The following experimental data were obtained for the reaction of NH4+ and NO2 in acidic NH, + (aq) + NO2 (aq) N2(g) +2 H20(€) [NH, ] (mol L-1) NO,-] (mol L-1) Rate = A[N2]/At (mol L-s) 0.0069 0.078 2.85 x 10-7 0.0069 0.039 1.43 x 10-7 0.0366 0.156 3.02 x 10-6 0.0186 0.156 1.54 x 10-6 Determine the rate law for this reaction. (Use k for the rate constant.) Rate = Calculate the rate constant. Rate constant =

The following experimental data were obtained for the reaction of NH4+ and NO2 in acidic NH, + (aq) + NO2 (aq) N2(g) +2 H20(€) [NH, ] (mol L-1) NO,-] (mol L-1) Rate = A[N2]/At (mol L-s) 0.0069 0.078 2.85 x 10-7 0.0069 0.039 1.43 x 10-7 0.0366 0.156 3.02 x 10-6 0.0186 0.156 1.54 x 10-6 Determine the rate law for this reaction. (Use k for the rate constant.) Rate = Calculate the rate constant. Rate constant =

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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