Chemical Equilibrium question bank (Chemistry)

$37.8 \mathrm{~g} \mathrm{~N}_2 \mathrm{O}_5$ was taken in a 1 L reaction vessel and allowed to undergo the following reaction at 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 18.65 bar. Then, $\mathrm{Kp}=$ ______ $\times 10^{-2}$ [nearest integer] Assume $\mathrm{N}_2 \mathrm{O}_5$ to behave ideally under these conditions. Given: $\mathrm{R}=0.082$ bar $\mathrm{L} \mathrm{mol}^{-1} \mathrm{~K}^{-1}$

For the given hypothetical reactions, the equilibrium constants are as follows : \(\begin{aligned} & \mathrm{X} \rightleftharpoons \mathrm{Y} ; \mathrm{K}_1=1.0 \\ & \mathrm{Y} \rightleftharpoons \mathrm{Z} ; \mathrm{K}_2=2.0 \\ & \mathrm{Z} \rightleftharpoons \mathrm{W} ; \mathrm{K}_3=4.0 \end{aligned}\) The equilibrium constant for the reaction \(\mathrm{X} \rightleftharpoons \mathrm{W}\) is