The oxidation of nitrogen monoxide by oxygen at 25 °C 2NO+O₂ → 2NO₂ is second order in NO and first order in O₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 9.66 x 10³ M³s¹. Using this value for the rate constant, the rate of the reaction when [NO] 6.42 x 103 M and [0₂]- 3.01 x 103 M would be M/s.

The oxidation of nitrogen monoxide by oxygen at 25 °C 2NO+O₂ → 2NO₂ is second order in NO and first order in O₂. Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate = In an experiment to determine the rate law, the rate constant was determined to be 9.66 x 10³ M³s¹. Using this value for the rate constant, the rate of the reaction when [NO] 6.42 x 103 M and [0₂]- 3.01 x 103 M would be M/s.

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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