In the Haber process nitrogen and hydrogen react to form ammonia. The forward reaction is exothermic.
N2(g)+3H2(g)⇌2NH3(g)\mathrm{N_{2}(g)} + 3\mathrm{H_{2}(g)} \rightleftharpoons 2\mathrm{NH_{3}(g)}N2(g)+3H2(g)⇌2NH3(g)
The reaction reaches a dynamic equilibrium. State how the rate of the forward reaction compares with the rate of the backward reaction at equilibrium.
Explain the effect of increasing the pressure on the equilibrium yield of ammonia.
Explain the effect of increasing the temperature on the equilibrium yield of ammonia.
Ammonia is removed from the equilibrium mixture. Predict the effect on the position of equilibrium and explain your answer.
30 dm3\mathrm{dm^{3}}dm3 of nitrogen reacts completely with hydrogen. All volumes are measured at the same temperature and pressure. Calculate the volume of hydrogen that reacts and the volume of ammonia formed.
43 exam-style questions on Edexcel GCSE Chemistry 6.3 Dynamic equilibria, covering 6.3.1 The Haber process as a reversible reaction, 6.3.2 Conditions and rate in industrial equilibria, and 6.3.3 Fertilisers and the preparation of ammonium sulfate. Each one has a worked solution and a mark scheme showing where the marks go.