6. The rate constant for the reaction, 2 N₂O5 (g) → 4 NO₂ (g) + O2 (g), doubles when the temperature is raised from 295.65 K to 300.62 K. (a) Determine the activation energy (in kJ/mol) for the reaction, assuming that the pre- exponential factor, A, in the Arrhenius equation is independent of temperature. (b) At what temperature would you predict this rate constant to increase by another factor of 10 relative to its value at 300.62 K?

6. The rate constant for the reaction, 2 N₂O5 (g) → 4 NO₂ (g) + O2 (g), doubles when the temperature is raised from 295.65 K to 300.62 K. (a) Determine the activation energy (in kJ/mol) for the reaction, assuming that the pre- exponential factor, A, in the Arrhenius equation is independent of temperature. (b) At what temperature would you predict this rate constant to increase by another factor of 10 relative to its value at 300.62 K?

Chemistry: The Molecular Science

5th Edition

ISBN:9781285199047

Author:John W. Moore, Conrad L. Stanitski

Publisher:John W. Moore, Conrad L. Stanitski

Chapter11: Chemical Kinetics: Rates Of Reactions

Section: Chapter Questions

Problem 11.ACP: (Section 11-5) A rule of thumb is that for a typical reaction, if concentrations are unchanged, a...

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