Questions: This chemical reaction is exothermic. High temperatures are usually not ideal for exothermic reactions. Look closely at the chemical reaction equation. Why do you think high temperatures are used in the Haber Process? What does increasing the temperature do to the reactant particles that would result in a higher product yield?

Solution Steps

The Haber Process is used to synthesize ammonia (\(\text{NH}_3\)) from nitrogen (\(\text{N}_2\)) and hydrogen (\(\text{H}_2\)) gases. The chemical equation for the reaction is: \[ \text{N}_2(g) + 3\text{H}_2(g) \rightleftharpoons 2\text{NH}_3(g) + \text{heat} \] This reaction is exothermic, meaning it releases heat.

In exothermic reactions, increasing the temperature generally shifts the equilibrium position to favor the reactants, according to Le Chatelier's Principle. This would typically reduce the yield of the product, which in this case is ammonia.

Despite the equilibrium considerations, increasing the temperature also increases the kinetic energy of the reactant particles. This results in more frequent and energetic collisions between \(\text{N}_2\) and \(\text{H}_2\) molecules, which can increase the rate of reaction.

In the Haber Process, a compromise temperature is chosen to balance the rate of reaction and the position of equilibrium. While high temperatures favor the reactants, they also significantly increase the reaction rate, leading to a higher overall yield of ammonia in a practical time frame.

Final Answer