a) Distinguish between a reversible reaction and an irreversible reaction, giving one example of each. (4 marks) b) For the gaseous equilibrium: 2SO2(g) + O2(g) ⇌ 2SO3(g) ΔH = -196 kJ/mol i) Write the expression for the equilibrium constant, Kp, for this reaction. (2 marks) ii) State what happens to the value of Kp when: I. The temperature is increased (1 mark) II. The pressure is increased (1 mark) III. A catalyst of vanadium(V) oxide is added (1 mark) c) At a certain temperature, the equilibrium partial pressures are: P(SO2) = 0.40 atm, P(O2) = 0.20 atm, P(SO3) = 0.80 atm Calculate the value of Kp and state its units. (4 marks) d) State TWO industrial conditions used in the Contact Process for the manufacture of sulphuric acid, and give a reason for each condition chosen. (3 marks)