0.108 g of finely divided copper was treated with an excess of ferric sulphate solution untill Cu was completely dissolved. The solution after the addition of excess dil `H_2SO_4`, required `33.7mL` of 0.1 N `KMnO_4` for complete oxidation. Find the equation which represents the reaction between metallic copper and ferric sulphate solution. `(Cu=63.7,Fe=56)`

Explanation

To solve the problem step by step, we need to determine the reaction between metallic copper (Cu) and ferric sulfate (Fe₂(SO₄)₃) and how it relates to the subsequent oxidation by potassium permanganate (KMnO₄).

### Step 1: Determine the milliequivalents of KMnO₄ used
Given that 33.7 mL of 0.1 N KMnO₄ was used, we can calculate the milliequivalents of KMnO₄.

\[ \text{Milliequivalents of KMnO₄} = \text{Volume (mL)} \times \text{Normality (N)} = 33.7 \, \text{mL} \times 0.1 \, \text{N} = 3.37 \, \text{meq} \]
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