Sulfur trioxide is manufactured during the Contact process.
The equation for the key reversible reaction is:
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)A vanadium(V) oxide catalyst is used in this reaction.
Which row correctly shows how adding the vanadium(V) oxide catalyst affects the rate of attainment of equilibrium and the equilibrium yield of sulfur trioxide (SO3\text{SO}_3SO3)?
Rate of attainment of equilibrium: decreases; Equilibrium yield of SO3\text{SO}_3SO3: increases
Rate of attainment of equilibrium: increases; Equilibrium yield of SO3\text{SO}_3SO3: does not change
Rate of attainment of equilibrium: increases; Equilibrium yield of SO3\text{SO}_3SO3: increases
Rate of attainment of equilibrium: decreases; Equilibrium yield of SO3\text{SO}_3SO3: does not change
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.