The table shows the percentage of ammonia in the equilibrium mixture for the Haber process under different conditions.
| Temperature / °C | 100 atm | 200 atm | 400 atm |
|---|---|---|---|
| 350 | 25 | 38 | 52 |
| 450 | 14 | 24 | 36 |
| 550 | 7 | 13 | 21 |
Statement 1: at each pressure shown, the percentage of ammonia falls as the temperature rises
Statement 2: the data show that the forward reaction is endothermic
Statement 3: starting from 450 ∘C450\,^\circ\mathrm{C}450∘C and 200 atm200\,\mathrm{atm}200atm, cooling to 350 ∘C350\,^\circ\mathrm{C}350∘C raises the percentage of ammonia more than raising the pressure to 400 atm400\,\mathrm{atm}400atm does
Which statements are correct?
1 only
1 and 3 only
2 and 3 only
1, 2 and 3
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.