`E^(c-)` of `Mg^(2+)|Mg,Zn^(2+)|Zn`, and `Fe^(2+)|Fe` are `-2.37V,-0.76V`, and `-0.44V`, respectively. Which of the following is correct ?

Options

A. `Mg` oxidize `Fe`
B. `Zn` oxidizes `Fe`
C. `Zn` reduces `Mg^(2+)`
D. `Zn` reduces `Fe^(2+)`

Explanation

To solve the problem, we need to analyze the given standard reduction potentials and determine which species can oxidize or reduce the others based on their reduction potentials.

### Step-by-Step Solution:

1. **Identify the Given Standard Reduction Potentials:**
- \( E^\circ \) of \( Mg^{2+}/Mg \) = -2.37 V
- \( E^\circ \) of \( Zn^{2+}/Zn \) = -0.76 V
- \( E^\circ \) of \( Fe^{2+}/Fe \) = -0.44 V

2. **Determine the Oxidizing and Reducing Agents:**
- The species with a higher (less negative) reduction potential is a better oxidizing agent.
- Among the given potentials, \( Fe^{2+}/Fe \) has the highest reduction potential (-0.44 V), making it the strongest oxidizing agent.
- The order of oxidizing power (from strongest to weakest) is:
- \( Fe^{2+}/Fe \) > \( Zn^{2+}/Zn \) > \( Mg^{2+}/Mg \)

3. **Evaluate Each Statement:**
- **Statement 1:** Mg will oxidize Fe.
- Incorrect, as Mg has a lower reduction potential than Fe.
- **Statement 2:** Zn will oxidize Fe.
- Incorrect, as Zn has a lower reduction potential than Fe.
- **Statement 3:** Zn will reduce Mg²⁺.
- Incorrect, as Zn cannot reduce Mg²⁺ since it has a lower reduction potential.
- **Statement 4:** Zn will reduce Fe²⁺.
- Correct, as Zn has a higher reduction potential than Mg and can reduce Fe²⁺.

4. **Conclusion:**
- The only correct statement is that **Zn will reduce Fe²⁺**, making option D the correct choice.

### Final Answer:
**The correct statement is:** Zn will reduce Fe²⁺.