Recall the reaction in lecture slides #42 and #43: 2 NO2CI(g) --> 2 NO2(g) + Cl2(g). The proposed mechanism from that example is below. (1) NO2CI(g) --> NO2(g) + CI(g) (2) NO2CI(g) + Cl(g) NO2(g) + Cl2(g) --> If step (1) is the rate-determining step for the reaction, what is the reaction rate law? rate = k [NO2CI] rate = k [NO2CI]? rate = k [NO2CI][CI] rate = k [NO2CI]² [NO2]² [Cl2] %3D There is not enough information provided to predict the rate law.

Recall the reaction in lecture slides #42 and #43: 2 NO2CI(g) --> 2 NO2(g) + Cl2(g). The proposed mechanism from that example is below. (1) NO2CI(g) --> NO2(g) + CI(g) (2) NO2CI(g) + Cl(g) NO2(g) + Cl2(g) --> If step (1) is the rate-determining step for the reaction, what is the reaction rate law? rate = k [NO2CI] rate = k [NO2CI]? rate = k [NO2CI][CI] rate = k [NO2CI]² [NO2]² [Cl2] %3D There is not enough information provided to predict the rate law.

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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Question

Recall the reaction in lecture slides #42 and #43: 2 NO2CI(g)
--> 2 NO2(g) + Cl2(g). The proposed
mechanism from that example is below.
(1) NO2CI(g)
--> NO2(g) + CI(g)
(2) NO2CI(g) + Cl(g)
NO2(g) + Cl2(g)
-->
If step (1) is the rate-determining step for the reaction, what is the reaction rate law?
rate = k [NO2CI]
rate =
k [NO2CI]?
rate =
k [NO2CI][CI]
rate = k [NO2CI]² [NO2]² [Cl2]
%3D
There is not enough information provided to predict the rate law.

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