$A$ solution that obeys Raoult's law is

Benzene and toluene form nearly ideal solutions. At $20\,^{\circ}C$,the vapour pressure of benzene is $75\,torr$ and that of toluene is $22\,torr$. The partial vapour pressure of benzene at $20\,^{\circ}C$ for a solution containing $78\,g$ of benzene and $46\,g$ of toluene in $torr$ is

$p_A$ and $p_B$ are the vapour pressure of pure liquid components,$A$ and $B,$ respectively of an ideal binary solution. If $x_A$ represents the mole fraction of component $A,$ the total pressure of 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: $22\, mm\, Hg$

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 $0.8$?

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