Find the number of moles of `KMnO_(4)` needed to oxidise one mole `Cu_(2)S` in acidic medium.
The reaction is `KMnO_(4) + Cu_(2)S rarr M n^(2+) + Cu^(2+) + SO_(2)`

Explanation

To find the number of moles of \( KMnO_4 \) needed to oxidize one mole of \( Cu_2S \) in acidic medium, we can follow these steps:

### Step 1: Write the balanced chemical equation
The reaction between potassium permanganate and copper sulfide can be represented as:
\[ KMnO_4 + Cu_2S \rightarrow Mn^{2+} + Cu^{2+} + SO_2 \]

### Step 2: Determine the oxidation states
In this reaction:
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