The reaction between nitrogen gas N2 and hydrogen gas H2 to produce ammonia gas NH3 is a reversible reaction and can be represented by the following equation:N2 g + 3H2 g 2NH3 g This reaction is governed by Le Chatelier's principle, which states that if a system at equilibrium is subjected to a change in pressure, temperature, or concentration of reactants or products, the system will adjust to counteract the change and restore equilibrium.In this case, increasing the pressure of the system will shift the equilibrium position to favor the side with fewer moles of gas. Since there are 4 moles of gas on the reactant side 1 mole of N2 and 3 moles of H2 and only 2 moles of gas on the product side 2 moles of NH3 , increasing the pressure will shift the equilibrium to the right, favoring the formation of ammonia.As a result, the reaction rate of nitrogen and hydrogen gases to produce ammonia will increase as the pressure is increased, given that the temperature and the amount of catalyst remain constant. Conversely, if the pressure is decreased, the reaction rate will decrease, and the equilibrium will shift to the left, favoring the dissociation of ammonia back into nitrogen and hydrogen gases.