If the vapor pressure of a solution formed by dissolving $1 \ mol$ of a non-volatile solute in $4 \ mol$ of a solvent is $24.0 \ kPa$,what will be the vapor pressure of the pure solvent in $kPa$?

At a certain temperature,$5 \ g$ of a non-electrolyte solute is dissolved in $100 \ g$ of water. The vapour pressure of the resulting solution is $2985 \ N/m^2$,and the vapour pressure of pure water is $3000 \ N/m^2$. Calculate the molar mass of the solute.

The vapour pressure of an aqueous solution of methanol is:

Vapour pressure of a solution of benzene $(P^o_{benzene} = 120 \ torr)$ and toluene $(P^o_{toluene} = 80 \ torr)$ having $2 \ moles$ of each is ......... $torr.$

The vapour pressure of a solvent decreases by $10 \ mm \ Hg$ if the mole fraction of a non-volatile solute is $0.2$. Calculate the vapour pressure of the pure solvent. (in $mm \ Hg$)

$A$ mixture of $3.0 \ mol$ of $Na_2O$ and $1.5 \ mol$ of $KO_2$ is dissolved in $1000 \ mL$ of water. The vapour pressure of the solution in $Torr$, at $100^{\circ}C$ is: