The oxidation of nitrogen monoxide by oxygen at 25 °C 2 NO + 022 NO2 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 of the reaction was determined to be 6.91×10o-4 Ms1 when [NO] = 5.26x103 M and [02] = 2.53x103 M. From this experiment, the rate constant is

The oxidation of nitrogen monoxide by oxygen at 25 °C 2 NO + 022 NO2 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 of the reaction was determined to be 6.91×10o-4 Ms1 when [NO] = 5.26x103 M and [02] = 2.53x103 M. From this experiment, the rate constant is

Chemistry by OpenStax (2015-05-04)

1st Edition

ISBN:9781938168390

Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser

Chapter12: Kinetics

Section: Chapter Questions

Problem 25E: Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following...

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