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6.2 Reversible reactions and dynamic equilibrium

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Question 31

Sulfur dioxide and oxygen form sulfur trioxide in a closed vessel. The forward reaction is exothermic.

2SO2(g)+O2(g)⇌2SO3(g)2\text{SO}_2\text{(g)} + \text{O}_2\text{(g)} \rightleftharpoons 2\text{SO}_3\text{(g)}2SO2​(g)+O2​(g)⇌2SO3​(g)

The mixture is allowed to reach equilibrium. The changes in parts (a) and (b) are made separately.

a.

Explain how heating the mixture causes the equilibrium amount of sulfur trioxide to decrease.

[2]
b.

The pressure inside the vessel is reduced at constant temperature. Explain why this lowers the equilibrium yield of sulfur trioxide.

[3]
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6.2 Reversible reactions and dynamic equilibrium Questions

  1. GCSE
  2. /Chemistry
  3. /6.2 Reversible reactions and dynamic equilibrium

109 exam-style questions on AQA GCSE Chemistry 6.2 Reversible reactions and dynamic equilibrium, covering 6.2.1 Reversible reactions, 6.2.2 Energy changes and reversible reactions, 6.2.3 Equilibrium, 6.2.4 The effect of changing conditions on equilibrium, 6.2.5 The effect of changing concentration, 6.2.6 The effect of temperature changes on equilibrium, and 6.2.7 The effect of pressure changes on equilibrium. Each one has a worked solution and a mark scheme showing where the marks go.

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