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 $P_A^{\circ} > P_B^{\circ}$):

For an ideal solution of two components $A$ and $B$,which of the following is true?

Which of the following will form an ideal solution?

At $300 \ K$,the vapour pressures of $A$ and $B$ liquids are $500 \ mm \ Hg$ and $400 \ mm \ Hg$ respectively. Equal moles of $A$ and $B$ are mixed to form an ideal solution. The mole fraction of $A$ and $B$ in the vapor state is respectively:

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

Vapour pressures of pure liquids $A$ and $B$ are $300$ and $800 \ torr$ respectively at $25^{\circ}C$. When these two liquids are mixed at this temperature to form a solution in which mole percentage of $B$ is $90$,the total vapour pressure is observed to be $720 \ torr$. Which of the following is true for this solution?