Q. No.The positive deviations from Raoult’s law mean the vapour pressure is:
1. Higher than expected.
2. Lower than expected.
3. As expected.
4. None of the above
2. Lower than expected.
3. As expected.
4. None of the above
The type of inter-molecular interactions present in:
| (a) | n-Hexane and n-octane | (i) | Van der Waal’s forces of attraction |
| (b) | NaClO4 and water | (ii) | Ion-dipole interaction |
| (iii) | Dipole-dipole interaction |
| (a) | (b) | |
| 1. | (i) | (ii) |
| 2. | (ii) | (ii) |
| 3. | (i) | (iii) |
| 4. | (iii) | (iii) |
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 |
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
The solubility of \(H_2S\) in water at STP is 0.195 m. The value of Henry's constant is:
| 1. | 274 atm | 2. | 285 atm |
| 3. | 295 atm | 4. | 278 atm |
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. |
Which law is applied when deep-sea divers use a breathing mixture of oxygen and less soluble helium to minimise the painful effects caused by the increased dissolution of gases in blood at high pressure?
| 1. | Raoult's law | 2. | Henry's law |
| 3. | Ideal gas Equation | 4. | All of the above |
| Type of solution | Example | ||
| a. | Solid in gas | i. | Aerated water |
| b. | Gas in liquid | ii. | Smoke |
| c. | Liquid in solid | iii. | Solution of hydrogen in palladium |
| d. | Gas in solid | iv. | Amalgams |
| a | b | c | d | |
| 1. | i | iii | iv | ii |
| 2. | ii | i | iv | iii |
| 3. | iii | i | iv | ii |
| 4. | iv | i | ii | iii |
A solution of glucose (M.W. = 180 g mol–1) in water is 10 % w/w. The mole fraction of each component in the solution is:
| 1. | Mole fraction of glucose - 0.44; mole fraction of water - 0.56 |
| 2. | Mole fraction of glucose - 0.056; mole fraction of water - 0.944 |
| 3. | Mole fraction of glucose - 0.011; mole fraction of water - 0.99 |
| 4. | Mole fraction of glucose - 0.36; mole fraction of water - 0.64 |
The type of molecular interactions in a solution of alcohol and water is:
| 1. | Electrostatic interaction | 2. | London dispersion forces |
| 3. | Hydrogen bonding | 4. | Ion-dipole interaction |
© 2026 GoodEd Technologies Pvt. Ltd.