GCSE Chemistry (AQA)

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The Haber Process: Equilibrium

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Using resources The Haber process and the use of NPK fertilisers

The Haber Process: Equilibrium

11:05 The Haber Process
Spec 4.10.4.1
Previous The Haber Process Next Reversible Reactions
  • Principles of dynamic equilibrium apply to the Haber process.
  • The Haber process produces ammonia from nitrogen and hydrogen.
  • The reaction is reversible; ammonia can break down back into nitrogen and hydrogen.
  • Changing temperature and pressure affects ammonia yield and production rate.
  • Commercial production of ammonia aims to maximize profits due to high demand in agriculture.
  • Increasing pressure increases ammonia yield at a constant temperature by shifting equilibrium to the side with fewer gas molecules.
  • The Haber process uses a pressure of 200 atmospheres as a compromise between yield and cost.
  • Higher pressures increase yield but require expensive equipment and energy.
  • Increasing temperature decreases ammonia yield at a given pressure by shifting equilibrium in the endothermic direction.
  • The Haber process uses a temperature of 450 degrees Celsius as a compromise between yield, rate, and cost.
  • Lower temperatures increase yield but slow down production.
  • An iron catalyst is used to increase reaction rate without affecting equilibrium position or yield.
  • Raw material costs, such as purified hydrogen and nitrogen, are significant in ammonia production.
  • Unreacted nitrogen and hydrogen are recycled to reduce costs and waste.

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