Adding a catalyst to a reaction does not affect the equilibrium position of the reaction. A catalyst works by lowering the activation energy of the reaction, which speeds up the rate at which the reaction reaches equilibrium. However, the equilibrium constant Kp remains the same, as it is only dependent on the temperature and the nature of the reactants and products.To calculate the equilibrium constant Kp of the reaction at 298 K, we would need the standard Gibbs free energy change G for the reaction. Unfortunately, the given information is not sufficient to calculate the equilibrium constant Kp directly. However, we can still discuss the effect of a catalyst on the equilibrium position.In the presence of a catalyst, the reaction will reach equilibrium faster, but the position of equilibrium will remain the same. This is because the catalyst affects both the forward and reverse reactions equally, allowing them to reach equilibrium more quickly without changing the equilibrium constant Kp .In conclusion, the presence of a catalyst will not affect the position of equilibrium for the redox reaction between iron III oxide and carbon monoxide. The equilibrium constant Kp will remain the same, and the reaction will simply reach equilibrium more quickly due to the lowered activation energy provided by the catalyst.