To analyze the effect on the equilibrium position of a redox reaction when the concentration of the reactants is decreased while the concentration of the products remains constant, we can use the Le Chatelier's Principle and the Nernst equation. Let's consider a generic redox reaction:aA + bB <=> cC + dDwhere A and B are reactants, C and D are products, and a, b, c, and d are their respective stoichiometric coefficients.Step 1: Write the expression for the equilibrium constant K and the reaction quotient Q K = [C]^c * [D]^d / [A]â * [B]^b Q = [C]^c * [D]^d / [A]â * [B]^b Step 2: Apply Le Chatelier's PrincipleAccording to Le Chatelier's Principle, if a change is applied to a system at equilibrium, the system will adjust itself to counteract the change and re-establish equilibrium. In this case, the concentration of the reactants A and B is decreased, so the system will shift towards the reactants to counteract the change and re-establish equilibrium.Step 3: Calculate the new reaction quotient Q' Since the concentration of the reactants is decreased, let's assume the new concentrations are [A'] and [B'].Q' = [C]^c * [D]^d / [A']â * [B']^b Step 4: Compare Q' with KIf Q' < K, the reaction will shift towards the products forward direction to re-establish equilibrium.If Q' > K, the reaction will shift towards the reactants reverse direction to re-establish equilibrium.If Q' = K, the reaction is already at equilibrium.Step 5: Analyze the effect on the equilibrium positionSince the concentration of the reactants A and B is decreased, the denominator in the Q' expression will be smaller than the denominator in the Q expression. Therefore, Q' > Q. Since the concentration of the products C and D remains constant, K remains the same. Now, since Q' > Q and Q' > K, the reaction will shift towards the reactants reverse direction to re-establish equilibrium.In conclusion, when the concentration of the reactants is decreased while the concentration of the products remains constant, the equilibrium position of a redox reaction will shift towards the reactants reverse direction to counteract the change and re-establish equilibrium.