If a chemical reaction involves equal numbers of gaseous reactants and products, and the total number of moles of gas remains constant, an increase in pressure will have no effect on the equilibrium position of the reaction. This is because the reaction will follow Le Chatelier's principle, which states that a system at equilibrium will adjust to counteract any changes in its conditions.In this case, since the number of moles of gas on both sides of the reaction is equal, the change in pressure will affect both the reactants and products equally. As a result, the equilibrium position will remain unchanged, and the reaction will continue to proceed at the same rate in both the forward and reverse directions.