thermal degradation of polyethylene modeled on tetracontane
TRANSCRIPT
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www.elsevier.com/locate/jaap
Available online at www.sciencedirect.com
J. Anal. Appl. Pyrolysis 81 (2008) 237–242
Thermal degradation of polyethylene modeled on tetracontane
Andras Nemeth *, Marianne Blazso, Peter Baranyai, Tamas Vidoczy
Chemical Research Center, Hungarian Academy of Sciences, Pusztaszeri ut 59-67, H-1025 Budapest, Hungary
Received 4 May 2007; accepted 30 November 2007
Available online 17 December 2007
Abstract
The thermal degradation of tetracontane as an idealized monodisperse ‘‘polymer’’ of 40 carbon atoms was modeled based on a detailed reaction
mechanism consisting of simultaneous or subsequent H-abstraction, b-scission and backbiting reactions (intramolecular H-shifts). A stiff
differential equation solver with a postprocessor program to compute the concentrations of each species and the contribution of each reaction to
their production was used. The model correctly predicts degradation at low conversion and indicates objectives for further research to improve
accuracy at higher conversions. Rate of production analysis quantifies reaction pathways contributing to the formation and consumption of species
and reveals specific H-abstraction and b-scission reactions, the complex impact of backbiting reactions, interdependence between production rates
of alkyl and alkenyl radicals, dominant role of small alkyl radicals. The data obtained by the model are compared to the experimental product
distribution of the degradation of high density polyethylene measured at 500 8C and 20 s reaction time in a micropyrolizer reactor.
# 2008 Elsevier B.V. All rights reserved.
Keywords: HDPE; Polyethylene; Pyrolysis; Thermal decomposition model; Low conversion
1. Introduction
Several methods to dispose plastic waste are extensively
studied nowadays, amidst them the thermal decomposition is a
favored alternative because of its versatility to recover
monomers, other valuable chemicals, fuel and energy as well
[1–3]. The kinetics of the process has been also intensively
studied and it is now accepted that in the case of hydrocarbon
polymers the decomposition proceeds by free radical mechan-
ism involving multistep chain reactions. The description of
elaborated reaction mechanism has been published decades ago
[4,5]. It consists of consecutive H-abstraction and b-scission
reactions producing alkanes, alkenes and dienes. The first
model taking into consideration the detailed reaction mechan-
ism for the thermal degradation of high density polyethylene
(HDPE) was published by Ranzi et al. [6]. In modeling, key
simplification was that the same rate constant was assigned to
all propagation reactions, and steady state radical concentration
was assumed to obtain the solution of the differential equation
system in closed form. For better fit to measured gas product
distribution intramolecular hydrogen shift, called backbiting –
* Corresponding author. Tel.: +36 1 4381100x116; fax: +36 1 4381145.
E-mail address: [email protected] (A. Nemeth).
0165-2370/$ – see front matter # 2008 Elsevier B.V. All rights reserved.
doi:10.1016/j.jaap.2007.11.012
missing from the earlier model – was added to the scheme by
Faravelli et al. [7]. Poutsma compiled a more elaborate set of
elementary reactions including b-scission of primary radicals,
rate constants based on critical review of experimental data and
theoretical considerations, simulated the thermal degradation
of a monodisperse model polymer of 19 degree of polymeriza-
tion to investigate the initial product distribution and the
functionality of the reaction mechanism [8]. For numerical
integration Monte Carlo method was used.
The present research was aimed to explore in what extent
modeled product distribution of thermal degradation of a
polymer of 40 carbon atoms (tetracontane) based on a detailed
reaction mechanism consisting of elementary reactions produ-
cing alkanes, alkenes, dienes complies with measured HDPE
degradation using a stiff differential equation solver for the
numerical integration. Further object was to reveal the impact
of b-scission, H-abstraction and isomerization reactions on
product distribution and the role of radicals by contribution
analysis.
