Modeling and Application of Catalytic Ignition in Internal Combustion Engines FINAL REPORT FEBRUARY 2004 Budget Number KLK312 N04-03 Prepared for OFFICE OF UNIVERSITY RESEARCH AND EDUCATION U.S. DEPARTMENT OF TRANSPORTATION Prepared by National Institute for Advanced Transportation Technology University of Idaho Judi Steciak and Steve Beyerlein
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Modeling and Application of Catalytic Ignition in Internal Combustion Engines
FINAL REPORT FEBRUARY 2004
Budget Number KLK312
N04-03
Prepared for
OFFICE OF UNIVERSITY RESEARCH AND EDUCATION U.S. DEPARTMENT OF TRANSPORTATION
Prepared by
National Institute for Advanced Transportation Technology University of Idaho
Judi Steciak and Steve Beyerlein
TABLE OF CONTENTS
TABLE OF FIGURES............................................................................................................. iii
LIST OF TABLES.................................................................................................................... v
LIST OF TABLES.................................................................................................................... v
The results show an increase in average catalyst temperature with the changes in the
power supply. As the heat input to the system increases, the average catalyst temperature
increases. In the laboratory experiments we observed a similar trend. The average
temperature obtained at the power level where surface reactions began using this two-
dimensional analysis is 605 K, 26 percent higher than the experimental average
temperature of 480 K.
Three-Dimensional FEA Model
A three-dimensional FEA model was generated to study the effects of conduction and
convection on the wire temperature. For our input parameters, we considered a platinum
Part II. Modeling Catalytic Ignition Conditions of Propane/Air Mixtures over Platinum Wires 27
catalyst (cylinder) of 508-micron diameter and 0.015. The top surface was kept at room
temperature, 25oC. The temperature profile is symmetrical; the bottom surface of the
FEA model corresponds to the intersection of the catalytic wire and the axial centerline of
the reactor tube. The average temperature obtained at the power level where surface
reactions began using this three-dimensional analysis is 495 K, only three percent higher
than the experimental average temperature of 480 K.
FIGURE 11 A three-dimensional propane air mixture FEA model of platinum temperature distribution.
A three-dimensional model allows specifying the boundary conditions more uniformly
throughout the entire surface area, whereas in a two-dimensional model, we can specify
the boundary conditions on only one of the four surfaces. Hence, a three-dimensional
analysis predicts the catalyst temperature more accurately than a two-dimensional
analysis. Figure 11 shows the temperature distribution along the length of the platinum
catalyst for a three-dimensional FEA model.
Part II. Modeling Catalytic Ignition Conditions of Propane/Air Mixtures over Platinum Wires 28
I.D FINDINGS; CONCLUSIONS; RECOMMENDATIONS Comparisons of Two-Dimensional and Three-Dimensional Results with the Experimental Results
Figure 12 compares the average catalyst wire temperature obtained experimentally with
that calculated by the two-dimensional and three-dimensional FEA models. Differences
between experiment and model may be due to modeling assumptions (the end
temperature of the wire is prescribed and thermal radiation is neglected) and uncertainty
in the convective heat transfer coefficient.
0
100
200
300
400
500
600
700
0.79 0.85 0.93 1.06 1.09 1.16 1.24 1.32
POWER (WATTS)
TEM
PER
ATU
RE
(K)
2-D ALGOR RESULTS
EXPERIMENTAL RESULTS
3-D ALGOR RESULTS
FIGURE 12 Catalyst temperatures versus changes in power supply.
The three-dimensional boundary conditions predict the catalyst temperature more
accurately than the two-dimensional boundary conditions. By conducting the FEA
propane-air mixture analysis, we learned that the axial conduction dominates radial
convection on the platinum catalyst. Because both two-dimensional and three-
dimensional results differ from the experimental results, it indicates that physical
assumptions such as a prescribed top surface temperature and negligible thermal
Part II. Modeling Catalytic Ignition Conditions of Propane/Air Mixtures over Platinum Wires 29
radiation, and uncertainties in the convective heat transfer coefficient are critical for
matching experimental conditions.
