Liquids $A$ and $B$ form an ideal solution. If $X_A$ and $Y_A$ are the mole fractions of $A$ in the solution and in vapour phase in equilibrium,respectively,then (Given $P_A^{\circ} > P_B^{\circ}$):

Two liquids $A$ and $B$ form an ideal solution. When they are mixed in a molar ratio of $1:1$,the vapor pressure of the solution at $300 \ K$ is $400 \ mm \ Hg$. When they are mixed in a molar ratio of $1:2$,the vapor pressure of the solution at the same temperature is $350 \ mm \ Hg$. The vapor pressures of pure liquids $A$ and $B$ are respectively:

Which of the following mixtures is an ideal solution?

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

Which of the following graphs does not represent the behavior of an ideal binary liquid solution?

Which condition is not satisfied by an ideal solution?