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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 by OpenStax (2015-05-04)
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
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Problem 49E: Nitroglycerine is an extremely sensitive explosive. In a series of carefully controlled experiments,...
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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-¹s-¹. Using this value for the rate constant, the rate of the reaction when [NH4+] 0.276 M and [NO₂] = 0.104 M would be M/s. =
Transcribed Image Text: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-¹s-¹. Using this value for the rate constant, the rate of the reaction when [NH4+] 0.276 M and [NO₂] = 0.104 M would be M/s. =
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