Shogo Kumagai,
Yuto Morohoshi,
Guido Grause,
Tomohito Kameda and
Toshiaki Yoshioka*
Graduate School of Environmental Studies, Tohoku University, 6-6-07 Aoba, Aramaki-aza, Aoba-ku, Sendai, Miyagi 980-8579, Japan. E-mail: yoshioka@env.che.tohoku.ac.jp
First published on 13th July 2015
Steam decomposition, a method employed for the depolymerization of polyesters, does not require solvents, catalysts, or high pressure. During steam decomposition, the fission of the ester group occurs by hydrolysis, whereas the ester group is cleaved without the action of water during pyrolysis, affording reduced monomer yields. Hence, elucidating the contribution of hydrolysis and pyrolysis to depolymerization in a steam atmosphere, as well as the effect of polyester structure on selectivity, will improve the accuracy of kinetic analyses and maximize monomer yields. In this study, the selectivities for pyrolysis and hydrolysis during the steam decomposition of polyethylene terephthalate (PET), polybutylene terephthalate (PBT), and polyethylene 2,6-naphthalate (PEN) were quantified using 18O-labeled steam at different steam concentrations and decomposition temperatures. The decomposition temperature strongly affected the hydrolysis selectivity for PET and PBT, whereas that for PEN was hardly affected. The selectivity for polyester hydrolysis increased with increasing steam concentration for both PET and PEN, with the exception of PBT. These results revealed that the selectivities for both pyrolysis and hydrolysis were significantly affected by the structure of the polyester. In addition, the thermogravimetric kinetic analysis of steam decomposition was consistent with the results of the 18O-labeling experiments.
On the other hand, pyrolysis is an attractive method because it only requires heat. Detailed mechanisms for the pyrolysis of aromatic polyesters have been reported previously. In this process, cyclic oligomers such as dimers, trimers, and tetramers are initially formed by intramolecular exchange.24–28 These oligomers are further decomposed by β-hydrogen transfer to the carbonyl carbon via six-membered ring intermediates,29,30 resulting in carboxylic acids such as terephthalic acid (TPA) and 2,6-naphthalene dicarboxylic acid (NDC), which can be used as feedstock for polyester synthesis. However, typically low recovery rates are obtained for these carboxylic acids, as vinyl esters that are simultaneously produced cannot be further pyrolyzed to carboxylic acids.
On the other hand, hydrolysis proceeds by the nucleophilic attack of the carbonyl carbon by water. Hence, hydrolysis enables the recovery of carboxylic acids in high yield. However, subcritical and supercritical conditions,2,13,19,23 as well as the addition of acid or base catalysts,4,6,7 are often required because under neutral conditions, the hydrolysis of polyesters is very slow,31–33 caused by their low water solubility. In addition, if polyester wastes contain additives such as metals or glass fillers, any solvent that is present must be regenerated after prolonged use as the additives accumulate in the medium. Finally, mixed polymers must be separated before the process. Hence, suitable plastics are limited for hydrolysis.
Herein, we examine the steam decomposition of polyesters, which exploits the advantages of both pyrolysis and hydrolysis. In this process, decomposition is conducted under steam at the pyrolysis temperature, allowing for the hydrolysis of polyesters at a speed more rapid as compared to that without catalysis at atmospheric pressure. On the other hand, inorganic additives can be separated as solids by the volatilization of organics.34 Furthermore, other plastics, which typically must be separated before solvolysis, can be simultaneously decomposed into oil and gas compounds.35 Hence, steam decomposition is a key technology for overcoming the obstacles of both pyrolysis and hydrolysis.
Hydrolysis and pyrolysis simultaneously occur during the steam decomposition of polyesters because it is conducted at high temperatures; the latter has a negative impact on the yield and selectivity of monomers. However, to the best of our knowledge, very little is known about the mechanism and kinetics of polyester decomposition under steam,3 although pyrolysis and hydrolysis have been widely reported. Thus, the manner in which pyrolysis affects hydrolysis still remains unclear, and vice versa. Hence, we developed a novel approach for quantifying the selectivities for pyrolysis and hydrolysis during the steam decomposition of PET using 18O-labeled steam (Scheme 1).36 Selectivity is calculated from the ratio of labeled and unlabeled TPA determined by gas chromatography-mass spectroscopy (GC-MS).
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Scheme 1 Identification of (a) pyrolysis and (b) hydrolysis products in the 18O-labeled steam decomposition of PET.36 |
In this study, the pyrolysis-versus-hydrolysis behavior of PET, PBT, and PEN during steam decomposition was investigated using our approach. Understanding this behavior is useful for predicting the decomposition mechanism and optimizing product yields. In addition, by the comparison of the three polyesters, the influence of the polymer structure on the pyrolysis and hydrolysis selectivities for each transformation was clarified during steam decomposition. For this purpose, the influence of steam concentration and decomposition temperature on the pyrolysis and hydrolysis selectivities in PET, PBT, and PEN was investigated using 18O-labeled steam. In addition, kinetic analyses of the steam decomposition of these polyesters were conducted by model-fitting techniques using a thermogravimetric analyzer. The results obtained from the 18O-labeling tests and kinetic analyses were compared for consistency. Our previously published letter briefly describes some of the results for PET.36 However, all experiments for PET were repeated and updated for an accurate comparison with the results for PBT and PEN under the same conditions.
18O-Labeled water (H218O) with a purity of >98% (SKChem Co., Ltd) was diluted to 10 wt% with ion-exchanged water and used for labeling experiments. 1-Methyl-3-nitro-1-nitrosoguanidine (Tokyo Chemical Industry Co., Ltd), methyl tert-butyl ether, and a 5 M NaOH solution (Kanto Chemical Co., Inc.) were purchased for the preparation of diazomethane. Tetrahydrofuran (THF) was obtained from Kanto Chemical Co.
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We confirmed that neither TPA nor NDC decomposed under the reaction conditions. In addition, the exchange of the 18O-labeled hydroxyl group of TPA and steam, and vice versa, was not observed when unlabeled TPA was exposed to 18O-labeled steam, because TPA underwent immediate sublimation and was carried beyond the heating zone. In contrast, a maximum of 5% exchange between the 18O-labeled hydroxyl group of NDC and steam, and vice versa, was observed under the conditions, caused by its higher sublimation temperature.
Both DMT and DMN were analyzed by GC-MS (Agilent Technologies; GC: HP6890; column: InertCap 5 MS/Sil; MS: HP5973, program: 50 °C (5 min) → 5 °C min−1 → 320 °C). The hydrolysis of the polyesters resulted in three mass peaks for each dimethyl dicarboxylate produced, corresponding to molecules containing two 16O isotopes, one 16O and one 18O isotope, or two 18O isotopes: m/z = 194, 196, and 198 for DMT and m/z = 244, 246, and 248 for DMN. For instance, Fig. 2 shows the MS spectra of the products obtained from pyrolysis and decomposition at a steam concentration of 50 vol%. The intensities of the peaks at m/z = 196, 198, 246, and 248 significantly increased in the presence of 18O-labeled steam.
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Fig. 2 MS spectra obtained from pyrolysis at a steam concentration of 50 vol% during the decomposition of (a) PET, (b) PBT, and (c) PEN. |
The selectivities for pyrolysis and hydrolysis to the steam decomposition of PET and PBT were calculated using eqn (2) and (4) and those of PEN were determined from eqn (3) and (4):
![]() | (2) |
![]() | (3) |
![]() | (4) |
The reacted conversion αr (αr = (W0 − W)/(W0 − Wf), where W0 [mg]: initial mass, W [mg]: actual mass, Wf [mg]: final mass) for each run was fitted to an integrated form of kinetic reaction models g(αr) taken from the solid-state reaction models37,39 summarized in Table 2 in our previous study.40 The theoretical αr vs. g(αr)/g(0.5) master plots of each model were compared with the experimental αr vs. t/t0.5 plot (reduced-time master plot), where t [min] is the actual time, and t0.5 [min] is a time of αr = 0.5, resulting in some possible models.41,42
The possible models selected by the reduced-time master plot method were further evaluated by the linearity rModel of t vs. g(α) plot based on the integrated form of eqn (5) under all conditions, where α is the conversion (α = 1 − W/W0). The reverse regression coefficient RModel [−] was calculated using eqn (6) for improving visualization, and then the three most probable reaction models were selected. The apparent reaction rate constant kapp [min−1] was determined from the slope of the t vs. g(α) plot, and the apparent activation energy Eapp [kJ mol−1] and pre-exponential factor k0 [min−1] were determined from the Arrhenius plot.
