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. N₂O5 NO₂ + 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.
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. N₂O5 NO₂ + 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.
Chemistry
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Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
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Chapter1: Chemical Foundations
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solve question 7
![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.](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2Fa50af9e4-75d3-4302-8305-ec9f1eb44db0%2Fe54b05e9-fdb3-49d8-825d-86a1934fc737%2F2y0mzxa_processed.jpeg&w=3840&q=75)
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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