N2O5( g) → 0{8) 2 NO2(g) + (8 F0 t1/2 = 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 1013 s-1, determine the value of k at 50°C.

N2O5( g) → 0{8) 2 NO2(g) + (8 F0 t1/2 = 20.5 h at 20°C and 3.5h at 40°C. (a) Calculate the activation energy of this reaction. (b) If the Arrhenius constant A = 2.5 x 1013 s-1, determine the value of k at 50°C.

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 101QRT

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Question

For the first-order reaction
N2O5( g)
• 2 NO:(8) +0x8)
t1/2 = 20.5 h at 20°C and 3.5h at 40°C.
(a) Calculate the activation energy of this reaction.
(b) If the Arrhenius constant A = 2.5 x 1013 s-1,
determine the value of k at 50°C.
3.

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