At $T \, ^\circ C$,the vapour density of $PCl_5$ is $104.25$. The degree of dissociation of $PCl_5$ 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?

If $PCl_{5(g)}$ is $40\%$ dissociated at equilibrium at $27\,^{\circ}C$ and $1\, atm$,then calculate the density of the equilibrium mixture at $27\,^{\circ}C$ and $1\, atm$ for the reaction: $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ (in $g\,L^{-1}$)

Gaseous $N_2O_4$ dissociates into gaseous $NO_2$ according to the reaction:
$N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$
At $300 \ K$ and $1 \ atm$ pressure,the degree of dissociation of $N_2O_4$ is $0.2$. If one mole of $N_2O_4$ gas is contained in a vessel,then the density of the equilibrium mixture is.......$g/L$

The vapour density of $N_2O_4$ in the equilibrium $N_2O_4 \rightleftharpoons 2NO_2$ is $40$. The degree of dissociation is:

The degree of dissociation $(\alpha)$ of $PCl_5$ obeying the equilibrium $PCl_5 \rightleftharpoons PCl_3 + Cl_2$ is related to the pressure at equilibrium by