2. Modeling
Initiation occurs by C–C homolysis in the tetracontane
polymer (P) backbone to form primary alkyl radicals (Rp�) at
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Table 1
Kinetic parameters used for modeling product distribution
Process A E k773
(i) 7.94 � 1014 77,000 1.86 � 10�7 s�1
(i)a 3.16 � 1013 67,000 4.77 � 10�6 s�1
A. Nemeth et al. / J. Anal. Appl. Pyrolysis 81 (2008) 237–242238
random position
P ! Rp� þ Rp
� (i)
In the propagation steps primary alkyl radicals have three
competitive fates:
(ii) 1.90 � 108 12,800 4.83 � 104 M�1 s�1(iii) 1.99 � 1013 27,800 1.66 � 105 s�1
(iii) 5.75 � 1012 30,100 2.01 � 104 s�1
(1) H Me(iv)14 1.58 � 1011 20,800 2.27 � 105 s�1
(iv)15 1.81 � 1010 13,700 2.57 � 106 s�1
(iv) 1.04 � 1010 14,300 1.00 � 106 s�1
-abstraction from the polymer forms n-alkanes (ANE) and
secondary alkyl radicals (Rs�)
Rp� þ P ! ANE þ Rs
� (ii)
16(v) 3.01 � 1014 31,700 3.76 � 105 s�1
(2) b (v)Me 1.10 � 1014 32,800 6.70 � 104 s�1(vi) 1.28 � 108 14,200 1.32 � 104 M�1 s�1
(vii) 1.90 � 108 12,800 4.83 � 104 M�1 s�1
-Scission produces ethene and smaller primary alkyl
radicals
Rp� ! C2H4þRp
� (iii)
(viii) 3.01 � 1014 31,700 3.76 � 105 s�1(viii) 1.10 � 1014 32,800 6.70 � 104 s�1
(3) a Me(ix) 3.01 � 1014 31,700 3.76 � 105 s�1
(x) 1.99 � 1013 27,800 1.66 � 105 s�1
(xi) 1.90 � 108 12,800 4.83 � 104 M�1 s�1
(xii) 4.18 � 1010 6,000 8.41 � 108 M�1 s�1
A units are M, s, and E units cal mol�1 as appropriate, index a denotes formation
nd rearrangement to create 5-, 6- and 7-membered rings
producing secondary alkyl radicals by 1-4, 1-5 and 1-6 H-
shifts called backbiting
Rp� ! Rs
� (iv)
b-scission of secondary alkyl radicals produces 1-alkenes
of an allyl type radical in initiation, Me methyl radical expelled in b-scissionand 14, 15, 16 denote 1,4-; 1,5-; 1,6-hydrogen shifts. Rate constants of initiation
and termination are from Ref. [4], of propagation from Ref. [6].
The
(ENE) and chain propagating primary alkyl radicals
Rs� ! ENE þ Rp
� (v)
Secondary alkyl radicals formed in backbiting reactions can
abstract hydrogen from the polymer
Rs� þ P ! ANE þ Rs
� (vi)
Diene (DIENE) formation is assumed to proceed according to a
similar scheme where primary alkyl radicals formed in the
previous propagation steps are converted by H-abstraction from
1-alkenes into secondary 1-alkenyl radicals (0Rs�)
Rp� þ ENE ! ANE þ 0Rs
� (vii)
Subsequent b-scission of the secondary 1-alkenyl radicals
forms either a, v-dienes and primary alkyl radicals in b-
scission away from the existing double bond,
0Rs� ! DIENE þ Rp
� (viii)
or 1-alkenes and primary v-alkenyl radicals (0Rp�) in b-scission
in the other direction
0Rs� ! ENE þ 0Rp
� (ix)
b-scission of the primary v-alkenyl radicals produces ethene
and smaller primary v-alkenyl radicals
0Rp� ! C2H4þ 0Rp
� (x)
H-abstraction from 1-alkenes by primary v-alkenyl radicals
(0Rp�) produces 1-alkenes and secondary 1-alkenyl radicals
0Rp� þ ENE ! 0Rs
� þ ENE (xi)
Termination, step (xii) is represented by recombination of all
radicals participating in the process.
This scheme has been applied to construct elementary
reactions in a systematic way including all possible radical
centers along the chain. At present, due to computational
constraints, decomposition of alkanes was not taken into
account, i.e. modeling was limited to low polymer conversion
and H-abstraction from the polymer by primary alkenyl radicals
and H-shifts toward an inner position though possible, albeit
with a lower probability, were also neglected. According to
these restrictions the reaction mechanism comprises of about
1000 species and 7500 elementary reactions.
Modeling degradation of tetracontane was performed with
kinetic parameters summarized in Table 1.
Initiation kinetic parameters were corrected to the number of
carbon atoms in tetracontane as detailed in [6], those for H-
abstraction multiplied with the factor of reaction path
degeneracy gH = 4 [8]. Kinetic parameters of diene formation
are assumed to be the same as assigned to the formation of
alkenes, derived for alkanes and alkenes of low carbon numbers
[9–13].
For computation the DASAC program package [14] was
used modeling tube reactor operating at constant pressure, the
dimensions of corresponding arrays extended to numbers of
species and reactions as required. Kinetic analysis of the
simulated data was assisted by a postprocessor program [15].
3. Experimental
Py-GC/MS experiments were performed at 500 8C for 20 s
in a Pyroprobe 2000 pyrolyser (Chemical Data System)
equipped with a platinum coil and quartz sample tube
interfaced to a gas chromatograph (Agilent 6890) coupled
with a mass selective detector (Agilent 5973) operating in
electron impact mode (EI) at 70 eV. The temperature of the GC/
MS interface was held at 280 8C.
A helium carrier gas of 20 ml/min flow rate purged the
pyrolysis chamber held at 250 8C. A split of the carrier gas
(1:20) was applied. The GC separation was carried out on a
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Fig. 2. Modeled product distribution of non-gaseous products backbiting
reactions excluded, residence time 20 s.
A. Nemeth et al. / J. Anal. Appl. Pyrolysis 81 (2008) 237–242 239
fused silica capillary column (Hewlett-Packard 5MS),
30 m � 0.25 mm. A temperature program from 50 to 300 8Cat 10 8C/min was applied with an isotherm period of 1 min at
50 8C and of 4 min at 300 8C.
4. Results and discussion
Because of different purpose of polyethylene pyrolysis,
experimental work available in literature is focused either on
gaseous products or on oil components (distillable, volatile non-
gaseous components) of the pyrolysate. We wanted to compare
the results of the present calculations on tetracontane to those of
experimental studies on polyethylene, thus the discussion of the
formation of gaseous and non-gaseous products is divided.
4.1. Non-gaseous products
Modeled distribution of non-gaseous products from tetra-
contane degradation is equimolar from carbon numbers of 8 to
35 (Fig. 1).
The exceptionally high molar ratio value of components of
36–37 carbon atoms is a modeling artifact, due to the choice of
tetracontane representing the polymer. Secondary alkyl radicals
formed from tetracontane undergo b-scission reactions, process
(v), however in case of CH3(CH2)37�CHCH3 there is only a
single possibility for b-scission (yielding the C37 primary alkyl
radical)
CH3�ðCH2Þ35�CH2�CH2��CH�CH3
! CH3�ðCH2Þ35��CH2þCH2¼CH�CH3
while for CH3(CH2)36�CHCH2CH3 the b-scission channel
yielding methyl radical is of much lower probability
CH3�ðCH2Þ34�CH2�CH2��CH�CH2�CH3
! CH3�ðCH2Þ34�CH2�CH2�CH¼CH2þ �CH3
than the other one yielding the C36 primary alkyl radical
CH3�ðCH2Þ34�CH2�CH2��CH�CH2�CH3
! CH3�ðCH2Þ34��CH2þCH2¼CH�CH2�CH3
Since the whole process is a long free radical chain process,
recombination (chain termination) has practically no effect on
Fig. 1. Modeled product distribution of non-gaseous products, residence time
20 s.
the stationary radical concentrations, the latter being deter-
mined by the consumption of the radicals in chain propagation
reactions. The secondary alkyl radicals formed from P have
only the b-scission as consuming reactions (besides the neg-
ligible termination reactions). Consequently reducing the cor-
responding rate constant (in case of the former one to one half,
in case of the latter one to about 65%) automatically means that
the stationary radical concentration is raised correspondingly.
