versión impresa ISSN 0327-0793
Lat. Am. appl. res. vol.40 no.4 Bahía Blanca oct. 2010
Limit of applicability of the monomer-enhanced mechanism for radical generation in persulfate initiated mechanism for radical generationin persulfate initiated polymerization of acrylamide
I. Rintoul† and C. Wandrey‡
† Instituto de Desarrollo Tecnológico para la Industria Química, Universidad Nacional del Litoral - Consejo Nacional de Investigaciones Científicas y Técnicas. Santa Fe, Argentina.
‡ Laboratoire de Médecine Régénérative et de Pharmacobiologie, Ecole Polytechnique Fédérale de Lausanne.
Abstract The limit of applicability of the monomer-enhanced mechanism as dominant mechanism ruling the initiation process of the polymerization of acrylamide (AM) initiated with potassium persulfate (K2S2O8) has been determined. The kinetics and mechanisms for radical generation were studied in solution at very low monomer and initiator concentrations. The transition of the initiation mechanism from dominant monomer-enhanced dissociation to dominant thermal decomposition of persulfate was observed. Both mechanisms contribute equally to radical generation at [AM] / [K2S2O8] ≈ 4.5. Thermal decomposition dominates at lower [AM] or higher [K2S2O8] and opposite variations promote the monomer-enhanced dissociation. This work also includes quantification of the rate coefficients, efficiencies and activation energies of the mentioned mechanisms, and the kinetics of AM polymerization when photochemically initiated with phenylbis(2,4,6-trimethylbenzoyl)-phosphine oxide.
Keywords Kinetics. Mechanism. Initiation. Acrylamide. Persulfate.
Polyacrylamide based products are commonly used as flocculants, thickening agents, additives in water-based paints and a multitude of other applications related to solid liquid separation, fluid control and surface modification (Myagchenkov and Kurenkov, 1991). Recently, they found applications in building and food industry, cosmetics, medicine and pharmacy (Dautzenberg et al., 1994; Hunkeler and Hernandez-Barajas, 1997).
Usually, polyacrylamides are synthesized through free radical polymerization of acrylamide (AM) in homogeneous or heterogeneous media using thermal, redox or photochemical initiators (Siyam, 2001; Kurenkov and Abramova, 1992). A widely used thermal initiator is potassium persulfate (K2S2O8). Important deviations from the ideal polymerization path have been observed for the polymerization of AM initiated with K2S2O8.
The literature describing the system AM/K2S2O8 is abundant. Though, frequently only experimental observations are presented without discussing or proposing neither mechanisms nor their ranges of applicability. Moreover, the majority of the literature investigated the system under conditions of industrial interests such as heterophase polymerization carried out at high monomer concentration, high polymerization rate and high conversion. These conditions are, definitely, far from those suited for the accurate identification of basic mechanisms, applicability ranges and kinetic parameters. Table 1 summarizes the values of α and β published by several authors along more than 50 years.
Table 1. Conditions, monomer and initiator exponents for AM polymerizations initiated with K2S2O8.
These parameters are the dependency orders of [AM] and [K2S2O8], respectively in the overall polymerization rate equation. (Odian, 1970):
The overall polymerization rate (Rp) is defined as the negative derivative of the monomer concentration with time: -d[M]/dt, [M] and [I] are the monomer and initiator concentrations (mol l-1), kp, ki, kt and fi are the rate coefficients for propagation (l mol-1 s-1), initiation (s-1), termination (l mol-1 s-1) and the dimensionless efficiency for radical generation. The temperature dependence of the rate coefficients can be expressed by an Arrhenius type relationship: k = A e(-E/RT). Here, A and E are the collision frequency factor (s-1) and the Arrhenius activation energy (KJ mol-1). In case of photopolymerization, fi is usually called the quantum yield of the initiator, Φ. Then, ki has to be expressed as the product of the molar absorptivity of the initiator, ε, (l mol cm-1) and the light intensity, I0 (mol l-1 s-1).
With the exception of Mahdavian et al. (2004), Stupenkova et al. (1991) and Kurenkov et al. (1978), β was reported as the ideal value: 0.5 whereas α varies from its approximately ideal value: 1.07 (Riggs and Rodriguez, 1967a) to a highly deviated value: 1.70 (Kurenkov et al., 1978).
