What is the rate law for this reaction? II II .C. HO, + НОCHЗ + H20 OCH3 Experiment [HCO2H], M [НОСН3], М Initial rate, M s-1 1 0.031 0.080 5.4 x 10-5 0.031 0.160 1.1 x 10-4 0.096 0.320 6.6 x 10-4 Rate = k[HCO2H]², k =2.4 x 10-2 M-1s-1 Rate = k[HCO2H][HOCH3], k = 2.2 x 10-2 M-1s-1 %3D Rate = k[HCO2H], k = 1.8 x 10-3 s-1 Rate = k[HCO2H], k = 1.1 x 10-3 s-1 2.
What is the rate law for this reaction? II II .C. HO, + НОCHЗ + H20 OCH3 Experiment [HCO2H], M [НОСН3], М Initial rate, M s-1 1 0.031 0.080 5.4 x 10-5 0.031 0.160 1.1 x 10-4 0.096 0.320 6.6 x 10-4 Rate = k[HCO2H]², k =2.4 x 10-2 M-1s-1 Rate = k[HCO2H][HOCH3], k = 2.2 x 10-2 M-1s-1 %3D Rate = k[HCO2H], k = 1.8 x 10-3 s-1 Rate = k[HCO2H], k = 1.1 x 10-3 s-1 2.
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 31E: The following data have been determined for the reaction: I+OCIIO+CI 1 2 3 [I] 0.10 0.20 0.30 [OCI]...
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![What is the rate law for this reaction?
II
II
.C.
HO,
+ HOCH3
+ H20
H
OCH3
Experiment
[HCO2H], M
[HOCH3], M
Initial rate, M s-1
1
0.031
0.080
5.4 x 10-5
0.031
0.160
1.1 x 10-4
3
0.096
0.320
6.6 x 10-4
O Rate = k[HCO2H]², k =2.4 x 10-2 M-1s-1
%3D
Rate = k[HCO2H][HOCH3], k = 2.2 x 10-2 M-1s-1
%3D
Rate = k[HCO2H], k = 1.8 x 103 s-1
%3D
Rate = k[HCO2H], k = 1.1 x 10-3 s°1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0a01e08b-df82-451a-8a4d-20a49d49636b%2F41c849a7-86d7-4d1b-aea3-3692f891f2f7%2Flyfqnra_processed.png&w=3840&q=75)
Transcribed Image Text:What is the rate law for this reaction?
II
II
.C.
HO,
+ HOCH3
+ H20
H
OCH3
Experiment
[HCO2H], M
[HOCH3], M
Initial rate, M s-1
1
0.031
0.080
5.4 x 10-5
0.031
0.160
1.1 x 10-4
3
0.096
0.320
6.6 x 10-4
O Rate = k[HCO2H]², k =2.4 x 10-2 M-1s-1
%3D
Rate = k[HCO2H][HOCH3], k = 2.2 x 10-2 M-1s-1
%3D
Rate = k[HCO2H], k = 1.8 x 103 s-1
%3D
Rate = k[HCO2H], k = 1.1 x 10-3 s°1
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