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

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?

Which of the following is appropriate for the solution made by mixing acetone and carbon disulphide?

Which of the following mixtures is a non-ideal solution?

Benzene and toluene form an ideal solution over the entire range of composition. The vapour pressure of pure benzene and toluene at $T \ K$ are $50 \ mmHg$ and $40 \ mmHg$,respectively. What is the mole fraction of toluene in the vapour phase when $117 \ g$ of benzene is mixed with $46 \ g$ of toluene? (Molar mass of benzene and toluene are $78 \ g \ mol^{-1}$ and $92 \ g \ mol^{-1}$,respectively)

Which of the following is a non-ideal solution?