In the reaction of `Zn + FeSO_(4) to ZnSO_(4) + Fe`

Options

A. Zn gets oxidized
B. Fe gets oxidized
C. Zn is oxidising agent
D. Zn and Fe both get oxidized

Answer

To analyze the reaction `Zn + FeSO₄ → ZnSO₄ + Fe`, we need to determine the oxidation states of the elements involved and identify which species is oxidized and which is reduced.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
- Reactants: Zinc (Zn) and Iron(II) sulfate (FeSO₄)
- Products: Zinc sulfate (ZnSO₄) and Iron (Fe)

2. **Assign Oxidation States**:
- For Zinc (Zn) in the reactants:
- Zn is in the elemental form, so its oxidation state is 0.
- For Iron (Fe) in FeSO₄:
- The sulfate ion (SO₄²⁻) has an oxidation state of -2.
- Since the overall charge of FeSO₄ is neutral, the oxidation state of Fe must be +2.
- For Zinc in ZnSO₄:
- Similar to FeSO₄, the sulfate ion remains -2, so Zn must be +2 to balance it.
- For Iron (Fe) in the products:
- In its elemental form, Fe has an oxidation state of 0.

3. **Determine Changes in Oxidation States**:
- Zinc (Zn): Changes from 0 (in reactants) to +2 (in products). This indicates that Zn is oxidized.
- Iron (Fe): Changes from +2 (in reactants) to 0 (in products). This indicates that Fe is reduced.

4. **Identify the Oxidizing and Reducing Agents**:
- The substance that gets oxidized (loses electrons) is the reducing agent. Here, Zn is oxidized, so it is the reducing agent.
- The substance that gets reduced (gains electrons) is the oxidizing agent. Here, Fe is reduced, so Fe²⁺ is the oxidizing agent.

5. **Conclusion**:
- In this reaction, Zn is oxidized to Zn²⁺, and Fe²⁺ is reduced to Fe. Therefore, Zn is the reducing agent, and Fe²⁺ is the oxidizing agent.

### Final Statements:
- Zn is oxidized (0 to +2).
- Fe is reduced (+2 to 0).
- Zn acts as the reducing agent.
- Fe²⁺ acts as the oxidizing agent.