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Haber Process

  • Balanced equation:
    • N2(g) + 3H2(g) (reversible) 2NH3(g)
  • Reaction is reversible and forms an equilibrium between reactants and products

  • Ammonia is crucial for the production of fertilisers which support global argiculture
  • Its also used in the production of:
    • Explosives
    • Pharmaceuticals
    • Textiles
    • Cleaning products

  • Raw materials for this process are both gases, and whilst nitrogen can be collected from the air, hydrogen isnt so easy to source
  • Feedstock: Methane (CH4) is currently the most common source of hydrogen
  • Natural gas is used because:
    • Abundant
    • Cost effective

Conditions for the Haber Process

  • 450oC (temperature)
  • 200 atm (pressure)
  • Iron (Fe) catalyst

  • Ammonia is cooled, condensed and collected reguarly
  • This pushes the equilibrium towards more ammonia production, maimising yield