`N_(2)O_(3) overset(R.T.) to NO+NO_(2)`

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 \( N_2O_3 \) at room temperature producing \( NO + NO_2 \), we will analyze the oxidation states of nitrogen in the reactants and products to determine the type of reaction.

### Step-by-Step Solution:

1. **Identify the Reactants and Products**:
The reactant is \( N_2O_3 \) and the products are \( NO \) (nitric oxide) and \( NO_2 \) (nitrogen dioxide).

2. **Determine the Oxidation States**:
- In \( N_2O_3 \), the oxidation state of nitrogen can be calculated as follows:
- Let the oxidation state of nitrogen be \( x \).
- The formula for \( N_2O_3 \) gives: \( 2x + 3(-2) = 0 \) (since oxygen has an oxidation state of -2).
- Solving this: \( 2x - 6 = 0 \) → \( 2x = 6 \) → \( x = +3 \).
- Therefore, the oxidation state of nitrogen in \( N_2O_3 \) is +3.
- In \( NO \), the oxidation state of nitrogen is +2.
- In \( NO_2 \), the oxidation state of nitrogen is +4.

3. **Analyze Changes in Oxidation States**:
- From \( N_2O_3 \) to \( NO \):
- The oxidation state changes from +3 to +2 (reduction).
- From \( N_2O_3 \) to \( NO_2 \):
- The oxidation state changes from +3 to +4 (oxidation).

4. **Identify the Type of Reaction**:
- Since one part of the reactant \( N_2O_3 \) is oxidized (to \( NO_2 \)) and another part is reduced (to \( NO \)), this is a classic example of a disproportionation reaction.
- In a disproportionation reaction, a single reactant is both oxidized and reduced, resulting in two different products.

5. **Conclusion**:
- The reaction \( N_2O_3 \) at room temperature producing \( NO + NO_2 \) is classified as a **disproportionation reaction**.

### Final Answer:
The correct option for the type of reaction is **disproportionation reaction**.

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