Consider the following reaction that follows a second order rate law. 2 NO2 (g) → 2 NO (g) + 02 (9) - f [NO2]0= = 0.0900 M and k = 0.543 M-1s-1, then what would be the concentration of NO2 after 1600 seconds? 9.52 x 10-3 M 1.14 × 10-3 M 2.91 × 10-3 M 7.64 × 10-3 M 2.51 × 10-3 M
Consider the following reaction that follows a second order rate law. 2 NO2 (g) → 2 NO (g) + 02 (9) - f [NO2]0= = 0.0900 M and k = 0.543 M-1s-1, then what would be the concentration of NO2 after 1600 seconds? 9.52 x 10-3 M 1.14 × 10-3 M 2.91 × 10-3 M 7.64 × 10-3 M 2.51 × 10-3 M
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
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
Section: Chapter Questions
Problem 89SCQ: The following statements relate to the reaction for the formation of HI: H2(g) + I2(g) 2 HI(g)Rate...
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![Consider the following reaction that follows a second order rate law.
2 NO2 (g) → 2 NO (g) + 02 (9)
If [NO2]0= 0.0900 M and k =
9.52 x 10-3 M
1.14 x 10-3 M
2.91 × 10-3 M
O 7.64 × 10-3 M
O 2.51 × 10-3 M
0.543 M-1s-1, then what would be the concentration of NO2 after 1600 seconds?](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F8afd3e8f-293d-45a8-8702-4440333f37df%2Fa299a89a-6c2d-41b4-82a5-9f3f19835623%2F6pcus15_processed.jpeg&w=3840&q=75)
Transcribed Image Text:Consider the following reaction that follows a second order rate law.
2 NO2 (g) → 2 NO (g) + 02 (9)
If [NO2]0= 0.0900 M and k =
9.52 x 10-3 M
1.14 x 10-3 M
2.91 × 10-3 M
O 7.64 × 10-3 M
O 2.51 × 10-3 M
0.543 M-1s-1, then what would be the concentration of NO2 after 1600 seconds?
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