What is the rate law for this reaction? II .C. HO, II + НОCHЗ + 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 0.096 0.320 6.6 x 10-4 Rate = k[HCO2H]², k =2.4 x 10-2 M-15-1 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 O Rate = k[HCO,H], k = 1.1 x 10-3 s-1 %3D %3D O=U
What is the rate law for this reaction? II .C. HO, II + НОCHЗ + 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 0.096 0.320 6.6 x 10-4 Rate = k[HCO2H]², k =2.4 x 10-2 M-15-1 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 O Rate = k[HCO,H], k = 1.1 x 10-3 s-1 %3D %3D O=U
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 29E: The rate constant for the ?rst-order decomposition at 45 C of dinitrogen pentoxide, N2O5, dissolved...
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![What is the rate law for this reaction?
II
+ HOCH3
+ H20
HO,
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
0.096
0.320
6.6 x 10-4
Rate = k[HCO2H]², k =2.4 x 10-2 M-1s°1
%3D
Rate %3D k[HCO2H)ІНОСН;|, k %3D 2.2 х 10:2 м-15-1
Rate = k[HCO2H], k = 1.8 x 10-3 s-1
O Rate = k[HCO2H], k = 1.1 x 10-3 s-1
O=U](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0a01e08b-df82-451a-8a4d-20a49d49636b%2F8cec0fb9-8392-4014-a1ef-f0f523f41ebc%2F7wql55u_processed.png&w=3840&q=75)
Transcribed Image Text:What is the rate law for this reaction?
II
+ HOCH3
+ H20
HO,
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
0.096
0.320
6.6 x 10-4
Rate = k[HCO2H]², k =2.4 x 10-2 M-1s°1
%3D
Rate %3D k[HCO2H)ІНОСН;|, k %3D 2.2 х 10:2 м-15-1
Rate = k[HCO2H], k = 1.8 x 10-3 s-1
O Rate = k[HCO2H], k = 1.1 x 10-3 s-1
O=U
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