Choose a false statement among the following:

1.	Raoult's law states that the vapour pressure of a component over a solution is proportional to its mole fraction.
2.	The osmotic pressure (\(\pi\)) of a solution is given by the equation \(\pi\)=MRT, where M is the molarity of the solution.
3.	The correct order of osmotic pressure for 0.10 M aqueous solution of each compound is BaCl2 > KCl > CH3COOH > sucrose.
4.	Two sucrose solutions of the same molarity prepared in different solvents will have the same depression in the freezing point.

On mixing, heptane, and octane form an ideal solution at 373 K, the vapor pressures of the two liquid components (Heptane and octane) are 105 kPa and 45 kPa respectively. Vapour pressure of the solution obtained by mixing 25.0 g of heptane and 35 g of octane will be:
(molar mass of heptane = 100 g mol⁻¹ and of octane =114 g 1 mol⁻¹)

1. 144.5 kPa

2. 72.0 kPa

3. 36.1 kPa

4. 96.2 kPa

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 %

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 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

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