The effect of AM on S2O8-2 during the radical generation process is considered to be responsible for α > 1. On the one hand, the cage-effect theory (Matheson, 1945) proposes that S2O8-2 undergoes decomposition immediately followed by recombination. Primary radicals remain trapped in a cage formed by solvent and monomer molecules. Accidentally, a primary radical reacts with a cage forming monomer yielding the radical outside of the cage. The higher the monomer concentration, the higher is the concentration of cage forming monomer molecules. Consequently, the higher the probability is for a radical to escape and initiate polymerization. On the other hand, the complex theory (Gee and Rideal, 1936) proposes the formation of a reversible associated complex between AM and S2O8-2 prior its dissociation in a primary radical, SO4-·, and an initial radical, SO4--AM·. In this case, the higher the monomer concentration, the more AM-S2O8-2 complex is formed and the higher is the production of free radicals. Although both theories are based on very different premises, they lead to an identical kinetic expression, which is generally referred as monomer-enhanced dissociation mechanism. The mechanism predicts α=1.5 and β=0.5.
In addition, thermal decomposition of the initiator also contributes to radical generation. Thus, the initiation process has to be considered as a result of two competing effects; thermal decomposition and monomer-enhanced dissociation of the initiator. This type of initiation process is usually called as hybrid mechanism (Hunkeler, 1991). The competing mechanisms are visible in Eq. (2).
Here, kd, ka, fd and fa are the rate coefficients for thermal decomposition of S2O8-2 (s-1), the association coefficient of the AM-K2S2O8 complex (s-1), and the dimensionless efficiencies for radical generation through thermal decomposition of S2O8-2 and AM-K2S2O8 dissociation, respectively. fa = 1 has been mechanistically demonstrated and reported for a number of situations (Manickam et al., 1979).
The hybrid mechanism predicts 1 ≤ α ≤ 1.5 Furthermore, it describes satisfactorily the kinetics of the polymerization of AM in emulsion, at very high monomer concentrations, [AM] = 6.7 mol l-1 and low initiator concentration, [K2S2O8] = 1.573 10-3 mol l-1 (Hunkeler, 1991). The extremely high monomer concentration and high monomer / initiator ratio ensures the hybrid mechanism to be governed by energetic factors since the probability that monomer and initiator approach is very high. However, as to the authors' knowledge, there is no evidence of the validity of the hybrid mechanism at very low monomer concentration and low monomer / initiator ratio. Under such conditions, frequency and energetic effects may become competitive and thus the system is expected to shift from non-ideal to ideal behavior. Actually, the polymerization of acrylic and methacrylic acids (Chapiro and Dulieu, 1977; Chapiro, 1973) which present significant deviations at high monomer concentrations, tend to "ideality" with the decrease of monomer concentration.
It is worth mentioning that some authors have explained the deviation of α from its ideal value assuming that the presence of AM could influence medium properties (Seabrook et al., 2005) such as pH (Cabaness et al., 1971; Currie et al., 1965; Pascal et al., 1990), solvent quality (Gromov et al., 1980) and ionic strength of the polymerization medium (Pascal et al., 1993) causing variations in kp. Later, the variation of kp were experimentally interpreted as a deviation of α. The effects were also explained by electrostatic interactions between monomers and terminal units of growing radicals, protonation of AM at low pH and hydrolysis of the amide group at high pH (Pascal et al., 1993). Changes in the flexibility, configuration, mobility and reactivity of growing radicals, changes in the nature of solvation shells and complex formation between the reacting species and solvent molecules were proposed (Pascal et al., 1993). Finally, favorable molecular orientation, high local monomer concentration in the proximity of the radical centre and dimerization of AM by H-bond formation were suggested (Gromov et al., 1980; Pascal et al., 1993). The experimental conditions of this study were selected in such a way that these effects resulted minimized or even avoided. Thus, exclusively information about the initiation mechanism should become significant.
The goal of the present study is to establish the limit or range of applicability of the hybrid mechanism for the polymerization of AM in solution initiated with K2S2O8.
White crystals of ultra pure AM, four times recrystallized purchased form Axon Lab, Switzerland, K2S2O8 puriss. > 99%, purchased from Fluka Chemie, Switzerland and an aqueous dispersion of phenylbis(2,4,6-trimethylbenzoyl)-phosphine oxide (C26H27O3P) purchased from Ciba Specialty Chemicals, Switzerland were selected as monomer, thermal and photochemical initiators respectively. ε and Φ of C26H27O3P were reported as 7900 l mol cm-1 and 0.40, respectively in a previous work (Rintoul and Wandrey, 2007). The water had Millipore quality (18.2 MOhm cm-1) and HPLC grade acetonitrile purchased from Axon Lab, Switzerland was used to precipitate the polymer in the withdrawn samples.
