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The rate constant for a certain reaction is measured at two different temperatures: temperature Assuming the rate constant obeys the Arrhenius equation, calculate the activation energy for this reaction. Round your answer to significant digits.

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Answer:

The question has some details missing which I have shown in the attached file.

Explanation:

The concept of arrehenius equation is used to calculate the activation energy.

  • Given T1 = 141.0 degree celsius = 414K and K1 = 3.3 x 10^8
  • T2 = 77 degree celsius = 350K and k2 = 1.1 x 10^8
  • R = 8.314
  • from Arrehenius equation;
  • ln(k2/k1) = -Ea/R [1/T2 - 1/T1]

  • Plugging the values ;
  • ln(1.1/3.3) = -Ea/8.314 [ 1/350 - 1/414]
  • Ea = 20.679KJ/mol = activation energy for this reaction

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