For a first order reaction, show that the time required for `99%` completion is twice the time required for the completion of `90%` of reaction.

Explanation

To show that the time required for 99% completion of a first-order reaction is twice the time required for 90% completion, we can follow these steps:

### Step 1: Understand the first-order reaction equation
For a first-order reaction, the relationship between time (T), the rate constant (k), and the concentrations is given by the equation:
\[ kT = 2.303 \log \left( \frac{A_0}{A_0 - x} \right) \]
where:
- \( A_0 \) = initial concentration
- \( A \) = concentration at time T
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