Show that for a first order reaction, time required for `99.99%` of the reaction to take place is 10 times the time required for the completion of half of the reaction.

Explanation

To show that for a first-order reaction, the time required for 99.99% of the reaction to take place is 10 times the time required for the completion of half of the reaction, we can follow these steps:

### Step 1: Understand the first-order reaction kinetics
The rate of a first-order reaction can be expressed using the integrated rate law:
\[ T = \frac{2.303}{k} \log \left( \frac{[A_0]}{[A_t]} \right) \]
where:
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