`KMnO_(4)` in excess on treatment with concentrated `H_(2)SO_(4)` forms a compound (X) which decomposes explosively on heating forming (Y). The (X) and (Y) are respectively.

Options

A. `Mn_(2)O_(7),MnO_(2)`
B. `Mn_(2)O_(7),Mn_(2)O_(3)`
C. `MnSO_(4),Mn_(2)O_(3)`
D. `Mn_(2)O_(3),MnO_(2)`

Explanation

To solve the question, we need to identify the compounds formed when potassium permanganate (KMnO₄) reacts with concentrated sulfuric acid (H₂SO₄) and subsequently decomposes upon heating.

### Step-by-Step Solution:

1. **Identify the Reaction**:
When potassium permanganate (KMnO₄) reacts with concentrated sulfuric acid (H₂SO₄), it forms manganese heptoxide (Mn₂O₇) and potassium sulfate (K₂SO₄) along with water (H₂O).

The balanced chemical equation for this reaction is:
\[ 2 KMnO₄ + 3 H₂SO₄ \rightarrow Mn₂O₇ + K₂SO₄ + 3 H₂O \]

Here, the compound formed (X) is manganese heptoxide (Mn₂O₇).

2. **Decomposition of Compound X**:
Manganese heptoxide (Mn₂O₇) is known to be highly explosive and decomposes upon heating. The decomposition reaction produces manganese dioxide (MnO₂) and oxygen gas (O₂).

The balanced equation for the decomposition is:
\[ 2 Mn₂O₇ \rightarrow 4 MnO₂ + O₂ \]

In this reaction, the product formed (Y) is manganese dioxide (MnO₂).

3. **Final Identification**:
- Compound X is Mn₂O₇ (manganese heptoxide).
- Compound Y is MnO₂ (manganese dioxide).

### Conclusion:
Thus, the compounds (X) and (Y) are:
- X = Mn₂O₇ (manganese heptoxide)
- Y = MnO₂ (manganese dioxide)