On mixing $10 \ mL$ $CCl_4$ and $10 \ mL$ benzene,the total volume of solution is

Two compounds form an ideal solution at room temperature. Which of the following are correct for this ideal solution?
$(A)$ $\Delta G_{mix} < 0$
$(B)$ $\Delta S_{mix} > 0$
$(C)$ $\Delta V_{mix} = 0$
$(D)$ $\Delta_{mix} H = 0$

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

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

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

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: