According to Le Chatelier's principle, if a change is applied to a system at equilibrium, the system will adjust itself to counteract the change and restore a new equilibrium. In the case of the reaction between nitrogen gas N and hydrogen gas H to form ammonia gas NH , the balanced chemical equation is:N g + 3H g 2NH g When the pressure of the system is increased, the equilibrium will shift to counteract this change. In this case, the equilibrium will shift towards the side with fewer moles of gas, as this will help to reduce the pressure. In the reaction above, there are 4 moles of gas on the reactants side 1 mole of N and 3 moles of H and 2 moles of gas on the product side 2 moles of NH .Therefore, when the pressure is increased, the equilibrium will shift towards the side with fewer moles of gas, which is the side with ammonia gas NH . As a result, the yield of ammonia gas will increase.In summary, increasing the pressure of the system will cause the equilibrium to shift towards the side with fewer moles of gas, which in this case is the ammonia gas NH . This will lead to an increase in the yield of ammonia gas, as predicted by Le Chatelier's principle.