The value of $K_p$ for the reaction,
$\mathrm{CaCO}_{3(\mathrm{~s})} \stackrel{\Delta}{\rightleftha

Question

The value of $K_p$ for the reaction, 
$\mathrm{CaCO}_{3(\mathrm{~s})} \stackrel{\Delta}{ightleftharpoons} \mathrm{CaO}_{(\mathrm{s})}+\mathrm{CO}_{2(\mathrm{~g})}$
 is $2.0 	imes 10^5 \mathrm{~Pa}$ at 1100 K . What is the pressure (in Pa ) of $\mathrm{CO}_2$ in equilibrium with $\mathrm{CaO}_{(s)}$ and $\mathrm{CaCO}_{3(s)}$ ?

Professor PC Thomas Classes · Answer

(b) : The given reaction is: 
$ \begin{aligned} & \mathrm{CaCO}_{3(\mathrm{~s})} \stackrel{\Delta}{ightleftharpoons} \mathrm{CaO}_{(\mathrm{s})}+\mathrm{CO}_{2(\mathrm{~g})} \ & K_C=\left[\mathrm{CO}_{2(\mathrm{~g})}ight]=P_{\mathrm{CO}_2} \end{aligned} $ 
Since $\left[\mathrm{CaCO}_{3(s)}ight]$ and $\left[\mathrm{CaO}_{(s)}ight]$ are both constant. 
$ 	herefore \quad P_{\mathrm{CO}_2}=2.0 	imes 10^5 \mathrm{~Pa} $