For the reaction: 2Y + T - B + H, the mechanism below is proposed, in which M is a reactive intermediate, and its concentration is maintained at some low steady-state throughout the reaction. 1.2Y M + B 2. T+ M → X + H Note that only the reverse reaction of step one is significant Determine the rate law for this reaction. Select one: O A. -d[T]/dt = kµ[Y][T]/(k₁' [B]+ k₂[T]) B._-d[T]/dt = ka[Y]²/k1'[B] + k2[T] C. -d[T]/dt = ka[Y]²[T]/[B] OD. -d[T]/dt = ka[Y]²/(kb [B]/[T] + 1)

For the reaction: 2Y + T - B + H, the mechanism below is proposed, in which M is a reactive intermediate, and its concentration is maintained at some low steady-state throughout the reaction. 1.2Y M + B 2. T+ M → X + H Note that only the reverse reaction of step one is significant Determine the rate law for this reaction. Select one: O A. -d[T]/dt = kµ[Y][T]/(k₁' [B]+ k₂[T]) B._-d[T]/dt = ka[Y]²/k1'[B] + k2[T] C. -d[T]/dt = ka[Y]²[T]/[B] OD. -d[T]/dt = ka[Y]²/(kb [B]/[T] + 1)

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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