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The reaction, 2 A2X4(g)   →    2 A2X3(g)  +  X2(g), was found to be first order.  The rate law, therefore, should be Select one: a. rate = k([A2X3]2[X2])/[A2X4]2 b. rate = k[A2X4]2 c. rate = k([A2X3][X2])/[A2X4] d. rate = k[A2X4] e. rate = k[A2X4]2/([A2X3]2[X2])

The reaction, 2 A2X4(g)   →    2 A2X3(g)  +  X2(g), was found to be first order.  The rate law, therefore, should be Select one: a. rate = k([A2X3]2[X2])/[A2X4]2 b. rate = k[A2X4]2 c. rate = k([A2X3][X2])/[A2X4] d. rate = k[A2X4] e. rate = k[A2X4]2/([A2X3]2[X2])

Chemistry
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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The reaction, 2 A2X4(g)   →    2 A2X3(g)  +  X2(g), was found to be first order.  The rate law, therefore, should be
Select one:
a.

rate = k([A2X3]2[X2])/[A2X4]2

b.

rate = k[A2X4]2

c.

rate = k([A2X3][X2])/[A2X4]

d.

rate = k[A2X4]

e.

rate = k[A2X4]2/([A2X3]2[X2])

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