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

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?

Which of the following statements about the composition of the vapour over an ideal $1:1$ molar mixture of benzene and toluene is correct? Assume that the temperature is constant at $25\ ^oC$. (Given,vapour pressure data at $25\ ^oC$,benzene $= 12.8\ kPa,$ toluene $= 3.85\ kPa$)

Benzene and toluene form nearly ideal solutions. At $20\,^{\circ}C$,the vapour pressure of benzene is $75\,torr$ and that of toluene is $22\,torr$. The partial vapour pressure of benzene at $20\,^{\circ}C$ for a solution containing $78\,g$ of benzene and $46\,g$ of toluene in $torr$ is

Explain non-ideal solutions and the occurrence of positive and negative deviations in non-ideal solutions.

An ideal solution was obtained by mixing methanol and ethanol. If the partial vapour pressure of methanol and ethanol are $2.619 \, kPa$ and $4.556 \, kPa$ respectively,the composition of the vapour (in terms of mole fraction) will be