT ln K

At equilibrium ∆G = 0, therefor

∆Gº = -RT ln K

-92.50 = -RT ln K

What happens to ln K as T is raised

92.50 / RT = ln K

So as T is raised, the value of ln K gets smaller and since K is (PCl3)(Cl2) / (PCl5), this ratio gets smaller or decreases. Does that help explain it?