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