The vapour pressure of pure benzene and toluene are $0.9 \ Bar$ and $0.85 \ Bar$ respectively. Calculate the vapour pressure of the solution prepared by dissolving $7.8 \ g$ of benzene in $180 \ g$ of toluene. (in $Bar$)

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 $20\,^{\circ}C,$ the vapour pressure of the resulting solution will be $.........\, mm$ of $Hg$.

If $Raoult's$ law is obeyed,the vapor pressure of the solvent in a solution is proportional to which of the following?

How many grams of glucose are required to prepare an aqueous solution of glucose having a vapor pressure of $23.324 \ mm \ Hg$ at $25^{\circ} C$ in $100 \ g$ of water? The vapor pressure of pure water at $25^{\circ} C$ is $23.8 \ mm \ Hg$.

At $50^{\circ} C$, the vapour pressure of pure benzene is $268 \ torr$. The number of moles of non-volatile solute per mole of benzene required to prepare a solution having a vapour pressure of $167 \ torr$ at the same temperature is (molar mass of benzene $= 78 \ g \ mol^{-1}$)

According to Raoult's law,the relative lowering of vapour pressure for a solution is equal to which of the following?