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

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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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С-2 (i) Write the rate formula for the following reaction in terms of both reactants and products. GaFa + 3 Cs > 3 CsF + Ga (ii) The following data is given for the decomposition of N2O5. 2N2OS(g) > 4NO2(g) + O2(g) [N2O5] (M) 0.0200 0.0142 0.0086 Time (second) 200 500 Determine the average rate of disappearance of N2Os between 0s and 200 s, and between 200 s and 500 s. (iii) Identify the reactant and product from the concentration vs. time graph as given below. Time (iv) A 11.5 M Solution of hydrochloric acid of volume 8 L needed to be diluted to reduce its concentration to 3.5 M. How much of water was added to do this? Concentration
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