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we following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH, + NO, N₂+ 2 H₂O xperiment [NH4] 0.554 0.554 I 2 3 4 1.11 1.11 k- MNO₂ la. M Initial Rate, M-s 8.61 x 10-5 1.72 x 10-5 1.73 x 10-5 3.45 x 10- Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for mor n and concentrations taken to the zero power do not appear Rate- 0.0500 0.100 0.0500 0.100 Ms

we following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH, + NO, N₂+ 2 H₂O xperiment [NH4] 0.554 0.554 I 2 3 4 1.11 1.11 k- MNO₂ la. M Initial Rate, M-s 8.61 x 10-5 1.72 x 10-5 1.73 x 10-5 3.45 x 10- Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for mor n and concentrations taken to the zero power do not appear Rate- 0.0500 0.100 0.0500 0.100 Ms

Chemistry
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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The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH₂+NO₂ → N₂+ 2 H₂O Experiment [NH4] MNO₂ lo. M Initial Rate, M-s 8.61 x 10-6 1.72 x 105 1.73 x 105 3.45 x 10-5 1 2 3 4 0.554 0.554 1.11 1.11 0.0500 0.100 0.0500 0.100 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate - k- M¹.8¹
Transcribed Image Text:The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH₂+NO₂ → N₂+ 2 H₂O Experiment [NH4] MNO₂ lo. M Initial Rate, M-s 8.61 x 10-6 1.72 x 105 1.73 x 105 3.45 x 10-5 1 2 3 4 0.554 0.554 1.11 1.11 0.0500 0.100 0.0500 0.100 Complete the rate law for this reaction in the box below. Use the form k[A] [B]", where '1' is understood for m or n and concentrations taken to the zero power do not appear. Don't enter 1 for m or n. Rate - k- M¹.8¹
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