For the reaction: NO2(g) → 1/2O2(g) + NO (g) The following data were obtained: [NO₂] (M) Natural Log [NO2] (M) 0.01 -4.605170186 100 Time (s) 0 50 100 300 200 0.00481 -5.337058195 0.00787 -4.844697217 127.064803 0.00649 -5.037492748 Concentration NO2 0.012 0.0038 -5.572754212 263.1578947 Determine the rate law of this reaction and the value of k, the rate constant. The graphs of the data appear below. 0.01 0.008 0.006 0.004 0.002 0 0 1/[NO2] 100 154.0832049 200 Time (s) 207.9002079 y=-1.97E-05x +9.15E-03 R² = 9.27E-01 1/[NO2] 300 250 200 150 8 100 50 。 300 0 50 400 100 Natural Log [NO2] 4.5 -4.7 -5.1 -5.3 -5.5 -5.7 0 y=0.5431x +99.833 R² = 1 150 200 Time (s) 100 250 200 Time (s) 300 350 y = -0.0032x-4.6679 R² = 0.9824 300 400

For the reaction: NO2(g) → 1/2O2(g) + NO (g) The following data were obtained: [NO₂] (M) Natural Log [NO2] (M) 0.01 -4.605170186 100 Time (s) 0 50 100 300 200 0.00481 -5.337058195 0.00787 -4.844697217 127.064803 0.00649 -5.037492748 Concentration NO2 0.012 0.0038 -5.572754212 263.1578947 Determine the rate law of this reaction and the value of k, the rate constant. The graphs of the data appear below. 0.01 0.008 0.006 0.004 0.002 0 0 1/[NO2] 100 154.0832049 200 Time (s) 207.9002079 y=-1.97E-05x +9.15E-03 R² = 9.27E-01 1/[NO2] 300 250 200 150 8 100 50 。 300 0 50 400 100 Natural Log [NO2] 4.5 -4.7 -5.1 -5.3 -5.5 -5.7 0 y=0.5431x +99.833 R² = 1 150 200 Time (s) 100 250 200 Time (s) 300 350 y = -0.0032x-4.6679 R² = 0.9824 300 400

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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