Describe the effects of increasing the 1)Pressure 2) Temperature of the following system and what effect this will have on the equilibrium position of this reversible reaction given the forward reaction is exothermic 3H2 + N2 <--> 2NH3

Overall the closed system will behave by Le Chantelier's Principal where the equilibrium moves to minimise change.

So in the first case increasing the pressure will move the equilibrium to the right as there are fewer moles of gas on the right compared to the left. In total there are 4 moles of gas on the left and 2 on the right. So to reduce the pressure of the gas it will try and reduce the total amount of gas.

In the second case it will move to the left as the forward reaction is exothermic it will give out heat so to take in more heat it will try to reduce this change and move it to the left as the backward reaction would be endothermic.