If a solution is prepared using the liquids mentioned in the previous question such that the mole fraction of $A$ is $0.8$,what will be the mole fraction of $A$ in the vapor phase?

At $300 \ K$,the vapor pressures of two pure liquids $A$ and $B$ are $150 \ mm \ Hg$ and $100 \ mm \ Hg$,respectively. If the mole fractions of $A$ and $B$ in the solution are equal,then the mole fraction of $B$ in the vapor phase at the same temperature is:

At $25\,^{\circ}C$,the vapour pressure of pure liquid $A$ $(mol. wt. = 40)$ is $100\, torr$,while that of pure liquid $B$ is $40\, torr$ $(mol. wt. = 80)$. The vapour pressure at $25\,^{\circ}C$ of a solution containing $20\, g$ of each $A$ and $B$ is .......... $torr$.

$18 \ g$ of glucose $(C_6H_{12}O_6)$ is added to $178.2 \ g$ of water. The vapour pressure of water for this aqueous solution at $100^\circ C$ is ........ $Torr$.

Calculate the relative lowering of vapour pressure of a solution containing $3 \ g$ urea in $50 \ g$ water. [ Molar mass of urea $= 60 \ g \ mol^{-1} ]$

For a solution of volatile liquids,the partial vapour pressure of each component in the solution is directly proportional to: