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Q. The decomposition of a hydrocarbon follows the equation $k=\left(4.5\times10^{11}s^{-1}\right)e^{-28000 K /T}.$ What will be the value of activation energy?

Chemical Kinetics

Solution:

Arrhenius equation, $k=Ae^{-Ea/ RT}$
Given equation is $k =\left(4.5\times10^{11}s^{-1}\right)$ $e^{-28000 K /T}$
Comparing both the equations, we get
$-\frac{E_{a}}{RT}$ $=-\frac{28000\, K }{T}$
$E_{a}$ $=28000 K\times R=28000 K\times8.314 J K^{-1}$ $ mol^{-1}$
$=232.79 \,KJ$ $mol^{-1}$