Assertion: Helium shows only positive deviations from ideal behaviour.
Reason: Helium is an inert gas.

Options

A. If both the statement are TRUE and STATEMENT-2 is the correct explanation of STATEMENT-1
B. If both the statement are TRUE but STATEMENT-2 is NOT the correct explanation of STATEMENT-1
C. If STATEMENT-1 is TRUE and STATEMENT-2 is FALSE
D. If STATEMENT-1 is FALSE and STATEMENT-2 is TRUE

Answer

To solve the question regarding the assertion and reason about helium's behavior as a gas, we will break down the concepts step by step.

### Step 1: Understanding the Assertion
The assertion states that "Helium shows only positive deviations from ideal behavior."

**Explanation**:
- An ideal gas follows the ideal gas law, represented by the equation \( PV = nRT \).
- Real gases deviate from this behavior due to intermolecular forces and the volume occupied by gas particles.
- Positive deviation occurs when the pressure of a real gas is greater than what is predicted by the ideal gas law, indicating weaker intermolecular forces.

### Step 2: Understanding the Reason
The reason states that "Helium is an inert gas."

**Explanation**:
- Helium is classified as an inert gas (noble gas) because it has a complete outer electron shell (1s² configuration), which makes it chemically nonreactive under standard conditions.
- While being an inert gas contributes to its behavior, it does not directly explain why it shows only positive deviations from ideal gas behavior.

### Step 3: Analyzing the Relationship
Now we need to analyze the relationship between the assertion and the reason.

**Explanation**:
- Both statements are true: helium does show positive deviations from ideal gas behavior, and it is indeed an inert gas.
- However, the reason does not explain the assertion. The positive deviation is primarily due to the weak intermolecular forces in helium, not its inert nature.

### Step 4: Conclusion
Based on the analysis, we conclude that:
- The assertion is true.
- The reason is true.
- The reason does not correctly explain the assertion.

Thus, the correct answer is that both statements are true, but the second statement is not a correct explanation of the first.

### Final Answer:
Both statements are true, but statement 2 is not a correct explanation of statement 1.

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