5. The overall reaction for the oxidation of NO to NO₂ is: 2NO(g) + O₂(g) → 2NO₂(g) The reaction proceeds by the following mechanism: NO + NO → N₂O₂ N₂O₂ → NO + NO N2O2 + O2 → NO₂ + NO₂ ka k'a kb (a) Verify that application of the steady-state approximation to the intermediate, N₂O2, results in the rate law: d[NO₂] 2kak [NO]²[0₂] dt ka + kb [0₂] (b) Show how the rate law simplifies (i) [0₂] is very large, and (ii) if [0₂] is very small. (c) Why might it be important to recognize how the rate law simplifies under the conditions of very large or very small [0₂]?
5. The overall reaction for the oxidation of NO to NO₂ is: 2NO(g) + O₂(g) → 2NO₂(g) The reaction proceeds by the following mechanism: NO + NO → N₂O₂ N₂O₂ → NO + NO N2O2 + O2 → NO₂ + NO₂ ka k'a kb (a) Verify that application of the steady-state approximation to the intermediate, N₂O2, results in the rate law: d[NO₂] 2kak [NO]²[0₂] dt ka + kb [0₂] (b) Show how the rate law simplifies (i) [0₂] is very large, and (ii) if [0₂] is very small. (c) Why might it be important to recognize how the rate law simplifies under the conditions of very large or very small [0₂]?
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 13.94QE
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