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191.

An aqueous dilute solution containing non-volatile solute boils at 100.52° C. What is the molality of solution?(Kb = 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


193.

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, Kb = 0.52 kg mol-1K; boiling temperature of water = 100°C).

  • 100.0052

  • 100.052

  • 100.0

  • 100.52


194.

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

           


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195.

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


196.

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

  • ΔHMix <0, ΔVMix > 0

  • ΔHMix >0, ΔVMix > 0

  • ΔHMix >0, ΔVMix < 0

  • ΔHMix <0, ΔVMix <0


197.

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


198.

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


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199.

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


200.

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


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