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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 by OpenStax (2015-05-04)
Chemistry by OpenStax (2015-05-04)
1st Edition
ISBN:9781938168390
Author:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Publisher:Klaus Theopold, Richard H Langley, Paul Flowers, William R. Robinson, Mark Blaser
Chapter12: Kinetics
Section: Chapter Questions
Problem 63E: Hydrogen iodide, HI, decomposes in the gas phase to produce hydrogen, H2, and iodine, I2. The value...
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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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