The osmotic pressure (in atm) of an aqueous solution containing 0.01 mol of NaCl (degree of dissociation 0.94 ) and 0.03 mol of glucose in 500 mL at $27^{\circ} \mathrm{C}$ is $\left(R=0.082 \mathrm{~L} \mathrm{~atm} \mathrm{~K}^{-1} \mathrm{~mol}^{-1}\right)$

Which of the following solution has highest amount of solute?

Observe the following statements

Statement I : The boiling point of 0.1 M urea solution is less than that of 0.1 M KCl solution.

Statement II : Elevation of boiling point is inversely proportional to molar mass of solute.

The correct answer is

At 300 K , the vapour pressure of toluene and benzene are 3.63 kPa and 9.7 kPa respectively. What is the composition of vapour in equilibrium with the solution containing 0.4 mole fraction of toluene?

(Assume the solution is ideal)