The still operative b-scission channel thus yields increased
amounts of the corresponding primary alkyl radicals (as com-
pared to the shorter ones), and since their main consumption is
hydrogen abstraction from the polymer, this leads automati-
cally to increased C37 and C36 alkane levels. Simultaneously,
propene and butene are formed in the b-scission in increased
amounts, as compared to longer alkenes.
Backbiting does not affect equimolarity of non-gaseous
products (Fig. 2).
The consumption of tetracontane, however, increases from
89% to 93% at 20 s residence time as the consequence that H-
abstraction by primary alkyl radicals is more effective than by
secondary ones.
The experimentally observed non-gaseous product distribu-
tion of HDPE pyrolysed at around 500 8C is somewhat different
from that predicted by the model. The main reason of the
difference is certainly due to the high experimental conversion.
Nevertheless, a quasi-equimolar formation of 1-alkenes is
Fig. 3. Py-GC/MS total ion chromatogram of HDPE pyrolysis at 500 8C and
20 s residence time.
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Fig. 4. Modeled product distribution of gaseous products, residence time 20 s.
Table 2
Yields of volatile products (wt%)
Measured [17] Modeled
Methane 0.09 0.021
Ethane 0.13 0.177
Ethene 0.64 0.461
Propane 0.19 0.215
Propene 0.37 0.385
Butane 0.04 0.243
Butene 0.35 0.438
A. Nemeth et al. / J. Anal. Appl. Pyrolysis 81 (2008) 237–242240
found in several carbon atom ranges, such as between C10–C13,
C14–C17, C18–C21, C22–C28 [16]. As an example the section of
the pyrolysis-gas chromatogram displaying the product
distribution of C18–C22 hydrocarbons obtained at 500 8C in a
micropyrolyser (see Section 3) is shown in Fig. 3.
The figure also demonstrates that experimental alkane–
alkene–diene ratios vary between 0.40:1:0.30 and 0.56:1:0.46.
Based on stoichiometric considerations [6,8], sequence of steps
((ii)–(v)) implies 1:1 alkane–alkene ratios if effects of end groups
in the polymer are ignored while 1:2:1 statistical ratio of alkanes–
alkenes–dienes if the product alkane and alkene molecules are
also decomposed by further H-abstraction and b-scission.
4.2. Gaseous products
Apart of ethene, alkenes are almost exclusively products of
b-scission of secondary tetracontyl radicals. The increase of
pentene, hexene and heptene (Fig. 4) is due to the already
discussed b-scission of secondary alkyl radicals formed in
backbiting reactions towards the farther end of the molecule.
This is illustrated for radical in position 5 involving the
favored six-membered ring transition state yielding 1-hexene
CH3�ðCH2Þn�CH2�CH2��CH�CH2�CH2�CH2�CH3
! CH3�ðCH2Þn��CH2þCH2¼CH�CH2�CH2�CH2�CH3
The b-scission in the direction to the nearer end of the molecule
results in propyl radical that forms propane after H-abstraction.
The quasi-equal contribution of the scissions in the two possible
directions is indicated by the nearly equal molar fraction values
obtained for hexene and propane. Moreover, a similarly
increased formation of the pairs of gaseous products (pen-
tene–ethane and heptene–butane) emerged from the model.
The increased rate of butene and propene originates from the
specific feature of b-scissions of tetracontyl radicals in position 3
or 2. Scissions of radical in position 3 is methyl cleavage to the
right
CH3�ðCH2Þ34�CH2�CH2��CH�CH2�CH3
! CH3�ðCH2Þ34�CH2�CH2�CH2¼CH þ �CH3
less effective than scission to the left producing 1-butene
CH3�ðCH2Þ34�CH2�CH2��CH�CH2�CH3
! CH3�ðCH2Þ34��CH2þCH2¼CH�CH2�CH3
For tetracontyl radical in position 2 b-scission is possible only
to the left with enhanced propene formation. Contrary to C2–C4
alkanes, production of methane is less, due to the less effective
b-scission yielding methyl radical compared to other primary
radicals. The contribution of b-scissions of all other tetracontyl
radicals between left and right is equal.
