Increasing the pressure on a reaction where the number of moles of gas increases will cause the equilibrium position to shift towards the side with fewer moles of gas. This can be explained using Le Chatelier's principle, which states that when a system at equilibrium is subjected to a change in pressure, temperature, or concentration of reactants and products, the system will adjust its equilibrium position to counteract the change.In this case, when the pressure is increased, the system will try to counteract the change by reducing the pressure. Since the side with fewer moles of gas has a lower pressure, the equilibrium will shift towards that side to minimize the effect of the increased pressure. This will result in the consumption of more reactants and the formation of fewer products with more moles of gas, ultimately leading to a new equilibrium position.