The table shows the percentage yield of product at equilibrium for a reaction between gases under different conditions.
| Temperature (°C) | Pressure (atmospheres) | Yield of product (%) |
|---|---|---|
| 300 | 50 | 38 |
| 300 | 100 | 52 |
| 400 | 50 | 21 |
| 400 | 100 | 33 |
Which equation could represent this reaction?
X(g)+Y(g)⇌2Z(g)\mathrm{X(g) + Y(g) \rightleftharpoons 2Z(g)}X(g)+Y(g)⇌2Z(g), forward reaction exothermic
2X(g)+Y(g)⇌2Z(g)\mathrm{2X(g) + Y(g) \rightleftharpoons 2Z(g)}2X(g)+Y(g)⇌2Z(g), forward reaction exothermic
2X(g)+Y(g)⇌2Z(g)\mathrm{2X(g) + Y(g) \rightleftharpoons 2Z(g)}2X(g)+Y(g)⇌2Z(g), forward reaction endothermic
X(g)⇌Y(g)+Z(g)\mathrm{X(g) \rightleftharpoons Y(g) + Z(g)}X(g)⇌Y(g)+Z(g), forward reaction exothermic
47 exam-style questions on OCR GCSE Chemistry 5.3 Equilibria, covering 5.3.1 Reversible reactions and dynamic equilibrium and 5.3.2 Changing the position of equilibrium. Each one has a worked solution and a mark scheme showing where the marks go.