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 of the following is true when components forming an ideal solution are mixed?

Which of the following mixtures forms 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?

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 graphs does not represent the behavior of an ideal binary liquid solution?