a) State Le Chatelier's Principle. (2 marks) b) Consider the following equilibrium reaction: N2(g) + 3H2(g) ⇌ 2NH3(g) ΔH = -92 kJ/mol State and explain the effect of each of the following changes on the position of equilibrium and on the yield of ammonia: i) Increasing the temperature (2 marks) ii) Increasing the pressure (2 marks) iii) Adding a catalyst (2 marks) iv) Removing ammonia as it is formed (2 marks) c) Write an expression for the equilibrium constant, Kc, for the reaction in (b) above. (1 mark) d) If the equilibrium concentrations at a certain temperature are: [N2] = 0.50 mol/dm³, [H2] = 1.50 mol/dm³, [NH3] = 2.00 mol/dm³ Calculate the value of Kc. (3 marks)