Ethene can be formed in b-scissions by primary alkyl and
alkenyl radicals.
Comparison to yields of C1–C4 products reported by Conesa
et al. [17] measured at 500 8C and 20 s reaction time in a CDS
Pyroprobe 1000 micropyrolizer is given in Table 2. The
pyrolysis conditions were the same as applied in this work
detailed in Section 3. The GC analysis was performed in
alumina column and with FID detector.
Agreement between measured and modeled yields of ethane,
ethene, propane, propene and butene is rather good, less so for
methane and butane.
4.3. Contribution analysis
The analysis is confined to small (1.5%) tetracontane
consumption (reaction time 0.1 s) where alkadiene formation
assumedly can be neglected, data of higher tetracontane
consumption are used at some instances to illustrate tendencies
as degradation proceeds. Computed reaction rates and their
contribution to the production of each species are expressed as
fraction of the total production (formation +, consumption �sign), neglecting reactions of less than 1% contribution.
Computed rates of alkenes of equimolar distribution are
3.05 � 10�3 M s�1 but 3.11 � 10�3 M s�1of heptene,
3.18 � 10�3 M s�1 of hexene, 3.80 � 10�3 M s�1 of pentene,
5.22 � 10�3 M s�1 of butene and 6.14 � 10�3 M s�1 propene
reflecting the already discussed effects of backbiting reactions
and specific features of b-scission. Contribution analysis also
quantified the ratio of contribution between scissions to right
and left of tetracontyl radicals in position 3 as 15:85.
Contributions to the degradation of the polymer at different
time points reveal the increasing role of small alkyl radicals as
the degradation proceeds. At 0.1 s, the highest contributors are
H-abstraction by primary alkyl radical of 37 carbon number
followed by ethyl radical, alkyl radical of 36 carbon number,
propyl and butyl radical. At 3.5 s the order still starts with H-
abstraction by the primary alkyl radical of 37 carbon atoms, but
followed by butyl radical. The rate of production of equimolar
alkanes is 3.00 � 10�3 M s�1, but that of heptatriacontane and
hexatriacontane (alkanes of 37 and 36 carbon number) are
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Fig. 5. Modeled diene–alkene ratios at 0.01, 0.1 and 3.5 s residence times.
A. Nemeth et al. / J. Anal. Appl. Pyrolysis 81 (2008) 237–242 241
5.95 � 10�3 M s�1 and 5.04 � 10�3 M s�1 higher than the
equimolar rate for reasons already discussed.
Nevertheless, the modeled 1:1 alkane–alkene ratio is rather
time independent in the non-gaseous fraction but the diene–
alkene ratio increases with time (Fig. 5).
Fig. 6. Reaction graph of the main reactio
The latter trend indicates that stepping forward from the
early state of degradation dominated by steps (ii) and (v) a
forthcoming research should address reactions of enhanced
fragmentation of alkane and alkene products and improvement
of the mechanism with special emphasis on diene formation.
n pathways, low polymer conversion.
