2H2(g) + O2(g) ⇌ 2H2O(g) ΔH = -ve
what happens to the equilibrium constant of the reaction above if the temperature is increased?

A.

it is unaffected

B.

it becomes zero

C.

it decrease

D.

it increase

Correct answer is C

This given equation shows the forward reaction is exothermic, which means an increase in temperature will cause the equilibrium position to shift to left to favor reactant formation, i.e K decreases