Half life of a first order chemical reaction is 69 hr at 300 K. Also , rate of this reaction is doubled as temperature is increased from 300 K to 310 K. Determine activation energy and pre - exponential factor for this reaction.

Explanation

To solve the problem step-by-step, we will follow the necessary calculations to determine the activation energy (Ea) and the pre-exponential factor (A) for the given first-order reaction.

### Step 1: Determine the rate constant (k1) at 300 K

The half-life (t1/2) of a first-order reaction is given by the formula:

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