The mixture which shows positive deviation from Raoult's law 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?

Liquid $M$ and liquid $N$ form an ideal solution. The vapour pressures of pure liquids $M$ and $N$ are $450 \ mmHg$ and $700 \ mmHg,$ respectively at the same temperature. Then the correct statement is: ( $x_M =$ mole fraction of $M$ in solution; $x_N =$ mole fraction of $N$ in solution; $y_M =$ mole fraction of $M$ in vapour phase; $y_N =$ mole fraction of $N$ in vapour phase)

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:

If liquids $A$ and $B$ form an ideal solution,which of the following statements is true?

What are the values of $\Delta H_{mix}$ and $\Delta V_{mix}$ for an ideal solution?