The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N2O5 and first order overall. The rate constant for the reaction at 70.°C is 6.82x10-3 s-1. The reaction is started with 0.300 mol of N2O5 in a 0.500L container. What is the rate law for this reaction? O a. rate = K[N₂05]² O b. rate k[NO2] O c. rate k[N205] O d. rate k[NO2][02] O e. rate = K[02]

The decomposition of N2O5 to NO2 and O2 is first order with respect to the reactant N2O5 and first order overall. The rate constant for the reaction at 70.°C is 6.82x10-3 s-1. The reaction is started with 0.300 mol of N2O5 in a 0.500L container. What is the rate law for this reaction? O a. rate = K[N₂05]² O b. rate k[NO2] O c. rate k[N205] O d. rate k[NO2][02] O e. rate = K[02]

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

Section: Chapter Questions

Problem 31QRT

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