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The oxidation of NO(g) to NO2(g): 2 NO(g) + O2(g) kobs 2 NO2(g) A mechanism of steps (a) - (c) is proposed below, all steps are elementary: k3 (a) NO(g) + NO(g) N2O2(g) k-3 (b) N2O2(g) → NO(g) + NO(g) k4 (c) N2O2(g) + O2(g) 2 NO2(g) Apply the steady-state approximation, find out the reaction rate law when the initial concertation of [O2] is high. Which step is rate-determining?

The oxidation of NO(g) to NO2(g): 2 NO(g) + O2(g) kobs 2 NO2(g) A mechanism of steps (a) - (c) is proposed below, all steps are elementary: k3 (a) NO(g) + NO(g) N2O2(g) k-3 (b) N2O2(g) → NO(g) + NO(g) k4 (c) N2O2(g) + O2(g) 2 NO2(g) Apply the steady-state approximation, find out the reaction rate law when the initial concertation of [O2] is high. Which step is rate-determining?

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
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
Section14.6: Reaction Mechanisms
Problem 2RC: A reaction is believed to occur by the following mechanism: Stepl: 2AI (Fast equilibrium) Step 2: I...
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The oxidation of NO(g) to NO2(g): 2 NO(g) + O2(g) kobs 2 NO2(g) A mechanism of steps (a) - (c) is proposed below, all steps are elementary: k3 (a) NO(g) + NO(g) → N2O2(g) k-3 (b) N2O2(g) → NO(g) + NO(g) k4 (c) N2O2(g) + O2(g) 2 NO2(g) Apply the steady-state approximation, find out the reaction rate law when the initial concertation of [02] is high. Which step is rate-determining?
Transcribed Image Text:The oxidation of NO(g) to NO2(g): 2 NO(g) + O2(g) kobs 2 NO2(g) A mechanism of steps (a) - (c) is proposed below, all steps are elementary: k3 (a) NO(g) + NO(g) → N2O2(g) k-3 (b) N2O2(g) → NO(g) + NO(g) k4 (c) N2O2(g) + O2(g) 2 NO2(g) Apply the steady-state approximation, find out the reaction rate law when the initial concertation of [02] is high. Which step is rate-determining?
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