Phosphine decomposes at $300 \ K$ and $3 \ atm$ as
$4PH_{3(g)} \rightleftharpoons P_{4(g)} + 6H_{2(g)}$
Calculate the vapour density of phosphine if it dissociates to the extent of $30 \%$.

The vapor density of a gas is $16$. If the ratio of specific heat at constant pressure to specific heat at constant volume is $1.4$,find its atomic weight.

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?

$0.1 \ mol$ of $H_2S_{(g)}$ is kept in a $0.4 \ L$ vessel at $1000 \ K$. For the reaction $2 H_2S_{(g)} \rightleftharpoons 2 H_{2(g)} + S_{2(g)}$,$K_c = 10^{-6}$. The percentage dissociation of $H_2S$ is.......$\%$

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 $g\,L^{-1}$)

In a $Victor \ Meyer$ experiment,$0.23 \ g$ of a volatile substance displaces $112 \ mL$ of air at $STP$. Calculate the vapor density of the substance.