The vapour pressure of pure $CHCl_3$ and $CH_2Cl_2$ are $200 \,atm$ and $41.5 \,atm$ respectively. The weights of $CHCl_3$ and $CH_2Cl_2$ are respectively $11.9 \,g$ and $17 \,g$. The vapour pressure of the solution will be (in $,atm$)

$18 \ g$ 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 vapour pressure of a solution containing a mixture of $2 \ mol$ of volatile liquid $A$ and $3 \ mol$ of volatile liquid $B$ at room temperature. $(P_{A}^{\circ} = 420 \ mm \ Hg, P_{B}^{\circ} = 610 \ mm \ Hg)$ (in $mm \ Hg$)

The vapor pressure of a dilute solution of glucose at $373 \ K$ is $750 \ mm \ of \ Hg$. The molality of the solution is:

How many grams of a non-volatile solute with a molar mass of $90$ must be dissolved in $97.5 \ g$ of water to cause a $2.5 \%$ decrease in vapour pressure?

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