Vapour pressure of $CCl_{4}$ at $25\,^{\circ} C$ is $143\, mm\, Hg$. $0.5\, g$ of a non-volatile solute (mol. wt. $65$) is dissolved in $100\, mL$ of $CCl_{4}$. Find the vapour pressure of the solution. (Density of $CCl_{4} = 1.58\, g / cm^{3}$)

The vapor pressure of a mixture of $300 \ mL$ of ethyl alcohol and propyl alcohol is $290 \ mm$. The vapor pressure of propyl alcohol is $200 \ mm$. If the mole fraction of ethyl alcohol is $0.6$,what will be its vapor pressure (in $mm$) at the same temperature?

At $300 \ K$,the vapour pressure of an ideal solution containing $3 \ mol$ of $A$ and $2 \ mol$ of $B$ is $600 \ torr$. At the same temperature,if $1.5 \ mol$ of $A$ and $0.5 \ mol$ of $C$ (non-volatile) are added to this solution,the vapour pressure of the solution increases by $30 \ torr$. What is the value of $p_B^o$?

The vapour pressure of pure water is $23 \text{ mmHg}$. The vapour pressure of an aqueous solution, which contains $10$ mass per cent of solute '$A$' having molecular weight $50$ is (in $\text{ atm}$)

$3 \ g$ of urea is dissolved in $45 \ g$ of $H_2O$. The relative lowering in vapour pressure is

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 $mm \ Hg$)