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6.3 Dynamic equilibria

6.3 Dynamic equilibria

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Question 13

In the industrial synthesis of methanol, carbon monoxide gas is reacted with hydrogen gas in a reversible reaction:

CO(g)+2H2(g)⇌CH3OH(g) \text{CO}(\text{g}) + 2\text{H}_2(\text{g}) \rightleftharpoons \text{CH}_3\text{OH}(\text{g}) CO(g)+2H2​(g)⇌CH3​OH(g)

The forward reaction is exothermic (releases heat energy).

The industrial conditions chosen for this synthesis are:

  • using excess hydrogen gas, rather than the exact 1:2 stoichiometric ratio
  • a pressure of 50 atm, rather than atmospheric pressure (1 atm)
  • a temperature of 250 °C, rather than room temperature.

Explain the effect of each of these chosen conditions on the equilibrium yield of methanol (CH3OH\text{CH}_3\text{OH}CH3​OH) and on the rate of reaching equilibrium.

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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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