Ongoing Research
The next step in the research is to include radiation losses in the three-dimensional model
that we have already generated, perform parametric studies for model sensitivity to a
prescribed end temperature and convective heat transfer coefficient, and compare with
the experimental results. Further efforts will be made to conduct transient heat transfer
analysis for this model using ALGOR. The basic aim will be to find a correlation
between the experimental wire temperatures achieved and FEA wire temperatures
calculated for the same power supply. The FEA propane air mixture analysis will be
helpful to determine the amount of power required to be supplied to the electrical system
in order to achieve a desired temperature. Further, the results of the FEA sensitivity
analysis will provide an insight into accommodating system modifications including
changing catalyst geometry, power supply and wall heating.
A platinum catalyst will be inserted into plug flow region, between 5.625 diameters and
11.625 diameters, identified by hot-wire analysis.
Future work will also include testing with other fuels including aqueous ethanol-air
mixtures. Data will be collected in order to determine the temperature of the platinum
catalyst required for ignition of a particular volumetric content of water in ethanol at a
specified equivalence ratio. Further investigation will be carried out in order to
understand the changes in ignition temperature for different volumetric concentrations of
aqueous ethanol at a constant excess air coefficient. This research aims at determining the
threshold point at which the ignition of aqueous ethanol fuel-air mixtures occur.
Acknowledgments In addition to a University Transportation Center grant from the US Department of
Transportation through NIATT, this research is sponsored by a DOD-EPSCOR grant.
Part II. Modeling Catalytic Ignition Conditions of Propane/Air Mixtures over Platinum Wires 30
PART III. THEORETICAL STUDY OF AQUEOUS ETHANOL-AIR COMBUSTION IN PLUG FLOW
III.A INTRODUCTION
The thermal decomposition and combustion kinetics of gas-phase ethanol oxidation were
modeled with a computer code. The output was compared with flow reactor data available
in the literature. Additional calculations were performed with different percentages of
water added to the fuel. Temperature, the consumption of ethanol, and the mole percent of
the major products carbon dioxide, water and excess oxygen (CO2, H2O and O2) and
intermediate species carbon monoxide, methane, acetylene, ethene, ethane, hydrogen, and
acetaldehyde (CO, CH4, C2H2, C2H4, C2H6, H2 and CH3CHO) were plotted as a function of
time. Reasonable agreement was found between the model and data for 100 percent ethanol
oxidation. Model results showed that combustion temperature dropped as water content
increased. Because dilution masked the impact of water on decomposition and combustion
kinetics, an analysis is underway to “dry” model results. The computer code is being
modified to include the kinetics of catalytic surface reactions.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 31
III.B DESCRIPTION OF PROBLEM
A detailed chemical kinetic mechanism developed for homogeneous ethanol oxidation was
examined using the HCT (Hydrodynamics, Combustion, and Transport) code developed at
Lawrence Livermore National Laboratory. The output was compared with combustion data
from a flow reactor available in the literature. Additional calculations were performed with
different percentages of water added to the fuel. Results show that combustion temperature
dropped as water content increased, with corresponding decreases in the rate of production
of stable intermediary species. The consumption of ethanol and the mole percent of major
products CO2, H2O and O2 and intermediate species CO, CH4, C2H2, C2H4, C2H6, H2 and
CH3CHO are plotted as a function of residence time. These calculations are a first step in
developing an understanding of cold starting and emissions from ethanol-water combustion
in air after catalytic ignition over platinum.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 32
III.C APPROACH AND METHODOLOGY
A catalytic igniter [Cherry, et al., 1990; Cherry, 1992; Cherry, et al., 1992] permits stable
combustion at fuel lean conditions in internal combustion engines [Morton, 2000]. The
igniter also supports combustion of high water content fuel, for example 70 percent
ethanol/30 percent water blends, and permits the combustion of heavy fuels in light
engines.
Water in fuel offers several advantages in lowering harmful combustion emissions. High
water content lowers combustion temperature, thus impeding the formation of thermal NO.
Due to the thermodynamics of CO oxidation, water also encourages the oxidation of CO to
CO2. Soot formation also appears to be inhibited in the presence of water [Hall-Roberts, et
al., 2000]. However, increased acetaldehyde emissions may be a problem during cold
starting since this species is a stable intermediary of the dominant path for gas-phase
ethanol combustion [Marinov, 1998; Egolfopoulos, et al., 1992; Norton and Dryer, 1992].
Our approach to assist in the development of the igniter takes three parallel paths:
a) Understanding the chemistry of catalytic ignition through detailed modeling and
plug-flow reactor studies
b) Working with stand-alone engines to improve igniter durability and
manufacturability, and modeling key characteristics for predicting future designs;
c) Creating demonstration vehicles for over-the-road testing and public outreach.
The work presented here describes our progress in modeling the impact of water on gas-
phase ethanol combustion. These calculations are a first step in developing an
understanding of ethanol water combustion after catalytic ignition over platinum. From
detailed modeling, a simplified model will be derived that improves a catalytic ignition-
timing model being developed to assist igniter designs for new engine applications.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 33
Hydrodynamics, Combustion, and Transport (HCT) Code
Our goal is to model the detailed chemical kinetics of platinum catalyzed ethanol-water
ignition. We are using the Hydrodynamics, Combustion, and Transport (HCT) code
developed at Lawrence Livermore National Laboratory. HCT is a finite-difference code
that calculates one-dimensional time-dependent problems involving gas hydrodynamics,
transport, and detailed chemical kinetics. It can calculate ignition occurrence, laminar
flame propagation, and species mole fractions. The code solves the coupled equations for
conservation of mass, momentum, energy, and conservation of each chemical species. The
inherently stiff set of equations is solved implicitly using the numerical method, LU
decomposition.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 34
FIGURE 13 Logic flow and file interaction for the MKCDAT, HCT, and HCTPLT programs
The HCT codes include MKCDAT, HCT and HCTPLT. Figure 13 shows the HCT
flowchart and the changes we made for plotting. HCT contains the main calculation
program. The input file, HCT.INP describes the combustion model, including reactions and
the species involved, initial conditions and boundary conditions, the model execution
method, and output files includes hsp0, defile0, and plot.xls. Among these output files,
hsp0 is an ASCII file that contains the simulation process, species mole fraction changes
and other information; dfile0 is a binary file for plotting with the HCTPLT program.
The MKCDAT code produces binary and ASCII chemistry data files, reads in.cdat and a
possible changes file (e.g. changes.195) and writes cdat (binary file required by the HCT
code) and out.cdat, which we rename in.cdat (for changes.195) for use in the next version.
The HCTPLT code is a post-processor plotter and requires NCAR and GPS graphics
library with input command file INPUT. Types of plots made include spatial and time.
Variables plotted are mole fractions, temperature, zone width, velocity, and flame position
and speed.
To satisfy more flexible and powerful plotting requirements, we made some changes in
HCT. When running HCT, the file plot.xls is produced so that with MS Excel or other data
analysis and graphics tools, we can plot powerfully and easily.
Theoretical Impact of Water on Gas-Phase Ethanol Combustion
For the flow reactor combustion of ethanol at atmospheric pressure, initial temperatures
near 1100 K and equivalence ratio φ = 0.61, 0.81 and 1.24, experimental profiles of stable
species mole fractions and temperature are reported by Norton and Dryer [1991].
The stable species CO2, O2, CO, C2H6, CH4, H2O, C2H5OH, H2, CH3CHO, C2H4, C2H2, and
temperature are plotted.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 35
CH3CH2OCH2CH2OH CH3CHOH
C2H5OH
CH2OC2H4 CH3CHO
HO2
C2H3
CH3COHCO
CH3
CH2O
C2H6 CH2O CH3OCH4 CH3OH
FIGURE 14 Species consumption path analysis for ethanol oxidation [Egolfopoulos, 1992; Norton and Dryer, 1991].
