Consider the following statements about the composition of the vapour over an ideal 1:1 molar mixture of benzene and toluene. The correct statement is:

Assume that the temperature is constant at 25 ^oC.
(Given, vapour pressure data at 25 °C, benzene = 12.8 kPa, toluene = 3.85 kPa)

1.	The vapour will contain a higher percentage of toluene.
2.	The vapour will contain equal amounts of benzene and toluene.
3.	Not enough information is given to make a prediction.
4.	The vapour will contain a higher percentage of benzene.

The boiling point of 0.2 mol kg^-1 solution of X in water is greater than the equimolal solution of Y in water. The correct statement in this case is:

The electrolyte having the same value of Van't Hoff factor (i) as that of Al₂(SO₄)₃  (if all are 100% ionized) is:

1. K₂SO₄
2. K₃[Fe(CN)₆]
3. Al(NO₃)₃
4. K₄[Fe(CN)₆]

The largest freezing point depression among the following O.10 m solutions is shown by:

The freezing point depression constant for water is 1.86 ^oC m^-1. If 5.00 g Na₂SO₄ is dissolved in 45.0 g H₂O, the freezing point is changed by -3.82 ^oC. The van’t Hoff factor for Na₂SO₄ is:

The van’t Hoff factor, i, for a compound that undergoes
dissociation and association in a solvent is, respectively:

1. Less than one and less than one.
2. Greater than one and less than one.
3. Greater than one and greater than one.
4. Less than one and greater than one.

An aqueous solution is 1.00 molal in KI. The vapour pressure of the solution can be increased by:

1. Addition of NaCl

2. Addition of Na₂SO₄

3. Addition of 1.00  molal Kl

4. Addition of water

A 0.0020 m aqueous solution of an ionic compound Co(NH₃)₅(NO₂)Cl freezes at -0.0073 ^oC. The number of moles of ions that 1 mol of ionic compound produces on being dissolved in water will be:
(K_f = -1.86 ^oC/m)

0.5 molal aqueous solution of a weak acid (HX) is 20 % ionised. The lowering in the freezing point of the solution will be:
[K_f for water = 1.86 K kg mol^-1]

1. -1.12 K

2. 0.56 K

3. 1.12 K

4. -0.56 K