Q. No.The amount of benzoic acid (C6H5COOH) required for preparing 250 mL of 0.15 M solution in methanol is:
1.
4.57 g
2.
3.57 g
3.
1.57 g
4.
12.57 g
The depression in the freezing point of water when 10 g of CH3CH2CHClCOOH is added to 250 g of water will be:
(Ka = 1.4 × 10–3, Kf = 1.86 K kg mol–1)
1. 0.32 K
2. 2.87 K
3. 0.65 K
4. 5.03 K
When 19.5 g of fluoroacetic acid (CH2FCOOH) is dissolved in 500 g of water, the observed depression in the freezing point was found to be 1.00 K. The Van’t Hoff factor and the dissociation constant of the fluoroacetic acid, respectively are: (Given: \(K_f\) for water = 1.86 K kg mol⁻¹, Molar mass of CH2FCOOH = 78 g mol⁻¹)
| 1. | 20.75 , 4.77 × 10–3 | 2. | 1.075 , 4.77 × 10–2 |
| 3. | 2.073 , 3.07 × 10–4 | 4. | 1.075 , 3.07 × 10–3 |
Henry’s law constant for the solution of methane in benzene at 298 K is 4.27 × 105 mm Hg. The mole fraction of methane in benzene at 298 K under 760 mm Hg will be:
1. 1.85 × 10–5
2. 192 × 10–4
3. 178 × 10–5
4. 18.7 × 10–5
100 g of liquid A (molar mass 140 g mol–1) was dissolved in 1000 g of liquid B (molar mass 180 g mol–1). The vapour pressure of pure liquid B was found to be 500 torr. If the total vapour pressure of the solution is 475 torr, the vapour pressure of pure liquid A will be:
| 1. | 326 torr | 2. | 226 torr |
| 3. | 360.7 torr | 4. | 280.7 torr |
Air consists primarily of nitrogen, which occupies approximately 79% by volume at 298 K under normal conditions. Water is in equilibrium with air at a total pressure of 10 atm and a temperature 298 K. The Henry's law constant for nitrogen in water at 298 K is given as 6.51 × 10⁷ mm Hg.
Determine the mole fraction of dissolved nitrogen in the water under these conditions:
| 1. | 12.4 × 10−5
|
2. | 9.22 × 10−5
|
| 3. | 3.54 × 10
|
4. | 4.96 × |
The amount of CaCl2 (i = 2.47) dissolved in 2.5 litre of water such that its osmotic pressure is 0.75 atm at 27 °C is:
| 1. | 1.02 g | 2. | 4.35 g |
| 3. | 2.87 g | 4. | 3.42 g |
Match the following type of intermolecular interactions present in the pair of compounds given:
| (a) | Methanol and Acetone | (i) | Van der Waal’s forces of attraction |
| (b) | Acetonitrile and Acetone | (ii) | Ion-dipole interaction |
| (iii) | Dipole-dipole interaction |
| (a) | (b) | |
| 1. | (iii) | (ii) |
| 2. | (ii) | (ii) |
| 3. | (iii) | (iii) |
| 4. | (iii) | (i) |
The solubility of gases in liquids generally decreases as temperature increases.
The primary reason for this behavior is:
| 1. | Dissolution of a gas in a liquid is an endothermic process. |
| 2. | Dissolution of a gas in a liquid is an exothermic process. |
| 3. | Gases are highly compressible. |
| 4. |
All of the above statements are correct. |
To minimize the painful effects accompanying deep sea diving, oxygen diluted with less soluble helium gas is used as breathing gas by the divers. This is an example of the application of:
| 1. | Raoult's law | 2. | Henry's law |
| 3. | Ideal gas Equation | 4. | All of the above |
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