`S+HNO_(3)(Dil.) to H_(2)SO_(4)+NOuarr`

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 given reaction \( S + HNO_3 \, (Dil.) \rightarrow H_2SO_4 + NO \), we will analyze the oxidation states of the elements involved and determine the type of reaction that occurs.

### Step-by-Step Solution:

1. **Identify Reactants and Products:**
- Reactants: Sulfur (S) and Dilute Nitric Acid (HNO₃).
- Products: Sulfuric Acid (H₂SO₄) and Nitric Oxide (NO).

2. **Determine Oxidation States:**
- In elemental form, Sulfur (S) has an oxidation state of 0.
- In HNO₃, Nitrogen (N) has an oxidation state of +5.
- In H₂SO₄, Sulfur (S) has an oxidation state of +6.
- In NO, Nitrogen (N) has an oxidation state of +2.

3. **Analyze Changes in Oxidation States:**
- For Sulfur:
- Changes from 0 (in S) to +6 (in H₂SO₄).
- This indicates that Sulfur is oxidized (loss of electrons).
- For Nitrogen:
- Changes from +5 (in HNO₃) to +2 (in NO).
- This indicates that Nitrogen is reduced (gain of electrons).

4. **Classify the Reaction:**
- Since both oxidation (of Sulfur) and reduction (of Nitrogen) are occurring simultaneously, this is classified as a **redox reaction**.
- Specifically, it can be categorized as an **intermolecular redox reaction** because it involves the transfer of electrons between different molecules (S and HNO₃).

5. **Eliminate Incorrect Options:**
- The reaction is not a disproportionation reaction (where a single substance is both oxidized and reduced).
- It is not a comproportionation reaction (where two different oxidation states of the same element react).
- It is not a thermal combination or decomposition reaction since the reaction occurs at room temperature without additional thermal energy.

6. **Final Conclusion:**
- The correct classification of the reaction is as an **intermolecular redox reaction**.