The table shows how the percentage of product in the equilibrium mixture changes with conditions for one reversible reaction in which all substances are gases.
| Temperature / °C | Pressure / atm | Percentage of product at equilibrium |
|---|---|---|
| 600 | 10 | 32 |
| 600 | 30 | 20 |
| 800 | 10 | 64 |
| 800 | 30 | 48 |
Which reaction could it be? The energy change of each forward reaction is given.
N2(g)+O2(g)⇌2NO(g)\mathrm{N_{2}(g) + O_{2}(g) \rightleftharpoons 2NO(g)}N2(g)+O2(g)⇌2NO(g), forward reaction endothermic
2O3(g)⇌3O2(g)\mathrm{2O_{3}(g) \rightleftharpoons 3O_{2}(g)}2O3(g)⇌3O2(g), forward reaction exothermic
CH4(g)+H2O(g)⇌CO(g)+3H2(g)\mathrm{CH_{4}(g) + H_{2}O(g) \rightleftharpoons CO(g) + 3H_{2}(g)}CH4(g)+H2O(g)⇌CO(g)+3H2(g), forward reaction endothermic
2NO2(g)⇌N2O4(g)\mathrm{2NO_{2}(g) \rightleftharpoons N_{2}O_{4}(g)}2NO2(g)⇌N2O4(g), forward reaction exothermic
45 exam-style questions on Edexcel GCSE Chemistry 5.2 Reversible reactions and equilibria, covering 5.2.1 Reversible reactions and dynamic equilibrium, 5.2.2 The Haber process, and 5.2.3 Changing the position of a dynamic equilibrium. Each one has a worked solution and a mark scheme showing where the marks go.