B. Polymer Synthesis
Syntheses were performed in a 100 ml glass reactor equipped with a stirrer, condenser, gas inlet and a heating/cooling jacket. A thermostat adjusted the reaction temperature within 1 ºK. Oxygen was removed from the initial monomer solution prior to the polymerization by purging with high purity N2 (O2 < 2 ppm) purchased from AirLiquide, Switzerland, during 30 min at 273 ºK. Afterwards, the temperature was increased to activate the thermal decomposition of K2S2O8 and to initiate the polymerizations. The reactions were performed isothermally. An UV lamp was immersed in the reactor to carry out photopolymerizations. The lamp had a primary out put at 254 nm and 540 erg s-1 cm-2 of intensity at the surface of the lamp (I0 = 5.16 10-8 mol l-1 s-1). Samples of 0.1 - 0.2 g were withdrawn each 5 min during 20 ± 5 s during the first hour of reaction to obtain highly reliable curves. The polymerizations were allowed to progress up to 2 hours of reaction time. A final sample was analyzed to get information about the limiting conversion.
C. Experimental Conditions
The effects related to pH, temperature, and solvents hypothesized by some authors as responsible for the non-ideal behavior of the AM/K2S2O8 system were minimized or avoided by preparing aqueous monomer solutions at pH = 4 to ensure electrochemical neutrality of AM and growing radicals (Cabaness et al., 1971; Currie et al., 1965; Pascal et al., 1990) and polymerizing between 303 - 323 ºK to expect the absence of H-bond effects (Gromov et al., 1980; Pascal et al., 1993; Rintoul and Wandrey, 2007). Solvent effects and ionic strength are not considered by using pure water and highly diluted monomer and initiator solutions.
The first series of experiments were performed in order to prove that thermal decomposition of K2S2O8 (series 1a) and C26H27O3P (series 1b) were insignificant during the degassing process. In series 1a, an AM/K2S2O8 solution was maintained at the degassing temperature (273 ºK) during 60 min under permanent N2 flow. In series 1b, an AM/C26H27O3P solution was maintained 60 min at 313 ºK, under permanent N2 flow without lighting the UV lamp. Furthermore, the possibility of monomer photolysis was evaluated (series 1c). Here, an initiator-free AM solution was illuminated with UV light during 380 min. Samples were withdrawn from the reactor to measure the monomer concentration and to determine if polymerization occurred. Series 1d served to ensure experimental reproducibility. Here, the same polymerization was repeated three times.
Series 2, 3 and 4 constitute the most important ex-periments to identify the effect of [AM] on Rp. For this purpose photo and thermal polymerizations of AM at different monomer concentrations and initiation mechanisms were performed. Series 5, served to obtain information about the influence of [K2S2O8] on the Rp. The effect of temperature was studied in series 6. Table 2 lists the conditions of all experiments performed.
Table 2. Summary of experimental conditions.
Series 1a-c: Exclusion of side effects; Series 1d: Experimental reproducibility; Series 2-4: Influence of monomer concentration; Series 5: Influence of initiator concentration; Series 6: Influence of temperature.
D. Determination of Residual Monomer Concentrations and Polymerization Rates
The residual monomer concentration of withdrawn samples served for determining the conversion (P) and for calculating Rp according to a detailed procedure (Rintoul and Wandrey, 2005). Most of conversion curves presented linearity (R2 > 0.99) until, at least, 20 min of reaction time. However, the best fitting was achieved by exponential decay regressions (always presenting R2 > 0.999). Then, Rp at the early stages of polymerization were calculated as the negative derivative of the exponential decay regressions of residual monomer concentration vs. reaction time plots. Limiting conversion values (P∞) were approached at 2 hours of reaction time.
The residual monomer concentration was determined using a HPLC system composed of L-7110 Merk-Hitachi pump (Hitachi, Japan) and SP6 Gynkotek UV detector (Gynkotec, Germany) operating at a wavelength of 197 nm. The stationary and mobile phases were LiChrosphere 100 RP-18 from Merk, Germany and 5 wt% acetonitrile aqueous solution with a flow rate of 1 ml min-1. The samples were first mixed with 4 ml of acetonitrile to precipitate and isolate the polymer from the solution. The residual monomer remains in solution. Subsequently, 20 μl of the supernatant were injected into the HPLC for analysis. The HPLC system was calibrated using AM standard solutions in the concentration range of 7 10-4 to 7 10-3 mol l-1. The standard solutions were prepared by sequential dilutions of 1 mol l-1 stock solution of AM. The peak area served as calibration parameter. Figure 1 shows a typical calibration curve.
Figure 1. HPLC calibration curve for AM at room temperature (298 ºK). Linear regression: Peak area = 0.158 [AM] + 0.117. R2 = 0.9991.
