For a reaction, the rate constant is `2.34 s^(-1)`. The half-life period for the reaction is

Options

A. 0.30 sec
B. 0.60 sec
C. 3.3 sec
D. Data is insufficient

Answer

To find the half-life period for a reaction with a given rate constant, we can follow these steps:

### Step 1: Identify the order of the reaction
The unit of the rate constant (K) is given as `s^(-1)`, which indicates that the reaction is a **first-order reaction**.

### Step 2: Use the formula for half-life of a first-order reaction
The half-life (t_half) for a first-order reaction can be calculated using the formula:
\[ t_{1/2} = \frac{0.693}{k} \]
where \( k \) is the rate constant.

### Step 3: Substitute the value of the rate constant into the formula
Given that the rate constant \( k = 2.34 \, s^{-1} \), we substitute this value into the formula:
\[ t_{1/2} = \frac{0.693}{2.34} \]

### Step 4: Perform the calculation
Now, we calculate the value:
\[ t_{1/2} = \frac{0.693}{2.34} \approx 0.296 \, seconds \]

### Step 5: Round the result
Rounding \( 0.296 \) seconds gives us approximately \( 0.30 \) seconds.

### Final Answer
Thus, the half-life period for the reaction is **0.30 seconds**.

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