g(α) = kappt | (5) |
RModel = −log(1 − r2Model) | (6) |
In this study, for focusing on the chain scission stage, kinetic analysis was conducted in the range 0.2 ≤ α ≤ 0.6 for avoiding an unstable temperature range (α < 0.2) and carbonization range (α > 0.6) as much as possible.
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Fig. 3 Selectivities of pyrolysis and hydrolysis as well as monomer yields obtained from (a) PET, (b) PBT, and (c) PEN at different temperatures at a steam concentration of 75 vol%. |
On the other hand, hydrolysis selectivity during the degradation of PBT was significantly influenced by the reaction temperature: it decreased from 81% at 320 °C to 27% at 440 °C. PBT exhibited hydrolysis selectivity higher than that of PET. The higher selectivity is possibly attributed to the easier access of steam to the ester bonds of PBT because its chain is more flexible than those of PEN and PET. The TPA yield was not influenced by the reaction temperature, and an average yield of 70% was obtained. In addition, char deposition was not observed over the investigated temperature range. The lack of influence of the decomposition temperature on the TPA yield is attributed to the production of TPA via β-scission.27 Because of its longer diol unit, PBT can undergo β-scission at both ends of the diol to release TPA (Scheme 2(a)). During the scission of the ester bond, ethylene-glycol-based polyesters with short diol units form vinyl esters, which prevent the same reaction at the opposite side. The degradation of the vinyl ester results in the simultaneous decarboxylation of the carboxylic acid (Scheme 2(b) and (c)).
The selectivities for pyrolysis and hydrolysis during the decomposition of PEN were not affected by the reaction temperature, although the NDC yield decreased from 81% at 380 °C to 61% at 440 °C. Char was deposited on the reactor walls under all conditions, suggesting that PEN easily forms char by pyrolysis, caused by its rigid structure. In addition, the vapor pressure of NDC was significantly lower than that of TPA. Hence, NDC might stay on the PEN surface longer than TPA on PET and PBT, resulting in the formation of char caused by the suppression of the access of steam to PEN. However, the constant selectivities indicate that hydrolysis was also accelerated with increasing temperature. Hence, the rigid PEN structure possibly becomes more flexible with increasing temperature, enhancing access to the ester bonds by the steam.
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Fig. 4 Selectivities of pyrolysis and hydrolysis as well as monomer yield obtained from (a) PET, (b) PBT, and (c) PEN at different steam concentrations at 400 °C. |
Neither the selectivities nor the TPA yield was influenced by the steam concentration during the steam decomposition of PBT, resulting in an average of 36% for the hydrolysis selectivity for a TPA yield of 69%. The influence of the steam concentration on hydrolysis selectivity might be hindered by the strong contribution by pyrolysis at 400 °C; among these materials, PBT exhibited the lowest pyrolysis onset temperature (352 °C). However, the flexible polymer chain afforded hydrolysis selectivity higher than that observed for PET. The constant TPA yields are due to β-scission from both ends of the long diol unit, as explained in the previous section.
In the case of PEN, only 38% NDC was recovered under pyrolysis conditions, caused by the significant production of char on the sample holder wall. Both the NDC yield and hydrolysis selectivity increased to 19%, with an NDC yield of 62% at a steam concentration of 25 vol%. The hydrolysis selectivity and NDC yield of PEN were slightly higher than those of PET even if structural features would lead to the presumption that PET, as compared to the others, undergoes hydrolysis at a more rapid rate, suggesting that the high thermal stability of PEN prevented pyrolysis. Both hydrolysis selectivity and NDC yield changed only slightly at steam concentrations between 25 and 50 vol%, which is possibly attributed to the strong hydrophobicity of the naphthalene ring and the rigid structure of the PEN chain, preventing contact between the ester groups and steam.43 However, the hydrolysis selectivity and NDC yield increased to 29% and 74%, respectively, at a steam concentration of 75 vol%, which is possibly attributed to overcoming the negative impact (strong hydrophobicity) of the PEN structure by the high steam concentration. In addition, the possible enhancement in acid hydrolysis by the deposited NDC is not negligible, caused by the fact that the residence time of NDC is longer than that of TPA.44
Fig. 5 summarizes the conversion plots of PET obtained at different isothermal temperatures under pyrolysis and at a steam concentration of 75 vol%, as one of the examples of results. The decomposition of PET was enhanced with increasing temperature and steam concentration. The same tendency was observed for the decomposition of PBT and PEN. Based on these TG results, master plots for all models under all conditions were drawn and compared with the experimental plot. Fig. 6 summarizes the experimental and master plots for each reaction model obtained from the decomposition of PET at 351 °C at a steam concentration of 75 vol%. These master plots coincided with g(αr)/g(0.5) = 0 at αr = 0, and g(αr)/g(0.5) = 1 at αr = 0.5. If there is a significant difference between the experimental observation and the master plot of each model, the models can be excluded from possible models. In Fig. 6, all power-law models and diffusion models were apparently inadequate models. In addition, chemical reaction models, except for F1/3 (g(αr) = 1 − (1 − αr)2/3) and F3/4 (g(αr) = 1 − (1 − αr)1/4), and Avrami–Eroféev models, except for A3/2 (g(αr) = [−ln(1 − αr)]2/3) were not suitable.
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Fig. 5 Conversion plots of PET at different temperatures under (a) pyrolytic condition and (b) a steam concentration of 75 vol%. |
Thus, possible models are narrowed down to F1/3, F3/4, R2·F1/2 (g(αr) = 1 −(1 − αr)1/2), R3·F2/3 (g(αr) = 1 −(1 − αr)1/3), and A3/2. Possible models for other conditions and other polyesters were selected by the same procedure, and Table 1 summarizes these models. The possible models did not change for the most part regardless of steam concentration and material. In addition, the reaction order of all possible chemical reaction models was less than 1. This might be caused by the influence of the simultaneous occurrence of the sublimation of TPA and NDC with polymer decomposition as sublimation has been demonstrated to be a zero-order reaction.45,46
