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 Kf and Kb 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]
1. | 40 | 2. | 60 |
3. | 80 | 4. | 20 |
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:
1. | P2 > P3 > P1 | 2. | P3 > P1 > P2 |
3. | P2 > P1 > P3 | 4. | P1 > P2 > P3 |
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:
Kb 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 % |