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

10th Edition

ISBN:9781305957404

Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste

Chapter1: Chemical Foundations

Section: Chapter Questions

Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...

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