The concentration of reaction products can affect the rate of a chemical reaction between X and Y according to Le Chatelier's principle and the law of mass action. Le Chatelier's principle states that if a dynamic equilibrium is disturbed by changing the conditions, the system will adjust itself to counteract the change and restore a new equilibrium. In the context of a chemical reaction, if the concentration of reaction products increases, the reaction will shift in the direction that reduces the concentration of the products, meaning the reverse reaction will be favored.The law of mass action states that the rate of a chemical reaction is proportional to the product of the concentrations of the reactants, each raised to the power of their stoichiometric coefficients. In a reversible reaction, both the forward and reverse reactions have their own rate laws. The overall rate of the reaction depends on the difference between the rates of the forward and reverse reactions.If the concentration of reaction products increases, the rate of the reverse reaction will increase according to the law of mass action. This will cause the net rate of the forward reaction X + Y products to decrease, as the reverse reaction products X + Y becomes more significant. Consequently, the rate of the chemical reaction between X and Y will be affected by the concentration of the reaction products.In summary, an increase in the concentration of reaction products will generally lead to a decrease in the rate of the forward chemical reaction between X and Y, as the system adjusts to restore equilibrium by favoring the reverse reaction.