Find out which of the following is the strongest oxidizing agent.

Options

A. `Cl^(-)`
B. `Mn^(2+)`
C. `MnO_(4)^(-)`
D. `Cr^(3+)`

Explanation

To determine which of the given options is the strongest oxidizing agent, 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 measured by its standard reduction potential (E°). The higher the reduction potential, the stronger the oxidizing agent.

### Step 2: Identify the Given Options
Assuming we have a list of substances (for example, MnO4^-, MnO2, etc.), we need to evaluate their standard reduction potentials.

### Step 3: Look Up Standard Reduction Potentials
We can look up the standard reduction potentials for the substances in the options. For example:
- MnO4^- + 8H^+ + 5e^- → Mn^2+ + 4H2O (E° = +1.51 V)
- MnO2 + 4H^+ + 2e^- → Mn^2+ + 2H2O (E° = +0.15 V)

### Step 4: Compare the Reduction Potentials
By comparing the standard reduction potentials, we can determine which substance has the highest potential. In this case, MnO4^- has the highest reduction potential (+1.51 V), indicating it is the strongest oxidizing agent among the options.

### Step 5: Conclusion
Based on the comparison of the standard reduction potentials, we conclude that MnO4^- is the strongest oxidizing agent.

### Final Answer
The strongest oxidizing agent among the given options is MnO4^-.

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