`NaNO_(3)+H_(2)SO_(4)(Conc.) overset(Hot) to Na_(2)SO_(4)+NO_(2)uarr+O_(2)uarr`

Options

A. For disproportionation reaction.
B. For comproportionation reaction.
C. For either intermolecular redox reaction or displacement reaction
D. For either thermal combination redox reaction or thermal decomposition redox reaction.

Answer

To solve the question regarding the reaction of sodium nitrate (NaNO₃) with concentrated sulfuric acid (H₂SO₄) when heated, we need to analyze the type of reaction taking place. The reaction can be represented as follows:

**Given Reaction:**
\[ \text{NaNO}_3 + \text{H}_2\text{SO}_4 \xrightarrow{\text{Hot}} \text{Na}_2\text{SO}_4 + \text{NO}_2 \uparrow + \text{O}_2 \uparrow \]

### Step-by-Step Solution:

1. **Identify the Reactants and Products:**
- Reactants: Sodium nitrate (NaNO₃) and concentrated sulfuric acid (H₂SO₄).
- Products: Sodium sulfate (Na₂SO₄), nitrogen dioxide (NO₂), and oxygen (O₂).

2. **Determine the Changes in Oxidation States:**
- In sodium nitrate (NaNO₃), nitrogen is in the +5 oxidation state.
- In nitrogen dioxide (NO₂), nitrogen is in the +4 oxidation state.
- The oxygen in the reactants is in the -2 oxidation state and remains -2 in the products (O₂).

3. **Classify the Reaction:**
- The nitrogen in NaNO₃ is being reduced from +5 to +4 (gaining electrons) to form NO₂.
- The oxygen is being oxidized from -2 to 0 (losing electrons) to form O₂.
- Since one element (nitrogen) is undergoing both oxidation and reduction, this is a **disproportionation reaction**.

4. **Conclusion:**
- The reaction is classified as a **disproportionation reaction** because a single species (nitrogen in NaNO₃) is being transformed into two different oxidation states (NO₂ and O₂).

### Final Answer:
The type of reaction is a **disproportionation reaction**.