Question 9 Consider the following reaction that follows a second order rate law. 2 NO2 (9) →2 NO (g) + O2 (g) If (NO210 = 0.0500 M and k = 0.543 M-1s-1, then what would be the concentration of NO2 after 1800 seconds? %3! %3D O 5.68 x 103 M O 1.77 x 103 M O 1.00 x 103 M O 2.05 x 103 M O 4.51 x 103 M
Question 9 Consider the following reaction that follows a second order rate law. 2 NO2 (9) →2 NO (g) + O2 (g) If (NO210 = 0.0500 M and k = 0.543 M-1s-1, then what would be the concentration of NO2 after 1800 seconds? %3! %3D O 5.68 x 103 M O 1.77 x 103 M O 1.00 x 103 M O 2.05 x 103 M O 4.51 x 103 M
Chemistry for Engineering Students
4th Edition
ISBN:9781337398909
Author:Lawrence S. Brown, Tom Holme
Publisher:Lawrence S. Brown, Tom Holme
Chapter11: Chemical Kinetics
Section: Chapter Questions
Problem 11.28PAE
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Question 9
Consider the following reaction that follows a second order rate law.
2 NO2 (g) → 2 NO (g) + O2 (g)
If (NO2]o = 0.0500 M and k = 0.543 M-1s-1, then what would be the concentration of NO2 after 1800 seconds?
O 5.68 x 10-3 M
O 1.77 x 10-3 M
O 1.00 x 10-3 M
O 2.05 x 10-3 M
O 4.51 x 10-3 M
A Moving to another question will save this response.
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Question 9
Consider the following reaction that follows a second order rate law.
2 NO2 (g) → 2 NO (g) + O2 (g)
If (NO2]o = 0.0500 M and k = 0.543 M-1s-1, then what would be the concentration of NO2 after 1800 seconds?
O 5.68 x 10-3 M
O 1.77 x 10-3 M
O 1.00 x 10-3 M
O 2.05 x 10-3 M
O 4.51 x 10-3 M
A Moving to another question will save this response.
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