If the student adds more N2 reactant to the reaction mixture, the equilibrium position will shift to the right, favoring the formation of NH3 product . This is in accordance with Le Chatelier's principle, which states that if a stress is applied to a system at equilibrium, the system will adjust to counteract the stress and re-establish equilibrium. In this case, the stress is the increased concentration of N2, and the system will respond by consuming more N2 and producing more NH3.On the other hand, if the student adds more NH3 product to the reaction mixture, the equilibrium position will shift to the left, favoring the formation of N2 and H2 reactants . This is also in accordance with Le Chatelier's principle, as the stress is the increased concentration of NH3, and the system will respond by consuming more NH3 and producing more N2 and H2.However, it is important to note that the equilibrium constant Kc for the reaction will not be affected by these changes in concentration. The equilibrium constant is a characteristic of the reaction and depends only on temperature. While the equilibrium position may shift in response to changes in concentration, the value of Kc remains constant.