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)

Principles of Modern Chemistry

8th Edition

ISBN:9781305079113

Author:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Publisher:David W. Oxtoby, H. Pat Gillis, Laurie J. Butler

Chapter18: Chemical Kinetics

Section: Chapter Questions

Problem 32P

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For the reaction A + B C, explain at least two ways in which the rate law could be zero order in chemical A.
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