Adding a catalyst to a chemical reaction does not affect the equilibrium position of the reaction. A catalyst works by lowering the activation energy of the reaction, which increases the rate at which the reaction proceeds. However, it does not change the thermodynamics of the reaction, meaning that the equilibrium constant K remains the same.In the redox reaction between potassium permanganate KMnO4 and oxalic acid H2C2O4 , the balanced equation is:2 KMnO4 + 5 H2C2O4 + 3 H2SO4 K2SO4 + 2 MnSO4 + 10 CO2 + 8 H2OAt equilibrium, the reaction quotient Q is equal to the equilibrium constant K . Adding a catalyst will not change the value of K, so the equilibrium position will remain the same.To further illustrate this, let's consider the reaction at equilibrium:aA + bB cC + dDThe equilibrium constant K is given by:K = [C]^c * [D]^d / [A]â * [B]^b where [A], [B], [C], and [D] are the equilibrium concentrations of the respective species, and a, b, c, and d are their stoichiometric coefficients.Since adding a catalyst does not change the value of K, the equilibrium concentrations of the reactants and products will remain the same. The only difference is that the reaction will reach equilibrium faster due to the presence of the catalyst.In conclusion, adding a catalyst to the redox reaction between potassium permanganate and oxalic acid will not affect the equilibrium position of the reaction. It will only increase the rate at which the reaction reaches equilibrium.