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Transcript of WHAT CAN KINETICS LEARN FROM NONSTATIONARY THERMODYNAMICS Miloslav Pekař Faculty of Chemistry...
![Page 1: WHAT CAN KINETICS LEARN FROM NONSTATIONARY THERMODYNAMICS Miloslav Pekař Faculty of Chemistry Institute of Physical and Applied Chemistry Brno University.](https://reader035.fdocuments.net/reader035/viewer/2022062517/56649e795503460f94b79a46/html5/thumbnails/1.jpg)
WHAT CAN KINETICS LEARN FROM NONSTATIONARY
THERMODYNAMICS
Miloslav Pekař
Faculty of ChemistryInstitute of Physical and Applied Chemistry
Brno University of TechnologyBrno, Czech Republic
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INTRODUCTION
• Evolution of experimental methods in chemical kinetics.
• Fine details of chemical processes and their mechanism can be obtained.
• Evolution of thermodynamics up to several general theories not limited by space or time homogeneity.
• Kinetics and thermodynamics – two different and independent, though complementary approaches to description of chemically reacting systems.
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INTRODUCTION
• Most often thermodynamic-equilibrium restrictions on chemical processes and rate equations are discussed.
• Rational thermodynamics + Samohýl new approach to chemical kinetics.
• Direct derivation of rate equations with new insights on the relationships between mechanism and kinetics.
• Overview of this method and its potential relevance in kinetic research and data treatment.
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ESSENCE – function
Rational thermodynamics proof:
for fluids with linear transport properties
reaction rate is function of only temperature and densities
or, alternatively, concentrations:
J = J(T,c)
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ESSENCE – approximationProved general function is approximated by a
polynomial of degree M:
McnZ n
01 0
,ν
kJ
),,,( 21 n ν
J = (J1, J2…, Jp)
p…number of independent reactions
n…number of components
),,,( 21 pkkk
ννννk
rate constants vector:
Z…number of polynomial terms
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ESSENCE – consistency
Fundamental thermodynamic requirement:
equilibrium concentrations found fromkinetic equilibrium condition, J = 0,
must accord with the values of equilibrium constants
restrictions on approximating polynomial follow
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ESSENCE – procedure
1. Independent reactions are selected.
2. Approximating polynomial of selected degree is constructed.
3. Equilibrium constants are used to express some concentrations as functions of remaining ones.
4. Modified polynomial should be zero for arbitrary equilibrium values of remaining concentrations.
5. Simplified polynomial results.
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EXAMPLES – adsorption “Atoms”: A, S“Components”: A, S, ASOne independent reaction; selected: A + S = AS
• second-degree polynomial standard mass-action law
• third-degree polynomial gives following rate equation:
)()()()( ASS12
SA120ASSA2AS002S
2AASA101AS
1SA110 ccKcckccKcckcKccckcKcckJ
JA = – J
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EXAMPLES – adsorption
interpretation of individual terms as reactions
A + AS = 2 A + S
2 AS = A + S + AS
A + 2 S = S + AS
)()()()( ASS12
SA120ASSA2AS002S
2AASA101AS
1SA110 ccKcckccKcckcKccckcKcckJ
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EXAMPLES – dissociation adsorption
for components A2, S, AS, A2S
two independent reactions are possible
selected
A2 + 2 S = 2 AS
A2 + S = A2S
second degree polynomial – two terms
A2 + S = A2S
A2S + S = 2 AS
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EXAMPLES – dissociation adsorption
third degree polynomial – nine terms
• both independent adsorptions included
• desorption by impact: A2 + A2S = 2 A2 + S
• desorption by surface mobility: AS + A2S = A2 + S + AS
• surface rearrangement: S + 2 A2S = 2 AS + A2S
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EXAMPLES – isomerisation
“Atoms”: A, S
“Components”: A, S, AS, RS, R lead to three independent reactions, e.g.:
A + S = AS
AS = RS
RS = R + S
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EXAMPLES – isomerisation
second degree polynomial may contain up to 9 terms, e.g.
A + S = ASA = R
A + AS = A + RSA + R = 2 R
AS + S = RS + SR + S = RS
AS + RS = 2 RSRS + R = AS + R
2 A = 2 R
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EXAMPLES – isomerisation
the term corresponding to AS + S = RS + S reads
)()()( RS1
2AS01100RS1
2ASS01100SRS1
2SAS01100 cKccKccccKcc kkk
and can be interpreted as surface reaction with concentration dependent rate “constant”
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EXAMPLES - CO oxidation
CO + ½ O2 = CO2
Atoms: C, O, S
Components: CO, O2, CO2, S, OS, COS
3 independent reactions are possible, e.g.:
O2 + 2 S = 2 OS
CO + S = COS
OS + COS = 2 S + CO2
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EXAMPLES - CO oxidation
second degree polynomial approximation:
)(
)()(
OSCO1
31
1COSO010001
SCO1
31
2OSCO100010COS1
2SCO100100
22
2
ccKKcc
ccKKcccKcc
k
kkJ
three reactions “appear”
CO + S = COS
CO + OS = CO2 + S
O2 + COS = CO2 + OS
O2 + 2 S = 2 OS
CO + S = COS
OS + COS = 2 S + CO2
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EXAMPLES - CO oxidation
)(
)()(
OSCO1
31
1COSO010001
SCO1
31
2OSCO100010COS1
2SCO100100
22
2
ccKKcc
ccKKcccKcc
k
kkJ
appearing in rate equation
CO + S = COS
CO + OS = CO2 + S
O2 + COS = CO2 + OS
selected
O2 + 2 S = 2 OS
CO + S = COS
OS + COS = 2 S + CO2
reactions “appearing” are combinations of reactions “selected”, but the terms in rate equation could not be combined in this way
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EXAMPLES - CO oxidation
rates of formation:
)(
)()(
OSCO1
31
1COSO010001
SCO1
31
2OSCO100010COS1
2SCO100100
22
2
ccKKcc
ccKKcccKcc
k
kkJ
3CO
1O
2CO 22 JJJJJJ
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EXAMPLES - CO oxidation
dissociative oxygen adsorption requires third degree polynomial:
• resulting rate equations are rather complicated and may contain up to twenty terms,
• many steps describe various displacements by attack of gaseous species onto adsorbed ones or various trimolecular reactions of low probability,
• rate constants of all these steps set to zero:
)()(
)()()(2OS
11
2SO010200
2SCO
13COSOS000011
OSCO1
31
1COSO010001SCO1
31
2OSCO100010COS1
2SCO100100
22
222
cKccccKcc
ccKKccccKKcccKcc
kk
kkkJ
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EXAMPLES - CO oxidation
five reactions can be identified:
CO + S = COS
CO + OS = CO2 + S
O2 + COS = CO2 + OS
OS + COS = 2 S + CO2
O2 + 2 S = 2 OS
)()(
)()()(2OS
11
2SO010200
2SCO
13COSOS000011
OSCO1
31
1COSO010001SCO1
31
2OSCO100010COS1
2SCO100100
22
222
cKccccKcc
ccKKccccKKcccKcc
kk
kkkJ
O2 + 2 S = 2 OS
CO + S = COS
OS + COS = 2 S + CO2
3CO
1O
2CO 22 JJJJJJ
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EXAMPLES - CO oxidation
adding also non-dissociatively adsorbed oxygen (O2S)
to the component list
four independent reactions are possible, e.g.:
O2 + 2 S = 2 OS
CO + S = COS
OS + COS = 2 S + CO2
O2 + S = O2S
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EXAMPLES - CO oxidation
in second degree polynomial approximation following reactions are found:
CO + S = COS
O2 + COS = CO2 + OS
O2 + S = O2S
S + O2S = 2 OS O2 + 2 S = 2 OS
CO + S = COS
OS + COS = 2 S + CO2
O2 + S = O2S
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EXAMPLES - CO oxidation
• For the oxidation itself only the first two steps are necessary.
• The last two can be viewed, in their reversed direction, as liberation of active sites occupied by oxygen
• For oxidation of one CO molecule only “a half” of oxygen molecule is needed.
• In the forward directions, the last two steps block the active sites.
CO + S = COS
O2 + COS = CO2 + OS
O2 + S = O2S
S + O2S = 2 OS
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PRINCIPAL FEATURES
• operates with independent reactions only, but resulting rate equations “contain” also other reactions, relevant for the kinetic description,
• kinetic equilibrium criteria are fulfilled with more general equation than usual Guldberg-Waage with no need for “kinetic” equilibrium constant,
• reaction mechanism for given set of species directly appears,
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PRINCIPAL FEATURES
• effects of other reactions or inert species on the rate of particular reaction are possible and naturally included,
• rates of all dependent reactions can be unambiguously expressed from the rates of selected independent reactions,
• independent reactions with “single simple” intermediate, i.e. intermediate which is sole product in one reaction (step) and sole reactant in another step, are not supported,
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PRINCIPAL FEATURES
• reaction orders are only whole numbers,
• importance of “additional” terms in the rate equation should be well assessed when the equilibrium constants of selected independent reactions are known,
• no need to determine the backward rate constant from kinetic experiments,
• not all rate constants must be positive (second law of thermodynamics).
)( ijkk
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APPLICATION SUGGESTIONS
(…see the following flowchart)
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Detection of “all” components in reacting mixture
atoms, components
number of independent reactions
Proposal of independent reactions stoichiometric matrix— chemical intuition— algebraic method (e.g. Hooyman’s)
Selection of degree of approximating polynomial (usual 2 or 3)+
rational thermodynamics method
rate equations for independent reactions
Rates of components’ reactions
“hidden” mechanism with kinetically significant reactions
Experimental tests and verificationsome
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LIMITATIONS
• function form is valid strictly only for the fluids with linear transport properties,
• polynomial approximation is purely formal, although it can be given (classical) kinetic interpretation,
• more complex rate equations with higher number of constants to be determined than usual,
• “all components” should be known,
• (non-unique rate equation).
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Acknowledgements
Ivan Samohýl(Institute of Chemical Technology, Prague)
Milan Roupec(Brno University of Technology, Brno)