The reaction H2S (g) + Br2 (g) → S (s) + 2 HBr (g) is second order for Br2. Which ofthe following "Trial 2" data will support this reaction order for bromine?Trial [H2S] (M) [Br2] (M) rate (MS-1)10.020.041.12 x 10-32?????????[H2S] = 0.02 M; [Br2] = 0.08 M; rate = 2.24 x 10-3 M s-1[H2S] = 0.04 M; [Br2] = 0.04 M; rate = 1.12 x 10-3 M s-1[H2S] = 0.02 M; [Br2] = 0.08 M; rate = 4.48 x 10-3 M s-1[H2S] = 0.02 M; [Br2] = 0.04 M; rate 1.12 x 10-3 M s 1=

1. Calculate the rate constant, k rate = k[H2S][Br2]2 From Trial 1: 1.12 x 10-3 = k [0.02][0.04]2…

Answered: The reaction H2S (g) + Br2 (g) → S (s)…

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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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: A. -d[T]/dt = k[Y][T]/(k₁' [B]+ k₂[T]) OB. -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) C
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