The production of nitrogen-based fertilisers relies on ammonia synthesised via the Haber process. In this industrial process, nitrogen and hydrogen gas react reversibly in a closed vessel:
N2(g)+3H2(g)⇌2NH3(g) \text{N}_2(\text{g}) + 3\text{H}_2(\text{g}) \rightleftharpoons 2\text{NH}_3(\text{g}) N2(g)+3H2(g)⇌2NH3(g)State one of the two key features of a reaction mixture once it has achieved a state of dynamic equilibrium.
30 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.