Methanol is industrially synthesized from synthesis gas according to the following reversible reaction:
CO(g)+2H2(g)⇌CH3OH(g)ΔH=−90 kJ mol−1 \text{CO}(\text{g}) + 2\text{H}_2(\text{g}) \rightleftharpoons \text{CH}_3\text{OH}(\text{g}) \quad \Delta H = -90\text{ kJ mol}^{-1} CO(g)+2H2(g)⇌CH3OH(g)ΔH=−90 kJ mol−1A copper-based catalyst (Cu/ZnO/Al2O3\text{Cu/ZnO/Al}_2\text{O}_3Cu/ZnO/Al2O3) is employed to accelerate the process.
Which row in the table correctly describes the effect of adding this catalyst on the activation energy of the reverse reaction (Ea, reverseE_{\text{a, reverse}}Ea, reverse) and the equilibrium yield of methanol?
| Activation energy of the reverse reaction (Ea, reverseE_{\text{a, reverse}}Ea, reverse) | Equilibrium yield of methanol | |
|---|---|---|
| A | Decreases | Does not change |
| B | Decreases | Increases |
| C | Does not change | Increases |
| D | Does not change | Does not change |
Row A
Row B
Row C
Row D
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.