A solution is prepared by dissolving 0.6 g of urea (molar mass = 60 g mol^–1) and 1.8 g of glucose (molar mass = 180 g mol^–1) in 100 mL of water at 27^oC. The osmotic pressure of the solution is :
(R = 0.08206 L atm K^–1 mol^–1)

1 g of a non-volatile non-electrolyte solute is dissolved in 100 g of two different solvents A and B whose ebullioscopic constants are in the ratio of 1 : 5. The ratio of the elevation in their boiling points, $${{\Delta {T_b}(A)} \over {\Delta {T_b}(B)}}$$, is :

At room temperature, a dilute solution of urea is prepared by dissolving 0.60 of urea in 360 g of water. If the vapour pressure of pure water at this temperature is 35 mm Hg, lowering of vapour pressure will be. (molar mass of urea = 60 g mol^–1)

Molal depression constant for a solvent is 4.0 kg mol^–1. The depression in the freezing point of the solvent for 0.03 mol kg^–1 solution of K₂SO₄ is :
(Assume complete dissociation of the electrolyte)