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 $\%$)?

The vapour density of a gas is $11.2$. The volume occupied by $11.2 \ g$ of the gas at $STP$ will be.....$L$

At temperature $T$,compound $AB_{2(g)}$ dissociates as $AB_{2(g)} \rightleftharpoons AB_{(g)} + \frac{1}{2} B_{2(g)}$ having degree of dissociation $x$ (small compared to unity). The correct expression for $x$ in terms of $K_p$ and $p$ is

For the reaction $PCl_5 \rightleftharpoons PCl_3 + Cl_2$,the degree of dissociation is inversely proportional to the square root of the system pressure. Assuming constant temperature,if the volume of the system increases to $16$ times its initial volume,the degree of dissociation becomes ....... times.

$AB_{3(g)}$ dissociates as:
$AB_{3(g)} \rightleftharpoons AB_{2(g)} + \frac{1}{2} B_{2(g)}$. When the initial pressure of $AB_3$ is $800 \ torr$ and the total pressure developed at equilibrium is $900 \ torr$,what percentage of $AB_{3(g)}$ is dissociated?

For the equations $(i) \ HCN + CCl_4 \rightarrow \alpha_1$ and $(ii) \ HCN + C_6H_6 \rightarrow \alpha_2$,which degree of dissociation is greater,$\alpha_1$ or $\alpha_2$?