Steam conc. [vol%] | Possible modelsa | Three best-fitting models | RModel | Eapp [kJ mol−1] | log![]() |
|
---|---|---|---|---|---|---|
a Determined by the reduced-time master plot method. | ||||||
PET | 0 | F1/3, F3/4, F1, R2, F1/2, R3, F2/3 | F1, A1 | 3.9 | 190.7 | 13.6 |
F3/4 | 3.2 | 190.6 | 12.9 | |||
R3, F2/3 | 3.0 | 190.6 | 13.0 | |||
25 | F1/3, F3/4, R2, F1/2, R3, F2/3 | F3/4 | 3.8 | 183.3 | 12.5 | |
R3, F2/3 | 3.6 | 183.3 | 12.6 | |||
R2, F1/2 | 3.1 | 183.2 | 12.8 | |||
50 | F1/3, F3/4, R2, F1/2, R3, F2/3 | R3, F2/3 | 4.3 | 137.6 | 9.0 | |
R2, F1/2 | 4.2 | 137.5 | 9.1 | |||
F3/4 | 3.9 | 137.6 | 8.8 | |||
75 | F1/3, F3/4, R2, F1/2, R3, F2/3, A3/2 | R3, F2/3 | 4.5 | 139.9 | 9.2 | |
R2, F1/2 | 3.8 | 139.9 | 9.3 | |||
F3/4 | 3.7 | 140.0 | 9.1 | |||
PBT | 0 | F1/3, F3/4, R2, F1/2, R3, F2/3, A3/2 | A3/2 | 4.0 | 177.6 | 13.3 |
R2, F1/2 | 3.8 | 177.5 | 12.9 | |||
F1/3 | 3.7 | 177.6 | 13.0 | |||
25 | F1/3, F3/4, R2, F1/2, R3, F2/3, A3/2 | F1/3 | 3.5 | 155.3 | 11.4 | |
R3, F2/3 | 3.2 | 154.9 | 11.1 | |||
F3/4 | 3.1 | 154.8 | 11.0 | |||
50 | F1/3, F3/4, R2, F1/2, R3, F2/3, A3/2 | A3/2 | 3.6 | 151.7 | 11.4 | |
F1/3 | 3.3 | 151.7 | 11.1 | |||
R2, F1/2 | 3.1 | 151.8 | 11.0 | |||
75 | F1/3, F3/4, R2, F1/2, R3, F2/3, A3/2 | A3/2 | 3.1 | 156.2 | 11.8 | |
F1/3 | 3.1 | 156.2 | 11.6 | |||
R2, F1/2 | 2.7 | 156.0 | 11.5 | |||
PEN | 0 | F1/3, F3/4, R2, F1/2, R3, F2/3, A3/2, A2 | F3/4 | 3.4 | 206.5 | 13.9 |
R3, F2/3 | 3.3 | 207.7 | 14.1 | |||
R2, F1/2 | 3.1 | 210.1 | 14.4 | |||
25 | F1/3, F3/4, R2, F1/2, R3, F2/3, A3/2 | R3, F2/3 | 3.6 | 182.1 | 12.4 | |
F3/4 | 3.6 | 182.2 | 12.3 | |||
R2, F1/2 | 3.3 | 182.0 | 12.5 | |||
50 | F1/3, F3/4, R2, F1/2, R3, F2/3, A3/2 | R3, F2/3 | 3.7 | 175.7 | 11.9 | |
R2, F1/2 | 3.6 | 175.8 | 12.0 | |||
F3/4 | 3.5 | 175.7 | 11.8 | |||
75 | F1/3, F3/4, R2, F1/2, R3, F2/3, A3/2 | A3/2 | 3.7 | 161.1 | 11.3 | |
R2, F1/2 | 3.7 | 161.0 | 10.9 | |||
F1/3 | 3.5 | 161.1 | 11.0 |
The possible models were further evaluated by their linearity of the plot of rModel of t vs. g(α). Table 1 lists the reverse regression coefficient for model fitting, RModel, of the three most probable reaction models for each condition. The three best-fitting models were well fitted, resulting in at least RModel = 3.0 (rModel = 0.999). The experimental error of the equipment was calculated to approximately RModel = ±0.03, suggesting that the difference of RModel = 0.1 is possible for considering a range of error. However, as the values of RModel determined under the same condition were similar despite the presence and absence of experimental error, the order of the three best-fitting models might not be important. Therefore, the change in the distribution of the model with respect to the materials and steam concentration change was mainly discussed. The apparent activation energy, Eapp, and the pre-exponential factor, k0, for each model were determined by the Arrhenius plot, which are summarized in Table 1. The linearity of the Arrhenius plot was at least 0.99 for all three best-fitting models.
The best-fitting model for PET pyrolysis was the first-order chemical reaction model (F1, g(α) = −ln(1 − α)). The apparent activation energy and logk0 were determined to be 190.7 kJ mol−1 and 13.6, respectively. These values are consistent with Ea = 197 kJ mol−1 and log
k0 = 13.8 reported by Saha et al.,47 which were also determined by fitting the F1 model for isothermal experimental results. On the other hand, even though various Eapp and k0 values were reported from non-isothermal experiments, which are also assigned to the first-order reaction.47–50 The reaction model shifted to phase-boundary models with increasing steam concentration. The rate-determining step of the phase-boundary model is the contraction of the reaction phase boundary. Particularly, the R2 and R3 models represent the contracting cylinder and sphere, respectively. Both shapes were comparable with the shape of the PET melt in the cylindrical sample holder. Hence, it suggested that hydrolysis is limited to the sample surface. The Eapp and log
k0 values were dramatically reduced to 139.9 kJ mol−1 and 9.2 at a steam concentration of 75 vol%, respectively. These values are higher than those previously determined under solvolytic hydrolysis,33 because pyrolysis simultaneously occurred during steam decomposition. The reduction of Eapp from 0 to 25 vol% was comparably small, whereas at 50 vol%, the lowest Ea value was observed, and higher steam concentrations exhibited no additional effect. This also indicates that the reaction mainly occurs at the sample surface. Eapp decreased with increasing steam concentration until steam saturation occurred at the sample surface. The calculated log
k0 values were approximately proportional to Eapp, suggesting the high reliability of the selected models and calculated kinetic values.51,52
During the degradation of PBT, the Avrami–Eroféev models A3/2 (where the rate-determining step is nucleation) were predominant. An Avrami order of 3/2 implied that heterogeneous spherical nucleation is predominant.53–55 Furthermore, this observation might be caused by the lower thermal stability of PBT, resulting in the rapid evolution of gas, which led to the nucleation of gas bubbles in the polymer matrix. Moreover, the flexible structure of PBT might allow for the rapid diffusion of steam into the plastic; hence, the reaction is not limited to the sample surface. Eapp and logk0 were determined to 177.6 kJ mol−1 and 13.3 under pyrolytic conditions, respectively. These values are smaller than those of PET, caused by the weaker C–O bond between the butyl groups and carboxyl oxygen in PBT.56 These values are comparable with the published data.57–59 Eapp and log
k0 values decreased to 155.3 kJ mol−1 and 11.1 at steam concentration of 25 vol%, respectively; these values remained constant even at higher steam concentrations, which is consistent with the behavior of the hydrolysis selectivity discussed in Section 3.2. The current Eapp values are higher than those obtained under solvolytic hydrolysis (88 kJ mol−1).57 In addition, Eapp and k0 of PBT in the presence of steam were higher than those of PET, suggesting the strong influence of pyrolysis on steam decomposition.
The most probable model for PEN pyrolysis was F3/4, resulting in Eapp = 206.5 kJ mol−1 and logk0 = 13.9. These values are comparatively lower than those calculated from the non-isothermal method,60 which is similar to the tendency exhibited by PET. With the addition of steam, the reaction model shifted to the phase-boundary-controlled reaction models R2 and R3. The reaction of PEN resembles that of PET, with the reaction limited to the sample surface, caused by the rigid and hydrophobic PEN structure. Under pyrolytic conditions, Eapp decreased from 206.5 kJ mol−1 to 182.1 kJ mol−1 at a steam concentration of 25 vol%. Moreover, at a steam concentration of 50 vol%, Eapp slightly decreased to 175.7 kJ mol−1, while at a steam concentration of 75 vol%, it further decreased to 161.1 kJ mol−1. This behavior is consistent with the hydrolysis selectivity obtained in Section 3.1. These Eapp values are higher than those obtained under solvolytic hydrolysis (110–120 kJ mol−1),61 caused by the influence of pyrolysis. The higher Eapp for both pyrolysis and hydrolysis during the decomposition of PEN as compared to that of PET and PBT is attributed to the higher thermal stability of the PEN structure.
Common reaction models such as F1/3, F3/4, R2 (F1/2), and R3 (F2/3) were selected by the reduced-time master plot method under all conditions. In these models, F3/4 was the best-fitted (rModel > 0.99) common reaction model under all conditions. Thus, the kapp values of each material at each set of conditions were calculated using F3/4 and plotted in Fig. 7. As a side note, kapp values calculated using other possible models also exhibited the same behavior even though kapp values differed according to the selected model. Thus, we concluded that the F3/4 model is appropriate for discussing kapp behavior.
