Yes, the concentration of reactants in a chemical reaction does affect the reaction yield. The relationship between the two variables can be explained using the principles of chemical equilibrium and the law of mass action.In a reversible chemical reaction, the rate of the forward reaction depends on the concentration of the reactants, while the rate of the reverse reaction depends on the concentration of the products. When the rates of the forward and reverse reactions are equal, the reaction is said to be at equilibrium.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. For a general reaction:aA + bB cC + dDThe equilibrium constant K can be expressed as:K = [C]^c [D]^d / [A]รข [B]^b where [A], [B], [C], and [D] represent the equilibrium concentrations of the respective species, and a, b, c, and d are their stoichiometric coefficients.The reaction yield is the amount of product formed at equilibrium. If the concentration of the reactants is increased, the reaction will shift towards the products to re-establish equilibrium, according to Le Chatelier's principle. This will result in a higher reaction yield. Conversely, if the concentration of the reactants is decreased, the reaction will shift towards the reactants, resulting in a lower reaction yield.However, it is important to note that the relationship between reactant concentration and reaction yield is not always linear, as it depends on the specific reaction and the stoichiometry involved. Additionally, other factors such as temperature, pressure, and the presence of catalysts can also affect the reaction yield.