The underlying thermosetting polymer is a resin being hardened due to the chemical reaction, called curing, leading to cross-links between existing polymer chains. Cross-linking affects (often decreases) the volume per mass, an increase in the overall stiffness, and at the same time altering the temperature due to an exothermal reaction. After mixing an agent to the resin, curing starts by using energy from the environment—mostly heat or radiation energy (UV light) is supplied to level off the temperature. Once the curing starts, from the viscous resin state until the so-called gel point, the curing process is fast. At the gel point the viscosity increases drastically so that we may call the material a solid and the curing process slows down; its rate asymptotically reaches zero at the fully cured state. Degree of cure is a difficult variable to measure. We start with a definition of this variable following [
52] by using theory of mixtures in a simplified manner. In a unit volume,
V, masses of resin, curing agent, and cured solid are introduced
\(m_\text {R}\),
\(m_\text {A}\), and
\(m_\text {S}\), respectively. Their values vary in time; but the sum is constant,
\(m = m_\text {R}+m_\text {A}+m_\text {S}\), throughout the curing process. We introduce mass fractions:
$$\begin{aligned} \begin{aligned} Y_\text {R} =&\frac{m_\text {R}}{m} \ , \ \ Y_\text {A} =&\frac{m_\text {A}}{m} \ , \ \ Y_\text {S} =&\frac{m_\text {S}}{m} \ , \end{aligned}\end{aligned}$$
(1)
leading to
$$\begin{aligned} \begin{aligned} \sum _\alpha Y_\alpha = Y_\text {R} +Y_\text {A} + Y_\text {S} = 1 . \end{aligned}\end{aligned}$$
(2)
Now we introduce the degree of cure,
\(\omega =\omega (t)\), as “measured” in time, giving the mass fraction of the solid
$$\begin{aligned} \begin{aligned} Y_\text {S} = \omega \ , \end{aligned}\end{aligned}$$
(3)
under the assumption that the initial mass of solid is zero,
\(Y_\text {S}(t=0)=0\), such that we have
$$\begin{aligned} \begin{aligned} Y_\text {R}(t=0) + Y_\text {A}(t=0) = 1 . \end{aligned}\end{aligned}$$
(4)
Consider that the ratio of masses,
\(Y_\text {R}(t=0)/Y_\text {A}(t=0)\), remains the same during the reaction. In other words, same molar mass is used for resin and agent. Now by using
\(z = Y_\text {R}(t=0)\), we obtain
$$\begin{aligned} \begin{aligned} Y_\text {R}(t) =&\,z (1-\omega ) , \\ Y_\text {A}(t) =&\,(1-z)(1-\omega ) , \\ Y_\text {S}(t) =&\,\omega . \end{aligned}\end{aligned}$$
(5)
Hence, the whole formulation for calculating the masses of constituents has been subsumed to the degree of cure (conversion degree),
\(\omega \). For obtaining its value, an evolution equation is developed dependent on the chemical reaction type. Epoxy resin reaction is based on autocatalysis mechanism [
53], effected by hydroxy groups formed during catalysis. Hence, the following evolution equation [
54] is found to be useful
where amplitudes,
\(A_\times \), activation energies,
\(E_\times \), and powers,
m,
n, are constant parameters to be determined. Universal gas constant,
R, is known. Temperature,
T, is the key variable altering kinetic rates,
\(k_\times \), and thus curing rate,
, significantly. We refer to [
55, Table 1] for parameter values of different materials. Obviously,
is used for determining the current degree of cure in each material point. This model fails to incorporate vitrification such that different mechanisms below and above glass transition temperature,
\(T_g\), are not modeled accurately. Especially curing at low temperatures (below 100
\(^\circ \)C) leads to incomplete conversion that is of paramount interest in fastening systems, where the hardening occurs in environmental conditions. A possible approach as in [
56] characterizes glassy and rubbery states occurring simultaneously. The idea was introduced in [
57] based on phenomenological observation combined with the free volume reduction during cure leading to decrease in mobility. Mobility plays a dominant role in the rubbery state as molecules collide and form a network via cross-linking. Beyond a cross-linking density, material vitrifies and in this glassy state the chemical rate is more dominant. By following [
58], we use only primary and secondary amines via autocatalysis and impurity catalysis (denoted by
c in index), collective kinetic rates,
\(K_1\),
\(K_{1c}\), involve diffusion controlled mechanism,
\(K_\text {diff}\), as well as chemically steered mechanism,
\(K_{1,\text {chem}}\),
\(K_{1c,\text {chem}}\), as suggested in [
59] as follows:
The diffusion rate is modeled by the
Williams‐
Landel‐
Ferry (WLF) equation based on [
60,
61] in the rubbery regime and greater than chemical rate in many orders in magnitude. In the glassy state, diffusion rate is nearly zero regarding chemical rate. This interplay delivers a realistic prediction of conversion degree,
\(\omega \), at low temperatures, where a so-called partial freezing inhibits to attain
\(\omega =1\). This model incorporates glass transition temperature, which is often determined by a fit function [
62] based on calorimetric measurements. For consistency, we follow [
58] and use the relation from [
63]
$$\begin{aligned} \begin{aligned} T_g = \exp \bigg ( \frac{ (1-\omega )\ln (T_{g,0}) + \Delta C \omega \ln (T_{g,\infty })}{ (1-\omega ) + \Delta C \omega } \Big ) \ , \end{aligned}\end{aligned}$$
(8)
with
\(\Delta C= \Delta c_\infty /\Delta c_0\) as the ratio of the heat capacity change at the glass transition temperature of the fully cured network with
\(\omega =1\),
\(T_{g,\infty }\) per the heat capacity change at the glass transition temperature of the monomer with
\(\omega =0\),
\(T_{g,0}\). The necessary coefficients for the evolution equations (
6), (
7) are determined by inverse analysis to data obtained by differential scanning calorimetry, we compile them from the literature as presented in Table
1. By knowing this mass fraction and the current mass density of the mixture, we can extract masses of each constituent by using Eq. (
5) with
z being the mass fraction of resin initially.
Table 1
Parameters for the evolution equation of the conversion degree,
\(\omega \), given in Eq. (
6) (upper part) and in Eq. (
7) (lower part) compiled from [
58]
Amplitude | \(A_1\) | \(1.7\times 10^{9}\) | 1/s |
Amplitude | \(A_2\) | \(280\times 10^{3}\) | 1/s |
Universal gas constant | R | 8.314 | J/(mol K) \(\hat{=}\) G/K |
Activation (energy) | \(E_1/R\) | \(12\times 10^{3}\) | K |
Activation (energy) | \(E_2/R\) | \(7\times 10^{3}\) | K |
Power constant | m | 0.6 | – |
Power constant | n | 1.2 | – |
Amplitude | \(A_3\) | \(10^{3.4}\) | 1/s |
Activation (energy) | \(E_3\) | 41.5 | kJ/mol \(\hat{=}\) kG |
Amplitude | \(A_4\) | \(10^{3.6}\) | 1/s |
Activation (energy) | \(E_4\) | 51.8 | kJ/mol \(\hat{=}\) kG |
Amplitude | \(k_{T_g}\) | \(3.8\times 10^{-5}\) | 1/s |
WLF parameter | \(C_1\) | 40 | – |
WLF parameter | \(C_2\) | 52 | K |
Ratio | \(\Delta C\) | 0.57 | – |
Monomer transition temperature | \(T_{g,0}\) | -10 | \(^\circ \)C |
Fully-cured transition temperature | \(T_{g,\infty }\) | 165 | \(^\circ \)C |