Using the information in the table, the rate law for the reaction 2 A(g) + B(g) → C(g) + D(g) is A) Rate = k[A][B] B) Rate = k[A] C) Rate = k[A]²[B] D) Rate = k[A][B]²
Using the information in the table, the rate law for the reaction 2 A(g) + B(g) → C(g) + D(g) is A) Rate = k[A][B] B) Rate = k[A] C) Rate = k[A]²[B] D) Rate = k[A][B]²
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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Using the information in the table, the rate law for the reaction 2 A(g) + B(g) → C(g) + D(g) is
A) Rate = k[A][B]
B) Rate = k[A]
C) Rate = k[A]²[B]
D) Rate = k[A][B]²
![Rate
[A]. (M)
[B], (M)
(M/min)
0.150
0.300
3.38 x 10-5
0.450
0.300
1.01 x 10-4
0.450
0.150
2.54 x 10-5](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F1243504b-5612-4510-ba6c-7b5ec7c70d6e%2F0915e5df-6ad4-47b9-a112-9ed7f6cfb5a7%2Fed4abt_processed.png&w=3840&q=75)
Transcribed Image Text:Rate
[A]. (M)
[B], (M)
(M/min)
0.150
0.300
3.38 x 10-5
0.450
0.300
1.01 x 10-4
0.450
0.150
2.54 x 10-5
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