3. The rate equation for the decomposition of N2O5(g) (forming NO2(g)) is: A[NO:]/At = k[N2O5]. The value of k is 5.0 × 104 s-1 for the reaction at a particular temperature. a) Calculate the half-life of N2O5(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[NO:]/At = k[N2O5]. The value of k is 5.0 × 104 s-1 for the reaction at a particular temperature. a) Calculate the half-life of N2O5(g) at that temperature. b) How long does it take for [N2O5] to decrease to one tenth of its original value?
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 25PS: The rate equation for the decomposition of N2O5 (giving NO2 and O2) is Rate = k[N2O5]. The value of...
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