The effect of increasing the concentration of product X on the reaction rate of the chemical reaction A + B -> X depends on whether the reaction is reversible or irreversible.1. If the reaction is irreversible proceeds only in the forward direction , the reaction rate will not be affected by the concentration of product X. In this case, the reaction rate depends only on the concentrations of reactants A and B.2. If the reaction is reversible can proceed in both forward and reverse directions , the reaction can be represented as A + B <-> X. In this case, increasing the concentration of product X will affect the reaction rate. According to Le Chatelier's principle, when the concentration of a product is increased, the equilibrium will shift to counteract the change, favoring the reverse reaction X -> A + B . This will result in a decrease in the forward reaction rate A + B -> X as the system tries to re-establish equilibrium.