Total vapour pressure of a mixture of $1 \, mol \, X$ $(P_x^o = 150 \, torr)$ and $2 \, mol \, Y$ $(P_y^o = 300 \, torr)$ is $240 \, torr$. In this case:

$A$ mixture of toluene and benzene forms a nearly ideal solution. Assume $p_{B}^{\circ}$ and $p_{T}^{\circ}$ to be the vapour pressures of pure benzene and toluene,respectively. The slope of the line obtained by plotting the total vapour pressure versus the mole fraction of benzene is $....$

$2 \ moles$ each of liquids $A$ and $B$ are dissolved to form an ideal solution. What will be the mole fraction of $B$ in the vapour phase? Given: $P_A^o = 120 \ torr, P_B^o = 80 \ torr$

Which one of the following non-ideal solutions shows negative deviation?

At $88\,^oC$,the vapor pressure of benzene is $900 \, \text{torr}$ and that of toluene is $360 \, \text{torr}$. What is the mole fraction of benzene in the mixture with toluene that will boil at $88\,^oC$ and $1 \, \text{atm}$ pressure,assuming it forms an ideal solution?

If vapour pressures of pure liquids $A$ and $B$ are $300$ and $800 \, torr$ respectively at $25 \, ^{\circ}C$. When these two liquids are mixed at this temperature to form a solution in which mole percentage of $B$ is $92$,then the total vapour pressure is observed to be $0.95 \, atm$. Which of the following is true for this solution?