The first order reaction has `k=1.5xx10^(-6)` per second at `200^(@)C` . If the reaction is allowed to ruf for 10 hours at the same temperature, what percentage of the initial concentration would have changed into the product? What is the half life period of this reaction ?

Explanation

To solve the problem step-by-step, we will first calculate the percentage of the initial concentration that has changed into the product after 10 hours, and then we will determine the half-life period of the reaction.

### Step 1: Determine the Half-Life of the Reaction

For a first-order reaction, the half-life (\( t_{1/2} \)) is given by the formula:

\[
t_{1/2} = \frac{0.693}{k}
...