The equilibrium position of the reaction N2 g + 3H2 g 2NH3 g will shift in response to an increase in pressure according to Le Chatelier's principle. This principle states that if a system at equilibrium is subjected to a change in pressure, temperature, or concentration of reactants and products, the system will adjust the equilibrium position to counteract the change.In this case, an increase in pressure will cause the equilibrium to shift in the direction that reduces the number of moles of gas particles. In the given reaction, there are 4 moles of gas on the reactant side 1 mole of N2 and 3 moles of H2 and 2 moles of gas on the product side 2 moles of NH3 . Since the product side has fewer moles of gas, the equilibrium will shift to the right, favoring the formation of NH3. This means that more N2 and H2 will react to form NH3, counteracting the increase in pressure.