1. Tardigrade
  2. Question
  3. Chemistry
  4. A arrow B The rate constants of the above reaction at 200 K and 300 K are 0.03 min -1 and 0.05 min -1 respectively. The activation energy for the reaction is J (Nearest integer) (Given: ln 10=2.3 R =8.3 JK -1 mol -1 log 5=0.70 log 3=0.48 log 2=0.30)

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Q. $A \rightarrow B$
The rate constants of the above reaction at $200 K$ and $300 K$ are $0.03 \min ^{-1}$ and $0.05 \min ^{-1}$ respectively. The activation energy for the reaction is __$J$
(Nearest integer)
(Given $: \ln 10=2.3$
$R =8.3 \,JK ^{-1} \,mol ^{-1}$
$\log 5=0.70$
$\log 3=0.48$
$\log 2=0.30)$

JEE MainJEE Main 2023Chemical Kinetics

Solution:

$\log \frac{ K _{300}}{ K _{200}}=\frac{ E _{ a }}{2.3 \times 8.314}\left(\frac{1}{ T _1}-\frac{1}{ T _2}\right) $
$ \log \frac{0.05}{0.03}=\frac{ Ea }{2.305 \times 8.314} \times\left[\frac{1}{200}-\frac{1}{300}\right] $
$E _{ a }=2519.88 J \Rightarrow E _{ a }=2520 J $