Assessment and Qualifications Alliance (AQA) GCSE Biology Paper 2 Practice Exam 2025 - Free AQA GCSE Biology Practice Questions and Study Guide

In the context of the Haber process, which synthesizes ammonia from nitrogen and hydrogen, temperature plays a crucial role in determining the position of equilibrium. The reaction is exothermic, meaning it releases heat when ammonia is produced. According to Le Chatelier's principle, if a change is applied to the conditions of an equilibrium system, the system will adjust to counteract that change and restore a new equilibrium.

When the temperature is lowered, the equilibrium shifts in the direction that produces heat—in this case, towards ammonia production. Therefore, lower temperatures favor the formation of ammonia. This is because the system seeks to release heat to counteract the reduction in temperature, thus driving the reaction towards the products, which include ammonia.

Conversely, higher temperatures would shift the equilibrium towards the reactants, as the increased heat effectively moves the system in a direction that absorbs heat, opposing the temperature rise.

Therefore, lower temperatures are indeed more favorable for the production of ammonia in the Haber process, making this understanding vital for optimizing industrial applications of the process.