to nitrogen dioxide and chlorine, according to the 2 NO₂Cl 2 NO2 + Cl2 The experimental rate law for this reaction is Rate = k [NO₂CI] Which, if any, of the following mechanisms are consistent with the observed rate law? More than one answer is possible. Write the overall reaction and rate law for each mechanism. a) NO₂CINO₂ + Cl (slow) CI+NO₂CI NO2 + Cl₂ (fast) 1) Nitryl chloride decomposes following reaction: b) 2 NO₂CI k2 N₂O4 c) 2 NO₂CI 2 NO₂ (slow) N₂O + CIO₂ N₂O4 N2O4 + Cl2 (fast equilibrium) k3 CIO2 + N₂O + CIO (fast equilibrium) + NOCI (fast equilibrium) NOCI+CIO → NO2 + Cl2 (slow)
to nitrogen dioxide and chlorine, according to the 2 NO₂Cl 2 NO2 + Cl2 The experimental rate law for this reaction is Rate = k [NO₂CI] Which, if any, of the following mechanisms are consistent with the observed rate law? More than one answer is possible. Write the overall reaction and rate law for each mechanism. a) NO₂CINO₂ + Cl (slow) CI+NO₂CI NO2 + Cl₂ (fast) 1) Nitryl chloride decomposes following reaction: b) 2 NO₂CI k2 N₂O4 c) 2 NO₂CI 2 NO₂ (slow) N₂O + CIO₂ N₂O4 N2O4 + Cl2 (fast equilibrium) k3 CIO2 + N₂O + CIO (fast equilibrium) + NOCI (fast equilibrium) NOCI+CIO → NO2 + Cl2 (slow)
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
Section: Chapter Questions
Problem 25E: Nitrogen monoxide reacts with chlorine according to the equation: 2NOCI(g)2NOCI(g) The following...
Related questions
Question
plz help me solve question 1
![Chem 102
Chapter 15 Workshop, Part 2: Kinetics
1) Nitryl chloride decomposes to nitrogen dioxide and chlorine, according to the
following reaction:
2 NO₂CI → 2 NO₂ + Cl₂
The experimental rate law for this reaction is Rate = k [NO₂CI]
Which, if any, of the following mechanisms are consistent with the observed rate law?
More than one answer is possible.
Write the overall reaction and rate law for each mechanism.
a) NO₂CINO₂ + Cl (slow)
k2
CI + NO₂CI NO₂ + Cl₂ (fast)
b) 2 NO₂Cl
k2
N₂O4
c) 2 NO₂CI
N₂O4 + Cl₂ (fast equilibrium)
2 NO₂ (slow)
N₂O + CIO₂
CIO2 + N₂O + CIO (fast equilibrium)
NO₂ + NOCI (fast equilibrium)
Dr. Harvey
k3
NOCI+ CIO NO₂ + Cl₂ (slow)
2) Given the following reaction mechanism,](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fd38dc3ae-53e5-4279-afed-9e69fa663b8c%2F04404afc-3353-4b10-b3e5-57b67e3290ae%2Fdnbbsm_processed.png&w=3840&q=75)
Transcribed Image Text:Chem 102
Chapter 15 Workshop, Part 2: Kinetics
1) Nitryl chloride decomposes to nitrogen dioxide and chlorine, according to the
following reaction:
2 NO₂CI → 2 NO₂ + Cl₂
The experimental rate law for this reaction is Rate = k [NO₂CI]
Which, if any, of the following mechanisms are consistent with the observed rate law?
More than one answer is possible.
Write the overall reaction and rate law for each mechanism.
a) NO₂CINO₂ + Cl (slow)
k2
CI + NO₂CI NO₂ + Cl₂ (fast)
b) 2 NO₂Cl
k2
N₂O4
c) 2 NO₂CI
N₂O4 + Cl₂ (fast equilibrium)
2 NO₂ (slow)
N₂O + CIO₂
CIO2 + N₂O + CIO (fast equilibrium)
NO₂ + NOCI (fast equilibrium)
Dr. Harvey
k3
NOCI+ CIO NO₂ + Cl₂ (slow)
2) Given the following reaction mechanism,
Expert Solution
This question has been solved!
Explore an expertly crafted, step-by-step solution for a thorough understanding of key concepts.
Step by step
Solved in 5 steps with 8 images
Knowledge Booster
Learn more about
Need a deep-dive on the concept behind this application? Look no further. Learn more about this topic, chemistry and related others by exploring similar questions and additional content below.Recommended textbooks for you
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry by OpenStax (2015-05-04)
Chemistry
ISBN:
9781938168390
Author:
Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:
OpenStax
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781337399074
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: The Molecular Science
Chemistry
ISBN:
9781285199047
Author:
John W. Moore, Conrad L. Stanitski
Publisher:
Cengage Learning
Chemistry for Engineering Students
Chemistry
ISBN:
9781337398909
Author:
Lawrence S. Brown, Tom Holme
Publisher:
Cengage Learning
Chemistry & Chemical Reactivity
Chemistry
ISBN:
9781133949640
Author:
John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:
Cengage Learning
Chemistry: An Atoms First Approach
Chemistry
ISBN:
9781305079243
Author:
Steven S. Zumdahl, Susan A. Zumdahl
Publisher:
Cengage Learning