At $STP$,the density of air is $0.001293 \ g \ mL^{-1}$. Its vapour density 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:

Before equilibrium is set up for the chemical reaction $N_2O_{4(g)} \rightleftharpoons 2NO_{2(g)}$,the vapour density $d$ of the gaseous mixture was measured. If $D$ is the theoretical value of vapour density,the variation of $\alpha$ with $D/d$ is given by the graph. What is the value of $D/d$ at point $A$?

The vapour density of undecomposed $N_2O_4$ is $46$. When heated,the vapour density decreases to $24.5$ due to its dissociation into $NO_{2(g)}$. The percentage dissociation of $N_2O_4$ is:

The density of air is $0.00130 \, g/mL$. What will be the vapor density of air?

If $D_T$ and $D_0$ are the theoretical and observed vapour densities at a definite temperature and $\alpha$ is the degree of dissociation of a substance,then $\alpha$ in terms of $D_0, D_T$ and $n$ (number of moles of product formed from $1 \, \text{mole}$ of reactant) is calculated by the formula: