`E^(@)` values of `Mg^(2+)//Mg` is `-2.37V,` of `Zn^(2+)//Zn` is `-0.76V` and `Fe^(2+)// Fe` is - `0.44V`
Which of the statement is correct ?

Options

A. Zn will reduce `Fe^(2+)`
B. Zn will reducing `Mg^(2+)`
C. Mg oxidises Fe
D. Zn oxidises Fe

Explanation

To solve the problem, we need to analyze the standard reduction potentials (E°) provided for the metals and determine which statements regarding their reducing and oxidizing abilities are correct.

### Step-by-Step Solution:

1. **Identify the Given Standard Reduction Potentials:**
- For \( \text{Mg}^{2+} + 2e^- \rightarrow \text{Mg} \): \( E° = -2.37 \, \text{V} \)
- For \( \text{Zn}^{2+} + 2e^- \rightarrow \text{Zn} \): \( E° = -0.76 \, \text{V} \)
- For \( \text{Fe}^{2+} + 2e^- \rightarrow \text{Fe} \): \( E° = -0.44 \, \text{V} \)

2. **Understand the Implications of the E° Values:**
- The more negative the E° value, the stronger the reducing agent. This means that:
- Magnesium (Mg) is the strongest reducing agent among the three because it has the most negative E° value (-2.37 V).
- Zinc (Zn) is the second strongest reducing agent (-0.76 V).
- Iron (Fe) is the weakest reducing agent (-0.44 V).

3. **Determine the Reducing and Oxidizing Abilities:**
- Since magnesium has the highest negative value, it can reduce both zinc and iron:
- \( \text{Mg} \) can reduce \( \text{Fe}^{2+} \) and \( \text{Zn}^{2+} \).
- Zinc can reduce iron because it has a more negative E° value than iron:
- \( \text{Zn} \) can reduce \( \text{Fe}^{2+} \).
- Iron cannot reduce magnesium or zinc because it has the least negative E° value:
- \( \text{Fe} \) cannot reduce \( \text{Mg}^{2+} \) or \( \text{Zn}^{2+} \).

4. **Evaluate the Statements:**
- **Statement 1:** Zn will reduce Fe\(^{2+}\). **(Correct)**
- **Statement 2:** Zn will reduce Mg\(^{2+}\). **(Incorrect)**
- **Statement 3:** Mg oxidizes Fe. **(Incorrect)**
- **Statement 4:** Zn oxidizes Fe. **(Incorrect)**

5. **Conclusion:**
- The only correct statement is that zinc will reduce iron.

### Final Answer:
The correct statement is: **Zn will reduce Fe\(^{2+}\)**.