What is the rate law for the following mechanism:NO (g) + Br2 (g) 2 NOB12 (g) (fast equilibrium)(rate of forward reaction: k1, rate of reverse reaction: k.1)NOB12 (g) + NO (g) → 2 NOB1 (g) (slow, rate: k2)Rate= k2 [NOB12[NO]O A.Rate= k1 [NO][Br2]B.Rate= (k1/k-1) [NO][Br2]Rate= k2 (k1k.1) [NOJ²[Br2]D.Rate= k2 [NO]?[Br2]

What is the rate law for the following mechanism: NO (g) + Br2 (2) 2 NOB12 (g) (fast equilibrium) (rate of forward reaction: k], rate of reverse reaction: k.1) NOB12 (g) + NO (g) → 2 NOB1 (g) (slow, rate: k2) Rate= k2 [NOB12][NO] OA. Rate= k1 [NO][Br2] B. OC. Rate= (k1/k.1) [NO][Br2] OD. O D. Rate= k2 (k1/k.1) [NO]²[Br2] OE. O E. Rate= k2 [Noj²[Br2]

What is the rate law for the following mechanism: NO (g) + Br2 (2) 2 NOB12 (g) (fast equilibrium) (rate of forward reaction: k], rate of reverse reaction: k.1) NOB12 (g) + NO (g) → 2 NOB1 (g) (slow, rate: k2) Rate= k2 [NOB12][NO] OA. Rate= k1 [NO][Br2] B. OC. Rate= (k1/k.1) [NO][Br2] OD. O D. Rate= k2 (k1/k.1) [NO]²[Br2] OE. O E. Rate= k2 [Noj²[Br2]

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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