The decomposition reaction of dinitrogen pentoxide (N2O5) is: 2 N2O5 → 4 NO2 (g) + O2 (g) a)Calculate the concentration of N2O5 remaining 460. s after the start of the decomposition at 65 oC when its initial concentration was 0.040 mol/L. The rate law for this reaction is rate=k[N2O5] with a rate constant of k=5.2x10-2 s-1. b)Calculate the half-life for this reaction.
The decomposition reaction of dinitrogen pentoxide (N2O5) is: 2 N2O5 → 4 NO2 (g) + O2 (g) a)Calculate the concentration of N2O5 remaining 460. s after the start of the decomposition at 65 oC when its initial concentration was 0.040 mol/L. The rate law for this reaction is rate=k[N2O5] with a rate constant of k=5.2x10-2 s-1. b)Calculate the half-life for this reaction.
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 77GQ: The decomposition of nitrogen dioxide at a high temperature NO2(g) NO(g) + O2(g) is second-order...
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The decomposition reaction of dinitrogen pentoxide (N2O5) is:
2 N2O5 → 4 NO2 (g) + O2 (g)
a)Calculate the concentration of N2O5 remaining 460. s after the start of the
decomposition at 65 oC when its initial concentration was 0.040 mol/L. The rate law for this
reaction is rate=k[N2O5] with a rate constant of k=5.2x10-2 s-1.
b)Calculate the half-life for this reaction.
2 N2O5 → 4 NO2 (g) + O2 (g)
a)Calculate the concentration of N2O5 remaining 460. s after the start of the
decomposition at 65 oC when its initial concentration was 0.040 mol/L. The rate law for this
reaction is rate=k[N2O5] with a rate constant of k=5.2x10-2 s-1.
b)Calculate the half-life for this reaction.
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