Can someone please explain this to me: If the system: CaCO3(s)CaO(s)+CO2(g) is at equilibrium, and the number of moles of CaO in the vessel is doubled, A. the reaction quotient, Q, is doubled B. the reaction quotient, Q, is halved C. the number of moles of CO2 present at equilibrium is halved D. the number of moles of CaCO3 present in the vessel increases E. The partial pressure of CO2 in the vessel remains unchanged

Question

Can someone please explain this to me:
If the system:
CaCO3(s)<>CaO(s)+CO2(g) 
is at equilibrium, and the number of moles of CaO in the vessel is doubled,
A. the reaction quotient, Q, is doubled
B. the reaction quotient, Q, is halved
C. the number of moles of CO2 present at equilibrium is halved
D. the number of moles of CaCO3 present in the vessel increases
E. The partial pressure of CO2 in the vessel remains unchanged

anonymous · Answer

sorry idk

anonymous · Answer

The answer is D. 

Le' Chatelier's Principle states that if a chemical system at equilibrium experiences a change in concentration, temperature, volume, or partial pressure, then the equilibrium shifts to counteract the imposed change and a new equilibrium is established.

Since the amount of CaO is increased, by Le' Chatelier's principle, the system will try to counter the increase in CaO by reducing the number of CaO. The equilibrium position shifts left, towards an increase in the formation of CaCO3 and a reduction in the number of Ca0.

anonymous · Answer

Thank you. I just was confused because I didn't know if it being a solid affected it or not.