For the balanced equation :
`8H^(+)(aq)+5Fe^(2+)(aq)+MnO_(4)^(-)(aq)rarr5Fe^(3+)(aq)+Mn^(2+)(aq)+4H_(2)O(l)`
Which statement is correct ?

Options

A. `Fe^(2+)` (aq) undergoes oxidation
B. `Fe^(2+)` (aq) is the oxidizing agent
C. `H^(+)` (aq) undergoes oxidation
D. `H^(+)` (aq) is the oxidizing agent

Answer

To determine which statement is correct regarding the balanced redox reaction:

\[ 8H^+(aq) + 5Fe^{2+}(aq) + MnO_4^{-}(aq) \rightarrow 5Fe^{3+}(aq) + Mn^{2+}(aq) + 4H_2O(l) \]

we will analyze the oxidation states and the roles of the species involved.

### Step 1: Identify the oxidation states
- **Iron (Fe)**:
- In \(Fe^{2+}\), the oxidation state is +2.
- In \(Fe^{3+}\), the oxidation state is +3.
- **Manganese (Mn)**:
- In \(MnO_4^{-}\), the oxidation state of Mn is +7 (since O is -2, the total for 4 O is -8, and to balance the -1 charge, Mn must be +7).
- In \(Mn^{2+}\), the oxidation state is +2.
- **Hydrogen (H)**:
- In \(H^+\), the oxidation state is +1.
- In \(H_2O\), the oxidation state of H is still +1.

### Step 2: Determine the changes in oxidation states
- **For Iron (Fe)**:
- \(Fe^{2+} \rightarrow Fe^{3+}\): The oxidation state increases from +2 to +3, indicating that Fe is oxidized.

- **For Manganese (Mn)**:
- \(MnO_4^{-} \rightarrow Mn^{2+}\): The oxidation state decreases from +7 to +2, indicating that Mn is reduced.

### Step 3: Identify the oxidizing and reducing agents
- **Oxidizing Agent**: The species that gets reduced is the oxidizing agent. Here, \(MnO_4^{-}\) is reduced to \(Mn^{2+}\).
- **Reducing Agent**: The species that gets oxidized is the reducing agent. Here, \(Fe^{2+}\) is oxidized to \(Fe^{3+}\).

### Step 4: Analyze the given statements
1. **Fe2+ undergoes oxidation**: This is correct since its oxidation state increases from +2 to +3.
2. **MnO4- is the oxidizing agent**: This is also correct since it gets reduced.
3. **H+ undergoes oxidation**: This is incorrect; H+ does not change its oxidation state in this reaction.
4. **H+ is the oxidizing agent**: This is incorrect; H+ does not act as an oxidizing agent in this reaction.

### Conclusion
The correct statement is that **Fe2+ undergoes oxidation**.

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