Changing the concentration of reactants in a chemical reaction can significantly affect the conversion of reactants into products. According to Le Chatelier's principle, if a system at equilibrium is subjected to a change in concentration, temperature, or pressure, the system will adjust to counteract the change and restore a new equilibrium.When the concentration of reactants is increased, the reaction will shift towards the products to re-establish equilibrium. This means that the rate of the forward reaction will increase, leading to a higher conversion of reactants into products. Conversely, if the concentration of reactants is decreased, the reaction will shift towards the reactants, decreasing the conversion of reactants into products.It is important to note that the effect of changing the concentration of reactants on the conversion of reactants into products depends on the reaction order. For a first-order reaction, the reaction rate is directly proportional to the concentration of the reactant. In this case, increasing the concentration of the reactant will lead to a faster reaction rate and a higher conversion of reactants into products. For a zero-order reaction, the reaction rate is independent of the concentration of the reactant, so changing the concentration will not affect the conversion of reactants into products.In summary, changing the concentration of reactants can affect the conversion of reactants into products by altering the reaction rate and shifting the equilibrium position. The extent of this effect depends on the reaction order and the specific reaction conditions.