A. Prerequisites, Reproducibility and Residual Monomer Concentration versus Time Plots
No polymerization was evidenced for series 1a-c. Contrarily, the three polymerizations of series 1d progressed near by linearly (R2 > 0.99) until approximately 30 min of reaction. A short induction time was present for some polymerizations as those presented exemplary in Fig. 2. Induction times were not taken into account for Rp calculations. Differences of less than 5.5% were found between the residual monomer concentrations at the corresponding time values. Furthermore, the slope -d[AM]/dt values presented differences of less than 3% demonstrating good experimental reproducibility.
Figure 2. Experimental reproducibility. [AM] = 0.2 mol l-1; [K2S2O8] = 3.2 10-3 mol l-1; T = 313 ºK. Rp = 2.33 10-5 (); 2.40 10-5 (); 2.29 10-5 ( ) mol l-1 s-1.
It was observed that Rp increases with the monomer concentration (series 2-4), initiator concentration (series 5) and temperature (series 6). The Rp of series 2 to 6 were calculated and plotted vs. the reaction parameter under study in Figs. 3 to 5.
Figure 3. Rp vs. [AM] for photochemically (series 2) and thermally initiated (series 3 and 4) polymerizations. [C26H27O3P] = 10-6 mol l-1 (); [K2S2O8] = 1.6 10-3 mol l-1 () and 3.2 10-2 mol l-1 (); T = 313 ºK.
Figure 4. Rp vs. [K2S2O8] (series 5). [AM] = 0.2 mol l-1; T = 313 ºK.
Figure 5. Ln(kd) () and ln(Rp) () vs. T-1 plots. [AM] = 0.2 mol l-1; [K2S2O8] = 3.2 10-2 mol l-1.
B. The Monomer Exponent
The logarithmic plots of Rp vs. [AM] for series 2 to 4 are presented in Fig. 3 according to: log (Rp) = α [AM] + b. The slopes of the linear regressions (R2 > 0.99) directly yield α which was obtained as 1.00, 1.34 and 1.33 for series 2, 3, and 4 and the intercept values, b, were obtained as -3.13, -3.61 and -3.77, respectively.
C. The kp/kt1/2 Ratio
The ideal value, α = 1, obtained for series 2 permitted to express Rp as a function of the batch composition ac cording to Eq. (1) adapted to the photopolymerizationcase where the photoinitiator does not suffer of mono-mer-enhanced dissociation. From this equation the intercept of the linear regression, b = -3.13, of series 2 can be expressed as:
The kp/kt1/2 ratio was calculated as 58 after introducing the values for b, Φ, ε, I0 and [C26H27O3P] into Eq. (3). Propagation and termination steps are considered as independent of the initiation step. Therefore, the kp/kt1/2 ratio obtained for photochemically initiated polymerizations may be valid for polymerizations using K2S2O8 as initiator.
D. The Thermal Decomposition Rate Coefficient
The dead-end polymerization technique (Tobolsky et al., 1960; Bohme and Tobolsky, 1966; Gobran et al., 1960) was used to calculate kd. The technique can be expressed as Eq. (4) where P and P∞ are the actual and limiting conversion values.
The value of kd was obtained as the slope when the left side of Eq. (4) was plotted vs. the reaction time. The experimentally obtained P∞ and the calculated kd values for series 3 to 6 are presented in Table 3.
Table 3. Limiting conversion (P∞) and dissociation constant of K2S2O8 (kd).
E. The AM-K2S2O8 Association Constant and The Efficiency for Thermal Decomposition
ka and fd were calculated employing Eq. (5). Equation (5) was obtained rearranging Eq. (2). The left side was calculated introducing the corresponding values of Rp, kp/kt1/2, [AM] and [K2S2O8]. Subsequently, it was plotted against [AM] and fitted with a linear regression. ka and fd resulted from the slope and intercept of the linear regression. Here, it was assumed fa = 1 as previously demonstrated by Hunkeler (1991) and Pascal et al., (1990).
Results from series 3 yielded fd = 3.7 10-4 and ka = 1.16 10-6 l mol-1 s-1 and for series 4 it was fd = 4.8 10-4 and ka = 1.04 10-6 l mol-1 s-1.
F. The Initiator Exponent
The logarithmic plot of Rp vs. [K2S2O8] is presented in Fig. 4. β= 0.38 for K2S2O8 was obtained as the slope of the linear regression (R2 > 0.99).
G. The Arrhenius Parameters
The values for the overall frequency factor, Ap = 1.56 106 s-1, overall activation energy, Ep = 53.77 KJ mol-1, the initiator decomposition frequency factor, Ad = 4.42109 s-1 and the activation energy for the thermal decom-position of K2S2O8, Ed = 78.62 KJ mol-1 were determined according the Arrhenius equation. The natural logarithms of Rp and kd obtained for series 6 were plotted vs. T-1 as presented in Fig. 5.
H. Thermal Decomposition vs. Monomer Enhanced Dissociation Analysis
Finally, the rates of radical generation by thermal decomposition and monomer-enhanced dissociation processes as function of monomer and initiator concentrations are presented in Fig. 6. The rate of radical generation due thermal decomposition and monomer-enhanced dissociation were calculated according to Eq. (2):
fd kd [K2S2O8] and fa ka [K2S2O8] [AM], respectively.
Figure 6. Rate of radical generation by thermal decomposition of K2S2O8 (circles) and monomer-enhanced dissociation of AM-K2S2O8 complex (squares) vs. [AM]. [K2S2O8] = 3.7 10-2 mol l-1 (full symbols) and 1.6 10-3 mol l-1 (empty symbols), T = 313 ºK.
Figure 6 shows that the contribution of radicals yielded to the reaction medium via thermal decomposition slightly decreases with the increment of the [AM]. Contrary, the contribution due to monomer-enhanced dissociation clearly increases with [AM]. Moreover, the radical contribution corresponding to thermal decomposition and monomer-enhanced dissociation mechanisms crossover at [AM] = 0.17 mol l-1 and 0.12 mol l-1 when polymerizations were carried out at [AM]/[K2S2O8] within the range 31-187 and 1.56-9.38, respectively.
A. Comparison Between Own Results and Literature Data
Table 4 presents own results and literature data. In the present contribution, the maximum monomer / initiator ratio is 187. Only, Mahdavian et al. (2004), Singh et al. (1979), Osmanov et al. (1980) and possibly Morgan (1946) with maximum monomer / initiator ratios about 140, 30, 180 and 320, respectively can be considered within the range used in the present contribution. However, the other reaction conditions and the subjects of the papers were not the same as those applied here. Mahdavian et al. (2004) studied the rate coefficients at high conversion, Singh et al. (1979) investigated the influence of Ag+ and Cu++ ions on the polymerization rate of AM, Osmanov et al. (1980) determined the kp/kt1/2 ratio and the very old article of Morgan (1946) is related to the influence of pH and AgNO3 on persulfate decomposition. Therefore, the comparison between own and literature data is relative since little is known about the system under low monomer / initiator ratio. However, the comparison may be useful to have an idea of magnitude orders and general perspective of the system.
Table 4. Comparison between own and literature parameters.
In general good agreement between the obtained kp/kt1/2 ratio, the frequency factor Ad and the activation energy Ed for the thermal decomposition of K2S2O8 and those from the literature was observed. The obtained kp/kt1/2 ratio, was slightly higher than that reported in the literature (Currie et al., 1965; Rintoul and Wandrey, 2007; Seabrook et al., 2005). The reason could be the extremely low monomer concentration used in the present study. In fact, kp was found to increase from 3.83 104 to 5.53 104 when the [AM] decreased from 2.81 to 0.32 mol l-1 (Seabrook et al., 2005). Therefore higher kp, and consequently higher kp/kt1/2, can be expected at [AM] < 0.3 mol l-1.
fd resulted one order of magnitude lower than the values found by Baer et al. (1972) and Hussain and Gupta (1977). However, very low initiator efficiencies were observed for persufate-based initiators due to the formation of cage products. Furthermore, an additional decrease in the initiator efficiency is expected when the [AM]/[K2S2O8] ratio decreases due to higher probability for radical transfer to the initiator, which also results in initiator wastage. In fact, the decrease of the initiator efficiency with the increase of the initiator concentration may be the cause for the apparent non-ideal initiator exponent, β = 0.38.
ka resulted 2 times higher than ka = 5.28 10-7 l mol-1 s-1 obtained by Hunkeler (1991). Such a difference may be due to the very low monomer/initiator ratio used here compared to Hunkeler's work. The overall frequency factor, Ap, resulted within the range proposed by Riggs and Rodriguez, (1967b) and the activation energy, Ep, agreed well with the values found by Lin, (2001).
The reaction order of [AM] for polymerizations initiated with K2S2O8 deviated significantly from unity (α = 1.34 and 1.33). Such deviation is coincident with the results presented in Table 1 and specially those obtained by Hunkeler (1991) and Kurenkov et al. (1987) with α = 1.34 and 1.37, respectively.
