The process ${\mathrm{CaCO}}_3\rightleftharpoons \mathrm{CaO}+{\mathrm{CO}}_2$ attains equilibrium in 11.2 lit. vessel at 1092 K and 2 atm. Now, initial number of moles of CaCO₃ cannot be.

The equation at its equilibrium,

CaCO_3​⇋CaO+CO_2​

K_P​=${\mathrm{P}}_{{\mathrm{CO}}_2}$

${\mathrm{P}}_{{\mathrm{CO}}_2}$=5 atm

Equilibrium constant is same.

 The moles of CO2​,

 nCO2​​=PV/RT​=2×11.2​/0.082×1092=0.25=1/4

 At equilibrium moles of CaCO₂​ = Moles ofCO2​

 The initial moles of CaCO3​ =1/4