For the reaction of H 2 with I 2 , the rate constant is 2.5 × 10 - 4 d m 3 m o l - 1 s - 1 at 327 o C and at 527 ° C is 1.0 d m 3 m o l − 1 s − 1 The activation energy for the reaction, in k J m o l −

Question

For the reaction of H 2 with I 2 , the rate constant is 2.5 × 10 - 4 d m 3 m o l - 1 s - 1 at 327 o C and at 527 ° C is 1.0 d m 3 m o l − 1 s − 1 The activation energy for the reaction, in k J m o l − 1 is: R = 8.314 J K - 1 m o l - 1

TestHub · Accepted Answer

T 2 = 527 o C ⇒ 800 k ; k 1 = 2.5 × 10 - 4 T 1 = 327 o C ⇒ 600 k ; k 2 = 1 According to Arrhenius Equation; ln ⁡ k 2 k 1 = - E a R 1 T 2 - 1 T 1 ln ⁡ 10 4 2.5 = E a R 1 600 - 1 800 ln ⁡ 4000 = E a 8.314 1 2400 E a = 165.431 k J , E a ≈ 166 k J / m o l

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