Question

A first order reaction is found to have a rate constant, $k=5.5\times {10}^{-14}{s}^{-1}$. Find the half-life of the reaction.

Answer 1

Given,

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

Half-life

Half-life for a first order reaction is given
by-

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

Put vale of k in above formula,

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

So, the half-life of the reaction is
$1.26\times {10}^{13}s$

Final answer: $t_{\frac{1}{2}}=1.26\times {10}^{13}s$