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Fig. 7 Apparent reaction constant kapp calculated using reaction model F3/4 at different steam concentrations: (a) PET, (b) PBT, and (c) PEN. |
It was assumed that kapp values estimated through the F3/4 model using data from reactions in the absence of steam were equivalent to the kapp of pyrolysis. The kapp of pyrolysis during the decomposition of PET increased at an accelerated pace along with the increase of reaction temperature (Fig. 7 (a)). kapp also increased when steam was added. This increment can be considered to correspond to hydrolysis; thus, the difference between the kapp of pyrolysis and the kapp of steam decomposition can be assumed to be the kapp of hydrolysis (assuming whole kapp = pyrolysis kapp + hydrolysis kapp). Fig. 8(a) plots the kapp of hydrolysis at 75 vol%. Interestingly, the hydrolysis rate did not significantly change in the investigated temperature range, suggesting that the hydrolysis rate is insensitive at these temperatures. Hence, this result reveals the presence of a crossing point at which the dominant reaction changes from hydrolysis to pyrolysis. The influence of the steam concentration on the hydrolysis rate is more obvious at lower temperatures as the influence of pyrolysis is comparatively weak. The behavior of both pyrolysis and hydrolysis rates observed in this section is well reflected in the selectivities for both processes obtained in Sections 3.1 and 3.2. The crossing-point temperatures observed in the 18O-labeling experiments and kinetic analyses were slightly different because steam contact efficiency was not identical for different instruments.
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Fig. 8 Pyrolysis and hydrolysis behavior of (a) PET, (b) PBT, and (c) PEN during the investigated temperature range at a steam concentration of 75 vol%. |
The behavior of the kapp of PBT was similar to that of PET, although the reaction rate was significantly higher, caused by the lower stability of PBT (Fig. 7(b)). The kapp of PBT pyrolysis was accelerated with increasing temperature, similar to PET. kapp was enhanced when steam was added, although it is unclear if there is any influence of steam concentration on the hydrolysis rate. The hydrolysis rate for PBT (Fig. 8(b)), similar to that for PET, was not sensitive to change in temperature. Hence, the dominant reaction changed from hydrolysis to pyrolysis with increasing reaction temperature. The selectivities obtained in Sections 3.1 and 3.2 are attributed to the changes in both pyrolysis and hydrolysis rates.
The kapp increase for pyrolysis during the decomposition of PEN was comparatively linear over the investigated temperature range (Fig. 7(c)). This might be caused by the high thermal stability of the PEN structure. On the other hand, the kapp of steam decomposition increased at an accelerated pace with increasing reaction temperature. Thus, both pyrolysis and hydrolysis rates were comparable through the investigated temperature range at a steam concentration of 75 vol% (Fig. 8(c)). The rigid PEN structure is expected to become flexible with increasing temperature, resulting in higher access of steam to the ester bonds. In addition, NDC might catalyze hydrolysis, caused by the fact that it exhibits vapor pressure lower than that of TPA. The pyrolysis and hydrolysis behavior correlated well with the selectivities obtained in Section 3.1. The enhancement of both rates results in constant selectivities for pyrolysis and hydrolysis with decreasing NDC. In addition, kapp did not exhibit any effect at steam concentrations between 25 and 50 vol%. However, kapp under a steam concentration of 75 vol% clearly increased. This behavior is consistent with the results obtained in section 3.2.
This study will be helpful toward the further improvement of the accuracy of the kinetic analyses of pyrolysis and hydrolysis and identification of the best conditions for the maximum process efficiency. Hydrolysis-predominant conditions are suitable for maximizing monomer yields, even with a lower reaction rate. In contrast, pyrolysis-predominant conditions enhance the complete reaction rate, which is suitable for reducing the reaction time. The results herein imply that these techniques can be applied for the evaluation of other transformations of polycondensation polymer, such as those of polycarbonates, polyamides, and polyimides.
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