34.2 g of cane sugar is dissolved in 180 g of water. The relative lowering of vapour pressure will be

(1) 0.0099

(2) 1.1597

(3) 0.840

(4) 0.9901

Lowering in vapour pressure is the highest for:

1. 0.2 m urea

2. 0.1 m glucose

3. 0.1 m MgSO₄

4. 0.1 m BaCl₂

The Vapour pressure of CCl₄ at 25°C is 143 mm Hg. 0.5 g of a non-volatile solute (mol. wt. 65) is dissolved in 100 ml of CCl₄. The vapor pressure of the solution is-

(Density of CCl₄ = 1 .58 g/cm³$)$ 

1. 141.93 mm Hg

2. 94.39 mm Hg

3. 199.34 mm Hg

4. 143.99 mm Hg

The vapour pressure of pure benzene and toluene are 160 and 60 torr respectively. The mole fraction of toluene in vapour phase in contact with an equimolar solution of benzene and toluene is -

The vapour pressure of a solvent decreases by 10 mm of mercury when a non-volatile solute was added to the solvent. The mole fraction of the solute in the solution is 0.2. What should be if the decrease in vapour pressure is to be 20 mm of mercury then the mole fraction of the solvent is [CBSE PMT 1998]

(1) 0.8

(2) 0.6

(3) 0.4

(4) None

Osmotic pressure is 0.0821 atm at a temperature of 300 K. Find concentration in mole/litre [Roorkee 1990]

(1) 0.033

(2) 0.066

(3) 0.33 × 10^–2

(4) 3

The osmotic pressure of 5 % (mass-volume) solution of cane sugar at 150 °C (mol. mass of sugar = 342 g/mole) is:

A solution containing 3.3 g of a substance in 125 g of benzene (b.p. 80°C) boils at 80.66°C. If K_b for one litre of benzene is 3.28°C, the molecular weight of the substance shall be 

1. 127.20

2. 131.20

3. 137.12

4. 142.72

The molal b.p. constant for water is $0{.513}^{o}Ckgmo{l}^{-1}$. When 0.1 mole of sugar is dissolved in 200 g of water, the solution boils under a pressure of 1 atm at

(1) 100.513°C

(2) 100.0513°C

(3) 100.256°C

(4) 101.025°C

An aqueous solution containing 1 g of urea boils at 100.25 °C. The aqueous solution containing 3 g of glucose in the same volume will boil at:
1. 100.75 °C
2. 100.5 °C
3. 100 °C
4. 100.25 °C