# Mole fraction of the component A in vapour phase is X1 and mole fraction of component A in liquid mixture is X2 then  (${\mathrm{P}}_{\mathrm{A}}^{0}$ = vapour pressure of pure A; ${\mathrm{P}}_{\mathrm{B}}^{0}$= vapour pressure of pure B), then total vapour pressure of the liquid mixture is- 1. $\frac{{\mathrm{P}}_{\mathrm{A}}^{0}{\mathrm{X}}_{2}}{{\mathrm{X}}_{1}}$ 2. $\frac{{\mathrm{P}}_{\mathrm{A}}^{0}{\mathrm{X}}_{1}}{{\mathrm{X}}_{2}}$ 3. $\frac{{\mathrm{P}}_{\mathrm{B}}^{0}{\mathrm{X}}_{1}}{{\mathrm{X}}_{2}}$ 4. $\frac{{\mathrm{P}}_{\mathrm{B}}^{0}{\mathrm{X}}_{2}}{{\mathrm{X}}_{1}}$

Subtopic:  Relative Lowering of Vapour Pressure |
58%
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pH of a 0.1 (M) monobasic acid is 2. Osmotic pressure at a given temperature T is-

1. 0.1RT

2. 0.11RT

3. 1.1RT

4. 0.01RT

Subtopic:  Osmosis & Osmotic Pressure |
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The vapour pressure of pure water at 298K is 23.76mm. The vapour pressure of a solution of sucrose(C12H22O11) in 5.56 moles of water is 23.392mm Hg. The mass of sucrose in the solution is

1. 15 g

2. 45 g

3. 30 g

4. 37.5 g

Subtopic:  Relative Lowering of Vapour Pressure |
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Among the following options, 0.1 M aqueous solution that will have the lowest freezing point is-

 1 Potassium Sulphate. 2 Sodium chloride. 3 Urea. 4 Glucose.

Subtopic:  Depression of Freezing Point |
68%
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The vapour pressure of toluene is 59.1 torr at 313.75 K and 298.7 torr at 353.15 K. Calculate, the molar heat of vaporisation.

1. 37888 J mol-1

2. 27188 J mol-1

3.  12834 J mol-1

4. 571328 J mol-1

Subtopic:  Raoult's Law |
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The vapour pressure of a pure liquid solvent A is 0.80 atm. When a non-volatile substance B is added to the solvent, its vapour pressure drops to 0.60 atm.
Mole fraction of the component B in the solution is:

 1 0.5 2 0.75 3 0.4 4 0.25
Subtopic:  Relative Lowering of Vapour Pressure |
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The lowest boiling point, if concentration is fixed at 0.1 M in aqueous solution, is given by which of the following solutions?

a. K2SO4

b. NaCl

c. Urea

d. Glucose

1. a, b

2. b, c

3. c, d

4. d, a

Subtopic:  Elevation of Boiling Point |
66%
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The boiling point of acetic acid is 118.1$°\mathrm{C}$ and its latent heat of vaporisation is 121 cal/gm. A solution containing 0.4344 gm anthracene in 44.16 gm acetic acid boils at 118.24$°\mathrm{C}$. What is the molecular wt. of anthracene ?

1. 122

2. 178

3. 105

4. 154

Subtopic:  Elevation of Boiling Point |
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Which solution will have the highest boiling point ?

1. 1 (M) C6H12O6 solution

2. 1 (M) NaCl solution

3. 1 (M) BaCl2 solution

4. 1 (M) CO(NH2)2 solution

Subtopic:  Van’t Hoff Factor |
63%
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A 2.0% solution by weight of urea in water shows a boiling point elevation of 0.18 deg [Molecular weight of urea=60]. Calculate the latent heat of vaporization per gram of water.

1. 495.3 cal/g

2. 560.3 cal/g

3. 525.8 cal/g

4. 501.3 cal/g

Subtopic:  Elevation of Boiling Point |
52%
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