A: On increasing temperature vapour pressure of solution increases.
R: Vapour pressure of ether is higher than alcohol.

Answer

To solve the given question, we need to analyze both the assertion (A) and the reason (R) provided.

### Step-by-Step Solution:

1. **Understanding Assertion (A)**:
- The assertion states that "On increasing temperature, vapor pressure of solution increases."
- **Explanation**: Vapor pressure is the pressure exerted by the vapor of a liquid in equilibrium with its liquid phase at a given temperature. When the temperature of a liquid increases, more molecules have enough energy to escape from the liquid phase to the vapor phase. This results in an increase in the number of vapor molecules, thereby increasing the vapor pressure.

2. **Conclusion about Assertion (A)**:
- The assertion is **correct** because increasing the temperature leads to an increase in vapor pressure.

3. **Understanding Reason (R)**:
- The reason states that "Vapor pressure of ether is higher than alcohol."
- **Explanation**: This statement is based on the intermolecular forces present in both substances. Ether has weaker dipole-dipole interactions compared to the strong hydrogen bonding present in alcohol. As a result, ether molecules can escape into the vapor phase more easily than alcohol molecules, leading to a higher vapor pressure for ether.

4. **Conclusion about Reason (R)**:
- The reason is also **correct** because it accurately describes the relationship between vapor pressure and the types of intermolecular forces in ether and alcohol.

5. **Relationship between Assertion and Reason**:
- While both the assertion and the reason are correct, the reason does not explain the assertion. The assertion discusses the effect of temperature on vapor pressure, while the reason compares the vapor pressures of two different substances (ether and alcohol) without addressing the temperature factor.

### Final Conclusion:
- Assertion (A) is correct.
- Reason (R) is correct, but it does not explain assertion (A).