The reaction of ammonium ion with nitrite ion in aqueous solution NH4++NO₂¯¯ → N₂ + 2H₂O is first order in NH4+ and first order in NO₂¯. 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 constant was determined to be 3.81 × 10-4 M¯¹s¹. Using this value for the rate constant, the rate of the reaction when [NH₂+] = 0.276 M and [NO₂¯] = 0.104 M would be M/s.

The reaction of ammonium ion with nitrite ion in aqueous solution NH4++NO₂¯¯ → N₂ + 2H₂O is first order in NH4+ and first order in NO₂¯. 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 constant was determined to be 3.81 × 10-4 M¯¹s¹. Using this value for the rate constant, the rate of the reaction when [NH₂+] = 0.276 M and [NO₂¯] = 0.104 M would be M/s.

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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