development of reliable, simple rate expressions from a microkinetic model of fts on cobalt calvin...
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![Page 1: Development of Reliable, Simple Rate Expressions from a Microkinetic Model of FTS on Cobalt Calvin H. Bartholomew, George Huber, and Hu Zou Brigham Young](https://reader036.vdocuments.site/reader036/viewer/2022062714/56649d455503460f94a21d1a/html5/thumbnails/1.jpg)
Development of Reliable, Simple Rate Expressions from a Microkinetic Model
of FTS on CobaltCalvin H. Bartholomew, George Huber, and Hu Zou
Brigham Young UniversityAnd
George Huber, Rahul Nabar, Peter Ferrin, Manos Mavrikakis, and James Dumesic
University of Wisconsin, Madison
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Background
Fischer-Tropsch Synthesis (FTS), is a key step in processes being developed and commercialized in the new GTL industry.
Improvements to GTL and FTS processes are facilitated by development of accurate, comprehensive reactor and kinetic models.
Rates and reactant/product compositions in a commercial FTS SBCR cover wide ranges; rates may vary 10-20 fold, H2/CO ratios 2 to 100.
Microkinetic models (MKMs) and/or Langmuir-Hinshelwood models (LHMs) are needed for reliable prediction of rates over the full range of conditions.
While MKMs are the most powerful predictors, given large computational requirements of a comprehensive FTS reactor model, a reliable LHM may be the best compromise.
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Kinetic Models for FTS on Cobalt
A dozen previous macrokinetic studies; each covers a narrow range of conditions.
Power law (PL) and LH rate expressions reported in previous studies may not be statistically valid since too many parameters were fitted to too few data.
Two microkinetic models for FTS on cobalt have been previously published. They have limited utility and have not been validated with a representative set of data.
Use of kinetic/thermo parameters from MCMs in building rate laws has been limited—hasn’t been done with Co FTS.
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Issues Addressed in This Talk
What is a viable approach to microkinetic model and rate-law development?
How can we use microkinetic models to develop better rate laws?
What factors limit the validity of previously reported rate laws and how might they be overcome?
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Surface ReactionSchemes and Kinetic
Models
Adsorption And Microcalorimetry
Heats, Coverages
Isotopic StudiesSSITKA and kinetics of
elementary steps
Detailed KineticsActivity, Selectivity,
Stability
XPS, XRD, MössbauerAlloy formation, oxidation
states, surface composition
IRSurface species
MicroscopySurface morphologyand composition
DFTElectronic structure of stable species, intermediates andtransition states
Microkinetic Model Development
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Information from MKM
Kinetic parameters for each elementary step
Site requirements
Predictions of rate over a wide range of conditions from solution of the differential equations
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Microkinetic Model for Fischer Tropsch Synthesis on Co(0001)
Rctn No. Reaction H eqK fA fE revA revE
1 H2+2*-->2H* -95.73 4.70E+02 1.0E+07 0.00
2 CO+*-->CO* -106.12 1.28E+01 1.0E+07 0.00
3 (rds) CO*+*-->C*+O* 36.47 9.24E-05 1.0E+13 90.52
4 C*+H*-->CH* + * -38.42 2.34E+04 1.0E+13 66.56
5 H* + O* --> OH* + * 43.82 1.30E-04 1.0E+13 106.12
6 OH* + H* --> H2O+ 2* 73.35 7.91E+01 1.0E+07 87.02
7 CH* + H* --> CH2* + * 13.21 8.29E-02 1.0E+13 42.45
8 CH2* + H* --> CH3* + * 44.56 3.73E-05 1.0E+13 53.06
9 CH3* + H* --> CH4 + 2* 3.78 3.85E+08 1.0E+07 123.34
10 CH2* + CH2* --> C2H4* + * 28.14 4.06E-04 1.0E+13 53.06
11 C2H4* + H* --> C2H5* + * 40.46 3.76E-04 1.0E+13 53.06
12 C2H5* + H* --> C2H6 + 2* 0.54 1.19E+10 1.0E+07 48.24
13 C2H4* + CH2* --> C3H6* + * -30.22 9.28E+02 1.0E+13 53.06
14 C3H6* + H* --> C3H7* + * 54.29 1.17E-05 1.0E+13 53.06
15 C3H7* + H* --> C3H8 + 2* 27.57 5.82E+08 1.0E+07 48.24
16 C2H4* --> C2H4+* 85.86 3.93E+01
17 C3H6* --> C3H6+* 114.80 1.95E+00 On Wisconsin
UWM
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Preferred Adsorption Sites and Binding Energies for Intermediates in CH4 Formation on Fe(110) and Co(0001) (Gokhale
and Mavrikakis, 2005; courtesy of the American Chemical Society)
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Kinetic Study: Statistical Design(H&B, BYU; Temperature 200C, Pressure Total = 20 atm.)
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250.025.0
50.075.0
)1(2
2
COH
COH
PPb
PPar
Rate Expression Derived from Original Carbide Mechanism
(Huber, 2000)
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0
10
20
30
40
50
60
70
80
0 10 20 30 40 50 60 70 80
Rate Measured (mole CO/h kg Co)
Ra
te C
alc
ula
ted
(m
ole
CO
/h k
g C
o) Model 1 Carbide
Model 2 Carbide
Power Law
Model Yates
Rate calculated vs. rate measured in this study for rate expressions derived from Carbide Theory, Power Law and rate expressions proposed by Yates and Satterfield.
