When the reaction: A + 2 B → C was studied, the experimental data was obtained and plotted. Based on these graphs, what is the experimental rate law? 0.06 0.06 0.05 0.05 0.04 0.04 0.03 0.03 0.02 0.02 0.01 0.01 0.2 0.4 0.6 0.8 1 0.2 0.4 0.6 0.8 [A]o (M) with [B] constant [B], (M) with [A] constant rate = k[A] rate = k[A][B] rate = k[A]²[B] %3D rate = k[A][B]2 %3D Initial Rate of Reaction (M/min) Initial Rate of Reaction (M/min)
When the reaction: A + 2 B → C was studied, the experimental data was obtained and plotted. Based on these graphs, what is the experimental rate law? 0.06 0.06 0.05 0.05 0.04 0.04 0.03 0.03 0.02 0.02 0.01 0.01 0.2 0.4 0.6 0.8 1 0.2 0.4 0.6 0.8 [A]o (M) with [B] constant [B], (M) with [A] constant rate = k[A] rate = k[A][B] rate = k[A]²[B] %3D rate = k[A][B]2 %3D Initial Rate of Reaction (M/min) Initial Rate of Reaction (M/min)
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 12PS: The reaction 2 NO(g) + 2 H2(g) N2(g) + 2 H2O(g) was studied at 904 C, and the data in the table...
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![When the reaction:
A + 2 B → C
was studied, the experimental data was obtained and plotted. Based on these graphs, what is the
experimental rate law?
0.06
0.06
0.05
0.05
0.04
0.04
0.03
0.03
0.02
0.02
0.01
0.01
0.2
0.4
0.6
0.8
1
0.2
0.4
0.6
0.8
1
[A]o (M) with [B] constant
[B]. (M) with [A] constant
rate =
k[A]
rate = k[A][B]
%3D
rate = k[A]?[B]
rate = k[A][B]?
Initial Rate of Reaction (M/min)
Initial Rate of Reaction (M/min)](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F84ae2f53-6ef3-4d1e-914e-c77779ee6da5%2F184c9507-36c0-4daf-a4b0-55c99c411069%2Fwue8x0t_processed.png&w=3840&q=75)
Transcribed Image Text:When the reaction:
A + 2 B → C
was studied, the experimental data was obtained and plotted. Based on these graphs, what is the
experimental rate law?
0.06
0.06
0.05
0.05
0.04
0.04
0.03
0.03
0.02
0.02
0.01
0.01
0.2
0.4
0.6
0.8
1
0.2
0.4
0.6
0.8
1
[A]o (M) with [B] constant
[B]. (M) with [A] constant
rate =
k[A]
rate = k[A][B]
%3D
rate = k[A]?[B]
rate = k[A][B]?
Initial Rate of Reaction (M/min)
Initial Rate of Reaction (M/min)
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