i) Write down the Equation for the Haber-Bosch process. Stating clearly the catalyst used. ii) Explain why high pressures are used for this reaction in industry iii) Explain the importance of the catalyst

i) N₂ (g) + 2H₂ (g) = 2NH_3ii) Le Chatelier’s Principle : If a dynamic equilibrium is disturbed by changing the conditions, the position of equilibrium moves to counteract the change. Pressure is a result of gas molecules hitting the side of the container, therefore a higher number of molecules results in a higher pressure. From Le Chatelier’s Principle if the pressure is increased, equilibrium will move in the direction which will counteract and reduce this pressure. There are 3 molecules of gas on the left hand side of the equation, compared to 2 molecules of gas (ammonia) on the right. Therefore, at higher pressures, equilibrium shifts in the forward direction, favouring the production of ammonia- which is the desired product.iii) Catalysts lower the activation energy of chemical reactions without undergoing chemical change themselves. They do not affect the position of equilibrium as they change the rate of reaction in both directions equally . This allows higher rate of reactions at lower temperature which is economically favourable.