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 & 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
Section14.3: Effect Of Concentration On Reaction Rate
Problem 1RC: The reaction NO(g) + 1/2 Cl2(g) NOCl(g) is first-order in [Cl2] and second-order with respect to...
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