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Table 4
Rate of production of the main reaction pathways (M s�1)
Process Residence time
0.01 s 0.1 s 3.5 s
Initiation (i) 1.89 � 10�5 1.83 � 10�5 1.09 � 10�5
H-transfer (ii) 8.89 � 10�2 8.80 � 10�2 5.63 � 10�2
b-Scission (iii) 5.35 � 10�4 5.37 � 10�4 5.65 � 10�4
H-shift (iv) 2.38 � 10�2 2.39 � 10�2 2.47 � 10�2
b-Scission (v) 1.09 � 10�1 1.08 � 10�1 7.85 � 10�1
H-transfer (vi) 2.19 � 10�2 2.19 � 10�2 2.24 � 10�2
H-transfer (vii) 1.82 � 10�6 2.03 � 10�5 6.41 � 10�4
b-Scission (viii) 1.76 � 10�6 1.97 � 10�5 6.18 � 10�4
b-Scission (ix) 1.61 � 10�6 1.80 � 10�5 5.65 � 10�4
b-Scission (x) 9.15 � 10�6 1.02 � 10�4 3.21 � 10�3
H-transfer (xi) 1.65 � 10�6 1.85 � 10�5 5.80 � 10�4
Termination (xii) 2.13 � 10�5 2.10 � 10�5 1.25 � 10�5
Table 3
Alkyl radical concentrations, molar fraction
Residence time
0.01 s 0.1 s 3.5 s
Methyl 2.8 � 10�11 2.8 � 10�11 3.1 � 10�11
Ethyl 1.1 � 10�10 1.1 � 10�10 1.3 � 10�10
Propyl 9.3 � 10�11 9.4 � 10�11 1.1 � 10�10
Butyl 9.0 � 10�11 9.0 � 10�11 1.1 � 10�10
Pentyl 8.7 � 10�11 8.8 � 10�11 1.0 � 10�10
Hexyl 8.5 � 10�11 8.6 � 10�11 1.0 � 10�10
C7–C35 alkyl 6.7 � 10�11 6.7 � 10�11 7.0 � 10�11
C36 alkyl 1.1 � 10�10 1.1 � 10�10 1.1 � 10�10
C37 alkyl 1.3 � 10�10 1.3 � 10�10 1.3 � 10�10
A. Nemeth et al. / J. Anal. Appl. Pyrolysis 81 (2008) 237–242242
At 1.5% tetracontane consumption the contribution of
primary alkyl radicals, and secondary alkyl radicals in position
5 and 6 to the formation of majority of alkanes is 0.80, 0.15 and
0.05, respectively. At 44% tetracontane consumption the
contribution of the above mentioned radicals changes to 0.70,
0.20 and 0.10, respectively. Contribution by secondary radicals
to the formation of hexane and pentane is less than the above
values, since 1,6-H-shift on hexyl carbon chain, 1,6 and 1,5-H-
shifts on pentyl cannot occur. C1–C4 alkanes are produced only
from the corresponding primary radicals by H-abstraction.
Concentration of alkyl radicals at 0.01, 0.1 and 3.5 s
residence times are summarized in Table 3 revealing quasi-
steady state radical concentration established within milli-
seconds.
Termination rates contribute less than 0.01% to radical
consumption for all types of radicals.
Reaction graph in Fig. 6 illustrates main reaction pathways
and corresponding rates of production at residence times 0.01,
0.1 and 3.5 s are summarized in Table 4.
Alkane production is dominated by arrow (ii), rate by arrow
(vi) is half of it even at higher tetracontane consumption.
b-Scission of secondary alkyl radicals, arrow (v) has the highest
rate at all conversion values studied, while the rate of
backbiting, arrow (iv) is almost a quarter of this value,
emphasizing the importance of such radical transformations.
Indeed, a secondary alkyl radical can yield several short
alkenes while cycling several times through arrows (v) and
(iv), contributing significantly to the increase of gaseous
products.
Though the sequences of the reaction mechanism are well
established in the literature and the compiled reactions are
thermochemically feasible, due to the complexity of the system
and scarcity of rate constants available as well as the scarcity of
current evidence the solution of the differential equation system
is not unique, the set represents only a possible reaction
mechanism. Sensitivity analysis can be informative in this
respect. Analysis of computed sensitivity coefficients reveals
that while both alkane and alkene concentrations are with order
of magnitude more sensitive to rate constants of b-scissions,
diene concentrations are sensitive to rate constants of
corresponding H-abstraction reactions. The system is most
sensitive to rate constants of b-scission of primary alkyl
radicals producing ethane. In our model these rate constant
values, together with those of the already discussed backbiting
reactions, are independent of the carbon chain lengths of the
reactants, more reliable experimental values would be needed
to improve the modeling, indicating priorities for further
research.
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