Vapour pressure of a pure solvent at $90\,^{\circ}C$ is $1020\, torr$. $A$ solution of $0.1\, m$ concentration has a vapour pressure of $1000\, torr$. What is the molecular weight of the solvent?

$A$ mixture of ethyl alcohol and propyl alcohol has a vapour pressure of $290 \, mm$ at $300 \, K$. The vapour pressure of propyl alcohol is $200 \, mm$. If the mole fraction of ethyl alcohol is $0.6$,its vapour pressure (in $mm$) at the same temperature will be:

Find the molar mass of a nonvolatile solute when $20 \ g$ of it is dissolved in $200 \ g$ of water at $300 \ K$. [Relative lowering of vapour pressure $= 0.02$]

If the total vapour pressure of the liquid mixture $A$ and $B$ is given by the equation: $P = 180X_A + 90 \, mm \, Hg$,then the ratio of the vapour pressure of the pure liquids $A$ and $B$ is given by:

The vapour pressure of water at $20^\circ C$ is $17.5 \ mm \ Hg$. If $18 \ g$ of glucose $(C_6H_{12}O_6)$ is added to $178.2 \ g$ of water at $20^\circ C$,what will be the vapour pressure of the resulting solution (in $mm \ Hg$)?

The vapour pressure of a solvent decreases by $10 \ mm$ of $Hg$ when a non-volatile solute is added to the solvent. The mole fraction of the solute in the solution is $0.2$. What should be the mole fraction of the solvent if the decrease in the vapour pressure is to be $20 \ mm$ of $Hg$?