The addition of a catalyst does not affect the equilibrium position of a redox reaction between potassium permanganate and oxalic acid. A catalyst only speeds up the rate at which the reaction reaches equilibrium, but it does not change the equilibrium constant or the position of the equilibrium itself.The redox reaction between potassium permanganate KMnO4 and oxalic acid H2C2O4 can be represented as follows:2 MnO4- + 5 H2C2O4 + 6 H+ -> 2 Mn2+ + 10 CO2 + 8 H2OTo understand the effect of a catalyst on this reaction, let's first consider the concept of equilibrium. At equilibrium, the rate of the forward reaction is equal to the rate of the reverse reaction, and the concentrations of the reactants and products remain constant.The equilibrium constant K for a reaction is given by the ratio of the concentrations of the products to the concentrations of the reactants, each raised to the power of their stoichiometric coefficients:K = [Mn2+]^2 * [CO2]^10 * [H2O]^8 / [MnO4-]^2 * [H2C2O4]^5 * [H+]^6 Now let's consider the role of a catalyst. A catalyst is a substance that increases the rate of a chemical reaction by lowering the activation energy barrier without being consumed in the reaction. It does this by providing an alternative reaction pathway with a lower activation energy. Importantly, a catalyst affects both the forward and reverse reactions equally, so the equilibrium constant remains unchanged.In the case of the redox reaction between potassium permanganate and oxalic acid, adding a catalyst will speed up the rate at which the reaction reaches equilibrium, but it will not change the equilibrium position itself. The concentrations of the reactants and products at equilibrium will remain the same, as will the equilibrium constant K .In summary, the addition of a catalyst does not affect the equilibrium position of the redox reaction between potassium permanganate and oxalic acid. It only speeds up the rate at which the reaction reaches equilibrium, without changing the equilibrium constant or the position of the equilibrium itself.