The plot of total vapour pressure as a function of mole fraction of the components of an ideal solution formed by mixing liquids $X$ and $Y$ is

$A$ solution contains $KCl$ in water. It is heated continuously and the vapour formed is removed continuously. The vapour pressure of the solution will be:

Which solution has the lowest vapor pressure?

Calculate the vapour pressure of pure volatile liquid $B$ $(P_B^o)$ at a given temperature if the mole fraction of liquid $B$ $(x_B)$ is $0.4$ and the vapour pressure of pure volatile liquid $A$ $(P_A^o)$ is $400 \ mm \ Hg$. The total vapour pressure of the solution is $P_{total} = 600 \ mm \ Hg$. (in $mm \ Hg$)

$A$ mixture of $3.0 \ mol$ of $Na_2O$ and $1.5 \ mol$ of $KO_2$ is dissolved in $1000 \ mL$ of water. The vapour pressure of the solution in $Torr$,at $100^{\circ}C$ is:

At a certain temperature,when some amount of glucose is dissolved in water,it is observed that the lowering in vapour pressure is $0.6 \ mm \ Hg$ for this solution. What will be the vapour pressure of the same glucose solution if its molality is $(\frac{1}{18}) \ mol \ kg^{-1}$ (in $mm \ Hg$)?