Industrial ammonia synthesis follows N₂(g) + 3H₂(g) ⇌ 2NH₃(g) with ΔH negative. Which single change shifts the equilibrium toward products AND increases the value of K?

Core Concept

With ΔH negative, heat behaves as a product of the forward reaction. Removing heat by cooling shifts the balance forward to replace it, and K grows because exothermic systems gain product favorability at lower temperature. Adding nitrogen or shrinking the volume also nudges the mixture toward products, yet neither touches K, which answers to temperature alone. Only the cooled reactor achieves both effects at once.