The vapour density of $PCl_5$ at $25^{\circ}C$ is $100$. Calculate the degree of dissociation at this temperature.

Ammonium carbamate $(NH_4COONH_2)$ when heated to $200 \ ^oC$ gives a mixture of $NH_3$ and $CO_2$ with a vapour density of $26$ at equilibrium. What is the degree of dissociation of ammonium carbamate?

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:

For the reaction $2A \rightleftharpoons B + 2C$,the degree of dissociation $(x)$ in terms of vapour density is:

What is the vapor density of a mixture containing $20\%\, NO_2$ by volume and $N_2O_4$?

Consider the following gas phase dissociation, $PCl_{5(g)} \rightleftharpoons PCl_{3(g)} + Cl_{2(g)}$ with equilibrium constant $K_P$ at a particular temperature and at pressure $P$. The degree of dissociation $(\alpha)$ for $PCl_{5(g)}$ is