1. HBr + 02 НООBr (slow) - (8) 2(g) () 2. HOOBr +HBr (fast) - (8) 2{HOB" + HBr H,O« +Brx} (fast) (8) (8) (8) 2(g) 4HB + O2→2H,0 +2Br, > (g) (8) Consider the above reaction mechanism. The rate-law equation from this reaction would be r = k[HBr]*[O,] r = k[HOB1]² - K[HBr]'[O,]' а. d. = k[HOB1]°[HBr] %3D b. e. impossible to tell from this information %3D с.

1. HBr + 02 НООBr (slow) - (8) 2(g) () 2. HOOBr +HBr (fast) - (8) 2{HOB" + HBr H,O« +Brx} (fast) (8) (8) (8) 2(g) 4HB + O2→2H,0 +2Br, > (g) (8) Consider the above reaction mechanism. The rate-law equation from this reaction would be r = k[HBr]*[O,] r = k[HOB1]² - K[HBr]'[O,]' а. d. = k[HOB1]°[HBr] %3D b. e. impossible to tell from this information %3D с.

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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Question

1.
HBr +O2 →HOOBF
2(g)
(slow)
2. НООBr + HBr,
(8)
2HOB" 2g)
(fast)
3. 2{НОBr + HBr,
T →H,O« +Br} (fast)
(8)
(g)
2(g)
4HB +0,→2H,O, +2Br%e
-
(3)
Consider the above reaction mechanism. The rate-law equation from this reaction would be
- K[HOB1]*[HBr]
K[HBr]*[O,]
= k[HOB1]²
r = k[HBr]'[O,]'
а.
r =
d.
=
b.
e. impossible to tell from this information
r =
с.

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