Select correct statement ?

Options

A. Heats orf vaporisation for a pure solvent and for a solution are similar because similar intermolecular forces between solvent molecules must be overcome in both case.
B. Entropy change between solution and vapour is smaller than the entropy change between pure solvent and vapour
C. Boiling point of the solution is larger than that of the pure solvent
D. All are correct statements

Explanation

To solve the question, we need to analyze each statement provided and determine whether they are correct or not. Let's break down the statements one by one.

### Step 1: Analyze the First Statement
**Statement:** Heats of vaporization for a pure solvent and for a solution are similar because similar intermolecular forces between solvent molecules must be overcome in both cases.

**Explanation:**
- In a pure solvent, the molecules interact only with each other (solvent-solvent interactions).
- In a solution, solvent molecules interact with both solvent and solute molecules (solvent-solvent and solvent-solute interactions).
- Although there may be slight differences in intermolecular forces due to the presence of solute, the dominant interactions are still between the solvent molecules. Thus, the heats of vaporization for both the pure solvent and the solution are approximately equal.

**Conclusion:** This statement is correct.

### Step 2: Analyze the Second Statement
**Statement:** Entropy change between solution and vapor is smaller than the entropy change between pure solvent and vapor.

**Explanation:**
- The entropy of a pure solvent is lower than that of a solution because the solution has solute particles that increase disorder.
- When transitioning from a pure solvent to vapor, the increase in entropy is significant because the vapor phase has the highest entropy.
- The difference in entropy change from pure solvent to vapor is greater than the difference from solution to vapor, since the solution already has a higher entropy than the pure solvent.

**Conclusion:** This statement is correct.

### Step 3: Analyze the Third Statement
**Statement:** Boiling point of the solution is larger than that of the pure solvent.

**Explanation:**
- The presence of solute in a solution increases the intermolecular forces (due to solute-solvent interactions).
- As a result, more energy (higher temperature) is required to break these intermolecular forces to reach the boiling point.
- Therefore, the boiling point of the solution is indeed higher than that of the pure solvent.

**Conclusion:** This statement is correct.

### Final Conclusion
Since all three statements have been analyzed and found to be correct, we can conclude that the answer to the question is:

**All statements are correct.**

### Answer: Option 4

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