Which of the following is not correct for an ideal solution?

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 $1000 \ torr$. Use the provided vapor pressure vs. temperature graph to find the answer. (in $^{\circ}C$)

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:

Which of the following mixture$(s)$ show$(s)$ positive deviation from Raoult's law at $35^{\circ}C$?
$(A)$ Carbon tetrachloride + methanol
$(B)$ Carbon disulphide + acetone
$(C)$ Benzene + toluene
$(D)$ Phenol + aniline

The solution which shows negative or positive deviation from Raoult's law is called:

$1 \, \text{mole}$ of liquid $A$ and $2 \, \text{mole}$ of liquid $B$ form a solution with a vapor pressure of $38 \, \text{torr}$. If the vapor pressures of pure $A$ and pure $B$ are $45 \, \text{torr}$ and $36 \, \text{torr}$ respectively,the solution will be: