Identify the correct oxidant and reductant in the following reaction :
`PbS+4H_(2)O_(2)toPbSO_(4)+4H_(2)O`

Options

A. pbs - Oxidant
`H_(2)O_(2)` - Reductant
B. pbs - Reductant
`PbSO_(4)` - Oxidant
C. PbS - Reductant
`H_(2)O_(2)` - Oxidant
D. `H_(2)O_(2)` - Oxidant
`H_(2)O` - Reductant

Explanation

To identify the correct oxidant and reductant in the reaction \( \text{PbS} + 4 \text{H}_2\text{O}_2 \rightarrow \text{PbSO}_4 + 4 \text{H}_2\text{O} \), we will follow these steps:

### Step 1: Understand Oxidation and Reduction
- **Oxidation** is defined as the gain of oxygen or the loss of electrons.
- **Reduction** is defined as the loss of oxygen or the gain of electrons.

### Step 2: Analyze the Reaction
The given reaction is:
\[ \text{PbS} + 4 \text{H}_2\text{O}_2 \rightarrow \text{PbSO}_4 + 4 \text{H}_2\text{O} \]

### Step 3: Identify Changes in Oxidation States
1. **Lead in PbS**:
- In PbS, lead (Pb) is in the oxidation state of +2.
- In PbSO4, lead (Pb) is also in the oxidation state of +2.
- Therefore, the oxidation state of lead does not change.

2. **Sulfur in PbS**:
- In PbS, sulfur (S) is in the oxidation state of -2.
- In PbSO4, sulfur (S) is in the oxidation state of +6.
- This indicates that sulfur is losing electrons (gaining oxygen), which means it is being oxidized.

3. **Hydrogen Peroxide (H2O2)**:
- In H2O2, oxygen is in the oxidation state of -1.
- In H2O, oxygen is in the oxidation state of -2.
- This indicates that oxygen in H2O2 is gaining electrons (losing oxygen), which means it is being reduced.

### Step 4: Identify the Oxidant and Reductant
- **Oxidant (Oxidizing Agent)**: The substance that is reduced (gains electrons) and causes oxidation in another substance. In this reaction, \( \text{H}_2\text{O}_2 \) is the oxidant because it is being reduced (losing oxygen).

- **Reductant (Reducing Agent)**: The substance that is oxidized (loses electrons) and causes reduction in another substance. In this reaction, \( \text{PbS} \) is the reductant because it is being oxidized (gaining oxygen).

### Conclusion
- **Oxidant**: \( \text{H}_2\text{O}_2 \)
- **Reductant**: \( \text{PbS} \)