The reaction,
`10FeSO_(4) + 2KMnO_(4) + 8H_(2)SO_(4) to 2MnSO_(4) + 5Fe_(2)(SO_(4))_(3) + K_(2)SO_(4) + 8H_(2)O` is an example of reaction of

Options

A. disproportionation
B. intermolecular redox
C. intramolecular redox
D. None of these

Explanation

To determine the type of reaction represented by the equation:

\[ 10 \text{FeSO}_4 + 2 \text{KMnO}_4 + 8 \text{H}_2\text{SO}_4 \rightarrow 2 \text{MnSO}_4 + 5 \text{Fe}_2(\text{SO}_4)_3 + \text{K}_2\text{SO}_4 + 8 \text{H}_2\text{O} \]

we need to analyze the oxidation states of the elements involved in the reaction.

### Step 1: Identify Oxidation States
- In \(\text{FeSO}_4\), iron (Fe) is in the +2 oxidation state.
- In \(\text{KMnO}_4\), manganese (Mn) is in the +7 oxidation state.
- In \(\text{MnSO}_4\), manganese (Mn) is in the +2 oxidation state.
- In \(\text{Fe}_2(\text{SO}_4)_3\), iron (Fe) is in the +3 oxidation state.

### Step 2: Determine Changes in Oxidation States
- Iron (Fe) changes from +2 in \(\text{FeSO}_4\) to +3 in \(\text{Fe}_2(\text{SO}_4)_3\). This indicates that iron is oxidized.
- Manganese (Mn) changes from +7 in \(\text{KMnO}_4\) to +2 in \(\text{MnSO}_4\). This indicates that manganese is reduced.

### Step 3: Identify the Type of Reaction
Since we have one element (iron) being oxidized and another element (manganese) being reduced, this reaction is classified as a redox reaction.

### Step 4: Classify Further
This reaction can also be classified as a **disproportionation reaction** because manganese in the +7 oxidation state is being reduced to +2 while simultaneously oxidizing iron from +2 to +3.

### Conclusion
Thus, the reaction is an example of a **disproportionation reaction**.

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