`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 question regarding the decomposition of \( N_2O_3 \) into \( NO \) and \( NO_2 \), we will follow these steps:

### Step-by-Step Solution:

1. **Identify the Reaction**:
The reaction given is:
\[ N_2O_3 \overset{(R.T.)}{\rightarrow} NO + NO_2 \]
This indicates that \( N_2O_3 \) is breaking down into two products: nitric oxide (\( NO \)) and nitrogen dioxide (\( NO_2 \)).

2. **Classify the Reaction**:
Since a single reactant (\( N_2O_3 \)) is decomposing into two products, this is classified as a **decomposition reaction**.

3. **Determine the Type of Decomposition**:
The reaction occurs at room temperature (R.T.), which indicates that it is a **thermal decomposition reaction**.

4. **Analyze Oxidation States**:
To further analyze the reaction, we need to determine the oxidation states of nitrogen in the reactants and products:
- In \( N_2O_3 \):
- Let the oxidation state of nitrogen be \( x \).
- The equation for the oxidation state is:
\[ 2x + 3(-2) = 0 \implies 2x - 6 = 0 \implies 2x = 6 \implies x = +3 \]
So, nitrogen in \( N_2O_3 \) has an oxidation state of +3.

- In \( NO \):
- The oxidation state of nitrogen is +2 (since oxygen is -2).

- In \( NO_2 \):
- The oxidation state of nitrogen is +4 (since oxygen is -2).

5. **Identify Oxidation and Reduction**:
- Nitrogen in \( N_2O_3 \) goes from +3 to +2 in \( NO \) (reduction).
- Nitrogen in \( N_2O_3 \) goes from +3 to +4 in \( NO_2 \) (oxidation).
- Since one species is oxidized and another is reduced, this is a **disproportionation reaction**.

6. **Conclusion**:
The correct classifications for the reaction are:
- It is a **decomposition reaction**.
- It is also a **disproportionation reaction**.

### Final Answer:
The reaction \( N_2O_3 \rightarrow NO + NO_2 \) is a **decomposition reaction** and a **disproportionation reaction**.