Assertion : Lower the cirtical temperature for a gas, more easily can it is liquefied.
Reason : Critical temperature is the temperature above which above which a gas cannot liquefied depending upon the pressure.

Options

A. If both assertion and reason are correct and reason is correct explanation for assertion
B. If both assertion and reason are correct and reason is not correct explanation for assertion
C. If assertion is correct but reason is incorrect
D. If assertion and reason are both incorreect.

Explanation

To solve the question, we need to evaluate both the assertion and the reason provided.

### Step 1: Analyze the Assertion
The assertion states: "Lower the critical temperature for a gas, more easily can it be liquefied."

- **Critical Temperature**: This is the temperature above which a gas cannot be liquefied, regardless of the pressure applied.
- If a gas has a lower critical temperature, it means that it requires a lower temperature to reach the liquid state. However, this does not imply that it can be liquefied easily. In fact, gases with lower critical temperatures often require higher pressures to be liquefied, making the assertion false.

### Step 2: Analyze the Reason
The reason states: "Critical temperature is the temperature above which a gas cannot be liquefied depending upon the pressure."

- This statement is partially correct as it defines critical temperature accurately. However, the phrase "depending upon the pressure" is misleading. The critical temperature itself is a fixed property of the gas and does not depend on pressure. Instead, it is the pressure that can be applied to liquefy a gas below its critical temperature. Therefore, this reason is also false.

### Step 3: Conclusion
- Since both the assertion and the reason are false, the correct answer is that both the assertion and the reason are incorrect.

### Final Answer
The answer is: **Both assertion and reason are false.** (Option D)

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