The reaction of sulfur dioxide with oxygen to produce sulfur trioxide is represented by the following reversible equation:
2SO2(g)+O2(g)⇌2SO3(g)ΔH=−197 kJ/mol 2\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{SO}_3(\text{g}) \quad \Delta H = -197\text{ kJ/mol} 2SO2(g)+O2(g)⇌2SO3(g)ΔH=−197 kJ/molA chemical plant originally carries out this reaction using a vanadium(V) oxide catalyst under the following conditions:
Explain what effect there would be on both the rate of attainment of equilibrium and the equilibrium yield of sulfur trioxide (SO3\text{SO}_3SO3) if the manufacturer changed the conditions to a lower temperature of 350 ∘C350\text{ }^\circ\text{C}350 ∘C and a higher pressure of 10 atm10\text{ atm}10 atm without changing the catalyst.
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.