CaCO3(s) <-> CaO(s) + CO2(g)

What would happen if CO2 was removed?
Would the reaction shift left? Does that mean CaCO3 increases and CaO and CO2 decrease ?

Keq=[CO2}

so if you remove the CO2, it tries to make more. shifts right.

This reaction is intereresting if one changes the temperature. The rightward reaction is endothermic, so think on that.

One other note, because the CaCO3 and CaO are solids they have no concentration, and are not in the expression for Keq, so adding, or removing either have no effect on equilibrium shifts.

If CO2 is removed from the reaction, according to Le Chatelier's principle, the system will try to counteract the change by shifting the equilibrium to the right to produce more CO2.

In this case, removing CO2 from the system will cause the reaction to shift to the right, towards the products side. As a result, more CaCO3 will be converted into CaO and CO2.

As the reaction shifts right, CaCO3 will decrease since it is being converted into CaO and CO2. However, CaO will increase since more of it is being formed, and CO2 will also increase as more of it is being produced.

In summary:
- CaCO3 will decrease
- CaO will increase
- CO2 will increase

In this reaction, the forward reaction is the formation of CaO and CO2 from CaCO3, while the reverse reaction is the formation of CaCO3 from CaO and CO2.

If CO2 is removed from the system, the equilibrium of the reaction will be disturbed. According to Le Chatelier's principle, when a reactant or product is removed, the reaction will shift in the direction that replenishes the removed substance.

In this case, since CO2 is a product of the reaction, its removal will cause the reaction to shift in the forward direction to produce more CO2. Consequently, the reaction will shift to the right, with CaCO3 decreasing and CaO and CO2 increasing.

To understand this, think of the reaction as a tug of war between reactants and products. If one product (CO2) is removed, it is like pulling on the reactants' side of the rope, causing the reaction to shift towards the products' side to counteract the disturbance.

It's important to note that the amount of shift will depend on the specific reaction conditions, such as temperature and pressure.