If a reaction has a rate constant of 3.7 x 10-3 s-1 at 25oC, and an activation energy of 43.6 kJ/mol, what will be the rate constant for this reaction at 75oC?

Question

Bradyn Daniels

Physics

27 January, 09:48

If a reaction has a rate constant of 3.7 x 10-3 s-1 at 25oC, and an activation energy of 43.6 kJ/mol, what will be the rate constant for this reaction at 75oC?

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Answers (1)

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Braylon Bean · Answer 1

The rate constant for the reaction at 75 °C = 4.6 * 10^ (-2) s^ (-1)

Explanation:

By Arrhenius equitation

k = Ae^ (-Ea / (RT))

Therefore

3.7 x 10-3 s-1 = A*e^ (43600J/mol / (8.3145*298))

Therefore A = 160900.320

Therefore at 75 °C T = 348.15 K and k = 160900.320*e^ (-43600 / (8.314*348.15)

k = 4.6 * 10^ (-2) s^ (-1)

the rate constant for this reaction at 75 °C is k = 4.6 * 10^ (-2) s^ (-1)

Which shows that the rate of reaction increases as temperature increases that is the proportions of effective collisions with energy equal to or greater than the activation energy increases.