B. The Hybrid Mechanism at Low Monomer Concentration
β deviated significantly from its ideal value in case of initiation with K2S2O8 while it reverted to ideality in case of initiation with C26H27O3P which certainly does not interact with AM during the photochemical dissociation process. Therefore, the deviation of β was evidently caused by monomeric influences on the rate of initiation. It suggests that the monomer participates actively in the initiator decomposition process. This effect may contribute to the support of the hybrid mechanism for persulfate-initiated AM polymerizations even at such low monomer concentration unlike the cited condition suggest ideal behavior.
Comparing the values obtained for kd = 3.8 10-4 and ka = 1.16 10-6 l mol-1 s-1 presented in Tables 3 and 4 it is clear that thermal decomposition of K2S2O8 occurs a hundred times faster than the dissociation of the AM-K2S2O8 complex. However, the very low efficiency of K2S2O8, fd = 3.7 10-4, decreases substantially the contribution of thermally generated radicals to the initiation of polymerization. Thus, both initiation mechanisms become competitive. The radical generation via monomer-enhanced dissociation of the initiator yields two free radicals, a free primary radical and a radical, that has already add the first monomer unit. Thus, the radicals do not form cage products justifying fa = 1 (Manickam et al., 1979).
The crossover for the thermal and monomer-enhanced contributions for radical generation shown in Fig. 6 shifted to lower [AM] when the [AM]/[K2S2O8] ratio was increased. This effect may indicate that polymerizations carried out at very high [AM]/[K2S2O8] such as those performed industrially are dominated by the monomer-enhanced mechanism. Moreover, under industrial conditions, it is usual to find more than 104 monomers per each initiator molecule, thus the probability of formation of monomer-initiator associates is very high. Contrary, the probability of finding a non-associated initiator molecule able to undergo thermal decomposition would be very low. Only at very low monomer and initiator concentrations the radical contribution due to thermal dissociation is higher than the contribution due to monomer-enhanced decomposition. This effect demonstrates that AM and K2S2O8 tend to associate and therefore, only at highly diluted systems they may occur as single molecules.
The hybrid mechanism describes satisfactorily the kinetics of the polymerization of AM initiated with K2S2O8 at very low monomer concentrations. Taking into account other studies carried out at higher monomer concentrations, it can be concluded that the hybrid mechanism rules the polymerization in the range of AM concentrations from 0.05 mol l-1 until its solubility limit.
The formation of a persulfate-AM complex is suggested as explanation for the deviations from the ideal monomer exponent found in persulfate-initiated polymerizations of AM. The kinetics of dissociation and subsequent release of radicals to the polymerization medium of such complex is slower than the corresponding kinetics for thermal decomposition and radical release of non-associated persulfate. However, it occurs with much higher efficiency. Therefore, the overall initiation rate is the result of both, thermal decomposition and monomer-enhanced dissociation processes supporting the idea of the hybrid mechanism.
The rate of radical generation by thermal decomposition and monomer-enhanced dissociation contribute equally to the initiation of polymerization when [AM] / [K2S2O8] ≈ 4.5 for polymerizations carried out at 313 K. At [AM] = 0.05 mol l-1 thermal decomposition dominates since about 80% of the radicals are generated by thermal decomposition. Contrary, 54% of the radicals are generated by monomer-enhanced dissociation at [AM] = 0.3 mol l-1. It lets expects the initiation process of polymerizations at very high [AM] / [K2S2O8] such as those performed under industrial conditions to be ruled mainly by the kinetics of the monomer-enhanced mechanism.
The authors thank the Swiss National Science Foundation (grants 2000-63395 and 200020-100250), the Universidad Nacional del Litoral and Consejo Nacional de Investigaciones Científicas y Técnicas for the financial support.
