Identify the mixture that shows positive deviations from Raoult's Law.

Which condition is not satisfied by an ideal solution?

Two liquids $A$ and $B$ form an ideal solution at temperature $T \ K$. At $T \ K$, the vapour pressures of pure $A$ and $B$ are $55 \ kNm^{-2}$ and $15 \ kNm^{-2}$ respectively. What is the mole fraction of $A$ in the solution of $A$ and $B$ in equilibrium with a vapour in which the mole fraction of $A$ is $0.8$?

At a particular temperature,the vapour pressures of two liquids $A$ and $B$ are respectively $120 \, mm$ and $180 \, mm$ of mercury. If $2 \, moles$ of $A$ and $3 \, moles$ of $B$ are mixed to form an ideal solution,the vapour pressure of the solution at the same temperature will be (in $mm$ of mercury):

Liquid $M$ and liquid $N$ form an ideal solution. The vapour pressures of pure liquids $M$ and $N$ are $450 \ mmHg$ and $700 \ mmHg,$ respectively at the same temperature. Then the correct statement is: ( $x_M =$ mole fraction of $M$ in solution; $x_N =$ mole fraction of $N$ in solution; $y_M =$ mole fraction of $M$ in vapour phase; $y_N =$ mole fraction of $N$ in vapour phase)

Which of the following plots does not represent the behavior of an ideal solution of $A$ and $B$?