The species decomposition paths for ethanol/air oxidation are shown in Fig. 14. We
developed these paths by integrating all reactions in the oxidation process and determining
the fraction of each species consumed by a particular reaction. C2H5OH is mainly attacked
by H, OH, O, CH3, C2H5 and HO2, which abstract H atom and produce three C2H5O
isomers CH3CHOH, CH2CH2OH and CH3CH2O:
C2H5OH + X -> {CH2CH2OH, CH3CHOH, CH3CH2O} +
XH {X = OH, H, CH3, HO2, C2H5} R1
The ethanol mechanism calculates the three distinct sites of hydrogen abstraction from the
ethanol molecule; subsequently the mechanism considers the reactions involving these
three isomers. CH3CHOH reacts with O, O2 and OH to produce acetaldehyde (CH3CHO).
CH2CH2OH decomposes to C2H4, which is the main step to produce ethane. CH3CH2O
thermally decomposes to CH3 with simultaneous product CH2O. The major products of
these three isomers reaction series and their subsequent reactions are expected to be
important in the mechanism.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 36
Detailed chemical kinetics model developed since 1990 have greatly improved the degree
of understanding of ethanol oxidation. The modeling studies of Borisov, et al. [1992] and
Norton and Dryer [1991] addressed the issue of three distinct H-atom abstraction sites in
ethanol as described above, and the resulting temperature dependent product distribution in
combustion. Egolfopoulos, et al. [1992] published the detailed kinetic scheme of the study
of ethanol in laminar-premixed flames, flow reactors, and shock tubes, and developed an
ethanol oxidation mechanism based on his methanol kinetics model. These models had
reasonable agreement with experimental data (Fig. 15).
FIGURE 15 Comparison between numerical calculations and experimental data for flow reactor studies of ethanol oxidation at φ = 0.81 [Egolfopoulos, 1992; Norton and Dryer, 1991].
More recently, Marinov [1998] studied ethanol oxidation at high temperature and
developed a detailed and improved model. The ethanol combustion mechanism reported by
Marinov [1998] was in particular agreement with experiment data in laminar flames, shock
tubes and jet-stirred reactors. Unfortunately his model was unable to reproduce the ethanol
consumption profile for φ = 0.61 in the flow reactor even considering the uncertainty in the
experimental induction time. Certainly for equivalence ratio φ = 0.81 and 1.24, numerical
results were time-shifted to match the experimental data from Norton and Dryer [1991]
correctly.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 37
Curran and Pitz [1997] modeled dimethyl ether CH3OCH3 (DME) combustion. This DME
kinetics model was rigorously tested through comparisons with experimental data. At high
temperature, the fuel consumption pathway for DME is similar to some degree to ethanol in
this model, since some dimethyl ether changes to ethanol at first, then ethanol reacts along
the reaction channels described by Norton and Dryer [1991], Egolfopoulos [1992],
Brorisov [1992], and Marinov [1998] (Fig. 13), while remaining DME reacts along its
decomposition channels. Hence, to some extent, this DME model can simulate ethanol
oxidation mechanism. However, the DME model is particularly developed for DME; using
it to predict ethanol oxidation requires additional effort. We modified the DME model with
more detailed ethanol decomposition reactions developed by Marinov [1998] and formed a
modified DME model. This model was used to simulate ethanol-water oxidation. The
results presented here show reasonably good agreement in comparison with plug-flow data
reported by Norton and Dryer [1991].
In our research about catalytic ethanol-water air oxidation, we first consider homogenous
oxidation at atmospheric pressure. The initial reactant mixture includes ethanol and air. We
examine the effect of increasing fuel-water content by varying the initial fuel from 100
percent ethanol and 0 percent water to 70 percent ethanol and 30 percent water in a plug
flow reactor. The numerical results for equivalence ratio φ = 0.81 were time-shifted by 15
msec.
0 20 40 60 80 1000.0
0.1
0.2
0.3
0.4
0.5
0.6
30% h2o
20% h2o
10% h2o
0% h2o
C2H5OH @T=1090, φ=0.81
Mol
e P
erce
nt
Time (msec)
FIGURE 16 C2H5OH vs. residence time at φ = 0.81.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 38
Although both the HCT simulation and the experimental data show steady consumption of
ethanol (Fig. 16), the data indicate a faster combustion rate than calculated by the
simulation. As water content increases, the rate of ethanol consumption decreases because
of lowered combustion temperature, as shown in Fig. 17.
