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 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 11.58PAE

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