At $363 \ K,$ the vapour pressure of $A$ is $21 \ kPa$ and that of $B$ is $18 \ kPa$. One mole of $A$ and $2 \ moles$ of $B$ are mixed. Assuming that this solution is ideal,the vapour pressure of the mixture is $....... \ kPa$. (Round off to the Nearest Integer).

Assuming the formation of an ideal solution,determine the boiling point of a mixture containing $1560 \ g$ benzene (molar mass $= 78 \ g/mol$) and $1125 \ g$ chlorobenzene (molar mass $= 112.5 \ g/mol$) against an external pressure of $1000 \ torr$ using the provided graph. (in $^{\circ}C$)

Which property is shown by an ideal solution?

Which of the following will form 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 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