The production of methanol from carbon monoxide and hydrogen is represented by the following reversible equation:
CO(g)+2H2(g)⇌CH3OH(g)ΔH=−91 kJ/mol \text{CO}(\text{g}) + 2\text{H}_2(\text{g}) \rightleftharpoons \text{CH}_3\text{OH}(\text{g}) \quad \Delta H = -91\text{ kJ/mol} CO(g)+2H2(g)⇌CH3OH(g)ΔH=−91 kJ/molAn industrial chemical plant originally carries out this synthesis using a copper-zinc catalyst under the following conditions:
Explain what effect there would be on both the rate of attainment of equilibrium and the equilibrium yield of methanol (CH3OH\text{CH}_3\text{OH}CH3OH) if the chemical plant operator changed the conditions to a higher temperature of 300 ∘C300\text{ }^\circ\text{C}300 ∘C and a lower pressure of 20 atm20\text{ atm}20 atm without changing the catalyst.
Practise Edexcel GCSE Chemistry Dynamic equilibria with exam-style questions for Foundation and Higher tier. 30 questions, matched to the Edexcel GCSE Chemistry (1CH0) specification and written in Paper 1 and Paper 2 style. Every question includes a full worked solution and mark scheme, so you can see where marks are awarded rather than just whether you got the answer right.
