37.8 g N_2 O_5 was taken in a 1 L reaction vessel and allowed to undergo the following reaction at 500 K 2 N_2 O_5( g ) ⇌ 2 N_2 O_4( g ) + O_2( g )…

$\displaystyle 37.8 \mathrm{~g} \mathrm{~N}_2 \mathrm{O}_5$ was taken in a $\displaystyle 1$ L reaction vessel and allowed to undergo the following reaction at $\displaystyle 500$ K $$2 \mathrm{~N}_2 \mathrm{O}_{5(\mathrm{~g})} \rightleftharpoons 2 \mathrm{~N}_2 \mathrm{O}_{4(\mathrm{~g})}+\mathrm{O}_{2(\mathrm{~g})} $$ The total pressure at equilibrium was found to be $\displaystyle 18.65$ bar. Then, $\displaystyle \mathrm{Kp}=$ $\displaystyle \_\_\_\_$ $\displaystyle \times 10^{-2}$ [nearest integer]Assume $\displaystyle \mathrm{N}_2 \mathrm{O}_5$ to behave ideally under these conditions. Given: $\displaystyle \mathrm{R}=0.082$ bar $\displaystyle \mathrm{L} \mathrm{mol}^{-1} \mathrm{~K}^{-1}$