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

What is the vapour density of $O_2$ gas?

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 dissociation equilibrium of a gas $AB_{2}$ can be represented as:
$2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$
The degree of dissociation is $x$ and is small compared to $1$. The expression relating the degree of dissociation $(x)$ with equilibrium constant $K_P$ and total pressure $P$ is:

The vapor density of a gas is $11.2$. At $N.T.P.$,$11.2 \ g$ of this gas occupies a volume of ............. $litres$.

At $NTP$,$5.6 \ L$ of a gas weighs $8 \ g$. The vapour density of the gas is: