Formation and Thermal Behavior of Polystyrene and Polystyrene/Clay Gels
Transcript of Formation and Thermal Behavior of Polystyrene and Polystyrene/Clay Gels
Full Paper
Formation and Thermal Behavior ofPolystyrene and Polystyrene/Clay Gels
Kai Chen, Ashley N. Baker, Sergey Vyazovkin*
DSC was used to study the thermal behavior of virgin PS as well as of PS/clay nanocompositesof exfoliated brush and of intercalated structure dissolved in carbon disulfide. Compared tovirgin PS, the behavior of the brushmaterial did not show any obvious difference, whereas theintercalated material demonstrated markedlylarger heats of gelation and gel melting. Isocon-versional kinetic analysis of the melting processrevealed that the activation energy was indepen-dent of the conversion for the gels prepared underisothermal conditions, whereas an increase in theactivation energy with the extent of conversionwas observed for the gels prepared under con-tinuous cooling conditions. The melting of thenonisothermally prepared gels apparentlyoccurred alongside with the formation of newgel structures.
Introduction
Gels are formed from polymer solutions (sols) as a result of
crosslinking of macromolecules. A transition from sol to
gel occurs at the point when the extent of crosslinking
becomes such that the solution loses its ability to flow.
When crosslinking occurs at the expense of relativelyweak
intermolecular forces it gives rise to thermoreversible or
physical gels. Such gels can be turned to sols and back to
gels by simply changing the temperature. It has been
reported[1] that solutions of atactic polystyrene (PS) in a
number of solvents can form thermoreversible gels.
Although the gel formation in some solvents has been
questioned by rheological tests,[2] gelation of PS solutions
in carbon disulfide (CS2) is an established experimental
K. Chen, A. N. Baker, S. VyazovkinDepartment of Chemistry, University of Alabama at Birmingham,901 S. 14th Street, Birmingham, AL 35294, USAE-mail: [email protected]
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fact.[3–5] The thermal behavior of PS/CS2 gels has been
studied[6,7] by using differential scanning calorimetry
(DSC) that allowed for determining the heats and
temperatures of the sol/gel (i.e., gelation) and gel/sol
(i.e., melting) conversion. In this work, DSC is applied to
study comparative thermal behavior of PS and PS/clay gels
formed from their respective solutions in CS2. To our
knowledge no systematic studies of the sol/gel and gel/sol
conversion in polymer/clay nanocomposite systems have
yet been conducted. Introduction of nanoparticles is
known to modify a wide variety of processes in polymers
such as glass transition, crystallization, melting and
degradation.[8–12] It is, therefore, quite naturally expected
that the processes of gelation and gel melting can too be
modified in the presence of clay nanoparticles. The
expectation is also supported by the frequently noted
similarities between the processes of gelation and crystal-
lization of polymers. For the latter, introduction of clay
nanoparticles has shown two opposing effects: accelera-
tion that can be linked to nucleating effect of the particles
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K. Chen, A. N. Baker, S. Vyazovkin
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and deceleration that can be associated with slowing
down of polymer chain mobility. Note that crosslinking of
macromolecules by forming crystallites in polymer solu-
tions is considered to be one of the major mechanisms of
gelation even for noncrystallizable polymers such as
atactic PS.[13]
In a previous paper,[14] we have reported on similarities
and differences in the thermal degradation and relaxation
behavior of two PS/montmorillonite clay nanocomposites,
one of which had an intercalated clay structure and the
other an exfoliated clay brush structure. The present work
extends a study of these two nanocomposites to the
thermal behavior of their respective gels and intends to
reveal possible effects of clay on the processes of the sol/
gel and gel/sol conversion. The paper also presents what
appears to be the first application of isoconversional
kinetic analysis[15] to the process of gel melting. The
analysis has been successful in providing physical insights
into a variety of relevant processes,[15] including chemical
crosslinking (curing), crystallization, glass transition, as
well as glass aging,[16] collagen denaturation,[17] gelation
of gelatin[18] and starch[19] solutions.
Experimental Part
Preparation and characterization of the PS/montmorillonite
(MMT) clay nanocomposites used in this study have been
described in detail elsewhere.[20–22] Briefly, the intercalated PS/
clay sample was prepared by a bulk polymerization technique.[20]
The organically modified MMT clay (under commercial name
Cloisite1 10A, containing a surfactant of dimethylbenzyl hydro-
genated tallow ammonium chloride) was used as received from
Southern Clay Product Inc. A radical initiator 2,20-azoisobutyroni-
trile (AIBN) and styrene monomer were mixed with the
organically modified MMT by stirring at room temperature under
flowing nitrogen gas. The bulk polymerization was carried out at
60 8C for 24 h and then at 80 8C for 24 h. The intercalated structure
of the resulting nanocomposites was confirmed by X-ray
diffraction (XRD)[20,23] and transmission electron microscopy
(TEM)[24] for the samples having different clay content. The
resulting material is further referred to as ‘‘intercalated’’ system.
The exfoliated PS/clay nanocomposite containing 1% byweight
of MMT was prepared by a solution surface-initiated polymeriza-
tion (SIP) method.[21,22] A monocationic initiator, (AIBN-analogue
compound with quaternized amine group at one end) was
intercalated inside the gallery of pristine MMT via a cation
exchange reaction in which the cationic end of the initiator was
ionically attached to the negatively charged silicate surface.[21]
The initiator-modified clay particles were mixed with styrene
monomer in THF solvent. At 60 8C, the in situ polymerization
under nitrogen atmosphere was directly initiated from the clay
surface[22] to which the initiators have been attached. In the final
products, the exfoliation of MMT clay and the attachment of the
initiator and PS chains onto the clay surface were demon-
strated[21,22] by XRD, infrared spectroscopy (IR), X-ray photoelec-
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tron spectroscopy (XPS) and atomic force microscopy (AFM). The
respective material is further referred to as ‘‘brush’’ system. The
brush system containing 1 wt.-% of clay was compared to the
intercalated system having 5 wt.-% of clay because these two
systems demonstrated significant similarity in a previous
study[14] of the processes of degradation and relaxation. For
comparison purposes, radically polymerized PS (Alfa Aesar) was
used as received and is referred to as ‘‘virgin’’ PS. The Mw of PS in
the intercalated system was determined[14] to be 1.61�105
g �mol�1. The Mw values are comparable to the previously
determined values for the brush system (0.90�105 g �mol�1)
and for virgin PS (1.00� 105 g �mol�1).[22]
High purity carbon disulfide (CS2, Spectranalyzed1, Fisher
Scientific) was used as solvent to make PS solutions. Pure PS and
PS/clay nanocomposites were dissolved in CS2 in hermetically
closed vials at the temperature of 45 8C over period of no less than
24 h to ensure complete dissolution. The concentration of resulting
solutions for all samples is 300 mg �mL�1 or�19 wt.-% (the density
of CS2 is 1.26 g � cm�3 [25]).
The gel formation and its melting behavior for all PS systems
were characterized by heat flux DSC (Mettler-Toledo, 822e).
Temperature, heat flow and tau-lag calibrations were performed
by using indium and zinc standards. The experiments were
conducted in the atmosphere of nitrogen flow (80 mL �min�1). A
typical sample size of PS solutionwas about 60–80mg. All samples
were hermetically sealed in 100 mL Al pans. The absence of leaks
was confirmed by measuring the sample mass before and after
each DSC run. The PS gels were formed under either isothermal or
continuous cooling conditions. Under isothermal condition, the PS
solutions were cooled down to �50 8C at a cooling rate of
10 8C �min�1, then the samples were held at this temperature for
30 min. Since no thermal events were detected during cooling at
10 8C �min�1, it is believed that either no PS gel was formed or it
was produced in a negligibly small amount undetectable by DSC.
That is, PS gels were predominately formed during the isothermal
hold at�50 8C. The gel formation processwas directlymeasured as
an exothermic DSC peak under continuous cooling conditions at a
very slow cooling rate of 1 8C �min�1. At this rate, the PS solutions
were cooled from 50 to �70 8C. Once PS gels were formed, either
under isothermal or continuous cooling condition, they were
immediately heated to 50 8C by using various heating rates: 5, 7.5,
10, 12.5, and 15 8C �min�1. The melting behavior of PS gel was
characterized by the melting peak temperature, the heat of
melting, and the effective activation energy of melting. All DSC
measurements were repeated at least 2 times.
Isoconversional Kinetic Computations
The DSC data on gel melting were subjected to isoconversional
kinetic analysis, for which purpose the effective activation energy,
Ea, was determined as a function of the extent of conversion, a, by
employing the advanced isoconversional method proposed by
Vyazovkin.[26,27] The method affords evaluating a Ea dependence
from a set of n experimental runs performed under different
temperature programs, Ti(t). The effective activation energy is
estimated at any given value of a by finding Ea, which minimizes
the function:
F Eað Þ ¼Xni¼1
Xnj 6¼i
J Ea; Ti tað Þ½ �J Ea; Tj tað Þ� � (1)
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Formation and Thermal Behavior of Polystyrene and Polystyrene/Clay Gels
where
Fig1 8CHersam
Macrom
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J Ea; Ti tað Þ½ � �Zta
ta�Da
exp�EaRTi tð Þ
� �dt (2)
In Equation 2, a varies fromDa to 1–Dawith a stepDa, typically
chosen to be 0.02. The integral, J, is calculated numerically by
using the trapezoid rule. Theminimization routine is performed at
each value of a to establish the dependence of the activation
energy on the extent of conversion. The mean relative error of the
Ea values determined in the present study was around 20% in
agreement with the results of the previous analysis[28] of the
method. The advanced isoconversional method has two crucial
advantages over the simpler isoconversional methods of Flynn
and Wall[29] and Ozawa.[30] First, it is capable of treating data
obtained under arbitrary temperature programs that secures its
validity in the case when a preset program is distorted by self-
heating or cooling of a sample. Second, because of performing
integration over small time segments (Equation 2) it eliminates a
systematic error[27] present in the Flynn and Wall and Ozawa
methods when Ea varies significantly with a.
Results and Discussion
Sol-to-Gel Conversion
Figure 1 presents data obtained on cooling of PS sols. It is
seen that in all three systems the exothermic process of
ure 1. Heat release detected by DSC on cooling PS sols at�min�1. Each curve is an average of five measurements.e and in all other figures the heat is given per gram ofple.
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crosslinking (sol/gel conversion) starts roughly below
�10 8C and continues down to �60 8C. Unexpectedly, theintercalated and brush samples have shown significantly
different behavior. The DSC peak for the brush sample
appears to be quite similar to that for the virgin PS sample.
There is no obvious difference in the respective heights and
width of the peaks. The integral heat for the brush sample
is only a little smaller (0.4 J � g�1) than that for the virgin
sample (0.5 J � g�1). Compared to the brush sample, the
peak for the intercalated sample is significantly taller and
its area is significantly larger (2.0 J � g�1). This means that
the presence of clay in the intercalated system promotes
the process of sol-gel conversion, whereas in the brush
system it shows no obvious effect. Such a difference is very
surprising because these two materials have previously
shown[14] very similar effects in terms of the thermal
degradation and glass transition behavior. Apparently, the
thermal behavior of these two systems changes in the
presence of the solvent. It should be recalled that the
interaction between PS and clay in these two materials is
of quite different nature. In the brush system the PS chains
are tethered to the clay surface via strong ionic forces. On
the other hand, in the intercalated system the PS chains are
attached to the organically modified clay surface primarily
via much weaker van der Waals forces. Therefore, in the
presence of the solvent some of the PS chainsmay separate
from the clay surface while in solution. As a result, the
nanoconfinement[14] of PS chains diminishes and their
mobility increases. Since the intercalated system has �5
times more clay than the brush system, it should have a
substantial vacant clay surface that may act as a site for
initiation of crosslinking when the temperature is lowered
below the gel temperature, Tgel. It seems quite reasonable
to expect that the dominant effect of intercalated clay
nanoparticles should be promoting the gel formation
because several PS chains anchored to a certain spot on the
clay surface would more readily crosslink than regular
chains in the solution.
However no enhanced crosslinking seems to be
observed in the brush system, in which the PS chains
are strongly bound to the surface. The reason for this is not
only the smaller clay content, but also that the clay surface
is effectively shielded by the dense brushwhose interchain
distance and grafting density are estimated[31] to be about
3.8 nm and 0.07 chains per nm2, respectively. In this
situation, the clay surface could only promote crosslinking
of the chains directly attached to the surface. However, this
effect is likely to be offset by the slow chainmobility due to
nanoconfinement of the PS chains that spreads much
farther away from the clay surface than in the case of the
intercalated system.[14] These reasons can explain why the
presence of clay in the brush system does not show any
obvious accelerating effect as in the case of the inter-
calated system.
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K. Chen, A. N. Baker, S. Vyazovkin
Figure 3. Heat absorption measured by DSC on 10 8C �min�1 heat-ing of PS gels prepared under isothermal and continuous coolingconditions. The curves for isothermally prepared gels are insidethe dashed rectangle.
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Melting of Gels Formed under Isothermal Conditions
According to rheological data,[4] PS-CS2 sols of a similar
concentration (200 g � L�1) and similar Mw of PS (1.8�105 g �mol�1) gel at Tgel around �17 8C. Similar to the rate
of polymer crystallization,[32,33] the rate of the gel formation
has a negative temperature dependence. That is, cooling a
PS/CS2 sol to a lower temperature leads to faster formation
of the gel.[4] In our study, we have tested three
temperatures (�20, �30, and �50 8C) to which PS/CS2 sols
were cooled and held for a certain time. Heating of the
resulting gels andmeasuring the heat of melting has given
us an idea about the amount of the gel formed. It has been
observed that the rate of the sol/gel conversion at �50 8Cwas markedly faster than at �30 and �20 8C. At the latter
temperature the melting effects have been barely detect-
able. Figure 2 demonstrates the evolution of the heat of
melting and the melting peak temperature of a virgin PS
gel as a function of the time of aging at �50 8C. It is seenthat both parameters continue evolving over a period of
8 h without reaching a plateau (i.e., equilibrium). The
amount of heat detected on melting of a gel aged for 8 h is
�0.25 J per gram of gel that corresponds approximately to
1.3 J per gram of PS. The amount of heat released on
melting of the gels aged for 30 min at �50 8C has been
found sufficient to perform a comparative study ofmelting
of the PS and PS/clay gels.
Figure 3 presents the melting DSC peaks for PS gels
formed after aging for 30 min at �50 8C. It is observed that
the peaks for the brush and virgin PS systems are quite
similar. Compared to these peaks, the peak for the
intercalated system is markedly larger. This result is
Figure 2. Evolution of the heat of melting and the melting peaktemperature in virgin PS gel aged at �50 8C for different periodsof time up to 8 h.
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consistent with the fact that the presence of clay in this
system promotes the process of crosslinking (Figure 1).
Being crosslinked to a greater extent the respective gel
should obviously demonstrate a larger heat ofmelting. The
heat of melting in either of the three systems has been
practically independent of the heating rate. Figure 4 shows
a representative set of the melting peaks for the brush
system at five different heating rates. The heating rate
average value of the heat of melting for this system is
Figure 4. Heat absorption measured by DSC on heating of thebrush sample at different heating rates. The numbers by the linesdenote the respective values of the heating rate.
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Formation and Thermal Behavior of Polystyrene and Polystyrene/Clay Gels
Figure 5. Effective activation energies evaluated as a function ofconversion for melting of the gels prepared under isothermalconditions.
�0.10 J � g�1. The same average value has been determined
for the virgin PS system. For melting of the intercalated
system, the heating rate average value is 50% larger, i.e.,
�0.15 J � g�1.
The gel melting data obtained at different heating rates
have been subjected to isoconversional analysis. Figure 5
presents the effective activation energies of the process as
a function of the gel to sol conversion in all three systems.
For each of these systems, the values of Ea are practically
independent of a that suggests that the gel melting
kinetics is limited by a single step pathway. The average
value of Ea for virgin PS system is �88 kJ �mol�1.
It is somewhat larger for the intercalated system
(�100 kJ �mol�1) and slightly smaller for the brush system
(�78 kJ �mol�1). However, these small differences are not
necessarily significant considering that, as mentioned in
above, the average error in Ea reaches 20%.
Figure 6. Heat absorption measured by DSC on heating of thevirgin sample at different heating rates. The numbers by the linesdenote the respective values of the heating rate.
Melting of Gels Formed on Continuous Cooling
The gels formed under nonisothermal conditions (constant
cooling rate 1 8C �min�1) demonstrate a complex melting
behavior which is quite different from that of the gels
formed isothermally. First of all, one can immediately see
(Figure 3) that for any of the three systems the DSCmelting
peaks are significantly broader than those for the
isothermally formed gels. The latter melt in the tempera-
ture range from �40 to �20 8C, whereas the former start
melting at around �50 8C and continue to melt up to 0 8C.As in the case of isothermally formed gels, the intercalated
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system shows a larger melting DSC peak than the virgin
and brush systems. On average the heats of melting of the
intercalated systems are about 2 times larger than those of
the virgin systems when compared at respectively similar
heating rates (Figure 6 and 7). This result is expected
considering the enhanced crosslinking process in the
intercalated system (Figure 1). Unexpected is the fact that
the melting peaks for the brush system have been
considerably smaller than those observed for the virgin
system. They have also consistently demonstrated a rather
poor signal to noise ratio because the process rate (i.e.,
intensity of DSC signal) has been quite low.
Another unexpected result is that the height and the
area of the DSC melting peaks have demonstrated a
systematic decrease with the heating rate (Figure 6 and 7).
The expectation has been that the integral heats ofmelting
should be comparable to the integral heats of the sol-gel
conversion in the respective systems (Figure 1). However,
the comparable heats could only be obtained at slow
heating rates around 2 8C �min�1, whereas at progressively
faster heating rates the heats of melting have been
consecutively smaller in all types of gels. We hypothesize
that this phenomenon is associated with the complex
structure of the gels formed on continuous cooling. It is
known that a sol cooled to and aged at a certain
temperature, Ta below Tgel forms a gel whose melting
point is larger than Ta (e.g., see Figure 2). Continuous
cooling of a sol is equivalent to going through a series of
very short aging periods at progressively smaller aging
temperatures. This would result in the formation of
various gel structures, having progressively smaller
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K. Chen, A. N. Baker, S. Vyazovkin
Figure 8. Effective activation energies evaluated as a function ofconversion for melting of the gels prepared under continuouscooling conditions.
Figure 7. Heat absorption measured by DSC on heating of theintercalated sample at different heating rates. The numbers bythe lines denote the respective values of the heating rate.
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melting temperatures. This type of behavior has been
observed for gelatin gels.[34] When the lower melting point
gel structures start melting on heating, they cannot form a
stable sol because the temperature is below Tgel. That
means that the just formed supercooled sol would tend to
form new gel structures, having a larger melting
temperature. Consequently, the endothermic heat flow
associated with the melting would partially be offset by
the exothermic heat flow related to the formation of the
new gel. Thus, the overall process of the gel melting can
be envisioned roughly as a competition of two pathways:
the gel to sol conversion and the new gel formation.
Because the two pathways are likely to have different
activation energies, a relative contribution of a larger
activation energy pathway to the overall process rate
would increase with increasing temperature. On the other
hand, the temperature of the melting process increases
with increasing the heating rate as can be seen from the
shift in the DSC peaks displayed in Figure 6 and 7.
Therefore, the decrease in the endothermic heat flow
observed upon increasing the heating rate is indicative of
an increasing contribution of the exothermic pathway
associated with the new gel formation. As the overall
endothermic heat flow becomes progressively smaller
with increasing the heating rate, the progressively larger
portion of the overall heat of melting falls below the
detection limit of the DSC instrument.
The fact that the melting occurs via more than one
pathway can be readily detected[15] by using isoconver-
sional kinetic analysis. The application of the latter to the
melting of the intercalated and virgin systems has resulted
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in the Ea dependencies shown in Figure 8. Because of the
poor signal to noise ratio the brush system melting data
have been unsuitable for the analysis. As seen in Figure 8,
both systems demonstrate increasing Ea dependencies
that are characteristic[35] of the competing pathways
kinetics. The initial stages of the melting yield effective
activation energy of around 45 kJ �mol�1 that apparently
represents disintegration of the least stable (low melting
temperature gel structures). As the melting proceeds the
effective activation energy of the overall processes quickly
rises which reflects an increasing relative contribution of
the pathway, having larger activation energy. According to
our hypothesis this is the exothermic pathway that leads
to the new gel formation. At any rate, isoconversional
analysis clearly demonstrates that the melting kinetics of
the gels formed on continuous cooling is definitely more
complex than of the gels formed isothermally. The latter
shows the Ea values that are practically independent of a
(Figure 5) which is characteristic of a single pathway
melting process.
Conclusion
Although the gel formation and gel melting in the system
PS/CS2 is accompanied by release and absorption of very
small amounts of heat, DSC has been found suitable for
detecting the effects of clay on the thermal behavior of PS/
clay/CS2 systems. The effect is dependent on the structure
of PS/clay composite. While negligible in the brush system,
the effect has been obvious in the intercalated system that,
DOI: 10.1002/macp.200800430
Formation and Thermal Behavior of Polystyrene and Polystyrene/Clay Gels
compared to the virgin PS system, has demonstrated a
significant increase in the heats of both gel formation and
gel melting. Significant differences have been discovered
in the melting behavior of the gels prepared under
isothermal and continuous cooling conditions. The melt-
ing of isothermally prepared gels appears to be dominated
by a single pathway of the gel/sol conversion. On the other
hand, the results obtained for the melting of the gels
prepared under continuous cooling conditions suggest
that the process occurs via competition of the gel/sol
conversion and the formation of new gel structures.
Acknowledgements: Support from the American Chemical SocietyPetroleum Research Fund under grant 46760-AC7 is gratefullyacknowledged, as is support for the SUMR Scholar (A. N. Baker)under grant 46760.01-AC7.
Received: August 25, 2008; Revised: September 24, 2008;Accepted: September 25, 2008; DOI: 10.1002/macp.200800430
Keywords: activation energy; differential scanning calorimetry(DSC); gelation; kinetics; nanoparticles
[1] H. M. Tan, A. Moet, A. Hiltner, E. Baer, Macromolecules 1983,16, 28.
[2] D. J. Plazek, T. Altares, J. Appl. Phys. 1986, 60, 2694.[3] J. Clark, S. T. Wellinghoff, W. G. Miller, Polym. Prepr. (Am.
Chem. Soc., Div. Polym. Chem.) 1983, 24, 86.[4] Y. S. Gan, J. Francois, J. M. Guenet, Makromol. Chem, Rapid
Commun. 1985, 6, 225.[5] D. J. Plazek, I. C. Chay, Polym. Prepr. (Am. Chem. Soc., Div.
Polym. Chem.) 1991, 32, 433.[6] J. Francois, J. Y. S. Gan, J. M. Guenet,Macromolecules 1986, 19,
2755.[7] X. M. Xie, A. Tanioka, K. Miyasaka, Polymer 1991, 32, 479.
Macromol. Chem. Phys. 2008, 209, 2367–2373
� 2008 WILEY-VCH Verlag GmbH & Co. KGaA, Weinheim
[8] S. S. Ray, M. Okamoto, Progr. Polym. Sci. 2003, 28, 1539.[9] M. Alcoutlabi, G. B. McKenna, J. Phys. : Condens. Matter 2005,
17, R461.[10] A. Leszczynska, J. Njuguna, K. Pielichowski, J. R. Banerjee,
Thermochim. Acta 2007, 453, 75.[11] C. Harrats, G. Groeninckx, Macromol. Rapid Commun. 2008,
29, 14.[12] D. R. Paul, L. M. Robertson, Polymer 2008, 49, 3187.[13] R. C. Domszy, R. Alamo, C. O. Edwards, L. Mandelkern, Macro-
molecules 1986, 19, 310.[14] K. Chen, C. A. Wilkie, S. Vyazovkin, J. Phys. Chem. B 2007, 111,
12685.[15] S. Vyazovkin, N. Sbirrazzuoli, Macromol. Rapid Commun.
2006, 27, 1515.[16] K. Chen, S. Vyazovkin, Chem. Phys. Lett. 2007, 448, 203.[17] S. Vyazovkin, L. Vincent, N. Sbirrazzuoli, Macromol. Biosci.
2007, 7, 1181.[18] K. Chen, S. Vyazovkin, Macromol. Biosci., DOI: 10.1002/
mabi.200800214.[19] K. Pielichowski, P. Tomasik, M. Sikora, Carbohydr. Polym.
1998, 35, 49.[20] J. Zhu, C. A. Wilkie, Polym. Int. 2000, 49, 1158.[21] X. Fan, C. Xia, R. C. Advincula, Colloid Surf. A 2003, 219, 75.[22] X. Fan, C. Xia, T. Fulghum, M. K. Park, J. Locklin, R. C. Advin-
cula, Langmuir 2003, 19, 916.[23] B. N. Jang, C. A. Wilkie, Polymer 2005, 46, 2933.[24] J. Zhu, F. M. Uhl, A. B. Morgan, C. A. Wilkie, Chem.Mater. 2001,
13, 4649.[25] Handbook of Chemistry and Physics, 83rd edition, D. R. Lide,
Ed., CRC Press, Roca Baton 2002.[26] S. Vyazovkin, J. Comput. Chem. 1997, 18, 393.[27] S. Vyazovkin, J. Comput. Chem. 2001, 22, 178.[28] S. Vyazovkin, C. A. Wight, Anal. Chem. 2000, 72, 3171.[29] H. Flynn, L. A. Wall, J. Res. Nat. Bur. Stand, A 1966, 70, 487.[30] T. Ozawa, Bull. Chem. Soc. Jan 1965, 38, 1881.[31] K. Chen, M. A. Susner, S. Vyazovkin, Macromol. Rapid Com-
mun. 2005, 26, 690.[32] J. M. Schultz, ‘‘Polymer Crystallization’’, ACS & Oxford Uni-
versity Press, Washington, D.C. 2001.[33] L. Mandelkern, ‘‘Crystallization of Polymers’’, 2nd edition, Vol.
2, Cambridge University Press, Cambridge 2004.[34] K. te Nijenhuis, Colloid Polym. Sci. 1981, 259, 1017.[35] S. Vyazovkin, Int. J. Chem. Kinet. 1996, 28, 95.
www.mcp-journal.de 2373