Given `E_(Cr^(3+)//Cr^(@))= -O*74V`,`E_(MnO_(4)^(-)//Mn^(2+))^(@) = 1.51V`
`E_(Cr_(2)O_(7)^(2-)//Cr^(3+))^(@)`= 1.33V , `E_(Cl//Cl^(-))^(@)= 1.36V`
Based on the given above , Strongest oxidising agent will be:

Options

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

Explanation

To determine the strongest oxidizing agent from the given standard electrode potentials, we will 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 indicated by its standard electrode potential (E°). The higher the E° value, the stronger the oxidizing agent.

### Step 2: List the Given Standard Electrode Potentials
We are provided with the following standard electrode potentials:
- \( E_{Cr^{3+}/Cr} = -0.74 \, V \)
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