A 100% 7:07 PM Wed Feb 5 Unanswered •1 attempt left For reaction 2A + 3B → 2C + D, following data of concentration and rate was obtained Trial Initial [A] Initial [B] Initial Rate (M/sec) 10.015 M 0.200 M 3.67 × 10^-6 20.030 МО.200 М 7.33 х 10^-6 3 0.015 M 0.400 M 1.47 × 10^-5 What is the rate law of the reaction? Rate = k[A][B] Rate = k[A]^2 Rate = k[B]^2 Rate = k[B][A]^2 %3D Rate = k[A][B]^2 Submit ш

A 100% 7:07 PM Wed Feb 5 Unanswered •1 attempt left For reaction 2A + 3B → 2C + D, following data of concentration and rate was obtained Trial Initial [A] Initial [B] Initial Rate (M/sec) 10.015 M 0.200 M 3.67 × 10^-6 20.030 МО.200 М 7.33 х 10^-6 3 0.015 M 0.400 M 1.47 × 10^-5 What is the rate law of the reaction? Rate = k[A][B] Rate = k[A]^2 Rate = k[B]^2 Rate = k[B][A]^2 %3D Rate = k[A][B]^2 Submit ш

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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A 100% 7:07 PM Wed Feb 5 3 ... Unanswered •1 attempt left Rate law of a reaction is experimentally determined as Rate = k [A]^2 [B] The unit of k is 1/(M^2-sec) 1/(M-sec) sec/M M/sec M^2/sec Submit
The rate of the reaction (A[CI/Ar) was measured in three trials with varying initial concentrations of the reactants. [B] (M) A[CV/AI (M/s) Trial order: 3 order: [A]o (M) 0.600 0.600 rate = k 1.20 0.250 0.500 0.500 What is the order of the reaction with respect to reactant A? 3.05 x 10-6 What is the rate law for this reaction? 1.22 x 10-5 What is the order of the reaction with respect to reactant B? 1.22 x 10-5
For the reaction A + B + C D + E, the following data were obtained: Exp. A, M B, M C,M rate, M/s 1 0.70 0.20 0.40 35 2 0.70 0.60 0.40 105 3 0. 20 0.10 0.20 5.0 4 0. 80 0.10 0.20 20 5 0.37 0.86 0.18 80 6 0.37 0.86 0.77 80 7 0.58 0.39 0.99 ? What is the rate in line 7? (i.e., fill in the rate in above chart) For the reaction A + B + C D + E, the following data were obtained: Exp. A, M B, M…
The following initial rate data were found for the reaction 2MnO4 +5H₂C2O4 + 6H+ → 2 Mn²+ [-] (M) {H+] (M) 1.00×10-3 1.0 1.00×10-3 1.0 2.00×10-3 1.0 2.00×10-3 2.0 Experiment 1 [MnO4-] (M) 1.00×10-3 2.00×10-3 2.00×10-3 2.00×10-3 The rate law for this reaction is 2 (ر) Rate = k[MnO4]²[H₂C₂O4][H+] Rate = k[MnO4]²[H₂C₂O4]5[H+]6 Rate = k[MnO4]²[H₂C₂O4] Rate = k[MnO4][H₂C₂O4][H+] Rate = k[MnO4]²[H₂C₂O4]² + 10 C Rate (M/s) 2.0×10-4 8.0×10-4 1.6x10-3 1.6×10-3
Combination # [IO3-]0 [H+]0 [I-]0 average dt(sec) Initial rate, M s-1 kR (including units) 1 0.010 0.00002 0.10 18.1 0.00055 2 0.020 0.00002 0.10 9.1 0.0022 3 0.010 0.00002 0.20 5.1 0.0020 4 0.010 0.00002 0.10 5.1 0.0020 1. Determine the orders x,y and z 2. Calculatethe rate constant, kR and average kR for combimnations 1-4 3. Write the experimenally determined rate law Rate =kR[IO3-]x [I-]y [H+]z
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Use the following data to determine the rate law and the rate constant of the reaction 3A+B-->C+D
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Consider this initial rate data at a certain temperature in the table for the reaction [OCI-], [I]o [OH-]o Initial rates OH (aq) OCI (aq) + I (aq) OI (aq) + Cl¯(aq) Trial (М) (М) (M/s) (М) 1 0.00185 0.00185 0.450 0.000494 0.00185 0.00324 0.450 0.000864 3 0.00350 0.00185 0.621 0.000676 0.00324 0.653 0.000596 4 0.00185