A high-T g epoxy−amine system based on diglycidyl ether of bisphenol A (DGEBA) and 4,4‘-methylenebis[3-chloro-2,6-diethylaniline] (MCDEA) was studied near the gel point in isothermal conditions from 80 to 180 °C by means of a rheological method, thus, below and above the glass transition temperature of the fully cured network, T g ∞ (T g ∞ = 177 °C). The lower limit of this temperature range is close to gel T g (gel T g = 50 °C), the temperature at which gelation and vitrification occur simultaneously. Close to the gel point, the power laws relating viscosity, η, to ε- k and the storage shear modulus, G‘, to ε z (ε = |x − x gel|/x gel) are verified above 150 °C. The scaling law ∂(log G*)/∂t proportional to ω-κ is verified only at 170 °C (κ = 0.25) and 180 °C (κ = 0.18). The exponents k and Δ are constant above 150 °C (k = 1.43 ± 0.03, Δ = 0.69 ± 0.01) and are very close to those found in the Rouse percolation model. Below 150 °C, these exponents diminish as the curing temperature decreases. The exponent z is frequency dependent at a given temperature, and its value z 0 for ω = 1 rad/s decreases with temperature. z 0 and κ are found to be more sensitive to the vitrification phenomenon than the parameters k and Δ. At 180 °C, thus above T g ∞, the values of exponents k, z 0, Δ, and κ are in good agreement with those derived from the percolation theory with macromolecular chains obeying the Rouse model. Below 150 °C, this behavior is no longer observed. These results are compared to those obtained for a low-T g epoxy−amine system for which only the gelation phenomenon occurs.
A flexible epoxy−amine system based on the diglycidyl ether of 1,4-butanediol (DGEBD) and 4,9-dioxa-1,12-dodecanediamine (4D) was studied between 40 and 70 °C by rheological and viscosimetric methods near the gel point. This temperature domain is located well above the maximum glass transition temperature of the fully cured network, for which T g ∞ = −12 °C. At the gel point, the theoretical extent of reaction, x gel, is equal to 0.5745, considering the reactivity ratio, n, of the secondary amines to the primary ones equal to 1.1 (equireactivity, n = 1). For the times corresponding to x gel, the rheological curves follow a classical behavior, i.e., (i) divergence of the viscosity in steady flow conditions, (ii) crossover of the tan δ curves measured as a function of time at several frequencies, and (iii) proportionality between G‘ and G‘‘ and the pulsation ωΔ (G‘(ω) and G‘‘(ω) are proportional to ωΔ). Above 50 °C, the exponent, Δ, is constant and equal to the average value of 0.70 ± 0.02. The width of the relaxation time spectrum is evaluated by studying the fully cured network. The highest value of Δ observed at low temperatures (40 °C) can be explained assuming that, in such a case, the longer relaxation times become similar to the observation times. Close to the gel point, the power laws η ∝ to ε- k and G‘ ∝ ε z (where ε = |x − x gel|/x gel), which govern the viscosity, η, and the elastic modulus, G‘, are verified within a large domain. The exponent k is constant with the temperature and is equal to 1.44 ± 0.03. The log G‘ vs f(log ε) curves display two linear domains, at least for low temperatures and high frequencies. In the second domain, the exponent z varies with frequency, but above 50 °C, its value of ω = 1 rad/s remains constant with the temperature (z 0 = 2.65 ± 0.02). The values of exponents k, z 0, and Δ are in good agreement with those obtained from the percolation theory with molecular chains obeying the Rouse model.
Chemical reaction kinetics of an aliphatic diepoxy-diamine system (DGEBD14D) has been studied between 50°C and 95 "C by two different calorimetric techniques; DSC in isothermal conditions on the one hand, conservation in thermostated tubes with successive extractions of samples studied by DSC in the dynamic temperature mode on the other hand.Experiments show that the kinetics determined by isothermal DSC are systematically faster than those obtained with the other technique, this advance starting during the initial phase of the reaction. We show that this gap comes from the mass difference between the samples used in the two techniques, and can be explained by two different reasons. On the one hand, there appears a delay in the attainment of the thermal equilibrium at the beginning of the kinetics in the thermostated tubes, the samples having a greater mass. On the other hand, experiments have shown that there is a catalytic effect caused by the contact of reactive system with air (probably due to the action of atmospheric water). The areaholume ratio of samples being greater for samples studied by isothermal DSC, the catalytic effect is favoured to a greater extent in the case of this technique, which induces a faster rate of reaction at the beginning of the kinetics.So, as the kinetic curves x = f (t) have different forms, they are described by different kinetic models. The Spacek-model adequately describes the kinetic curves determined by isothermal DSC, with exponent values p = 1.20 and q = 0.45. The curves obtained by the technique of conservation in thermostated tubes are well described by the second order autocatalytic model, the ratio of the reactivities of primary and secondary amines having the value n = 1.1. Furthermore the Tg variation curve with the extent of reaction in the thermostated tubes agrees very well with the equation proposed by Pascault and Williams. CCC OOO3-3146/95/$07.00 13 J. P. Eloundou, M. Feve, D. Harran, J. P. Pascault ZUSAMMENFASSUNG:Die Reaktionskinetik eines aliphatischen Diepoxy/Diamin-Systems (DGEBDMD) wurde zwischen 50 "C and 95 "C nach zwei unterschiedlichen kalorimetrischen Methoden untersucht, zum einen mit Differentialkalorimetrie (DSC) unter isothermen Bedingungen, zum anderen durch DSC mit Rmperaturerhdhung, nachdem die Proben unterschiedlich lange in thermostatisierten Rohren aufbewahrt wurden.Die kinetischen Parameter aus den isothermen Messungen deuten auf eine schnellere Reaktion, bereits ab der Startphase, hin als die Ergebnisse der dynamischen Methode. Dieser Unterschied wird durch die Massendifferenz der Proben bei den einzelnen Verfahren verursacht und hat zwei Grunde. Erstens verzogert sich die Einstellung des thermischen Gleichgewichts bei den Proben mit der groBeren Masse in den thermostatisierten Rohren. Zweitens wird die Reaktion von der Luft (wahrscheinlich aufgrund der Wirkung der Luftfeuchtigkeit) katalysiert. Das Verhaltnis von Probenoberflache zu Probenmasse ist bei der isothermen Methode grorjer als bei dem dynamischen Verfahren, so daB sich der kata...
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