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.

Vapour density of a gas is $5.6$,volume of $5.6 \ g$ of it at $STP$ is ............... $L$

Consider the following reaction in a sealed vessel at equilibrium with concentrations of $N_2 = 3.0 \times 10^{-3} \ M$,$O_2 = 4.2 \times 10^{-3} \ M$,and $NO = 2.8 \times 10^{-3} \ M$.
$2 \ NO_{(g)} \rightleftharpoons N_{2_{(g)}} + O_{2_{(g)}}$
If $0.1 \ mol \ L^{-1}$ of $NO_{(g)}$ is taken in a closed vessel,what will be the degree of dissociation $(\alpha)$ of $NO_{(g)}$ at equilibrium?

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

$3.2 \text{ moles of hydrogen iodide are heated in a closed vessel at } 444^{\circ}C \text{ until equilibrium is reached. If the degree of dissociation at this temperature is } 22\%, \text{ then the number of moles of hydrogen iodide remaining at equilibrium will be:}$

The vapour density of completely dissociated $NH_4Cl$ would be