For a reaction with ΔH∘>0 and ΔS∘>0, which statement best describes how the equilibrium constant K changes as temperature is increased?
a) K decreases because the term TΔS∘ adds to ΔH∘, so ΔG∘ increases with temperature.
b) K remains less than 1 at all temperatures because both ΔH∘ and ΔS∘ are positive.
c) K increases because the free-energy term −TΔS∘ becomes more negative at higher temperatures.
d) K decreases because the term −RTΔH∘ becomes more negative as T increases.