The rate law for the reaction below was determined using the method of initial rates, to be: Rate = k[F2][NO2]. F2(g) + 2NO2(g) –→ 2NO2F(g) You have repeated the reaction and recorded the concentration of [NO2] as a function of time. Sketch the plots of the appropriately treated data that could be used to confirm that reaction is 1st order, and not 2nd or zero order in NO2.

The rate law for the reaction below was determined using the method of initial rates, to be: Rate = k[F2][NO2]. F2(g) + 2NO2(g) –→ 2NO2F(g) You have repeated the reaction and recorded the concentration of [NO2] as a function of time. Sketch the plots of the appropriately treated data that could be used to confirm that reaction is 1st order, and not 2nd or zero order in NO2.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.50QE

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