Standard potentials (E°) for some half-reactions are given below:
`Sn^(4+) + 2e rightarrow Sn^(2+) , E^(@) = + 0.15V`
`2Hg^(2+) + 2e rightarrow Hg_(2)^(2+) , E^(@) = 0.92 V`
`pbo_(2) + 4H^(+) + 2e rightarrow pb^(2+)+ 2H_(2)O , E^(@) = + 1.45 V`
Based on the above , Which one of the following statement is correct?

Options

A. `Sn^(4+)` is stronger oxidation agent than `pb^(4+)`
B. `Sn^(2+)` is a stronger reducing agent than `Hg_(2)^(2+)`
C. `pb^(2+)` is a stronger oxidation agent than `pb^(4+)`
D. `pb^(2+) is a stronger reducing agent than `sn^(2+)`

Explanation

To solve the problem, we need to analyze the given standard potentials (E°) for the half-reactions and determine which statement is correct based on the strength of oxidizing and reducing agents.

### Step-by-Step Solution:

1. **Identify the Standard Potentials (E°)**:
- For the half-reaction: \( \text{Sn}^{4+} + 2e^- \rightarrow \text{Sn}^{2+} \), \( E° = +0.15 \, \text{V} \)
- For the half-reaction: \( 2\text{Hg}^{2+} + 2e^- \rightarrow \text{Hg}_2^{2+} \), \( E° = +0.92 \, \text{V} \)
- For the half-reaction: \( \text{PbO}_2 + 4\text{H}^+ + 2e^- \rightarrow \text{Pb}^{2+} + 2\text{H}_2\text{O} \), \( E° = +1.45 \, \text{V} \)

2. **Determine the Strength of Oxidizing Agents**:
- The higher the E° value, the stronger the oxidizing agent.
- Comparing \( \text{Sn}^{4+} \) (0.15 V) and \( \text{Pb}^{4+} \) (1.45 V):
- Since \( \text{Pb}^{4+} \) has a higher E° value, it is a stronger oxidizing agent than \( \text{Sn}^{4+} \).
- Comparing \( \text{Sn}^{4+} \) (0.15 V) and \( \text{Hg}^{2+} \) (0.92 V):
- \( \text{Hg}^{2+} \) is also a stronger oxidizing agent than \( \text{Sn}^{4+} \).

3. **Determine the Strength of Reducing Agents**:
- The lower the E° value (more negative), the stronger the reducing agent.
- For \( \text{Sn}^{2+} \), the E° for oxidation is \( -0.15 \, \text{V} \).
- For \( \text{Hg}_2^{2+} \), the E° for oxidation is \( -0.92 \, \text{V} \).
- Since \( -0.15 \, \text{V} \) (for \( \text{Sn}^{2+} \)) is higher than \( -0.92 \, \text{V} \) (for \( \text{Hg}_2^{2+} \)), \( \text{Sn}^{2+} \) is a stronger reducing agent than \( \text{Hg}_2^{2+} \).

4. **Evaluate the Statements**:
- **Statement 1**: \( \text{Sn}^{4+} \) is a stronger oxidizing agent than \( \text{Pb}^{4+} \) - **Incorrect**.
- **Statement 2**: \( \text{Sn}^{2+} \) is a stronger reducing agent than \( \text{Hg}^{2+} \) - **Incorrect**.
- **Statement 3**: \( \text{Pb}^{2+} \) is a stronger oxidizing agent than \( \text{Pb}^{4+} \) - **Incorrect**.
- **Statement 4**: \( \text{Pb}^{2+} \) is a stronger reducing agent than \( \text{Sn}^{2+} \) - **Correct**.

### Conclusion:
The correct statement is **Statement 4**: \( \text{Pb}^{2+} \) is a stronger reducing agent than \( \text{Sn}^{2+} \).