Increasing the concentration of a reactant in a redox reaction will affect the position of the equilibrium and the concentration of products at equilibrium, but it will not change the equilibrium constant.When the concentration of a reactant is increased, the system will respond by shifting the position of the equilibrium to counteract the change, according to Le Chatelier's principle. In this case, the equilibrium will shift towards the products to consume the excess reactant. As a result, the concentration of products at equilibrium will increase, while the concentration of the reactants will decrease.However, the equilibrium constant K remains unchanged, as it is only affected by changes in temperature. The equilibrium constant is a ratio of the concentrations of products to reactants, raised to their respective stoichiometric coefficients in the balanced chemical equation. Although the concentrations of reactants and products change when the reactant concentration is increased, the ratio of their concentrations at the new equilibrium position will still be equal to the equilibrium constant.