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. The decomposition of N₂O5 in carbon tetrachloride has been studied: 2 N₂Os (g) → 2 N₂O4 (g) + O₂(g) The concentration of N₂O5 is monitored for 1200 seconds and measured every 400 seconds. The data are tabulated below: time(s) [N₂O5] (M) 1.40 400.0 1.10 800.0 0.87 1200.0 0.68 (a) Fill the blanks in the table. Note that the last column is the average rate of reaction. (b) Briefly explain why the rates are decreasing. 0.0 Δt(s) A[N₂O5](M) Rate =L A[N₂O5]/At(M/s) -

. The decomposition of N₂O5 in carbon tetrachloride has been studied: 2 N₂Os (g) → 2 N₂O4 (g) + O₂(g) The concentration of N₂O5 is monitored for 1200 seconds and measured every 400 seconds. The data are tabulated below: time(s) [N₂O5] (M) 1.40 400.0 1.10 800.0 0.87 1200.0 0.68 (a) Fill the blanks in the table. Note that the last column is the average rate of reaction. (b) Briefly explain why the rates are decreasing. 0.0 Δt(s) A[N₂O5](M) Rate =L A[N₂O5]/At(M/s) -

Chemistry for Engineering Students
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 11.69PAE: In Chapter 3, we discussed the conversion of biomass into biofuels. One important area of research...
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. The decomposition of N₂O5 in carbon tetrachloride has been studied: 2 N₂O5 (g) → 2 N₂O4 (g) + O₂(g) The concentration of N₂O5 is monitored for 1200 seconds and measured every 400 seconds. The data are tabulated below: [N₂O5] (M) 0.0 1.40 400.0 1.10 800.0 0.87 1200.0 0.68 (a) Fill the blanks in the table. Note that the last column is the average rate of reaction. (b) Briefly explain why the rates are decreasing. time(s) At(s) Rate =- A[N₂O5]/At(M/s) A[N₂O5](M)
Transcribed Image Text:. The decomposition of N₂O5 in carbon tetrachloride has been studied: 2 N₂O5 (g) → 2 N₂O4 (g) + O₂(g) The concentration of N₂O5 is monitored for 1200 seconds and measured every 400 seconds. The data are tabulated below: [N₂O5] (M) 0.0 1.40 400.0 1.10 800.0 0.87 1200.0 0.68 (a) Fill the blanks in the table. Note that the last column is the average rate of reaction. (b) Briefly explain why the rates are decreasing. time(s) At(s) Rate =- A[N₂O5]/At(M/s) A[N₂O5](M)
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