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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
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?
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
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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