Calculated and measured values are in reasonable agreement.
NSSE = 4-8 x 10-5 for several sets of data.
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-20
-15
-10
-5
0
5
10
15
20
0 5 10 15 20 25
Run #Normalized deviation from average value (%) versus run number. (Normalized deviation from average value = (value – average value) /average value x 100) [Huber and Bartholomew, 2005].
Deviations are within + or – 5%.
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Correlation between A and B for Model 1 derived from Carbide Theory. Ellipse indicates 95 % confidence limit for each constant.
Results of Nonlinear Regression
Conclusion: A and B (a and b) in rate equation cannot be specified!
a = 81.1 ± 43 b = 1.0 ± 0.4
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This is a Can of Worms!
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Solution to Dilemma?
Use MKM to specify all variables except one
Use nonlinear regression to determine the unspecified parameter
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Microkinetic Model for Fischer Tropsch Synthesis on Co(0001)
Rctn No. Reaction H eqK fA fE revA revE
1 H2+2*-->2H* -95.73 4.70E+02 1.0E+07 0.00
2 CO+*-->CO* -106.12 1.28E+01 1.0E+07 0.00
3 (rds) CO*+*-->C*+O* 36.47 9.24E-05 1.0E+13 90.52
4 C*+H*-->CH* + * -38.42 2.34E+04 1.0E+13 66.56
5 H* + O* --> OH* + * 43.82 1.30E-04 1.0E+13 106.12
6 OH* + H* --> H2O+ 2* 73.35 7.91E+01 1.0E+07 87.02
7 CH* + H* --> CH2* + * 13.21 8.29E-02 1.0E+13 42.45
8 CH2* + H* --> CH3* + * 44.56 3.73E-05 1.0E+13 53.06
9 CH3* + H* --> CH4 + 2* 3.78 3.85E+08 1.0E+07 123.34
10 CH2* + CH2* --> C2H4* + * 28.14 4.06E-04 1.0E+13 53.06
11 C2H4* + H* --> C2H5* + * 40.46 3.76E-04 1.0E+13 53.06
12 C2H5* + H* --> C2H6 + 2* 0.54 1.19E+10 1.0E+07 48.24
13 C2H4* + CH2* --> C3H6* + * -30.22 9.28E+02 1.0E+13 53.06
14 C3H6* + H* --> C3H7* + * 54.29 1.17E-05 1.0E+13 53.06
15 C3H7* + H* --> C3H8 + 2* 27.57 5.82E+08 1.0E+07 48.24
16 C2H4* --> C2H4+* 85.86 3.93E+01
17 C3H6* --> C3H6+* 114.80 1.95E+00 On Wisconsin
UWM
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2
50.075.0
)1(2
CO
COH
Pb
PPar
Approach
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0.0
10.0
20.0
30.0
40.0
50.0
0.00 10.00 20.00 30.00 40.00 50.00
Measured Rate
Fit
Dat
a
Data points: 11Chi-squared: 0.20Chi-distr.prob. = 1.00
Huber and Bartholomew
r = a PH2^0.75 PCO^0.5 / (1 + b PCO)^2
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0.0
5.0
10.0
15.0
20.0
25.0
30.0
0.0 5.0 10.0 15.0 20.0 25.0 30.0
Experimental TOF
Cal
cula
ted
TO
F
Zennaro et al.
Data points: 9Chi-squared: 0.15Chi-distr.prob. = 1.00
r = a PH2 0̂.75 PCO 0̂.5 / (1 + b PCO) 2̂
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Conclusions Dilemma: Typical approach to fitting kinetic
data to LHE may lead to highly correlated constants; standard errors are large and constants are unspecified.
Solution: use constants from theory or MKM to specify all but one constant, which can be fitted by nonlinear regression.
For Co(0001) CO dissociation is rds and CO is masi. On stepped sites C + H could be rds.
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BYU Catalysis Group Spring 2005
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Thanks for listening.
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Kinetic expression Mechanistic Implications References
Cobalt Catalysts
C1 2
-0.2 0.7CO CO Hr a P P
CO inhibits reaction; CO strongly adsorbed; high CO
Ribiero et al., 1997; Zennaro et al., 2000
C2 2CO H
COCO
21
a P Pr
bP
high CO; enolic mechanism;
hydrogenation of HCOH (rds) Yates and Satterfield, 1991; Zennaro et al., 2000
C3 CO H2
COCO1
m na P Pr
bP
,
m = 0.5 – 0.6, n = 0.6 – 0.9
moderate CO; Eley-Rideal; stepwise hydrogenation of Cs
Iglesia et al., 1993b.; Peluso et al., 2001
C4 2
0.5 0.5CO H
CO0.5
CO
21
a P Pr
b P
high CO; Cs + Hs and
Os + Hs are rds’s
Sarup, 1989; Keyser et al., 2000; Huber, 2000; Huber and Bartholomew 2005
Representative Simple Reaction Rate Equations for CO Consumption in FTS on Co Catalysts