Please explainAnswer is a 34. Given the mechanism shown, what would be the rate law?2 NO → N₂O₂N₂O₂ + Br₂ → 2NOBra. rate = k[NO][Br₂]b. rate = k[N₂O₂] [Br₂]c. rate = k[NO] [N₂O₂][Br₂]d. rate k[NO][Br₂]e. rate = k[NO]fast, equilibriumslow

The objective of the question is to determine the rate law of the given mechanism.

34. Given the mechanism shown, what would be the rate law? 2 NO → N₂O₂ N₂O₂ + Br₂ → 2NOBr a. rate k[NO]¹[Br₂] = b. rate = k[N₂O₂] ² [Br₂] c. rate = k[NO][N₂O₂][Br.] d. rate k[NO][Br₂] = e. rate = k[NO] fast, equilibrium slow

34. Given the mechanism shown, what would be the rate law? 2 NO → N₂O₂ N₂O₂ + Br₂ → 2NOBr a. rate k[NO]¹[Br₂] = b. rate = k[N₂O₂] ² [Br₂] c. rate = k[NO][N₂O₂][Br.] d. rate k[NO][Br₂] = e. rate = k[NO] fast, equilibrium slow

Chemistry for Engineering Students

4th Edition

ISBN:9781337398909

Author:Lawrence S. Brown, Tom Holme

Publisher:Lawrence S. Brown, Tom Holme

Chapter11: Chemical Kinetics

Section: Chapter Questions

Problem 11.36PAE: The reaction NO(g) + O,(g) — NO,(g) + 0(g) plays a role in the formation of nitrogen dioxide in...

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Please explain

Answer is a

34. Given the mechanism shown, what would be the rate law?
2 NO → N₂O₂
N₂O₂ + Br₂ → 2NOBr
a. rate = k[NO][Br₂]
b. rate = k[N₂O₂] [Br₂]
c. rate = k[NO] [N₂O₂][Br₂]
d. rate k[NO][Br₂]
e. rate = k[NO]
fast, equilibrium
slow

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