The reaction of nitrogen monoxide with ozone at 25 °C NO + O3 → NO₂ + O₂ is first order in NO and first order in 03. Complete the rate law for this reaction in the box below. Use the form k[A]m [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate= [NO][0₂] -1 S In an experiment to determine the rate law, the rate constant was determined to be 1.15 × 10² M²¹s¹. Using this value for the rate constant, the rate of the reaction when [NO] = 0.182 M and [O3] = 0.0192 M would be 0.402 M/s.

The reaction of nitrogen monoxide with ozone at 25 °C NO + O3 → NO₂ + O₂ is first order in NO and first order in 03. Complete the rate law for this reaction in the box below. Use the form k[A]m [B]", where '1' is understood for m, n ... (don't enter 1) and concentrations taken to the zero power do not appear. Rate= [NO][0₂] -1 S In an experiment to determine the rate law, the rate constant was determined to be 1.15 × 10² M²¹s¹. Using this value for the rate constant, the rate of the reaction when [NO] = 0.182 M and [O3] = 0.0192 M would be 0.402 M/s.

Chemistry: Principles and Practice

3rd Edition

ISBN:9780534420123

Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer

Chapter13: Chemical Kinetics

Section: Chapter Questions

Problem 13.50QE

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