At a certain temperature,the vapour density of $N_2O_4$ is $30$. Find the percentage of dissociation of $N_2O_4$ at this temperature.

The value of $K_P$ for the equilibrium reaction ${N_2}{O_4}_{(g)} \rightleftharpoons 2N{O_2}_{(g)}$ is $2$. The percentage dissociation of ${N_2}{O_4}_{(g)}$ at a pressure of $0.5 \ atm$ is

For the reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the correct relation between degree of dissociation $(\alpha)$ of $N_2O_{4(g)}$ and equilibrium constant,$K_p$ is $(P=$ total pressure of mixture $)$

$A$ gas has the formula $[CO]_x$. If its vapor density is $70$,what is the value of $x$?

The vapor density of a gas is $35.5$. What is the volume occupied by $3.55 \, g$ of this gas at $N.T.P$?

The equation $\alpha = \frac{D - d}{(n - 1)d}$ represents the degree of dissociation. For which of the following reactions is this equation valid,where $D$ is the theoretical vapour density and $d$ is the observed vapour density?