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

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: $22\, mm\, Hg$

Which of the following mixtures shows positive deviation from ideal behavior?

$A$ solution of two miscible liquids showing negative deviation from Raoult's law will have :

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 $A$ and $B$ form an ideal solution. The vapour pressure of pure liquids $A$ and $B$ are $350 \ mm \ Hg$ and $750 \ mm \ Hg$ respectively at the same temperature. If $x_A$ and $x_B$ are the mole fractions of $A$ and $B$ in the solution,and $y_A$ and $y_B$ are the mole fractions of $A$ and $B$ in the vapour phase,then: