The rate law for the reaction 2 NO (g) + Cl2 (g) ⇄ 2 NOCl (g) is given by the rate=k[NO][Cl2]. A mechanism involving these steps has been proposed for the reactionNO (g) + Cl2 (g) ⇄ NOCl2 (g)NOCl2 (g)+ NO (g) ⇄ 2 NOCl (g)(2a) If this mechanism is correct, what does it imply about the relative rates of these two steps (e.g. How do the rates of reaction compare? Which is slow?)(2b) What is the reaction intermediate in this mechanism?
The rate law for the reaction 2 NO (g) + Cl2 (g) ⇄ 2 NOCl (g) is given by the rate=k[NO][Cl2]. A mechanism involving these steps has been proposed for the reactionNO (g) + Cl2 (g) ⇄ NOCl2 (g)NOCl2 (g)+ NO (g) ⇄ 2 NOCl (g)(2a) If this mechanism is correct, what does it imply about the relative rates of these two steps (e.g. How do the rates of reaction compare? Which is slow?)(2b) What is the reaction intermediate in this mechanism?
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 11.64PAE: 11.64 HBr is oxidized in the following reaction: 4 HBr(g) + O2(g) —• 2 H2O(g) + 2 Br,(g) A proposed...
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The rate law for the reaction 2 NO (g) + Cl2 (g) ⇄ 2 NOCl (g) is given by the rate=k[NO][Cl2]. A mechanism involving these steps has been proposed for the reaction
NO (g) + Cl2 (g) ⇄ NOCl2 (g)
NOCl2 (g)+ NO (g) ⇄ 2 NOCl (g)
(2a) If this mechanism is correct, what does it imply about the relative rates of these two steps (e.g. How do the
(2b) What is the reaction intermediate in this mechanism?
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