Looking for classes? Ksquare Career Institute, Bengaluru →
Half-life period of a first-order reaction is 1386 seconds. The specific rate constant of the reaction is
A
$5.0\times10^{-2}\ s^{-1}$
B
$5.0\times10^{-3}\ s^{-1}$
C
$0.5\times10^{-2}\ s^{-1}$
D
$0.5\times10^{-3}\ s^{-1}$
Detailed Solution
For a first order reaction: $t_{1/2} = \frac{0.693}{k}$
$k = \frac{0.693}{t_{1/2}} = \frac{0.693}{1386}$
$k = 5.0\times10^{-4}\ s^{-1}$
$k = 0.5\times10^{-3}\ s^{-1}$
$k = \frac{0.693}{t_{1/2}} = \frac{0.693}{1386}$
$k = 5.0\times10^{-4}\ s^{-1}$
$k = 0.5\times10^{-3}\ s^{-1}$