3. The rate equation for the decomposition of N2O5(g) (forming NO2(g)) is: A[NO2]/At = k[N2O5]. The value of k is 5.0 × 104 s-' for the reaction at a particular temperature. a) Calculate the half-life of N2Os(g) at that temperature. b) How long does it take for [N2O5] to decrease to one tenth of its original value?

3. The rate equation for the decomposition of N2O5(g) (forming NO2(g)) is: A[NO2]/At = k[N2O5]. The value of k is 5.0 × 104 s-' for the reaction at a particular temperature. a) Calculate the half-life of N2Os(g) at that temperature. b) How long does it take for [N2O5] to decrease to one tenth of its original value?

Chemistry: Principles and Reactions

8th Edition

ISBN:9781305079373

Author:William L. Masterton, Cecile N. Hurley

Publisher:William L. Masterton, Cecile N. Hurley

Chapter11: Rate Of Reaction

Section: Chapter Questions

Problem 58QAP: If the activation energy of a reaction is 9.13 kJ, then what is the percent increase in the rate...

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