If the vapor density of a volatile substance relative to $CH_4$ is $4$,then find the molecular mass of that substance.

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

The vapour density of a mixture containing $NO_2$ and $N_2O_4$ is $27.6$. The mole fraction of $NO_2$ in the mixture is:

$A$ mixture of $NO_2$ and $N_2O_4$ has a vapour density of $38.3$ at $300 \ K$. What is the number of moles of $NO_2$ in $100 \ g$ of the mixture?

At $444\,^oC$,the equilibrium constant $K$ for the reaction $2AB_{(g)} \rightleftharpoons A_{2(g)} + B_{2(g)}$ is $\frac{1}{64}$. The degree of dissociation of $AB$ will be .....$\%$

At $200 \, ^\circ C$,the observed vapour density $(V.D.)$ of $PCl_5$ is $60$. The degree of dissociation $(\alpha)$ of $PCl_5$ is ..........$\%$ (Given: Molar mass of $PCl_5 = 208.5 \, g/mol$).