In a Victor Meyer's experiment,$0.23 \ g$ of a volatile solute displaces $112 \ mL$ of air at $NTP$. What is the vapor density of the substance?

$3.2$ moles of hydrogen iodide were heated in a sealed bulb at $444\,^{\circ}C$ till the equilibrium was reached. The degree of dissociation of $HI$ at this temperature was found to be $22\%$. The number of moles of hydrogen iodide present at equilibrium are

If the density of air at $STP$ is $0.001293 \, g \, mL^{-1}$,what will be its vapor density?

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

If the vapor density of a volatile substance relative to $CH_4$ is $4$,then find the molecular mass of that substance.

Given is a concentrated solution of a weak electrolyte $A_{x}B_{y}$ of concentration '$c$' and dissociation constant '$K$'. The degree of dissociation is given by: