Which species are oxidised and reduced in the reaction?
`FeC_(2)O_(4)+KMnO_(4)rarrFe^(3+)+CO_(2)+Mn^(2+)`

Options

A. Oxidised:Fe,C,Reduced:Mn
B. Oxidised:Fe,Reduced:Mn
C. Reduced:Fe,Mn,Oxidised:C
D. Reduced:C,Oxidised:Mn,Fe

Answer

To determine which species are oxidized and reduced in the reaction:

\[ \text{FeC}_2\text{O}_4 + \text{KMnO}_4 \rightarrow \text{Fe}^{3+} + \text{CO}_2 + \text{Mn}^{2+} \]

we will follow these steps:

### Step 1: Identify the oxidation states of the elements in the reactants and products.

- In **FeC₂O₄** (ferrous oxalate):
- Iron (Fe) is in the +2 oxidation state.
- Each carbon (C) in oxalate (C₂O₄) is in the +3 oxidation state (calculated as follows: let the oxidation state of C be \( x \); then \( 2x + 4(-2) = 0 \) leads to \( 2x - 8 = 0 \) or \( x = +4 \)).

- In **KMnO₄** (potassium permanganate):
- Manganese (Mn) is in the +7 oxidation state.

### Step 2: Identify the oxidation states in the products.

- In **Fe³⁺**:
- Iron (Fe) is in the +3 oxidation state.

- In **CO₂**:
- Each carbon (C) is in the +4 oxidation state.

- In **Mn²⁺**:
- Manganese (Mn) is in the +2 oxidation state.

### Step 3: Determine the changes in oxidation states.

- **Iron (Fe)**:
- Changes from +2 (in FeC₂O₄) to +3 (in Fe³⁺). This is an increase in oxidation state, indicating that iron is **oxidized**.

- **Carbon (C)**:
- Changes from +3 (in C₂O₄) to +4 (in CO₂). This is also an increase in oxidation state, indicating that carbon is **oxidized**.

- **Manganese (Mn)**:
- Changes from +7 (in KMnO₄) to +2 (in Mn²⁺). This is a decrease in oxidation state, indicating that manganese is **reduced**.

### Step 4: Conclusion

In this reaction:
- **Oxidized species**: Iron (Fe) and Carbon (C)
- **Reduced species**: Manganese (Mn)

### Final Answer:
- The species that are oxidized are Fe and C, while the species that is reduced is Mn.

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