AP Chem

For the following equilibrium system, which of the following changes will form more CaCO3?
CO2(g) + Ca(OH)2(s) <--> CaCO3(s) + H2O(l)
deltaH(rxn) = -113 kJ

My choices are:
a) Decrease temperature at a constant pressure (no phase change)

B) Increase volume at a constant temperature

C) Increase partial pressure of CO2

D) Remove one-half of the initial CaCO3

I was thinking that it would be A, C, and D. Is that correct?

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  1. A and C are right. Removing 1/2 CaCO3 won't affect the equilibrium AS LONG AS there is a smidgen of CaCO3 solid present. A speck must be present to attain equilibrium; more or less than that has no effect.

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  2. Is that because it's a solid and not a gas?

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