Question

The chemical reaction which occurs during the Haber process is:
Nitrogen + Hydrogen Ammonia
N2(g) + 3H2(g) 2NH3(g)
Use Le Chatelier’s principle to explain what would happen if you raised the
temperature of this reaction.

Answer 1

According to Le Chatelier's principle, if you increase the temperature of a chemical reaction that involves gases, the equilibrium will shift in the direction that consumes heat. In the case of the Haber process, the forward reaction (N2 + 3H2 → 2NH3) is exothermic, meaning it releases heat. Therefore, raising the temperature would shift the equilibrium towards the reactants (N2 and H2) in an attempt to consume the excess heat. This would result in a decrease in the yield of ammonia and a lower conversion rate of the reactants to products. In industrial applications of the Haber process, the temperature is typically maintained at around 450°C to achieve a good balance of equilibrium yield and reaction rate.