`N_(2)+O_(2) overset("High temp.")toNOuarr`-Heat.

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 problem regarding the reaction of nitrogen and oxygen at high temperature to form nitric oxide (NO), we will analyze the reaction step by step.

### Step-by-Step Solution:

1. **Identify the Reactants and Products:**
- The reactants are nitrogen gas (N₂) and oxygen gas (O₂).
- The product formed is nitric oxide (NO).

2. **Determine the Conditions of the Reaction:**
- The reaction occurs at high temperature, which is indicated in the question.

3. **Assign Oxidation States:**
- In the reactants:
- Nitrogen (N₂) has an oxidation state of 0 (elemental form).
- Oxygen (O₂) also has an oxidation state of 0 (elemental form).
- In the product (NO):
- Nitrogen has an oxidation state of +2.
- Oxygen has an oxidation state of -2.

4. **Analyze the Changes in Oxidation States:**
- Nitrogen is oxidized from 0 to +2 (loss of electrons).
- Oxygen is reduced from 0 to -2 (gain of electrons).

5. **Classify the Reaction:**
- Since there is both oxidation and reduction occurring, this reaction is classified as a **redox reaction**.
- Additionally, since two reactants combine to form a single product (NO), it is also classified as a **combination reaction**.

6. **Identify the Type of Combination Reaction:**
- Given that the reaction is carried out at high temperature, it can be specifically categorized as a **thermal combination reaction**.

7. **Conclusion:**
- The reaction is a **redox reaction** and a **thermal combination reaction**.

### Final Answer:
The reaction \( N_2 + O_2 \overset{\text{High temp.}}{\rightarrow} NO + \text{Heat} \) is classified as both a **redox reaction** and a **thermal combination reaction**.

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