The reaction of nitrogen dioxide with fluorine 2NO2+ F2 → 2NO₂F is first order in NO₂ and first order in F2. 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 of the reaction was determined to be 1.40 × 10-³ M s¹, when [NO₂] = 2.36 M and [F₂] = 4.12 M. From this experiment, the rate constant is M¹.s-¹.
The reaction of nitrogen dioxide with fluorine 2NO2+ F2 → 2NO₂F is first order in NO₂ and first order in F2. 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 of the reaction was determined to be 1.40 × 10-³ M s¹, when [NO₂] = 2.36 M and [F₂] = 4.12 M. From this experiment, the rate constant is M¹.s-¹.
Chemistry
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ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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![The reaction of nitrogen dioxide with fluorine
2NO2+ F2 → 2NO₂ F
is first order in
NO2 and first order in
F2.
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 of the reaction was determined to be
1.40 × 10-³ M.s¹, when
[NO₂] = 2.36 M and
[F₂]
= 4.12 M. From this experiment, the rate constant is
M¹. s-¹](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0a6c9e0c-0b6a-4785-ae3f-5e292bd65bb9%2F9ce57992-7317-4316-ae73-7fb1e667476a%2Fy7kqh9h_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The reaction of nitrogen dioxide with fluorine
2NO2+ F2 → 2NO₂ F
is first order in
NO2 and first order in
F2.
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 of the reaction was determined to be
1.40 × 10-³ M.s¹, when
[NO₂] = 2.36 M and
[F₂]
= 4.12 M. From this experiment, the rate constant is
M¹. s-¹
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