0 10 20 30 40 50 60 70 80 90 100
1100
1125
1150
1175
1200
1225
1250
1275
1300
1325
30% h2o
20% h2o
10% h2o0% h2o
Temperature @T=1090, φ=0.81
Tem
pera
ture
(K)
Time (msec)
FIGURE 17 Temperature vs. residence time at φ = 0.81.
0 20 40 60 80 1000.2
0.4
0.6
0.8
1.0
1.2
1.4
1.6
1.8
2.0
2.2
2.4
30% h2o
20% h2o
10% h2o
0% h2o
O2 @T=1090, φ=0.81
Mol
e P
erce
nt
Time (msec)
FIGURE 18 O2 vs. residence time at φ = 0.81.
Figure 18 shows that the HCT prediction is in reasonable agreement with experimental
data. As the amount of water increases in the fuel, the consumption rate of O2 becomes
lower in concert with corresponding decreases in the rate of ethanol decomposition and
temperature. Closer comparison between Fig. 17 and 18 shows that once the temperature
starts to increase abruptly, the consumption of O2 increases quickly.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 39
0 20 40 60 80 1000.0
0.1
0.2
0.3
0.4
0.5
0.6
0.7
0.8
0.9
30% h2o
20% h2o
10% h2o
0% h2o
CO @T=1090, φ=0.81
Mol
e P
erce
nt
Time (msec)
FIGURE 19 CO vs. residence time at φ=0.81.
CO mole percent is plotted as a function of residence time in Fig. 19. With 10 percent and
more water, the rate of CO formation slows in comparison with the 0 percent water
condition and the CO peaks are not so abrupt as in 0 percent water. The peak production of
CO is coincident with the rapid temperature increase.
The CO oxidation reactions include the following:
2 2CO +O CO + O R2→
2
2
O + H2O OH + OH R3CO + OH CO + H R4H + O OH + O R5
→→
→
Glassman [1987] indicated that with the peroxy radical HO2 present, another route for CO
oxidation is possible:
2 2CO + HO CO + HO R6→
In Fig. 19, HCT shows that CO2 mole faction with 0 percent water in initial condition is in
reasonable agreement with the experimental data. The abrupt increase of production of CO2
is in good conformity to the temperature curve in Fig. 16, for 0 percent water, 10 percent
water, 20 percent water and 30 percent water. The CO2 formation rate increases abruptly in
concert with the abrupt temperature change. And with the increase of water, the final CO2
fraction decreases because of dilution due to the large amount of water present.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 40
0 20 40 60 80 1000.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
30% h2o
20% h2o10% h2o
0% h2o
CO2 @T=1090, φ=0.81
Mol
e P
erce
nt
Time (msec)
FIGURE 20 CO2 vs. residence time at φ = 0.81.
Reactions R2-R6 shows the mechanism between CO and CO2. Reaction 2 is the initiator of
the chain sequence; the fastest and the dominant CO oxidation mechanism is R4 [Turns,
1996]. As water content increases, thermodynamic equilibrium considerations argue that
the reaction R4 is pushed further towards reactants. However, chemical kinetics
calculations show that with increase in water, the reaction temperature decreases
considerable in Fig. 20, which causes the severe decrease in the CO2 production rate.
In Fig. 21, the formation reaction R7 of C2H6, methyl radical recombination
3 3 2 6CH + CH C H R7→
is the major contributor to C2H6 [Egolfopoulos, 1992], following the ethanol decomposition
path in Fig. 13. The key reactions involving C2H6 include
2 6 2 5 2
2 6 2 5
2 6 2 5 2
C H + H C H + H R8C H + O C H + OH R9C H + OH C H +H O R10
→→→
Figure 20 shows the general tendency for the addition of H2O to lower the reaction speed.
