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 |
The major component of air is nitrogen with approximately 79% by volume at 298 K. The water is in equilibrium with air at a pressure of 10 atm. At 298 K. if the Henry’s law constant for nitrogen at 298 K is 6.51 × 107 mm respectively, then the composition of nitrogen in air will be :
1. 12.4 × 10−5
2. 9.22 × 10−5
3. 3.54 × 10−5
4. 4.96 × 10−5
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 |
The type of inter molecular interactions present in
(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 a gas in a liquid decreases with an increase in temperature because:
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. |
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 |
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 |
The example of gas in a solid type solution is:
1. Solution of hydrogen in palladium.
2. Ethanol dissolved in water.
3. Camphor vapours in N2 gas.
4. Amalgams.
1. | \(\text X_{\text{mole fraction}}=\frac{\text n_{\text{solute}}}{\text n_{\text{solution}}}\) |
2. | \(\text{Molarity}=\frac{\text{amount of solute (g)}}{\text{volume of solution (mL)}}\) |
3. | \(\text{Molality}=\frac{\text{Number of mole of solute}}{\text{amount of solvent (kg)}}\) |
4. | \(\text{Mass percentage}=\frac{\text{mass of the component in the solution}}{\text{Total mass of the solution}}\times100 \) |
The density of 68 % nitric acid by mass in an aqueous solution is 1.504 g mL–1. The molarity of the acid solution would be:
1. 15.24 M
2. 16.23 M
3. 14.52 M
4. 13.45 M