When `N_(2)` is converted into `NH_(3)`, the equivalent weight of nitrogen will be:

Options

A. (a)`1.67`
B. (b)`2.67`
C. (c )`3.67`
D. (d)`4.67`

Explanation

To find the equivalent weight of nitrogen when it is converted from \(N_2\) to \(NH_3\), we can follow these steps:

### Step 1: Determine the change in oxidation state
- In \(N_2\), the oxidation state of nitrogen is 0.
- In \(NH_3\), the oxidation state of nitrogen is +3.
- The change in oxidation state for one nitrogen atom is \(3 - 0 = 3\).

### Step 2: Calculate the total change for two nitrogen atoms
- Since there are two nitrogen atoms in \(N_2\), the total change in oxidation state is:
\[ \text{Total change} = 2 \times 3 = 6 \]

### Step 3: Determine the molecular weight of nitrogen
- The molecular weight of \(N_2\) is calculated as:
\[ \text{Molecular weight of } N_2 = 2 \times \text{Atomic weight of nitrogen} = 2 \times 14 = 28 \text{ g/mol} \]

### Step 4: Calculate the equivalent weight
- The equivalent weight is given by the formula:
\[ \text{Equivalent weight} = \frac{\text{Molecular weight}}{N \text{ factor}} \]
- Here, \(N \text{ factor} = 6\) (from Step 2).
- Therefore, the equivalent weight of nitrogen is:
\[ \text{Equivalent weight} = \frac{28}{6} \approx 4.67 \text{ g/equiv} \]

### Final Answer
The equivalent weight of nitrogen when \(N_2\) is converted into \(NH_3\) is approximately **4.67 g/equiv**.

---