The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+NO₂ → N₂+ 2 H₂O Experiment [NH4+, MNO₂ ]o, M Initial Rate, M. s-¹ 1.45 x 10-6 2.89 x 10-6 1 2 3 4 Rate = 0.128 0.128 0.255 0.255 k = 0.0358 0.0715 0.0358 0.0715 M-¹.8-¹ -6 2.88 x 107 5.76 x 10 Complete the rate law for this reaction in the box below. Use the form [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. -6
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution: NH4+NO₂ → N₂+ 2 H₂O Experiment [NH4+, MNO₂ ]o, M Initial Rate, M. s-¹ 1.45 x 10-6 2.89 x 10-6 1 2 3 4 Rate = 0.128 0.128 0.255 0.255 k = 0.0358 0.0715 0.0358 0.0715 M-¹.8-¹ -6 2.88 x 107 5.76 x 10 Complete the rate law for this reaction in the box below. Use the form [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. -6
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:
NH4+NO₂ → N₂ + 2 H₂O
Experiment [NH4+]o, M [NO₂ ]o, M Initial Rate, M. s-1
0.0358
1.45 x 10-6
0.0715
0.0358
0.0715
1
2
3
4
Rate =
0.128
0.128
0.255
0.255
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.
k =
2.89 x 10-6
2.88 x 10-6
5.76 x 10-6
M-1.s-1
![Use the References to access important values if needed for this question.
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution:
NH4++NO₂ → N₂+ 2 H₂O
Experiment [NH4+]o, M [NO₂ lo. M Initial Rate, M. s-¹
0'
0.0358
1.45 x 10-6
0.0715
0.0358
0.0715
1
2
3
4
Rate =
0.128
0.128
0.255
0.255
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.
k =
2.89 x 10-6
2.88 x 10-6
5.76 x 10-6
-1
M-¹.8-¹](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F88b4235c-2b0d-4459-88fc-1ffa51a7c481%2Fe1b9d3cd-e26e-47af-833e-70bb594604ba%2Fd5d20up_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Use the References to access important values if needed for this question.
The following initial rate data are for the reaction of ammonium ion with nitrite ion in aqueous solution:
NH4++NO₂ → N₂+ 2 H₂O
Experiment [NH4+]o, M [NO₂ lo. M Initial Rate, M. s-¹
0'
0.0358
1.45 x 10-6
0.0715
0.0358
0.0715
1
2
3
4
Rate =
0.128
0.128
0.255
0.255
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.
k =
2.89 x 10-6
2.88 x 10-6
5.76 x 10-6
-1
M-¹.8-¹
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