The strongest oxidizing agent among the following is

Options

A. `K_(2)Cr_(2)O_(7)`
B. `MnO_(2)`
C. `KMnO_(4)`
D. `Cl_(2)`

Explanation

To determine the strongest oxidizing agent among the given options, we will compare the standard reduction potentials of each species. The species with the highest reduction potential is the strongest oxidizing agent.

### Step-by-Step Solution:

1. **Identify the Compounds**: The given compounds are:
- Potassium Dichromate (K2Cr2O7)
- Manganese Dioxide (MnO2)
- Potassium Permanganate (KMnO4)
- Chlorine (Cl2)

2. **Write the Reduction Reactions and Their Potentials**:
- For **Potassium Dichromate (K2Cr2O7)**:
\[ \text{Cr}_2\text{O}_7^{2-} + 14\text{H}^+ + 6\text{e}^- \rightarrow 2\text{Cr}^{3+} + 7\text{H}_2\text{O} \quad E^\circ = +1.33 \text{ V} \]
- For **Manganese Dioxide (MnO2)**:
\[ \text{MnO}_2 + 4\text{H}^+ + 2\text{e}^- \rightarrow \text{Mn}^{2+} + 2\text{H}_2\text{O} \quad E^\circ = +1.23 \text{ V} \]
- For **Potassium Permanganate (KMnO4)**:
\[ \text{MnO}_4^{-} + 8\text{H}^+ + 5\text{e}^- \rightarrow \text{Mn}^{2+} + 4\text{H}_2\text{O} \quad E^\circ = +1.51 \text{ V} \]
- For **Chlorine (Cl2)**:
\[ \text{Cl}_2 + 2\text{e}^- \rightarrow 2\text{Cl}^- \quad E^\circ = +1.36 \text{ V} \]

3. **Compare the Reduction Potentials**:
- Potassium Dichromate: +1.33 V
- Manganese Dioxide: +1.23 V
- Potassium Permanganate: +1.51 V
- Chlorine: +1.36 V

4. **Determine the Strongest Oxidizing Agent**:
- The highest reduction potential is for Potassium Permanganate (KMnO4) at +1.51 V. Therefore, it is the strongest oxidizing agent among the given options.

### Conclusion:
The strongest oxidizing agent among the given options is **Potassium Permanganate (KMnO4)**.