22 NO2(3) + O3(g) → NO3(g) + O2(g) (fast)4NO3(g) – 2N205(g) + O2(g) (slow)NO2(3) + O3(g) → NO3(g) + O2(g) (fast)NO3(g) + NO2(g) N205(g) (slow)NO2(g) + O3(g) NO3(g) + O2(g) (slow)4NO3(g) → 2N205(g) + O2(g) (fast)NO2(g) + O3(g)→ NO3(g) + O2(g) (slow)NO3(g) + NO2(g)→N2O5(g) (fast)79°FClearesc13)17fol21%23&5.8. One of the reactions that occurs in polluted air in urban areas is 2NO2(g) +O3(g) → N2O5(g) + O2(g). Assume that a species with theformula NO3 is involved in the mechanism, and the observed rate law for the overall reaction is rate = k[NO2][O3].Propose a mechanism for this reaction that includes the species NO3 and is consistent with the observed rate law.NO2(s) + O3(g) – NO3(g) + O2(g) (fast)4NO3(g) → 2N2O5(g) + O2(g) (slow)NO2(g) + O3(g) NO3(g) + O2(g) (fast)NO3(g) + NO2(3) → N2O5(g) (slow)NO2(8) + O3(g) – NO3(g) + O2(g) (slow)4NO3(g) → 2N2O5(g) + O2(g) (fast)NO2(3) + O3(g) – NO3(g) + O2(g) (slow)7.19-A1217fno12Apri scdeletefA /S19ED $TLLL%234.7.8.11

Rate law is experimentally calculated quality. A reaction completes in several steps then ,slow…

eg) – 2N2O5(g) + O2(g) (slow) g) + O3(g) → NO3(g) + O2(g) (fast) (g) + NO2(g) N2O5(g) (slow) z(g) + O3(g) → NO3(g) + O2(g) (slow) D3l8) 2N205(g) + O2(g) (fast) P2(g) + O3lg) → NO3(g) + O2(g) (slow) D3(g) + NO2(g) –→ N2O5(g) (fast)

eg) – 2N2O5(g) + O2(g) (slow) g) + O3(g) → NO3(g) + O2(g) (fast) (g) + NO2(g) N2O5(g) (slow) z(g) + O3(g) → NO3(g) + O2(g) (slow) D3l8) 2N205(g) + O2(g) (fast) P2(g) + O3lg) → NO3(g) + O2(g) (slow) D3(g) + NO2(g) –→ N2O5(g) (fast)

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

Section11.7: Reaction Mechanisms

Problem 11.12E

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