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6.2 Reversible reactions and dynamic equilibrium

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Question 32

Sulfur dioxide, oxygen and sulfur trioxide form an equilibrium mixture in a sealed vessel.

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 temperature remains constant as the pressure is increased. After equilibrium is restored, which statement about the amount of sulfur dioxide is correct?

[1]
A

It stays constant because sulfur dioxide and sulfur trioxide have equal coefficients

B

It decreases because higher pressure favours the side with fewer gas molecules

C

It increases because higher pressure favours the side with more gas molecules

D

It stays constant because the total number of sulfur atoms is the same on each side

Markscheme

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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