Statement-1: A compound with odd number of nitrogen always contains odd molecular weight.
and
Statement-2: Nitrogen has odd molecular mass.

Answer

To analyze the statements given in the question, we will break down the reasoning step by step.

### Step 1: Understanding Statement-1
**Statement-1** claims that a compound with an odd number of nitrogen atoms always has an odd molecular weight.

To verify this, we can consider examples of compounds with an odd number of nitrogen atoms and calculate their molecular weights.

**Example 1: Aniline (C6H5NH2)**
- Carbon (C): 6 atoms × 12 g/mol = 72 g/mol
- Hydrogen (H): 7 atoms × 1 g/mol = 7 g/mol
- Nitrogen (N): 1 atom × 14 g/mol = 14 g/mol

Calculating the total molecular weight:
\[ 72 + 7 + 14 = 93 \text{ g/mol} \]
93 is an odd number.

**Example 2: Ammonia (NH3)**
- Nitrogen (N): 1 atom × 14 g/mol = 14 g/mol
- Hydrogen (H): 3 atoms × 1 g/mol = 3 g/mol

Calculating the total molecular weight:
\[ 14 + 3 = 17 \text{ g/mol} \]
17 is also an odd number.

Thus, for compounds with an odd number of nitrogen atoms, the molecular weight is indeed odd.

### Step 2: Understanding Statement-2
**Statement-2** claims that nitrogen has an odd molecular mass.

To verify this, we need to look at the atomic mass of nitrogen:
- The atomic mass of a nitrogen atom (N) is 14 g/mol, which is an even number.

Additionally, if we consider nitrogen gas (N2), the molecular mass would be:
- Nitrogen gas (N2): 2 × 14 g/mol = 28 g/mol, which is also even.

Since both the atomic mass of nitrogen and the molecular mass of nitrogen gas are even, this statement is incorrect.

### Conclusion
- **Statement-1** is correct: A compound with an odd number of nitrogen atoms does indeed have an odd molecular weight.
- **Statement-2** is incorrect: Nitrogen does not have an odd molecular mass, as its atomic mass is even.

### Final Answer
- Statement-1 is true.
- Statement-2 is false.