A homogeneous ideal gaseous reaction $\mathrm{AB}_{2(\mathrm{~g})} \rightleftharpoons \mathrm{A}_{(\mathrm{g})}+2 \mathrm{~B}_{(\mathrm{g})}$ is carried out in a 25 litre flask at $27^{\circ} \mathrm{C}$. The initial amount of $\mathrm{AB}_{2}$ was 1 mole and the equilibrium pressure was $1.9$ atm. The value of $K_{P}$ is $x \times 10^{-2}$. The value of $x$ is__________ .(Integer answer)
$\mathrm{AB}_{2}=\mathrm{A} \quad+\quad 2 \mathrm{~B}$
$1.9 \times 25=\mathrm{n}_{\mathrm{T}} \times 0.08206 \times 300$
$\mathrm{n}_{\mathrm{T}}=1.93=1+2 \alpha$
$\alpha=0.465$
$\mathrm{Kp}=\frac{\left(\frac{0.465}{1.93} \times 19\right)\left(\frac{0.93}{1.93} \times 1.9\right)^{2}}{\left(\frac{0.535}{1.93} \times 1.9\right)}$
$\simeq 73 \times 10^{-2} \mathrm{~atm}^{2}$