Which of the following contains maximum number of nitrogen atoms ?

Options

A. `22.4 L` of `N_(2)` at STP
B. 500 mL of `2.0 M NH_(3)`
C. `6.02 xx 10^(23)` molecules of `NO_(2)`
D. 1.00 mol of `NH_(4)Cl`

Explanation

To determine which option contains the maximum number of nitrogen atoms, we will analyze each option step by step.

### Step-by-Step Solution:

1. **Option 1: 22.4 liters of N2 at STP**
- At Standard Temperature and Pressure (STP), 1 mole of any gas occupies 22.4 liters.
- Since we have 22.4 liters of N2, this means we have 1 mole of N2.
- Each molecule of N2 contains 2 nitrogen atoms.
- Therefore, the number of nitrogen atoms = 1 mole of N2 × 2 atoms/molecule = 2 moles of nitrogen atoms.
- In terms of atoms, this is equal to 2 × 6.022 × 10²³ = 1.2044 × 10²⁴ nitrogen atoms.

2. **Option 2: 500 ml of 2.0 M NH3**
- Molarity (M) = moles of solute/volume of solution (in liters).
- Volume = 500 ml = 0.5 liters.
- Moles of NH3 = Molarity × Volume = 2.0 moles/liter × 0.5 liters = 1 mole of NH3.
- Each molecule of NH3 contains 1 nitrogen atom.
- Therefore, the number of nitrogen atoms = 1 mole of NH3 × 1 atom/molecule = 1 mole of nitrogen atoms = 6.022 × 10²³ nitrogen atoms.

3. **Option 3: 6.02 × 10²³ molecules of NO2**
- The number of molecules given is 6.02 × 10²³, which is equal to 1 mole of NO2.
- Each molecule of NO2 contains 1 nitrogen atom.
- Therefore, the number of nitrogen atoms = 1 mole of NO2 × 1 atom/molecule = 1 mole of nitrogen atoms = 6.022 × 10²³ nitrogen atoms.

4. **Option 4: 1 mole of NH4Cl**
- 1 mole of NH4Cl contains 1 nitrogen atom (from the NH4+ ion).
- Therefore, the number of nitrogen atoms = 1 mole of NH4Cl × 1 atom/molecule = 1 mole of nitrogen atoms = 6.022 × 10²³ nitrogen atoms.

### Conclusion:
- Option 1 (22.4 liters of N2 at STP) contains the maximum number of nitrogen atoms, which is 2 moles of nitrogen atoms (1.2044 × 10²⁴ nitrogen atoms).
- Therefore, the correct answer is **Option 1**.