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The activation energy of a reaction at a given temperature is found to be 2.303

The activation energy of a reaction at a given temperature is found to be 2.303 RT J mol⁻¹.The ratio of rate constant to the Arrhenius factor is

Options

(a) 0.01
(b) 0.1
(c) 0.02
(d) 0.001

Correct Answer:

0.1

Explanation:

Arrhenius equation K=A.e(-Eₐ/RT)

⇒In K =In A -Eₐ/RT slop = -Eₐ/R

so,activation energy of reaction can be determined from the slop of In K vs 1/T

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