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6.3 Dynamic equilibria

6.3 Dynamic equilibria

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Question 15

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)⇌CH3​OH(g)ΔH=−91 kJ/mol

An industrial chemical plant originally carries out this synthesis using a copper-zinc catalyst under the following conditions:

  • temperature: 200 ∘C200\text{ }^\circ\text{C}200 ∘C
  • pressure: 100 atm100\text{ atm}100 atm

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}CH3​OH) 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.

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Markscheme

6.3 Dynamic equilibria Questions

  1. GCSE
  2. /Chemistry
  3. /6.3 Dynamic equilibria

60 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.

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