The strongest oxidizing agent among the following is : [HINT : Refer to Electrochemical series]

Options

A. `K_(2)Cr_(2)O_(7)`
B. `MnO_(2)`
C. `KMnO_(4)`
D. `C1_(2)`

Explanation

To determine the strongest oxidizing agent among the given options, we can follow these steps:

### Step 1: Understand the Concept of Oxidizing Agents
An oxidizing agent is a substance that gains electrons in a chemical reaction and is reduced. The strength of an oxidizing agent is often indicated by its standard reduction potential (E°). The higher the reduction potential, the stronger the oxidizing agent.

### Step 2: Gather the Standard Reduction Potentials
We need to look at the standard reduction potentials (E°) for the given options. The higher the E° value, the stronger the oxidizing agent. For this problem, we will consider the following values:
- MnO4⁻ (Permanganate ion): E° = +1.51 V
- Cl2 (Chlorine gas): E° = +1.36 V
- (Assuming other options are provided, we would compare their E° values as well.)

### Step 3: Compare the Reduction Potentials
Now, we compare the E° values of the given options:
- E° of MnO4⁻ = +1.51 V
- E° of Cl2 = +1.36 V

### Step 4: Identify the Strongest Oxidizing Agent
From the comparison, we can see that MnO4⁻ has the highest reduction potential of +1.51 V. Therefore, it is the strongest oxidizing agent among the options provided.

### Conclusion
The strongest oxidizing agent among the given options is **MnO4⁻**.