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The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2 → N2 + 2 H2O Experiment 0.776 0.776 1.55 1.55 NO2l, M 4.80x10-2 9.60x10-2 4.80×10-2 9.60x10-2 Initial Rate, Ms1 1.29×10-5 2.58x10-5 2.57x10-5 5.15x10-4 Complete the rate law for this reaction in the box below. Use the form k A m B n where T is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m 01 In Rate = From these data, the rate constant is 1--1

The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2 → N2 + 2 H2O Experiment 0.776 0.776 1.55 1.55 NO2l, M 4.80x10-2 9.60x10-2 4.80×10-2 9.60x10-2 Initial Rate, Ms1 1.29×10-5 2.58x10-5 2.57x10-5 5.15x10-4 Complete the rate law for this reaction in the box below. Use the form k A m B n where T is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m 01 In Rate = From these data, the rate constant is 1--1

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section: Chapter Questions
Problem 90IL: The acid-catalyzed iodination of acetone CH3COCH3(aq) + I2(aq) CH3COCH2I(aq) + HI(aq) is a common...
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The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2 → N2 + 2 H2O Experiment 0.776 0.776 1.55 1.55 NO2l, M 4.80x10-2 9.60x10-2 4.80×10-2 9.60x10-2 Initial Rate, Ms1 1.29×10-5 2.58x10-5 2.57x10-5 5.15x10-4 Complete the rate law for this reaction in the box below. Use the form k A m B n where T is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m 01 In Rate = From these data, the rate constant is 1--1
Transcribed Image Text:The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution NH4+ + NO2 → N2 + 2 H2O Experiment 0.776 0.776 1.55 1.55 NO2l, M 4.80x10-2 9.60x10-2 4.80×10-2 9.60x10-2 Initial Rate, Ms1 1.29×10-5 2.58x10-5 2.57x10-5 5.15x10-4 Complete the rate law for this reaction in the box below. Use the form k A m B n where T is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m 01 In Rate = From these data, the rate constant is 1--1
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