An aqueous dilute solution containing non-volatile solute boils at 100.52° C. What is the molality of solution?(K_b = 0.52 kg mol^-1K, boiloing temperature of water = 100° C)

• 0.1 m

• 0.01 m

• 0.001 m

• 1.0 m

192.

The experimental depression in freezing point of a dilute solution is 0.025 K. If the van't Hoff factor (i) is 2.0, the calculated depression in freezing point (in K) is

• 0.00125

• 0.025

• 0.0125

• 0.05

The molality of an aqueous dilute solution containing non-volatile solute is 0.1 m. What is the boiling temperature (in °C) of solution? (Boiling point elevation constant, K_b = 0.52 kg mol^-1K; boiling temperature of water = 100°C).

• 100.0052

• 100.052

• 100.0

• 100.52

The vapour pressure of a non-ideal two component solution is given below

When helium gas is allowed to expand into vaccum, heating effect is observed. The reason for this is (assume He as a non ideal gas)

• He is an inert gas

• The inversions temperature of helium is very high

• The inversion temperature of helium is very low

• He has the lowest boiling point

Which of the following conditions are correct for real solutions showing negative deviation from Raoult's law?

• ΔH_Mix <0, ΔV_Mix > 0

• ΔH_Mix >0, ΔV_Mix > 0

• ΔH_Mix >0, ΔV_Mix < 0

• ΔH_Mix <0, ΔV_Mix <0

Molal depression constant for a solvent is 4.0 K 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)

• 0.24 K

• 0.12 K

• 0.18 K

• 0.36 K

For the solution of the gases w, x, y and z in water at 298 K, the Henrys law constants (K_H) are 0.5, 2, 35 and 40 kbar, respectively. The correct plot for the given data is :

The osmotic pressure of a dilute solution of an ionic compound XY in water is four times that of a solution of 0.01 M BaCl₂ in water. Assuming complete dissociation of the given ionic compounds is water, the concentration of XY (in mol L^-1 ) in solution is 

• 4 × 10^-4

• 16 × 10^-4

• 4 × 10^-2

• 6 × 10^-2

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

• 0.28mmHg

• 0.031 mmHg

• 0.027Hg

• 0.017mmHg