Consider the reaction: AB(g) → B(g) +A(g) with the rate law Rate = K[AB]2 and the rate constant k = 5.0 x 10-2 M-1s-1 3.What is the initial rate when the concentration of [AB] = 2.0 M a. 1.0 x 10-1 Ms-1 b. 2.0 x 10-1 Ms-1 c. 1.0 Ms-1 d. 2.0 Ms-1 e. 5.0 x 10-2 MS-1

Consider the reaction: AB(g) → B(g) +A(g) with the rate law Rate = K[AB]2 and the rate constant k = 5.0 x 10-2 M-1s-1 3.What is the initial rate when the concentration of [AB] = 2.0 M a. 1.0 x 10-1 Ms-1 b. 2.0 x 10-1 Ms-1 c. 1.0 Ms-1 d. 2.0 Ms-1 e. 5.0 x 10-2 MS-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

Chapter12: Chemical Kinetics

Section: Chapter Questions

Problem 100AE: Consider a hypothetical reaction between A and B: A + B products Use the following initial rate...

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At 40C, H2O2 (aq) will decompose according to the following reaction: 2H2O2(aq)2H2O(l)+O2(g) The following data were collected for the concentration of H2O2 at various times. Times(s) [H2O2](mol/L) 0 1.000 2.16 104 0.500 4.32 104 0.250 a. Calculate the average rate of decomposition of H2O2 between 0 and 2.16 104 s. Use this rate to calculate the average rate of production of O2(g) over the same time period. b. What are these rates for the time period 2.16 104 s to 4.32 104 s?
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