`E^(@)` of `Fe^(2 +) //Fe = - 0.44 V, E^(@) ` of `Cu //Cu^(2+) = -0.34 V` .
Then in the cell

Options

A. `Cu^(2+)` Oxidizes Fe
B. `Fe^(2+)` oxidizes Cu
C. Cu Reduces `Fe^(2+)`
D. Fe reduces `Cu^(2+)`

Answer

To solve the question, we need to analyze the given standard reduction potentials and determine the correct statements regarding the redox reactions between Fe and Cu ions.

### Step-by-Step Solution:

1. **Identify the Given Standard Reduction Potentials:**
- For the reaction \( \text{Fe}^{2+} + 2e^- \rightarrow \text{Fe} \), the standard reduction potential \( E^\circ = -0.44 \, \text{V} \).
- For the reaction \( \text{Cu}^{2+} + 2e^- \rightarrow \text{Cu} \), the standard reduction potential \( E^\circ = -0.34 \, \text{V} \).

2. **Convert the Oxidation Potential of Cu:**
- The oxidation potential of \( \text{Cu}^{2+} \) can be derived from its reduction potential:
\[ E^\circ \text{ (oxidation of Cu)} = -E^\circ \text{ (reduction of Cu)} = -(-0.34 \, \text{V}) = +0.34 \, \text{V} \]

3. **Determine the Reaction Tendencies:**
- A more positive \( E^\circ \) value indicates a stronger tendency to be reduced (act as an oxidizing agent).
- A more negative \( E^\circ \) value indicates a stronger tendency to be oxidized (act as a reducing agent).

4. **Analyze the Reactions:**
- Since \( E^\circ \text{ (Fe)} = -0.44 \, \text{V} \) (more negative), Fe will act as a reducing agent and will oxidize (lose electrons).
- Since \( E^\circ \text{ (Cu)} = +0.34 \, \text{V} \) (more positive), Cu will act as an oxidizing agent and will reduce (gain electrons).

5. **Evaluate the Statements:**
- **Statement 1:** \( \text{Cu}^{2+} \) oxidizes Fe.
- Incorrect, because \( \text{Cu}^{2+} \) is a strong oxidizing agent and will not oxidize Fe.
- **Statement 2:** \( \text{Fe}^{2+} \) oxidizes Cu.
- Incorrect, because \( \text{Fe}^{2+} \) cannot oxidize Cu as it is a weaker oxidizing agent.
- **Statement 3:** Cu reduces \( \text{Fe}^{2+} \).
- Incorrect, because Cu does not donate electrons; it gains electrons instead.
- **Statement 4:** Fe reduces \( \text{Cu}^{2+} \).
- Correct, because Fe donates electrons to \( \text{Cu}^{2+} \), reducing it to Cu.

### Conclusion:
The correct statement is that **Fe reduces \( \text{Cu}^{2+} \)**.