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 $\%$)?

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

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

If the density of a gas at $NTP$ is $0.00445 \ g/mL$,then its vapor density and molecular weight are respectively:

$AB_{3(g)}$ 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?

Total number of moles for the reaction $2HI \rightleftharpoons H_2 + I_2$ at equilibrium,if $\alpha$ is the degree of dissociation,is: