The rate coefficient for the reaction CH₂O(g) + O(g) → HCO(g) + OH(g) was measured as a function of temperature. The results are: k(300 K) = 1.77 x 10-13 cm³ molec-¹ s-¹ k(500 K) = 1.38 x 10-12 cm³ molec-¹ s-¹ Determine the Arrhenius expression for the rate coefficient and make an energy diagram labeling the important points on the plot. AfH°298 (CH₂O) = -115.90 kJ mol-¹ AfH 298 (HCO) = 43.51 kJ mol-¹ AfH 298 (O) = 249.18 kJ mol-¹ AfH°298 (OH) = 38.99 kJ mol-¹

The rate coefficient for the reaction CH₂O(g) + O(g) → HCO(g) + OH(g) was measured as a function of temperature. The results are: k(300 K) = 1.77 x 10-13 cm³ molec-¹ s-¹ k(500 K) = 1.38 x 10-12 cm³ molec-¹ s-¹ Determine the Arrhenius expression for the rate coefficient and make an energy diagram labeling the important points on the plot. AfH°298 (CH₂O) = -115.90 kJ mol-¹ AfH 298 (HCO) = 43.51 kJ mol-¹ AfH 298 (O) = 249.18 kJ mol-¹ AfH°298 (OH) = 38.99 kJ mol-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

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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