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The rate constant of a first order react...

The rate constant of a first order reaction follows the equation `logk(s^(-1))=22.3-(12.16xx10^(3))/(T)K`
Find the activation energy of the reaction.

Text Solution

Verified by Experts

According to the Arrhenius equation,
`logk=logA-(E_(a))/(2.303R)xx(1)/(T)" "... [1]`
Comparing the given equation with equation[1] gives `(E_(a))/(2.303R)=12.16xx10^(3)`
or , `E_(a)=12.16xx10^(3)xx2.3030xx8.314"J.mol"^(-1)`
`-232.32"kJ.mol"^(-1)`
Thus the activation energy of the reaction `=232.82"kJ.mol"^(-1)`
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Knowledge Check

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