Q. No.| 1. | formation of hydrogen bonding between acetone and chloroform. |
| 2. | increase in the escaping tendency of molecules of each component. |
| 3. | stronger intermolecular forces between chloroform molecules than those between chloroform and acetone molecules. |
| 4. | repulsive forces. |
| A. | An ideal solution thus formed obeys Raoult's law throughout the composition range. |
| B. | Mixture of chloroform and acetone shows negative deviation from Raoult's law. |
| C. | Mixture of aniline and phenol shows positive deviation from Raoult's law. |
| 1. | A and C only |
| 2. | A and B only |
| 3. | B and C only |
| 4. | A only |
| Assertion (A): | For an ideal solution formed by mixing liquids P and Q, \(\Delta_{mix} H = 0\) and \(\Delta_{mix} V = 0\) |
| Reason (R): | No interactions occur between P and Q |
| 1. | (A) is not correct but (R) is correct |
| 2. | Both (A)and (R) are correct and (R) is the correct explanation of (A) |
| 3. | Both (A) and (R) are correct but (R) is NOT the correct explanation of (A) |
| 4. | (A) is correct but (R) is not correct |
[Given: The vapour pressures of pure \(\text X\) and \(\text Y\) are \(63\) torr and \(78\) torr respectively]
| 1. | The solution is ideal. |
| 2. | The solution has a volume that is greater than the sum of individual volumes. |
| 3. | The solution shows positive deviation. |
| 4. | The solution shows negative deviation. |
The correct option for the value of vapour pressure of a solution at 45 C with benzene to octane in a molar ratio 3:2 is:
[At 45 C vapour pressure of benzene is 280 mm Hg and that of octane is 420 mm Hg. Assume Ideal gas]
| 1. | 336 mm of Hg | 2. | 350 mm of Hg |
| 3. | 160 mm of Hg | 4. | 168 mm of Hg |
1. Benzene + Toluene
2. Acetone + Chloroform
3. Chloroethane + Bromoethane
4. Ethanol + Acetone
For an ideal solution, the correct option is:
1. at constant T and P
2. at constant T and P
3. at constant T and P
4. at constant T and P
The correct statement regarding a solution of two components A and B exhibiting positive deviation from ideal behaviour is :
| 1. | Intermolecular attractive force between A-A and B-B are stronger than those between A-B |
| 2. | ∆mixH = 0 at constant T and P |
| 3. | ∆mixV = 0 at constant T and P |
| 4. | Intermolecular attractive forces between A-A and B-B are equal to those between A-B |
1. \(\Delta H_{\text{Mix}}=0\)
2. \(\Delta U_{\text{Mix}}=0\)
3. \(\Delta P=P_{\text{obs.}}-P_{\text{(Calculated by Raoult's law)}}=0\)
4. \(\Delta G_{\text{Mix}}=0\)
Calculate the vapour pressure of a solution prepared by mixing 25.5 g of chloroform (CHCl₃) and 40 g of dichloromethane (CH₂Cl₂) at 25°C.
Given:
Vapour pressure of pure CHCl₃ = 200 mmHg
Vapour pressure of pure CH₂Cl₂ = 415 mmHg
Molar mass of CHCl₃ = 119.5 g mol⁻¹
Molar mass of CH₂Cl₂ = 85 g mol⁻¹
| 1. | 90.40 mm Hg | 2. | 119.5 mm Hg |
| 3. | 348 mm Hg | 4. | 173.9 mm Hg |
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