A first order reaction is found to have a rate constant, $k = 5.5 × 10^{-14} s^{-1}$. The half life of the reaction will be:

$1.26 × 10^{13} s$

The correct answer is Option (2) → $1.26 × 10^{13} s$

For a first-order reaction, the half-life is given by:

$t_{1/2} = \frac{0.693}{k}$

Given:

$k = 5.5 \times 10^{-14}\ \text{s}^{-1}$

$t_{1/2} = \frac{0.693}{5.5 \times 10^{-14}} = 0.126 \times 10^{14} = 1.26 \times 10^{13}\ \text{s}$