Dinitrogen pentoxide decomposes according to the reaction 2N2O5 (g) 4NO2(g) + O2(g) At 45°C the rate constant is 6.2 x 10 s The reaction is first order. a What is the rate law for the reaction? Rate = k[NO2] [O2] %3D O Rate = k[N2O5]*NO2]*[O2] O Rate = k[N2 05] %3D O Rate = k[N205] %3D

Dinitrogen pentoxide decomposes according to the reaction 2N2O5 (g) 4NO2(g) + O2(g) At 45°C the rate constant is 6.2 x 10 s The reaction is first order. a What is the rate law for the reaction? Rate = k[NO2] [O2] %3D O Rate = k[N2O5]NO2][O2] O Rate = k[N2 05] %3D O Rate = k[N205] %3D

Chemistry

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

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Question

17a.)

Dinitrogen pentoxide decomposes according to the reaction
2N2O5 (9) → 4NO2(9) + O2(9)
At 45°C the rate constant is 6.2 x 10 s. The reaction is first order.
4.
-1
a What is the rate law for the reaction?
Rate = k[NO2]*[O2]
Rate = k[N2O5]° NO,] [O2]
k[N2 O;]
%3D
Rate = k[N2 O;]
Rate = k[N2 O5]

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