200 mL of an aqueous solution contains 1.26 g of protein. The osmotic pressure of this solution at 300 K is found to be 2.57 × 10^–3 bar. The molar mass of protein will be:

(R = 0.083 L bar mol^–1 K^–1):

1.	61038 g mol–1	2.	51022 g mol–1
3.	122044 g mol–1	4.	31011 g mol–1

A solution of urea (molar mass 56 g mol^–1) boils at 100.18 ºC at atmospheric pressure. If K_f and K_b for water are 1.86 and 0.512 K kg mol^–1 respectively, the above solution will freeze at:

1. –6.54 ºC

2. –0.654 ºC

3. 6.54 ºC

4. 0.654 ºC

If 8 g of a non-electrolyte solute is dissolved in 114 g of n-octane to reduce its vapor pressure to 80 %, the molar mass (in g mol^–1) of the solute is -

[Molar mass of n-octane is 114 g mol^–1]

The following solutions were prepared by dissolving 10 g of glucose (C₆H₁₂O₆) in 250 ml of water (P₁), 10 g of urea (CH₄N₂O) in 250 ml of water (P₂) and 10 g of sucrose (C₁₂H₂₂O₁₁) in 250 ml of water (P₃). The decreasing order of osmotic the pressure of these solutions is:

The correct option for the value of vapour pressure of a solution at 45 $°$C with benzene to octane in a molar ratio 3:2 is:

[At 45 $°$C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume Ideal gas]
1. 336 mm of Hg
2. 350 mm of Hg
3. 160 mm of Hg
4. 168 mm of Hg

The mole fraction of ethylene glycol (C₂H₆O₂) in a solution containing 20% of C₂H₆O₂ by mass is-

1. 0.932

2. 0.0672

3. 0.832

4. 0.732

If N₂ gas is bubbled through water at 293 K, how many millimoles of N₂ gas would dissolve in 1 litre of water?
(Partial pressure of nitrogen = 0.987 bar, Henry’s law constant for N₂ at 293 K = 76.48 kbar).

1. 0.716 mmol

2. 0.616 mmol

3. 0.726 mmol

4. 0.516 mmol

The boiling point of benzene is 353.23 K. When 1.80 g of a non-volatile solute was dissolved in 90 g of benzene, the boiling point is raised to 354.11 K. The molar mass of the solute is-

K_b for benzene is 2.53 K kg mol^–1

1. 55 g mol^–1
2. 64 g mol^–1
3. 58 g mol^–1  
4. 68 g mol^–1

45 g of ethylene glycol (C₂H₆O₂) is mixed with 600 g of water. The freezing point of the solution is -

1. 268.15 K
2. 270.95 K
3. 272.75 K
4. 267.15 K

The mole fraction of glucose (C₆H₁₂O₆) in an aqueous binary solution is 0.1. The mass percentage of water in it to the nearest integer is-
1. 44%
2. 49 %
3. 47 %
4. 41 %