Q03: Consider the following mechanism: k₁ N₂05 (8) NO2(g) + NO 3 (8) k₂ NO2(g) + NO3(g) → NO (g) +NO2(g) + O2(g) k3 NO(g) + NO3(g) 2NO2(g) Apply S.S. approximation to derive the rate law of the production of O2(g), given that the intermediates are NO and NO3.
Q03: Consider the following mechanism: k₁ N₂05 (8) NO2(g) + NO 3 (8) k₂ NO2(g) + NO3(g) → NO (g) +NO2(g) + O2(g) k3 NO(g) + NO3(g) 2NO2(g) Apply S.S. approximation to derive the rate law of the production of O2(g), given that the intermediates are NO and NO3.
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 13.88QE
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Question
Consider the following mechanism:
N2O5(8) NO2(g) + NO3 (8) K-1
NO2(g) + NO3(g) NO(g) + NO2(g) + O2(g)
k3 - NO (g) + NO3(g) 2NO2(g)
Apply S.S. approximation to derive the rate law of the production of O2(g), given that the intermediates are NO and NO3.
Transcribed Image Text:Q03: Consider the following mechanism:
k₁
N₂O5(g) NO2(g) + NO3(g)
k₂
NO2(g) + NO3(g) → NO(g) + NO2(g) + O2(g)
K-1
k3
NO(g) + NO3(g) → 2NO2(g)
Apply S.S. approximation to derive the rate law of the production of O2(g), given that the
intermediates are NO and NO3.
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