`NH_(3)+Ocl^(ɵ)toN_(2)H_(4)+Cl^(ɵ)`
On balancing the above equation in basic solution, using integral coefficient, which of the following whole number of will be the coefficient of `N_(2)H_(4)`?

Options

A. 1
B. 2
C. 3
D. 4

Explanation

To balance the chemical equation \( \text{NH}_3 + \text{OCl}^- \rightarrow \text{N}_2\text{H}_4 + \text{Cl}^- \) in a basic solution using integral coefficients, we can follow these steps:

### Step 1: Identify Oxidation States
First, we need to determine the oxidation states of the elements involved in the reaction:
- In \( \text{NH}_3 \), nitrogen (N) has an oxidation state of -3.
- In \( \text{OCl}^- \), chlorine (Cl) has an oxidation state of +1.
- In \( \text{N}_2\text{H}_4 \), nitrogen (N) has an oxidation state of -2.
- In \( \text{Cl}^- \), chlorine (Cl) has an oxidation state of -1.

### Step 2: Identify Oxidation and Reduction
Next, we can identify which species are oxidized and reduced:
- Nitrogen in \( \text{NH}_3 \) is oxidized from -3 to -2 (oxidation).
- Chlorine in \( \text{OCl}^- \) is reduced from +1 to -1 (reduction).

### Step 3: Write Half-Reactions
Now, we can write the half-reactions for oxidation and reduction:
1. **Oxidation Half-Reaction**:
\[ 2 \text{NH}_3 \rightarrow \text{N}_2\text{H}_4 + 2 \text{H}^+ + 2 e^- \]
2. **Reduction Half-Reaction**:
\[ \text{OCl}^- + 2 \text{H}_2\text{O} + 2 e^- \rightarrow \text{Cl}^- + 2 \text{H}^+ \]

### Step 4: Combine Half-Reactions
Now, we combine the two half-reactions:
- The electrons cancel out:
\[ 2 \text{NH}_3 + \text{OCl}^- + 2 \text{H}_2\text{O} \rightarrow \text{N}_2\text{H}_4 + \text{Cl}^- + 2 \text{H}^+ \]

### Step 5: Simplify the Equation
After canceling out the common species (2 \( \text{H}^+ \) on both sides), we get:
\[ 2 \text{NH}_3 + \text{OCl}^- \rightarrow \text{N}_2\text{H}_4 + \text{Cl}^- \]

### Step 6: Determine Coefficient of \( \text{N}_2\text{H}_4 \)
From the balanced equation, we can see that the coefficient of \( \text{N}_2\text{H}_4 \) is **1**.

### Final Answer
The coefficient of \( \text{N}_2\text{H}_4 \) in the balanced equation is **1**.

---