The vapour pressure of a solvent $A$ is $0.80 \, atm$. When a non-volatile substance $B$ is added to this solvent its vapour pressure drops to $0.6 \, atm$. What is the mole fraction of $B$ in the solution?

The boiling points of $C_6H_6, CH_3OH, C_6H_5NH_2$ and $C_6H_5NO_2$ are $80 \ ^oC, 65 \ ^oC, 184 \ ^oC$ and $212 \ ^oC$ respectively. Which will show the highest vapour pressure at room temperature?

Which of the following aqueous solutions will show maximum vapour pressure at $300 \text{ K}$?

The vapor pressure of pure $A$ is $10 \ torr$. When $1 \ g$ of $B$ is dissolved in $20 \ g$ of $A$ at the same temperature,the vapor pressure of the solution becomes $9 \ torr$. If the molar mass of $A$ is $200 \ g/mol$,the molar mass of $B$ is ............ $amu$.

Why is the vapour pressure of an aqueous solution of glucose lower than that of pure water?

The boiling points of $C_6H_6$,$CH_3OH$,$C_6H_5NH_2$,and $C_6H_5NO_2$ are $80 \, ^\circ C$,$65 \, ^\circ C$,$184 \, ^\circ C$,and $212 \, ^\circ C$ respectively. Which one exhibits the maximum vapor pressure at room temperature?