$2 \ moles$ each of liquids $A$ and $B$ are dissolved to form an ideal solution. What will be the mole fraction of $B$ in the vapour phase? Given: $P_A^o = 120 \ torr, P_B^o = 80 \ torr$

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

Two liquids $A$ and $B$ form an ideal solution. What will be the vapor pressure of a solution containing a mole ratio of $A$ and $B$ as $3:1$ in $torr$? $(Given: P_A^o = 24 \ torr, P_B^o = 40 \ torr)$

On mixing $10 \ mL$ of acetone with $40 \ mL$ of chloroform,the total volume of the solution is

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 $^{\circ}C$)

$A$ binary liquid solution is prepared by mixing $n$-heptane and ethanol. Which one of the following statements is correct regarding the behaviour of the solution?