# How does equilibrium change when the products are solid and gas?

$$\ce{CaCO3(s) <=> CaO(s) + CO2(g)}$$

How will the amount of each element change if the pressure is increased?

My guess is that the equilibrium will shift to the left, because the right side has 1 gas molecule. I know my solution contradicts with La Chateliers principles, but there is no gas on the left. So how will the the amount of the elements on the right decreased and the the solid on the left increase? Pressure has only has effect on gas.