The degree of dissociation of a weak acid is $7.2 \times 10^{-4}$. What is the value of its percent dissociation in a $0.025 \ M$ solution (in $\%$)?

Ammonium carbamate $(NH_2COONH_4)$ when heated to $200\,^{\circ}C$ gives a mixture of $NH_3$ and $CO_2$ with a vapour density of $13.0$ at equilibrium. What is the degree of dissociation of ammonium carbamate?

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

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

At temperature $T$,a compound $AB_{2(g)}$ dissociates according to the reaction $2AB_{2(g)} \rightleftharpoons 2AB_{(g)} + B_{2(g)}$ with a degree of dissociation $x$,which is very small compared to unity. The value of $x$ is:

$2SO_3 \rightleftharpoons 2SO_2 + O_2$. Initially,$3$ moles of $SO_3$ were heated. If the degree of dissociation of $SO_3$ is $40\%$,find the total number of moles at equilibrium.