In the industrial production of sulfur trioxide, sulfur dioxide reacts with oxygen in a closed system to establish a reversible reaction:
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)Which of the following statements is correct when this reaction reaches dynamic equilibrium?
The rate of the forward reaction is greater than the rate of the reverse reaction.
The amounts of sulfur dioxide, oxygen, and sulfur trioxide remain constant.
The concentrations of all reactants and products become equal.
The forward and reverse reactions stop completely.
30 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.