10.5. The rate of formation of the product of a reaction is found to give a nonlinear Arrhenius plot, the line being convex to the 1/T axis (i.e., the activation energy is higher at higher temperatures). Suggest a reason for this type of behavior. (Hint: For this and the following problem, consider the possibility of two parallel reactions and of two consecutive reactions having different activation energies.)
10.5. The rate of formation of the product of a reaction is found to give a nonlinear Arrhenius plot, the line being convex to the 1/T axis (i.e., the activation energy is higher at higher temperatures). Suggest a reason for this type of behavior. (Hint: For this and the following problem, consider the possibility of two parallel reactions and of two consecutive reactions having different activation energies.)
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
Section: Chapter Questions
Problem 1RQ: Define and explain the differences between the following terms. a. law and theory b. theory and...
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solve question 5
Transcribed Image Text:10.4. A reaction of stoichiometry
A+B=Y + Z
is found to be second order in A and zero order in B.
Suggest a mechanism that is consistent with this
behavior.
10.5. The rate of formation of the product of a reaction is
found to give a nonlinear Arrhenius plot, the line being
convex to the 1/T axis (i.e., the activation energy is higher
at higher temperatures). Suggest a reason for this type of
behavior. (Hint: For this and the following problem,
consider the possibility of two parallel reactions and of
two consecutive reactions having different activation
energies.)
10.6. An Arrhenius plot is concave to the 1/T axis (i.e., it
exhibits a lower activation energy at higher temperatures).
Suggest a reason for this type of behavior.
10.7. Nitrogen pentoxide reacts with nitric oxide in the gas
phase according to the stoichiometric equation
N₂O5 + NO = 3NO₂
The following mechanism has been proposed.
N₂O5NO₂ + NO3
NO₂ + NO3
N₂O5
NO + NO3 → 2NO₂
Assume that the steady-state treatment can be applied to
NO3, and derive an equation for the rate of consumption of
N₂O5.
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