One mole of `KMnO_(4)` is used for complete oxidation of `FeSO_(4), FeC_(2)O_(4)` and `H_(2)C_(2)O_(4)` respectively and separately. Pick up the correct statement.

Options

A. 5 mole of `FeSO_(4)` can be oxidised
B. 3/5 mole of `FeC_(2)O_(4)` can be oxidized
C. 5/3 mole of `FeC_(2)O_(4)` can be oxidized
D. 2.5 mole of `H_(2)C_(2)O_(5)` canbe oxidized

Answer

To solve the problem, we need to determine how many moles of `FeSO4`, `FeC2O4`, and `H2C2O4` can be oxidized by one mole of `KMnO4`. Let's go through the steps systematically.

### Step 1: Understand the oxidation reactions
We need to write the balanced chemical equations for the oxidation of `FeSO4`, `FeC2O4`, and `H2C2O4` by `KMnO4`.

### Step 2: Balance the reaction for `FeSO4`
The balanced reaction for the oxidation of `FeSO4` by `KMnO4` is:
\[ \text{MnO}_4^- + 8 \text{H}^+ + 5 \text{Fe}^{2+} \rightarrow \text{Mn}^{2+} + 5 \text{Fe}^{3+} + 4 \text{H}_2\text{O} \]
From this equation, we can see that 1 mole of `KMnO4` oxidizes 5 moles of `FeSO4`.

### Step 3: Balance the reaction for `H2C2O4`
The balanced reaction for the oxidation of `H2C2O4` (oxalic acid) by `KMnO4` is:
\[ 2 \text{KMnO}_4 + 5 \text{H}_2\text{C}_2\text{O}_4 + 6 \text{H}_2\text{SO}_4 \rightarrow 2 \text{MnSO}_4 + 10 \text{CO}_2 + 8 \text{H}_2\text{O} \]
From this equation, we can see that 1 mole of `KMnO4` oxidizes 2.5 moles of `H2C2O4`.

### Step 4: Balance the reaction for `FeC2O4`
The balanced reaction for the oxidation of `FeC2O4` by `KMnO4` can be written as:
\[ 6 \text{KMnO}_4 + 5 \text{FeC}_2\text{O}_4 + 24 \text{H}_2\text{SO}_4 \rightarrow 3 \text{K}_2\text{SO}_4 + 6 \text{MnSO}_4 + 5 \text{Fe}_2\text{SO}_4 + 20 \text{CO}_2 + 24 \text{H}_2\text{O} \]
From this equation, we can see that 1 mole of `KMnO4` oxidizes 2.5 moles of `FeC2O4`.

### Conclusion
From the balanced equations, we can summarize:
- 1 mole of `KMnO4` can oxidize **5 moles of `FeSO4`**.
- 1 mole of `KMnO4` can oxidize **2.5 moles of `H2C2O4`**.
- 1 mole of `KMnO4` can oxidize **2.5 moles of `FeC2O4`**.

### Final Answer
Thus, the correct statements based on the oxidation capabilities of `KMnO4` are:
- Option A: 5 moles of `FeSO4` can be oxidized by 1 mole of `KMnO4`.
- Option C: 2.5 moles of `H2C2O4` can be oxidized by 1 mole of `KMnO4`.
- Option D: 2.5 moles of `FeC2O4` can be oxidized by 1 mole of `KMnO4`.