The rate constant for the decomposition of nitrogen dioxide NO2(g) > NO (g) + 1/2 02(g) with a laser beam is 1.79 1/M: min. Find the time, in seconds, needed to decrease 2.14 M of NO2 to 1 M. Hint: What is the order of the reaction? How can you determine that? Units of k?
The rate constant for the decomposition of nitrogen dioxide NO2(g) > NO (g) + 1/2 02(g) with a laser beam is 1.79 1/M: min. Find the time, in seconds, needed to decrease 2.14 M of NO2 to 1 M. Hint: What is the order of the reaction? How can you determine that? Units of k?
Chemistry & Chemical Reactivity
10th Edition
ISBN:9781337399074
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter14: Chemical Kinetics: The Rates Of Chemical Reactions
Section14.7: Reaction Mechanisms
Problem 14.14CYU: One possible mechanism for the decomposition of nitryl chloride, NO2CI, is What is the overall...
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![The rate constant for the decomposition of nitrogen dioxide NO2(g) > NO (g) + 1/2 O2(g) with a
laser beam is 1.79 1/M: min. Find the time, in seconds, needed to decrease 2.14 M of NO2 to 1 M.
Hint: What is the order of the reaction? How can you determine that? Units of k?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0bbbbd3b-3a87-492d-8c19-9415e4831697%2F7b68d178-e997-4868-aed4-40efa3334cc4%2Fjb67fha_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The rate constant for the decomposition of nitrogen dioxide NO2(g) > NO (g) + 1/2 O2(g) with a
laser beam is 1.79 1/M: min. Find the time, in seconds, needed to decrease 2.14 M of NO2 to 1 M.
Hint: What is the order of the reaction? How can you determine that? Units of k?
Expert Solution
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Step 1
To solve this first we have determine the order of reaction by using rate law
Rate = K[A]n
Where K = rate constant
n = order of reaction
[A] = concentration of reactant
So from this equation
K = Rate /[A]n we will get n
Then according to that order of reaction we will calculate the time taken .
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