Can you mark my answer for Q8 on this paper:
Link to the paperMark Scheme LinkMy Answer:As the pressure is increased, the percentage of ammonia yielded increases. For example, at a pressure of 1 atmospheres, the percentage yield was 0.2%, whereas at 50 atmospheres, the percentage yield had increased to 9.5%. This is because increasing the pressure causes a greater likelihood of particle collisions and, thus, shifts the position of equilibrium to the right, in favour of the forward reaction.
On the other hand, as the temperature is increased, the percentage of ammonia yielded decreases. For example, at a temperature of 400 degrees celsius, the percentage yield was 50%, whereas at 550 degrees celsius, the percentage yield decreased to 17%. This is because increasing the temperature moves the position of the equilibrium in the direction of the endothermic reaction. In this case, the forward reaction is exothermic and therefore the backward reaction will be endothermic. In the endothermic reaction, the products are on the left hand side so the equilibrium will move to the left.
Questions:I don't really understand why the equilibrium moves in the direction of the endothermic reaction when the temperature is increased - why not in the direction of the exothermic reaction?
Also, if I added this to my answer to the question, would it be incorrect or unnecessary?
As the temperature is increased, the percentage yield of ammonia decreases - so less products is made. This means that the equilibriumwill move to the left as the concentration of the reactants will be higher than the concentration of theproducts.