HCT simulation also correctly describes the fast decrease of C2H6 after the mole fraction
apex, but significantly underestimates the amount of ethane produced.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 41
0 20 40 60 80 1000
20
40
60
80
100
120
140
160
180
200
220
240
30% h2o20% h2o
10% h2o
0% h2o
C2H6 @T=1090, φ=0.81
Mol
e P
PM
Time (msec)
FIGURE 21 C2H6 vs. residence time at φ = 0.81.
0 20 40 60 80 1000
200
400
600
800
1000
1200
1400
30% h2o20% h2o
10% h2o
0% h2o
C2H4 @T=1090, φ=0.81
Mol
e P
PM
Time (msec)
FIGURE 22 C2H4 vs. residence time at φ = 0.81.
The main reactions involved in C2H4 and C2H2 include
2 4 2 2 2
2 4 2 3
2 4 2 4 2 3 2 5
C H + M C H + H + M R11C H + M C H + H + M R12
C H + C H C H +C H R13
→→
→
and
2 3 2 2 2
2 3 2
2 3 2 2 2 2
2 3 2
C H + H C H + H R14 C H + O H CO + H R15C H + O C H + HO R16C H + M C H
C→→→→ 2 + H + M R17
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 42
In Fig. 22, the HCT simulation shows that C2H4 production mainly follows the
decomposition of CH2CH2OH in Fig. 13. Ethene’s consumption follows R11-R17 and the
path about C2H4 in Fig. 13, and quickly disappears with the abrupt increase of temperature.
Figure 23 shows significant difference between the simulated C2H2 mole fraction and the
experimental data for the case with pure ethanol (0 percent water). One reason for the
difference is the difficulty reading the exact experimental data from Norton and Dryer
[1992] due to the graphics scale. As the temperature decreases with increasing water
content, the production rate of acetylene slows. At a fixed temperature, the rate of C2H2
production decreases abruptly. The dominant reactions here are
2 2 2
2 2 2
2 2 2
C H + M C H + H + M R18C H + O HCCO + OH R19C H + O HCO + HCO R20
→→→
It is clear that C2H2 production is closely connected with C2H4 directly in R11through R17
and through the intermediary C2H3.
0 20 40 60 80 1000
10
20
30
40
30% h2o
20% h2o
10% h2o
0% h2o
C2H2 @T=1090, φ=0.81
Mol
e P
PM
Time (msec)
FIGURE 23 C2H2 vs. residence time at φ = 0.81.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 43
0 20 40 60 80 1000
200
400
600
800
1000
1200
30% h2o
20% h2o
10% h2o0% h2o
CH3CHO @T=1090, φ=0.81
Mol
e P
PM
Time (msec)
FIGURE 24 CH3CHO vs. residence time at φ = 0.81.
The reactions that directly affect the production and consumption of CH3CHO are
3 3
2 2
3 3
CH CHOH + X -> CH CHO + XH R21 {X=O , O, H, OH and HO }CH CHOH + M -> CH CHO + H + M R22
and
3 3
2 2
3 2
CH CHO + X -> CH CO + XH R23 {X=O , O, H, OH and HO }CH CHO + X -> CH CHO + XH R24
3 2
{X=CH , O, H, OH and HO }
Egolfopoulos, et al. [1992] developed a CH3CHO reaction channel and Marinov [1998]
further refined this channel. The production reactions R21 and R22 of CH3CHO, following
the production of CH3CHOH, directly result from the ethanol decomposition in Fig. 16.
The CH3CHO consumption reactions R23 and R24 are sensitive to temperature. Hence
with 10 percent, 20 percent, and 30 percent H2O, the rate of decrease of acetaldehyde
production is steep. In Fig. 24, HCT shows that the modified ethanol mechanism is in
reasonable agreement with the experimental data for CH3CHO.
The intermediate H2 reaction mechanism connects with many reactions and intermediate
and stable species in the modified DME mechanism because of the importance of H, O and
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 44
OH chemistry. The rate of H2 formation increases steadily before the temperature reaches
its sharp increase (Fig. 25). Higher H2O content slows the rate of H2 formation. The
experiment data and HCT simulation are in reasonable agreement at the 0 percent fuel
water case.
