The molar volume of liquid benzene (density= 0.877 g ml^-1) increases by a factor of 2750 as it vapourises at 20$°\mathrm{C}$. At 27$°\mathrm{C}$ when a non-volatile solute (that does not dissociate) is dissolved in 54.6cm3 of benzene, vapour pressure of this solution, is found to be 98.88 mm Hg. calculate the freezing point of the solution.

Given: Enthalpy of vapourisation of benzene(l)=394.57 Jg^-1. Enthalpy of fusion of benzene (l) = 10.06 kJ mol^-1 Molal depression constant for benzene=5.0 K kg mol^-1.

1. 177.65 K

2. 277.65 K

3. 517.65 K

4. 237.15 K

The depression in the freezing point of water when 10 g of CH₃CH₂CHClCOOH is added to 250 g of water is -K_a=1.4 X 10^-3, K_f=1.86K kg mol^-1

1. 0.15$°\mathrm{C}$

2. 2.15$°\mathrm{C}$

3. 1.15$°\mathrm{C}$

4. 0.65$°\mathrm{C}$

The ratio of the vapour pressure of a solution to the vapour pressure of the solvent is

1. Equal to the mole fraction of the solvent

2. Proportional to the mole fraction of the solute

3. Equal to the mole fraction of the solute

4. None of the above

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. $\frac{{\mathrm{P}}_{\mathrm{B}}^0{\mathrm{X}}_2}{{\mathrm{X}}_1}$

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

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

Among the following options, 0.1 M aqueous solution that will have the lowest freezing point is-

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

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:

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