Assertion (R): At low concentration equimolar solutions of non electrolytes are isotonic and have equal osmotic pressure.
Reason (R): Osmotic pressure is directly proportional to temperature of solution.

Explanation

To solve the question regarding the assertion and reason, we will analyze both statements step by step.

### Step 1: Analyze the Assertion
**Assertion (A)**: "At low concentration, equimolar solutions of non-electrolytes are isotonic and have equal osmotic pressure."

- **Explanation**: Non-electrolytes do not dissociate into ions in solution. When two solutions are equimolar (having the same molarity) and are non-electrolytes, they will exert the same osmotic pressure at low concentrations. This is because osmotic pressure is a colligative property, which depends on the number of solute particles in a solution, not their identity, provided the solutions are at the same temperature.

### Step 2: Analyze the Reason
**Reason (R)**: "Osmotic pressure is directly proportional to the temperature of the solution."

- **Explanation**: The formula for osmotic pressure (π) is given by the equation:
\[ \pi = C \cdot R \cdot T \]
where:
- \( \pi \) is the osmotic pressure,
- \( C \) is the molar concentration of the solution,
- \( R \) is the ideal gas constant,
- \( T \) is the absolute temperature in Kelvin.

From this equation, we can see that osmotic pressure is indeed directly proportional to temperature, assuming concentration remains constant.

### Step 3: Conclusion
- Both the assertion and reason are correct statements.
- However, the reason does not provide a direct explanation for the assertion. The assertion is about isotonic solutions at low concentrations, while the reason discusses the relationship between osmotic pressure and temperature.

### Final Answer
- **Assertion (A)**: True
- **Reason (R)**: True
- **Conclusion**: Both the assertion and reason are correct, but the reason is not the correct explanation for the assertion.

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