The reaction of nitrogen monoxide with ozone at 25 °CNO + O3 NO2 + 02is first order in NO and first order in 02.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) andconcentrations taken to the zero power do not appear.Rate =In an experiment to determine the rate law, the rate constant was determined to be 111 M-ls1.Using this value for the rate constant, the rate of the reaction when [NO] = 0.117 M and [O3] =Ms4.59x10-2 M would be

In this above Questions, already we know the order with respect to reactants So ; Rate law is Rate…

ogen monoxide with ozone at 25 °C + 02 and first order in O3. law for this reaction in the box below. "B]"... , where '1' is understood for m, n ... (don't enter 1) and n to the zero power do not appear. determine the rate law, the rate constant was determined to be rote of the reaction when [NO] = 0.117 M

ogen monoxide with ozone at 25 °C + 02 and first order in O3. law for this reaction in the box below. "B]"... , where '1' is understood for m, n ... (don't enter 1) and n to the zero power do not appear. determine the rate law, the rate constant was determined to be rote of the reaction when [NO] = 0.117 M

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 115QRT

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