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Ammonia, the Haber process and fertilisers

Inorganic chemistry and industrial processes · Lesson 4 of 5

Lesson 4 of 5

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Lesson 4 of 5 · Inorganic chemistry and industrial processes

Ammonia, the Haber process and fertilisers

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By the end you’ll be able to

describe the Haber process as the reversible reaction of nitrogen with hydrogen to form ammonia and write the balanced symbol equation $$\mathrm{N_2 + 3H_2 \rightleftharpoons 2NH_3}$$
explain how temperature, pressure and the iron catalyst affect the rate and equilibrium position in the Haber process and justify the use of compromise industrial conditions

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describe ammonia as a feedstock for fertiliser production and identify fertilisers that supply nitrogen, phosphorus and potassium to improve plant growth

describe how ammonium salts are produced by reacting ammonia with acids and apply this to named examples such as ammonium sulfate or ammonium nitrate

evaluate the benefits of fertiliser use for crop yield against environmental issues such as eutrophication or energy use in manufacture

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