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_(a) propa^(@)`
D. None of these

Explanation

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

### Step 1: Write the Reaction
The decomposition of \( N_2O_5 \) is given as:
\[ 2N_2O_5 \rightarrow 4NO_2 + O_2 \]

### Step 2: Determine Molecularity
Molecularity refers to the number of reactant molecules that participate in a single step of a reaction. In this case, we have 2 molecules of \( N_2O_5 \) reacting to form products. Therefore, the molecularity of this reaction is:
- **Molecularity = 2** (since 2 molecules of \( N_2O_5 \) are involved)

### Step 3: Identify the Order of Reaction
The question states that the reaction follows first-order kinetics. In first-order reactions, the rate of reaction is directly proportional to the concentration of one reactant.

### Step 4: Analyze the Options
1. **Option 1: The reaction is bimolecular.**
- This is correct because there are 2 molecules of \( N_2O_5 \) involved in the reaction.

2. **Option 2: The reaction is unimolecular.**
- This is incorrect as there are 2 molecules involved, not 1.

3. **Option 3: The time is directly proportional to the concentration to the power 0.**
- This is correct because in first-order reactions, the half-life is independent of the initial concentration, which can be interpreted as being proportional to concentration raised to the power of 0.

4. **Option 4: None of these.**
- This is incorrect since we have already identified correct options.

### Conclusion
The correct answers are:
- Option 1: The reaction is bimolecular.
- Option 3: The time is directly proportional to the concentration to the power 0.