Nitrogen is an inert molecule due to low bond dissociation enthalpy.

Explanation

### Step-by-Step Solution:

1. **Understanding the Question**: The statement claims that nitrogen is an inert molecule due to low bond dissociation enthalpy. We need to analyze this statement to determine its validity.

2. **Structure of Nitrogen**: Nitrogen exists as a diatomic molecule (N₂). In this molecule, two nitrogen atoms are bonded by a triple bond (N≡N).

3. **Bond Dissociation Enthalpy**: The bond dissociation enthalpy is the energy required to break a bond. In the case of nitrogen, the triple bond is very strong, meaning it has a high bond dissociation enthalpy.

4. **Energy Requirement for Bond Breaking**: Because the triple bond in nitrogen is strong, a significant amount of energy is required to break this bond. This means that at room temperature, there is generally not enough energy available to break the N≡N bond.

5. **Inertness of Nitrogen**: Due to the high bond dissociation enthalpy, nitrogen does not readily react with other substances at room temperature. This characteristic contributes to its inertness.

6. **Conclusion**: The original statement is incorrect. Nitrogen is an inert molecule due to its high bond dissociation enthalpy, not low. Therefore, the claim that nitrogen is inert because of low bond dissociation enthalpy is false.

### Final Answer:
The statement is false. Nitrogen is an inert molecule due to its high bond dissociation enthalpy, which makes it difficult to break the strong triple bond between nitrogen atoms.

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