The decomposition of `N_(2)O_(5)` occurs as, `2N_(2)O_(5) rarr4NO_(2)+O_(2)` and follows `I` order kinetics, hence:

Options

A. The reaction is bimolecular
B. The reaction is unimolecular
C. `t_(1//2) prop a^(0)`
D. None of these

Explanation

To solve the question regarding the decomposition of \( N_2O_5 \) and its kinetics, we can follow these steps:

### Step-by-Step Solution:

1. **Identify the Reaction and its Order**:
The decomposition reaction given is:
\[ 2N_2O_5 \rightarrow 4NO_2 + O_2 \]
It is stated that this reaction follows first-order kinetics.

2. **Understanding Reaction Order**:
First-order kinetics means that the rate of reaction is directly proportional to the concentration of one reactant. In this case, the order of the reaction is 1.

3. **Determine Molecularity**:
Molecularity refers to the number of reactant molecules involved in the rate-determining step of the reaction. Here, since two molecules of \( N_2O_5 \) are involved in the reaction, the molecularity is 2.

4. **Relate Order and Molecularity**:
In this case, we have a first-order reaction with a bimolecular step (two molecules). This is characteristic of a pseudo-unimolecular reaction, where one reactant is in excess, and the reaction appears to be first-order with respect to the other reactant.

5. **Expression for Half-Life**:
For a first-order reaction, the half-life (\( t_{1/2} \)) is given by:
\[ t_{1/2} = \frac{0.693}{k} \]
where \( k \) is the rate constant. The half-life is independent of the initial concentration for first-order reactions.

6. **Conclusion**:
Since the reaction is first-order, and the molecularity is 2, we conclude that this reaction is an example of a pseudo-unimolecular reaction.

### Final Answer:
The decomposition of \( N_2O_5 \) follows first-order kinetics and is an example of a pseudo-unimolecular reaction.

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