Rate = K[A][B] [A] (M) 0.100 0.100 0.200 [B] (M) Rate (M/s) 0.100 0.200 0.100 5.0 x 10-³ 1.0 x 10-² 5.0 x 10-3 and it A) m = 1, n = 1 B) m = 0, n = 0 C) m = 0, n = 2 D) m = 0, n = 1 E) m = 2, n = 1
Rate = K[A][B] [A] (M) 0.100 0.100 0.200 [B] (M) Rate (M/s) 0.100 0.200 0.100 5.0 x 10-³ 1.0 x 10-² 5.0 x 10-3 and it A) m = 1, n = 1 B) m = 0, n = 0 C) m = 0, n = 2 D) m = 0, n = 1 E) m = 2, n = 1
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 11.25PAE: For each of the rate laws below, what is the order of the reaction with respect to the hypothetical...
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![Rate = k[A]m[B]n
[A] (M)
0.100
0.100
Given the rate law and table below, what are the values of m and n?
0.200
[B] (M) Rate (M/s)
0.100
0.200
5.0 x 10³
1.0 x 10-²
0.100 5.0 x 10-3
A) m = 1, n = 1
B) m = 0, n = 0
C) m = 0, n = 2
D) m = 0, n = 1
E) m = 2, n = 1](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F2485abad-9bb4-442d-b61c-92b3f0f3d54b%2F78911b8d-bdc0-4312-912c-6b3a27003854%2F29q9l4b_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Rate = k[A]m[B]n
[A] (M)
0.100
0.100
Given the rate law and table below, what are the values of m and n?
0.200
[B] (M) Rate (M/s)
0.100
0.200
5.0 x 10³
1.0 x 10-²
0.100 5.0 x 10-3
A) m = 1, n = 1
B) m = 0, n = 0
C) m = 0, n = 2
D) m = 0, n = 1
E) m = 2, n = 1
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