If you add more CO₂(g) to an equilibrium mixture of CaCO₃(s) , CaO(s) and CO₂(g) in a hot closed vessel, which way would you expect the equilibrium to shift ? CaCO₃(s)
CaO(s) + CO₂(g)

Question

If you add more CO₂(g) to an equilibrium mixture of CaCO₃(s), CaO(s) and CO₂(g) in a hot closed vessel, which way would you expect the equilibrium to shift ? CaCO₃(s) CaO(s) + CO₂(g)

Quizplus · Accepted Answer

According to Le Chatelier's principle, if more of a product is added to an equilibrium mixture, the equilibrium will shift to the side with fewer moles of gas in order to counteract the increase in pressure. In this case, adding more CO₂(g) would increase the amount of gas in the mixture, therefore the equilibrium would shift towards the reactant side to decrease the amount of gas and relieve the increased pressure.

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