Which of the following is an ideal solution?

If 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 $92$,then the total vapour pressure is observed to be $0.95 \, atm$. Which of the following is true for this solution?

An ideal solution has two components $A$ and $B$. If $A$ is more volatile than $B$,then the correct relation between mole fraction of $A$ in liquid $(X_A)$ and vapour phase $(Y_A)$ is:

At $T(K)$,the vapour pressures of two liquids,heptane and octane are $106 \ kPa$ and $47 \ kPa$ respectively. If $25 \ g$ of heptane and $57 \ g$ of octane form an ideal solution,at $T(K)$ the vapour pressure of solution in $kPa$ is :

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

$5$ moles of liquid $X$ and $10$ moles of liquid $Y$ make a solution having a vapour pressure of $70 \ torr$. The vapour pressures of pure $X$ and $Y$ are $63 \ torr$ and $78 \ torr$ respectively. Which of the following is true regarding the described solution?