In the equilibrium mixture CaCO3(s) ----- CaO (s) + CO2 (g) at 27 C is 2 atm - Chemistry - Equilibrium

Question

In the equilibrium mixture CaCO3(s) -----> CaO (s) + CO2 (g) at
27 °C is 2 atm What will be the pressure of CO2 when 2 moles of
CO2 are added to equilibrium mixture (Ans is 2 atm please explain
how?)

Vartika Jain · Accepted Answer

Dear Student,

CaCO3(s)     ↔    CaO(s)     +    CO2(g)Since, CaCO3 and CaO both are solids, therefore here Kp is determined by CO2 onlyKp=p(CO2)At equilibrium, Kp=2 atmAccording to Le Chatelier's Principle, when 2 moles of CO2 are added i
e
 the concentration of product is increased, then the reaction will move in backward direction in order to form more reactants but once the pressure of CO2 is 2 atm, the reaction would have reached equilibrium
 Therefore equilibrium pressure of CO2 is 2 atm

In the equilibrium mixture CaCO3(s) -----> CaO (s) + CO2 (g) at 27 °C is 2 atm. What will be the pressure of CO2 when 2 moles of CO2 are added to equilibrium mixture. (Ans is 2 atm please explain how?)