Number of moles of ferrous sulphate oxidised by 1 mole of potassium permanganate in acidic medium is

Options

A. `2/5`
B. `5/2`
C. `1/5`
D. 5

Answer

To determine the number of moles of ferrous sulfate (FeSO4) oxidized by 1 mole of potassium permanganate (KMnO4) in acidic medium, we can follow these steps:

### Step 1: Write the balanced chemical equation
The reaction between potassium permanganate and ferrous sulfate in acidic medium can be represented as follows:

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

### Step 2: Balance the equation
Balancing the equation involves ensuring that the number of atoms of each element is the same on both sides. The balanced reaction is:

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

### Step 3: Analyze the stoichiometry
From the balanced equation, we see that:
- 2 moles of KMnO4 react with 10 moles of FeSO4.

### Step 4: Determine the ratio
To find out how many moles of FeSO4 are oxidized by 1 mole of KMnO4, we can set up a ratio based on the balanced equation:

\[ \frac{10 \text{ moles of FeSO}_4}{2 \text{ moles of KMnO}_4} = 5 \text{ moles of FeSO}_4 \text{ per mole of KMnO}_4 \]

### Conclusion
Thus, 1 mole of potassium permanganate oxidizes 5 moles of ferrous sulfate in acidic medium.

### Final Answer
The number of moles of ferrous sulfate oxidized by 1 mole of potassium permanganate in acidic medium is **5 moles**.

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