By passing `H_(2)S` in acidified `KMnO_(4)` solution we get

Options

A. (a) `S`
B. (b) `K_(2)S`
C. (c) `MnO_(2)`
D. (d) `K_(2)SO_(3)`

Explanation

To solve the question regarding the reaction that occurs when hydrogen sulfide (H₂S) is passed through acidified potassium permanganate (KMnO₄) solution, we can follow these steps:

### Step 1: Identify the Reactants
The reactants in this reaction are:
- Hydrogen sulfide (H₂S)
- Acidified potassium permanganate (KMnO₄) in the presence of sulfuric acid (H₂SO₄)

### Step 2: Understand the Reaction Conditions
The reaction takes place in an acidic medium due to the presence of sulfuric acid. KMnO₄ acts as an oxidizing agent in this acidic environment.

### Step 3: Write the Balanced Chemical Equation
The balanced chemical equation for the reaction can be written as follows:

\[ 2 \, KMnO_4 + 3 \, H_2SO_4 + 5 \, H_2S \rightarrow K_2SO_4 + 2 \, MnSO_4 + 8 \, H_2O + 5 \, S \]

### Step 4: Analyze the Oxidation and Reduction
In this reaction:
- H₂S is oxidized to sulfur (S), where sulfur changes from an oxidation state of -2 in H₂S to 0 in elemental sulfur.
- KMnO₄ is reduced; manganese changes from an oxidation state of +7 in KMnO₄ to +2 in MnSO₄.

### Step 5: Identify the Products
From the balanced equation, we can identify the products:
- Potassium sulfate (K₂SO₄)
- Manganese(II) sulfate (MnSO₄)
- Water (H₂O)
- Elemental sulfur (S)

### Step 6: Choose the Correct Answer
Among the options provided:
- Option A: Sulfur (S) - This is a product of the reaction.
- Option B: K₂S - This is not produced in the reaction.
- Option C: MnO₂ - This is not produced in the reaction.
- Option D: K₂SO₃ - This is not produced; instead, K₂SO₄ is formed.

Thus, the correct answer is **Option A: Sulfur (S)**.

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