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Haber Process

Haber Process. Making of ammonia from its elements. Uses of Ammonia. Fertilisers , fibers, plastics, nitric acid (explosives), household cleaners, detergents. N 2 and H 2. Ammonia. Chemical monitoring. Equilibrium. To produce ammonia:

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Haber Process

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  1. Haber Process Making of ammonia from its elements

  2. Uses of Ammonia Fertilisers, fibers, plastics, nitric acid (explosives), household cleaners, detergents

  3. N2 and H2 Ammonia Chemical monitoring

  4. Equilibrium To produce ammonia: Increase pressure (it will tend to decrease the number of moles of gas) Decrease temperature (it will tend to increase temperature)

  5. Increasing pressure increases the frequency of successful collisions • Compromise: Construction of strong pipes to maintain high pressures is not economical. Pressure needs to be lessened Pressure

  6. Lower temperature produces the highest yield of ammonia (~90%) but at a very slow rate (months!) as there is insufficient kinetic energy for a collision • Compromise: Use slightly higher temperatures to yield smaller amounts quickly. Temperature

  7. Catalysts speed the forward and reverse reaction. • It does not change the position of equilibrium • Compromise: A catalyst makes it possible to use lower temperatures Catalyst

  8. Magnetite Catalyst (Fe3O4)

  9. Conditions: Increase reactants (but must maintain 1:3 ratio) Pressure: 25 MPa (25,000 Pa) Temperature: 400oC Magnetite Catalyst Product is removed

  10. Yield of ammonia: ~15–20% per cycle. After 5–6 cycles about 98% of the reactants are converted to ammonia.

  11. Sources of H2 and N2

  12. Why Monitor? Efficiency and safety

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