8. The thermal decomposition of nitric oxide at elevated temperatures 2NO → N₂+02 has been studied in a batch reactor where at temperatures below 2000K the rate expression that applies to low conversions is: r = kCm05 Co At high conversions, or when the initial mixture contains a high concentration of O2 the rate expression is given by: r = k' Cм0.5 C15C0,5 To explain these kinetics the following chain reaction mechanism has been proposed: Initiation: Propagation: 2NON₂O +0 k₂ E1=272.0 kJ/mol 0+ NO O₂+ N E₂-161.0 kJ/mol N+NO N₂+0 E3-1.4 kJ/mol K4 20+ MO₂+M E4=14.0 kJ/mol ks Termination: where M is any molecule capable of the energy transfer necessary to stabilize the oxygen molecule. Once appreciable amounts of O2 are present in the reaction mixture, the initiation reaction that is the primary source of atomic oxygen is no longer the first reaction. Instead, the following reaction begins to dominate the chain initiation process: Initiation (high O2): ks NO +0₂ NO₂+0 E5=198.0 kJ/mol a. Determine whether the proposed mechanism is consistent with the two limiting forms of the rate expression indicated above. b. If it is consistent how are the rate constants k and k' related to the rate constants of the mechanistic equations? c. What are the values of the experimental activation energy that are predicted at high and low conversions of NO? [related reference: Wu and Yeh, Int. J. of Chem. Kinetics, 28, 89, 1996)]
8. The thermal decomposition of nitric oxide at elevated temperatures 2NO → N₂+02 has been studied in a batch reactor where at temperatures below 2000K the rate expression that applies to low conversions is: r = kCm05 Co At high conversions, or when the initial mixture contains a high concentration of O2 the rate expression is given by: r = k' Cм0.5 C15C0,5 To explain these kinetics the following chain reaction mechanism has been proposed: Initiation: Propagation: 2NON₂O +0 k₂ E1=272.0 kJ/mol 0+ NO O₂+ N E₂-161.0 kJ/mol N+NO N₂+0 E3-1.4 kJ/mol K4 20+ MO₂+M E4=14.0 kJ/mol ks Termination: where M is any molecule capable of the energy transfer necessary to stabilize the oxygen molecule. Once appreciable amounts of O2 are present in the reaction mixture, the initiation reaction that is the primary source of atomic oxygen is no longer the first reaction. Instead, the following reaction begins to dominate the chain initiation process: Initiation (high O2): ks NO +0₂ NO₂+0 E5=198.0 kJ/mol a. Determine whether the proposed mechanism is consistent with the two limiting forms of the rate expression indicated above. b. If it is consistent how are the rate constants k and k' related to the rate constants of the mechanistic equations? c. What are the values of the experimental activation energy that are predicted at high and low conversions of NO? [related reference: Wu and Yeh, Int. J. of Chem. Kinetics, 28, 89, 1996)]
Introduction to Chemical Engineering Thermodynamics
8th Edition
ISBN:9781259696527
Author:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Publisher:J.M. Smith Termodinamica en ingenieria quimica, Hendrick C Van Ness, Michael Abbott, Mark Swihart
Chapter1: Introduction
Section: Chapter Questions
Problem 1.1P
Related questions
Question
![8. The thermal decomposition of nitric oxide at elevated temperatures
2NO → N₂+02
has been studied in a batch reactor where at temperatures below 2000K the rate
expression that applies to low conversions is:
r = kCm05 Co
At high conversions, or when the initial mixture contains a high concentration of O2 the
rate expression is given by:
r = k' Cм0.5 C15C0,5
To explain these kinetics the following chain reaction mechanism has been proposed:
Initiation:
Propagation:
2NON₂O +0
k₂
E1=272.0 kJ/mol
0+ NO O₂+ N
E₂-161.0 kJ/mol
N+NO N₂+0
E3-1.4 kJ/mol
K4
20+ MO₂+M
E4=14.0 kJ/mol
ks
Termination:
where M is any molecule capable of the energy transfer necessary to stabilize the oxygen
molecule.
Once appreciable amounts of O2 are present in the reaction mixture, the initiation
reaction that is the primary source of atomic oxygen is no longer the first reaction.
Instead, the following reaction begins to dominate the chain initiation process:
Initiation (high O2):
ks
NO +0₂ NO₂+0 E5=198.0 kJ/mol
a. Determine whether the proposed mechanism is consistent with the two limiting
forms of the rate expression indicated above.
b. If it is consistent how are the rate constants k and k' related to the rate constants of
the mechanistic equations?
c. What are the values of the experimental activation energy that are predicted at
high and low conversions of NO?
[related reference: Wu and Yeh, Int. J. of Chem. Kinetics, 28, 89, 1996)]](/v2/_next/image?url=https%3A%2F%2Fcontent.bartleby.com%2Fqna-images%2Fquestion%2F0efff925-8d44-4087-926b-fe71bc58fe4c%2Ffa5d551f-1940-4a67-a53f-e0d9b522a2ba%2F9rd0x7_processed.png&w=3840&q=75)
Transcribed Image Text:8. The thermal decomposition of nitric oxide at elevated temperatures
2NO → N₂+02
has been studied in a batch reactor where at temperatures below 2000K the rate
expression that applies to low conversions is:
r = kCm05 Co
At high conversions, or when the initial mixture contains a high concentration of O2 the
rate expression is given by:
r = k' Cм0.5 C15C0,5
To explain these kinetics the following chain reaction mechanism has been proposed:
Initiation:
Propagation:
2NON₂O +0
k₂
E1=272.0 kJ/mol
0+ NO O₂+ N
E₂-161.0 kJ/mol
N+NO N₂+0
E3-1.4 kJ/mol
K4
20+ MO₂+M
E4=14.0 kJ/mol
ks
Termination:
where M is any molecule capable of the energy transfer necessary to stabilize the oxygen
molecule.
Once appreciable amounts of O2 are present in the reaction mixture, the initiation
reaction that is the primary source of atomic oxygen is no longer the first reaction.
Instead, the following reaction begins to dominate the chain initiation process:
Initiation (high O2):
ks
NO +0₂ NO₂+0 E5=198.0 kJ/mol
a. Determine whether the proposed mechanism is consistent with the two limiting
forms of the rate expression indicated above.
b. If it is consistent how are the rate constants k and k' related to the rate constants of
the mechanistic equations?
c. What are the values of the experimental activation energy that are predicted at
high and low conversions of NO?
[related reference: Wu and Yeh, Int. J. of Chem. Kinetics, 28, 89, 1996)]
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