1. Baer, M., J.A. Caskey and A. Fricke, "A kinetic study of acrylamide polymerization initiated by 4.4'-azo-bis-4-cyanopentanoic acid in aqueous solution," Makromol. Chem., 158, 27-37 (1972). [ Links ]
2. Bohme R.D. and A.V. Tobolsky, Encyclopedia of Polymer Science and Technology., John Wiley & Sons, New York (1966). [ Links ]
3. Cabaness, W.R., T. Yen-Chin Lin and C. Parkanyi, "Effect of pH on the reactivity ratios in the copolymerization of acrylic acid and acrylamide," J. Polym. Sci. Part A-1, 9, 2155-2170 (1971). [ Links ]
4. Chapiro, A., "Polymerization and copolymerization in associated monomer aggregates," Eur. Polym. J., 9, 417-427 (1973). [ Links ]
5. Chapiro, A. and J. Dulieu, "Influence of solvents on the molecular association and on the radiation initiated polymerization of acrylic acid," Eur. Polym. J., 13, 563-577 (1977). [ Links ]
6. Chiriac, A.P. and C.I. Simionescu, "Magnetic field polymerization," Prog. Polym. Sci., 25, 219-258 (2000). [ Links ]
7. Currie, D.J., F.S. Daiton and W.S. Watt, "The effect of pH on the polymerization of acrylamide in water," Polymer, 6, 451-453 (1965). [ Links ]
8. Dautzenberg, H., W. Jaeger, J. Kötz, B. Philipp, C. Seidel and D. Stscherbina, Polyelectrolytes formation, Characterization and Application, Verlag, Munich (1994). [ Links ]
9. Friend, J.P. and A.E. Alexander, "Effect of surfactants on the polymerization of acrylamide in aqueous solutions," J. Polym. Sci. Part A-1, 6, 1833-1839 (1968). [ Links ]
10. Geczy, I. and H.I. Nasr, "Polymerization of acrylamide with the redox system K2S2O8-ascorbic acid in aqueous solution at room temperature," Acta Chim. Acad. Sci. Hungaricae, 70, 319-327 (1971). [ Links ]
11. Gee, G. and E.K. Rideal, "The kinetics of polymerisation processes. Part III. The effects of catalysts and inhibitors," Trans. Farad. Soc., 32, 666-674 (1936). [ Links ]
12. Giz, A., H. Catalgil-Giz, A. Alb, J.L. Brousseau and W.F. Reed, "Kinetics and mechanisms of acrylamide polymerization from absolute online monitoring of polymerization reaction," Macromolecules, 34, 1180-1191 (2001). [ Links ]
13. Gobran, R.H., M.B. Berenbaum and A.V. Tobolsky, "Bulk polymerization of isoprene: kinetic constant from the dead-end theory," J. Polym. Sci., 46, 431-440 (1960). [ Links ]
14. Gromov, V.F., N.I. Galperina, T.O. Osmanov, P.M. Khomikovski and A.D. Abkin, "Effect of solvent on chain propagation and termination reaction rates in radical polymerization," Eur. Polym. J., 16, 529-535 (1980). [ Links ]
15. Hunkeler, D., "Mechanism and kinetics of the persulfate-initiated polymerization of acrylamide," Macromolecules, 24, 2160-2171 (1991). [ Links ]
16. Hunkeler, D., and J. Hernandez-Barajas, Handbook of thermoplastics, Marcel Dekker, New York (1997). [ Links ]
17. Hussain, M.M. and A. Gupta, "Kinetics of aqueous polymerization of acrylamide initiated by ceric ammonium sulfate/2-mercaptoethanol redox system," J. Macromol. Sci. Part A: Chem., 11, 2177-2187 (1977). [ Links ]
18. Kang, S.C., Y.J. Choi, H.Z. Kim, J.B. Kyong and D.K. Kim, "Kinetics of Acrylamide Solution Polymerization Using Potassium Persulfate as an Initiator by in situ IR," Macromol. Res., 12, 107-107 (2004). [ Links ]
19. Kurenkov, V.F., T.M. Osipova, E.V. Kuznetsov and V.A. Myagchenkov, "Polymerization of acrylamide using potassium persulfate as initiator," Vysokomol. Soedin. Seriya B, 20, 647-650 (1978). [ Links ]
20. Kurenkov, V.F., T.A. Baiburdov and L.L. Stupenkova, "Adiabatic polymerization of acrylamide in aqueous solutions initiated by the system K2S2O8Na2S2O5," Polym. Sci. USSR, 29, 388-392 (1987). [ Links ]
21. Kurenkov, V.F. and L.I. Abramova, "Homogeneous polymerization of acrylamide in solutions," Polym. Plast. Tech. Eng., 31, 659-704 (1992). [ Links ]
22. Kurenkov, V.F. and O.A. Antonovich, "Radical polymerization of acrylamide in aqueous-dimethyl sulfoxide solutions in the presence of sodium acetate," Russian J. Appl. Chem., 76, 280-283 (2003). [ Links ]
23. Lin, H.R., "Solution polymerization of acrylamide using potassium persulfate as an initiator: kinetic studies, temperature and pH dependence," Eur. Polym. J., 37, 1507-1510 (2001). [ Links ]
24. Mahdavian, A.R., M. Abdollahi and H.R. Bijanzadeh, "Kinetic study of radical polymerization. III. Solution polymerization of acrylamide by 1H-NMR," J. Appl. Polym. Sci., 93, 2007-2013 (2004). [ Links ]
25. Manickam, S.P., K. Venkatarao and N.R. Subbaratnam, "Peroxo salts as initiators of vinyl polymerization-2," Eur. Polym. J., 15, 483-487 (1979). [ Links ]
26. Matheson, M.S., "Chain initiation in catalyzed polymerization," J. Chem. Phys., 13, 584-585 (1945). [ Links ]
27. Morgan, L.B., "Transient molecular species occurring in persulfate oxidations," Trans. Farad. Soc., 42, 169-183 (1946). [ Links ]
28. Myagchenkov, V.A. and V.F. Kurenkov, "Applications of acrylamide polymers and copolymers: a review," Polym. Plast. Tech. Eng., 30, 109-135 (1991). [ Links ]
29. Odian, G., Principles of polymerization, McGraw-Hill, New York (1970). [ Links ]
30. Osmanov, T.O., V.F. Gromov, P.M. Komikovsky and A.D. Abkin, "Solution polymerization of acrylamide in the presence of Lewis acids," Polym. Sci. USSR, 22, 739-748 (1980). [ Links ]
31. Pascal, P., D.H. Napper, R.G. Gilbert, M.C. Piton and M.A. Winnik, "Pulsed laser study of the propagation kinetics of acrylamide and methacrylamide in water," Macromolecules, 23, 5161-5163 (1990). [ Links ]
32. Pascal, P., M.A. Winnik, D.H. Napper and R.G. Gilbert, "Pulsed laser study of the propagation kinetics of acrylamide and its derivatives in water," Macromolecules, 26, 4572-4576 (1993). [ Links ]
33. Pohl, K. and F. Rodríguez, "Adiabatic polymerization of acrylamide using a persulfate-bisulfite redox couple," J. Appl. Polym. Sci., 26, 611-618 (1981). [ Links ]
34. Rasmussen, J.K., S.M. Heilmann, P.E. Toren, A.V. Pocius and T.A. Kotnour, "Kinetics and mechanism of the interaction of potassium peroxydisulfate and 18-crown-6 in aqueous media," J. Am. Chem. Soc., 105, 6845-6849 (1983). [ Links ]
35. Riggs, J.P. and F. Rodriguez, "Polymerization of acrylamide initiated by the persulfate-thiosulfate redox couple," J. Polym. Sci. Part A-1, 5, 3167-3181 (1967a). [ Links ]
36. Riggs, J.P. and F. Rodriguez, "Persulfate-initiated polymerization of acrylamide," J. Polym. Sci. Part A-1, 5, 3151-3165 (1967b). [ Links ]
37. Rintoul, I. and C. Wandrey, "Polymerization of ionic monomers in polar solvents: kinetics and mechanism of the free radical copolymerization of acrylamide/acrylic acid," Polymer, 46, 4525-4532 (2005). [ Links ]
38. Rintoul, I. and C. Wandrey, "Magnetic field effects on the free radical solution polymerization of acrylamide," Polymer, 48, 1903-1914 (2007). [ Links ]
39. Seabrook, S.A., M.P. Tonge and R.G. Gilbert, "Pulsed laser polymerization study of the propagation kinetics of acrylamide in water," J. Polym. Sci. Part A: Polym. Chem., 43, 1357-1368 (2005). [ Links ]
40. Singh, U.C., S.P. Manickam and K. Venkatarao, "Koperverteilung und ausscheidungsverhalten von monomerem und polymerem sulfadiazinacrylamid," Makromol. Chem., 180, 595-602 (1979). [ Links ]
41. Siyam, T., "Development of acrylamide polymers for the treatment of waste water" Des. Monom. Polym., 4, 107-168 (2001). [ Links ]
42. Stearn, A.E., E.M. Irish and H. Eyring, "A theory of diffusion in liquids, " J. Phys. Chem., 44, 981-995 (1940). [ Links ]
43. Stupenkova, L.L., T.A. Baiburdov, V.F. Gromov and E.N. Teleshov, "Inverse suspension polymerization of acrylamide," Polym. Sci. USSR, 33, 1388-1394 (1991). [ Links ]
44. Tobolsky, A.V., C.E. Rodgers and R.D. Brickman, "Dead-end radical polymerization II," J. Am. Chem. Soc., 82, 1277-1280 (1960). [ Links ]
45. Trubitsyna, S.N., I. Ismailov and M.A. Askarov, "Polymerization of acrylamide in the presence of potassium persulphate at low temperatures," Polym. Sci. USSR, 20, 2926-2931 (1978). [ Links ]
Received: November 2, 2009.
Accepted: December 9, 2009.
Recommended by Subject Editor: Ricardo Gómez.