The Haber process for the production of ammonia relies on high temperatures and pressures.Which of these,high temperatures or pressures,actually reduce the yield of the reaction at equilibrium?
N₂(g) + 3H₂(g) ⇌ 2NH₃(g)
ΔH° = −92.2 kJ

Question

Quizplus · Accepted Answer

According to Le Chatelier's Principle, increasing the temperature of an endothermic reaction will shift the equilibrium position towards the right, favoring the forward reaction. Therefore, high temperatures will increase the rate of the forward reaction, but decrease the yield of the reaction at equilibrium. On the other hand, high pressures will favor the side with fewer moles of gas, which in this case is the product side. Therefore, high pressures would actually increase the yield of the reaction at equilibrium.

The Haber Process for the Production of Ammonia Relies on High