On mixing $10 \ mL$ of acetone with $40 \ mL$ of chloroform,the total volume of the solution is

$1 \, \text{mole}$ of liquid $A$ and $2 \, \text{mole}$ of liquid $B$ form a solution with a vapor pressure of $38 \, \text{torr}$. If the vapor pressures of pure $A$ and pure $B$ are $45 \, \text{torr}$ and $36 \, \text{torr}$ respectively,the solution will be:

Which statement about the composition of vapour over an ideal $1:1$ molar mixture of benzene and toluene is correct? Assume the temperature is constant at $25\,^{\circ}C$. Vapour pressure data $(25\,^{\circ}C)$:
Benzene: $75\, mm\, Hg$
Toluene: $22\, mm\, Hg$

At $27^o C$,the vapor pressure of pure liquid $A$ is $70 \ torr$. It forms an ideal solution with $B$. The mole fraction of $B$ is $0.2$ and the vapor pressure of the solution at $27^o C$ is $84 \ torr$. What is the vapor pressure of pure liquid $B$ at $27^o C$ (in $torr$)?

Which one is an example of an ideal solution from the following?

Which pair of liquids shows positive deviation from Raoult's law?