A homogeneous ideal gaseous reaction AB_2( g ) ⇌ A_( g ) +2 B_( g ) is carried out in a 25 litre flask at 27°C. The initial amount of AB_2 was 1 mole…

A homogeneous ideal gaseous reaction $\displaystyle \mathrm{AB}_{2(\mathrm{~g})} \rightleftharpoons \mathrm{A}_{(\mathrm{g})}+2 \mathrm{~B}_{(\mathrm{g})}$ is carried out in a $\displaystyle 25$ litre flask at $\displaystyle 27$°C. The initial amount of $\displaystyle \mathrm{AB}_2$ was $\displaystyle 1$ mole and the equilibrium pressure was $\displaystyle 1.9$ atm. The value of $\displaystyle \mathrm{K}_{\mathrm{p}}$ is $\displaystyle x \times 10^{-2}$. The value of $\displaystyle x$ is \_\_\_\_. (Integer answer) $\displaystyle \left[\mathrm{R}=0.08206 \mathrm{dm}^3 \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right]$