The reaction 2N₂O(g) → O₂(g) +4NO₂(g) is first order in N205. For this reaction at 45°C, the rate constant k = 1.0 × 10-5 s-1, where the rate law is defined as A[N₂Os] At Rate =- -= * [N₂0s] For a particular experiment ([N2O5]0= 7.0 × 10−1 M), calculate [N205] after 2.7 × 105 seconds. a. 2.7 M Ob.1.0 × 10-3 M O c. 9.6 M Od. 6.7 x 10-5 M e. 0.14 M
The reaction 2N₂O(g) → O₂(g) +4NO₂(g) is first order in N205. For this reaction at 45°C, the rate constant k = 1.0 × 10-5 s-1, where the rate law is defined as A[N₂Os] At Rate =- -= * [N₂0s] For a particular experiment ([N2O5]0= 7.0 × 10−1 M), calculate [N205] after 2.7 × 105 seconds. a. 2.7 M Ob.1.0 × 10-3 M O c. 9.6 M Od. 6.7 x 10-5 M e. 0.14 M
Chemistry: Principles and Practice
3rd Edition
ISBN:9780534420123
Author:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Publisher:Daniel L. Reger, Scott R. Goode, David W. Ball, Edward Mercer
Chapter13: Chemical Kinetics
Section: Chapter Questions
Problem 13.57QE: The decomposition of ozone is a second-order reaction with a rate constant of 30.6 atm1 s1 at 95 C....
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![The reaction
2N₂O5 (8)→O₂(g) + 4NO₂(g)
is first order in N205. For this reaction at 45°C, the rate constant k = 1.0 × 10-5 s-1, where the rate law is defined as
A[N₂Os]
At
= [N₂O₁]
For a particular experiment ([N205]0 = 7.0 × 10−1 M), calculate [N205] after 2.7 × 105 seconds.
a. 2.7 M
Ob.1.0 x 10-3 M
O c. 9.6 M
Od. 6.7 x 10-5 M
O e. 0.14 M
Rate =-](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fe49ecbb2-f25c-46ea-84a1-b0b9efe71122%2F03d6efde-0868-451d-992a-de8e32e47880%2Fwsq0e9_processed.jpeg&w=3840&q=75)
Transcribed Image Text:The reaction
2N₂O5 (8)→O₂(g) + 4NO₂(g)
is first order in N205. For this reaction at 45°C, the rate constant k = 1.0 × 10-5 s-1, where the rate law is defined as
A[N₂Os]
At
= [N₂O₁]
For a particular experiment ([N205]0 = 7.0 × 10−1 M), calculate [N205] after 2.7 × 105 seconds.
a. 2.7 M
Ob.1.0 x 10-3 M
O c. 9.6 M
Od. 6.7 x 10-5 M
O e. 0.14 M
Rate =-
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