Assertion: The value of van der Waals constant a is larger for ammonia than for nitrogen.
Reason: Hydrogen bonding is present in ammonia.

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 assertion and reason question regarding the van der Waals constant \( a \) for ammonia and nitrogen, we will analyze both the assertion and the reason step by step.

### Step 1: Understand the Assertion
The assertion states that "The value of van der Waals constant \( a \) is larger for ammonia than for nitrogen."

**Explanation:**
- The van der Waals constant \( a \) is a measure of the strength of intermolecular forces in a substance. A larger \( a \) value indicates stronger intermolecular attractions.
- Ammonia (NH₃) has stronger intermolecular forces compared to nitrogen (N₂) due to hydrogen bonding.

### Step 2: Understand the Reason
The reason states that "Hydrogen bonding is present in ammonia."

**Explanation:**
- Ammonia has a nitrogen atom bonded to three hydrogen atoms. The nitrogen is highly electronegative, which leads to the formation of hydrogen bonds between ammonia molecules.
- Hydrogen bonding significantly increases the intermolecular forces in ammonia, making it a polar molecule.

### Step 3: Compare Ammonia and Nitrogen
- **Ammonia (NH₃):**
- Polar molecule due to the presence of hydrogen bonding.
- Strong intermolecular forces lead to a higher van der Waals constant \( a \).

- **Nitrogen (N₂):**
- Non-polar molecule with weak London dispersion forces as the only type of intermolecular force.
- Lower van der Waals constant \( a \) compared to ammonia.

### Step 4: Conclusion
Since the assertion is true (the value of \( a \) for ammonia is indeed larger than for nitrogen) and the reason is also true (hydrogen bonding is present in ammonia), we conclude that:

- Both the assertion and reason are correct.
- The reason correctly explains the assertion.

### Final Answer
Both the assertion and reason are true, and the reason is the correct explanation of the assertion.

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