Factors affecting Kp (pressure constant)
If there is a high gas pressure in the environment the reaction is taking place in, $K_\mathrm{p}$ will shift towards the side of the reaction that has fewer gas molecules, as it is "fighting against" the high pressure, in a way. So in your case, since only one side has gas (the product side) if you increase the pressure of $\ce{CO2}$ or any other gas, the equilibrium will shift towards the reactant side.