`E^(o)` value of `Mg^(2+)|Mg,Fe^(2+)|Fe and Zn^(2+) | Zn" are " - 2.37 V, - 0.44 and - 0.76 V` respectively. The correct statement is :

Options

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

Answer

To solve the question regarding the standard electrode potentials (E°) of the given half-cells, we will analyze the values provided and determine the correct statement based on the reduction potentials.

### Step-by-Step Solution:

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

2. **Understand the Meaning of E° Values**:
- The more negative the E° value, the less likely the species is to be reduced (i.e., it has a higher tendency to oxidize).
- Conversely, a less negative or more positive E° value indicates a greater tendency to be reduced.

3. **Rank the Electrode Potentials**:
- From the values:
- \( \text{Mg}^{2+}/\text{Mg} \) has the lowest reduction potential (-2.37 V), indicating it is the strongest reducing agent.
- \( \text{Zn}^{2+}/\text{Zn} \) is next (-0.76 V).
- \( \text{Fe}^{2+}/\text{Fe} \) has the highest reduction potential (-0.44 V), indicating it is the weakest reducing agent among the three.

4. **Determine Which Species Can Reduce Others**:
- Since \( \text{Mg} \) is the strongest reducing agent, it can reduce both \( \text{Zn}^{2+} \) and \( \text{Fe}^{2+} \).
- \( \text{Zn} \) can reduce \( \text{Fe}^{2+} \) to \( \text{Fe} \) because \( -0.76 \, \text{V} \) (Zn) is less negative than \( -0.44 \, \text{V} \) (Fe).
- \( \text{Fe} \) cannot reduce \( \text{Zn} \) or \( \text{Mg} \) because its reduction potential is higher than both.

5. **Conclusion**:
- The correct statement is that \( \text{Zn} \) can reduce \( \text{Fe}^{2+} \) to \( \text{Fe} \).

### Final Answer:
The correct statement is: **Zn reduces Fe²⁺ to Fe.**

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