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The colorless gas N2O4 decomposes to the brown gas NO2 in a first order-reaction: N2O4(g) → 2 NO2(g) a) The rate constant k is 4.5 × 10³ s-l at 274 K and 1.00 × 104 s-l at 283 K. What is the activation energy, Ea for this reaction? b) Use a graphical method to calculate the value of k at 298 K. c) Is this reaction an elementary step?

The colorless gas N2O4 decomposes to the brown gas NO2 in a first order-reaction: N2O4(g) → 2 NO2(g) a) The rate constant k is 4.5 × 10³ s-l at 274 K and 1.00 × 104 s-l at 283 K. What is the activation energy, Ea for this reaction? b) Use a graphical method to calculate the value of k at 298 K. c) Is this reaction an elementary step?

Chemistry: Principles and Reactions
Chemistry: Principles and Reactions
8th Edition
ISBN:9781305079373
Author:William L. Masterton, Cecile N. Hurley
Publisher:William L. Masterton, Cecile N. Hurley
Chapter11: Rate Of Reaction
Section: Chapter Questions
Problem 67QAP: For the reaction 2N2O(g)2N2(g)+O2(g) the rate constant is 0.066 L/mol min at 565C and 22.8 L/mol min...
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The colorless gas N2O4 decomposes to the brown gas NO2 in a first order-reaction: N2O4(g) - →2 NO2(g) a) The rate constant k is 4.5 × 10³ s-' at 274 K and 1.00 × 104 s-l at 283 K. What is the activation energy, Ea for this reaction? b) Use a graphical method to calculate the value of k at 298 K. c) Is this reaction an elementary step?
Transcribed Image Text:The colorless gas N2O4 decomposes to the brown gas NO2 in a first order-reaction: N2O4(g) - →2 NO2(g) a) The rate constant k is 4.5 × 10³ s-' at 274 K and 1.00 × 104 s-l at 283 K. What is the activation energy, Ea for this reaction? b) Use a graphical method to calculate the value of k at 298 K. c) Is this reaction an elementary step?
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