0 20 40 60 80 1000.00
0.05
0.10
0.15
0.20
0.25
0.30
30% h2o
20% h2o
10% h2o0% h2o
H2 @T=1090, φ=0.81
Mol
e P
erce
nt
Time (msec)
FIGURE 25 Water vs. residence time at φ = 0.81.
0 20 40 60 80 1000.0
0.2
0.4
0.6
0.8
1.0
1.2
1.4
1.6
1.8
2.0
0% h2o
H2O @T=1090, φ=0.81
Mol
e P
erce
nt
Time (msec)
FIGURE 26 Water vs. residence time at φ = 0.81.
The water routes in the oxidation mechanism are connected to many other reactions and are
not included here. The experiment data and HCT simulation are in reasonable agreement at
the 0 percent fuel water case for the production of water in combustion (Fig. 26). The plot
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 45
does not include simulation with increased water in the fuel because the fuel-water
overwhelms the plot and obscures slight changes in mole percent with time.
As shown in Fig. 27 for CH4, its production mainly follows the reaction R25:
3 4CH + H + M -> CH + M R25
Methane consumption mainly reverses to the production of CH3 again. Once the abrupt
temperature increase starts, most of CH3 is consumed, which leads to an abrupt drop in CH4
production.
0 20 40 60 80 1000
200
400
600
800
1000
1200
1400
30% h2o
20% h2o
10% h2o
0% h2o
CH4 @T=1090, φ=0.81
Mol
e P
PM
Time (msec)
FIGURE 27 CH4 vs. residence time at φ =0.81.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 46
III.D FINDINGS; CONCLUSIONS; RECOMMENDATIONS
The development of a catalytic igniter that permits stable combustion of high water-
content ethanol in internal combustion engines has promoted a need for fundamental
understanding of Pt-catalytic ethanol water ignition chemistry. As a first step in
developing a heterogeneous model, the HCT code was used with an ethanol oxidation
mechanism to model gas-phase ethanol-water-air combustion.
A modified ethanol mechanism was based on an existing dimethyl ether mechanism,
and included the species consumption path analysis for ethanol oxidation.To gain
confidence in the ethanol oxidation mechanism, simulated gas-phase ethanol-air
combustion was compared with experimental data from a plug flow reactor.
Due to the uncertainty in experimental induction time, the simulation results were
“time-shifted.” The calculations are in reasonable agreement with experimental data
obtained with 100 percent ethanol, with the exception of intermediate species C2H6,
(overperdicted) and C2H2 (underpredicted), and slower C2H5OH decomposition. The
simulation shows that as more water is added to ethanol, the reaction temperature
decreases and the rate of the oxidation process decreases. The addition of water results
in lower peak valued of intermediate species because of dilution.
Future Plans
1. Refine the ethanol-air combustion mechanism as new information and insights
become available to improve agreement with data at φ=0.81. Compare an improved
model with data available at φ=0.61 and 1.24.
2. Search for and evaluate hydrocarbon-Pt surface reaction data, especially that for
initial ethanol-Pt decomposition reactions. Find characteristics of Pt-hydrocarbon
oxidation that will be useful in developing a Pt-ethanol-water oxidation mechanism.
3. Develop a 1-D model for catalyst surface reactions through a literature search and
theoretical analysis of surface chemistry.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 47
4. Modify the HCT code to model the coupled homogeneous-heterogeneous
catalytically assisted ignition of ethanol-water fuel.
5. Compare the result with ethanol-water-air plug flow experiments in a reactor that is
being developed.
6. Derive simplifications that can be used to improve a catalytic ignition timing model
being developed to assist igniter designs for new engine applications
Acknowledgements
Drs. C. Westbrook, W. Pitz and L. Chase of Lawrence Livermore National Laboratory
provided valuable assistance understanding the operation of HCT and its application.
Part III: Theoretical Study of Aqueous Ethanol-Air Combustion in Plug Flow 48
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