1. Tardigrade
  2. Question
  3. Chemistry
  4. The rate constant of the first-order reaction, i.e., decomposition of ethylene oxide into CH 4 and CO may be described by the following equation: log k s -1=14.34 -(1.25 × 104/ T ) K Find the energy of activation (in kJ / mole ). Report answer till the nearest integer.

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Q. The rate constant of the first-order reaction, i.e., decomposition of ethylene oxide into $CH _{4}$ and $CO$ may be described by the following equation: $\log\, k\, s ^{-1}=14.34$ $-\frac{1.25 \times 10^{4}}{ T } K$
Find the energy of activation (in $kJ / mole$ ). Report answer till the nearest integer.

NTA AbhyasNTA Abhyas 2022

Solution:

$\log \,k =14.34-\frac{1.25 \times 10^{4}}{ T } K$
Comparing with the standard form of Arrhenius equation:
$\log k=\log A-\frac{ Ba }{2.303 RT }$
$\frac{ Ea }{2.303 R }=1.25 \times 10^{4} $
$ Ea =\frac{2.303 \times 8.314 \times 1.25 \times 10^{4}}{1000} kJ / mole$
$ Ea =239.34\, kJ / mole$