$A$ mixture of benzene and toluene forms

Liquids $A$ and $B$ form an ideal solution. The vapour pressure of pure $A$ and $B$ are $50 \ mm \ Hg$ and $32 \ mm \ Hg$ respectively at $300 \ K$. One mole of liquid $A$ is mixed with $1$ mole of liquid $B$. What is the approximate mole fraction of $A$ in the vapour phase?

When does a mixture containing components $A$ and $B$ show negative deviation from Raoult's law?

An ideal solution has two components $A$ and $B$. If $A$ is more volatile than $B$ and also $P_A^o > P_T$,then the correct relation between mole fraction of $A$ in liquid $(x)$ and vapour $(y)$ phase is

$A$ liquid mixture contains $10 \ moles$ of $A$ $(P_A^0 = 200 \ mm \ Hg)$ and $10 \ moles$ of $B$ $(P_B^0 = 100 \ mm \ Hg)$. The vapour pressure over the liquid mixture is $160 \ mm \ Hg$. Which statement is correct?

In a binary ideal solution of liquids $A$ and $B$ at a constant temperature,the mole fraction of $A$ in the liquid phase is $0.7$ and in the vapor phase is $0.4$. If $P_A^o + P_B^o = 90 \, mm$,then the vapor pressures of pure liquids $A$ and $B$ at that temperature are respectively: