9. A possible mechanism for a reaction is 1. 2 NO N₂O₂ 2. N₂O₂ + H₂ → N₂O + H₂O 3. N₂O + H₂ → N₂ + H₂O (fast reaction) (slow reaction) (fast reaction) a. What is the molecularity of the slow step? b. What is the overall reaction? c. Are there any intermediates? If yes, identify the intermediate(s). d. Are there any catalysts? If yes, identify the catalyst (s). e. What is the rate law for the overall reaction based on this mechanism?

9. A possible mechanism for a reaction is 1. 2 NO N₂O₂ 2. N₂O₂ + H₂ → N₂O + H₂O 3. N₂O + H₂ → N₂ + H₂O (fast reaction) (slow reaction) (fast reaction) a. What is the molecularity of the slow step? b. What is the overall reaction? c. Are there any intermediates? If yes, identify the intermediate(s). d. Are there any catalysts? If yes, identify the catalyst (s). e. What is the rate law for the overall reaction based on this mechanism?

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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If the activation energy of a reaction increases, what happens to the rate constant (k)? A.the rate constant decreases B.the rate constant stays the same C. there isn't enough information to predict what happens to the rate constant D. the rate constant increases
D and E solutions?
Consider the following mechanism: Cl2 → Cl+ + Cl- Cl- + H2S → HCl + HS- Cl+ + HS- → HCl + S What is the role of Cl+? A. product B. intermediate C. catalyst D. reactant
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of the following all are valid uits for a reaction rate except g/s mol/L mol/L-hr M/s mol/hr
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The following is the proposed mechanism for a given reaction: Step 1: NO + 02 2 NO, (fast, reversible) Step 2: NO, + NO 2 N20 (slow) What is the rate law for the overall reaction? A. O rate = k[NO][NO] В. k[NO||0, rate = C. O rate = D.O rate = E. O rate = k[NO]|0:)
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