Yi
Cheng
*
Nanjing University of Science and Technology, Nanjing, 210094, P.R.China. E-mail: chengyi20@yahoo.com.cn
First published on 2nd July 2010
Ordinarily, Thermogravimetry (TG) or Differential Thermal Analysis (DTA) or Differential Scanning Calorimetry (DSC) can describe only the change of α or △T or q with T(t), and Simultaneous Thermal Analysis (STA) provides two curves, (α∼ T(t) curve and △T or q∼ T(t) curve, in a single test (T is temperature; q is the heat flow; t is time). This work proposes a Simultaneous Kinetic Method, or simply SKM method aimed at STA tests. In the SKM method, the values of the activation energy (E) and reaction mechanism function can be calculated and determined by a trial and error method using the differential kinetic equation. When the values of αm at the different heating rate are different, for example the heat degradation of polyamide 6 (PA6), the SKM method provides a more accurate activation energy than that calculated by the Kissinger equation.
The Kissinger method2 is a well known differential method in thermal analysis. The main supposition is that ln[−f′(αp)] is zero or constant. But many researchers have proved that ln[−f′(αp)] is not a constant.3–9Ref. 10 suggests the use of differential methods when the experimental curve is fluctuating.
Since the values of αp and Tp can be obtained directly from STA, a differential method similar to the Kissinger method, but even more exact than that, is proposed here.
(1) |
At a peak temperature (Tp) of a curve of either differential thermal analysis DTA or differential scanning calorimetry DSC, d2α/dT2 = 0, the differential rate equation, eqn (1), may be expressed as:
(2) |
Usually, because f(α)is unknown and the value of αp cannot be obtained directly from just a DTA or DSC curve, eqn (2) cannot be solved.
Kissinger1 suggested that choosing f(α) = (1 − α)n and assuming n(1 − αp)n−1 ≈ 1, then ln[−f′(α)] = 0. Hence, eqn (2) can be re-expressed as:
(3) |
(4) |
In fact, n(1 − αp)n−1 ≠ 1 or f′(αp) ≠ C1(constant) in many reactions. Hence, the activation energy can not calculated exactly by Kissinger eqn (3) and (4) for many reactions.
Now, with the development of thermal analysis techniques, the STA technique can give TG and DTA (or DSC) curves in one experimental set-up, which are α ∼ T(t) and either ΔT ∼ T(t) or q ∼ T(t) (q is the heat flow mw/mg). In this case, the values of Tp and corresponding αp can easily be determined.
By varying the linear heating rate, a series of αp and Tp values are obtained. From any of the f(α), the reaction active energy (E) can be calculated from eqn (2). The f(α) can assume any reaction mechanism function, such as the reaction order equation, Johnson–Mehl–Avrami equation, the one-dimensional diffusion equation, the two-dimensional diffusion equation, Jander equation, Ginstling–Brounshtein equation, random equation, etc.10 From the different f(α), we can get a series of E values. Comparing the deviation of E for different f(α) and analyzing the rationality of f(α), E and f(α) can be determined. This method is called the Simultaneous Kinetic Method (SKM).
To illustrate SKM's application, it is applied to analysis degradation of polyamide 6.
Fig. 1 The STA curves of PA6 at 5, 10 and 20 K min−1 (the heating rate increasing from left to right). |
β/K min−1 | 5 | 10 | 20 |
---|---|---|---|
1 − αp | 0.431 | 0.372 | 0.333 |
T p/K | 712.24 | 729.65 | 745.48 |
β T/K | α | ||||||||
---|---|---|---|---|---|---|---|---|---|
0.10 | 0.20 | 0.30 | 0.40 | 0.50 | 0.60 | 0.70 | 0.80 | 0.90 | |
5 | 665.5 | 685.2 | 695.2 | 702.5 | 708.5 | 713.9 | 719.0 | 724.4 | 731.0 |
10 | 677.7 | 698.2 | 709.0 | 716.5 | 722.9 | 728.2 | 733.4 | 738.5 | 745.0 |
20 | 689.5 | 710.5 | 721.9 | 729.9 | 736.2 | 741.9 | 747.2 | 752.5 | 758.9 |
(5) |
ln(β/T2p) − ln(2 − 2αp) = ln(AR/Es2) − Es2/RTp (L = 2) | (6-1) |
ln(β/T2p) − ln(6αp − 6α2p) = ln(AR/Es2) − Es2/RTp (L = 3) | (6-2) |
(6-3) |
By the SKM method, the activation energies for different reaction orders and reaction mechanism functions can be calculated separately.
ΔEmax is the maximum deviation between the activation energy at same reaction order. From Table 3, ΔEmax is seen to decrease with increasing n when f(α) = (1 − α)n. Usually, it is impossible for n to exceed 5, so it is unsuitable to assume f(α) = (1 − α)n in describing the thermal degradation of PA6. For the alternative f(α) function, the smallest value of ΔEmax was obtained when L = 2 and the value of Es of PA6 should then be 206.79 kJ mol−1.
n | L | |||||||
---|---|---|---|---|---|---|---|---|
1 | 2 | 3 | 4 | 5 | 2 | 3 | 4 | |
E 5/10(kJ mol−1) | 160 | 197 | 233 | 270 | 307 | 197 | 172 | 148 |
E 5/20(kJ mol−1) | 172 | 206 | 241 | 275 | 309 | 206 | 185 | 164 |
E 10/20(kJ mol−1) | 186 | 217 | 249 | 281 | 312 | 217 | 200 | 183 |
ΔEmax(kJ mol−1) | 26 | 21 | 16 | 11 | 6 | 21 | 28 | 35 |
E s/kJ mol−1 | 173 | 207 | 241 | 275 | 309 | 207 | 186 | 165 |
The Ozawa equation is given below:
(7) |
The activation energy of PA6 calculation by Ozawa, Kissinger and SKM method are listed in Table 4 and 5. Where E0 is calculated by Ozawa method according to the data in Table 2; Ek is calculated by Kissinger method according to the data in Table 1; Es is calculated by SKM method according to the data in Table 1.
E/kJ mol−1 | 0.10 | 0.20 | 0.30 | 0.40 | 0.50 | 0.60 | 0.70 | 0.80 | 0.90 | |
---|---|---|---|---|---|---|---|---|---|---|
E 5/10 | 203 | 202 | 196 | 197 | 195 | 199 | 201 | 208 | 213 | 201 |
E 5/20 | 210 | 212 | 206 | 205 | 206 | 207 | 209 | 213 | 218 | 209 |
E 10/20 | 217 | 221 | 217 | 214 | 219 | 216 | 218 | 218 | 223 | 218 |
E/kJ mol−1 | E k | E s1(n = 5) | E s2 (L = 2) | |
---|---|---|---|---|
E 5/10 | 201 | 160 | 307 | 197 |
E 5/20 | 209 | 172 | 309 | 207 |
E 10/20 | 218 | 186 | 312 | 217 |
ΔEmax | 17 | 26 | 6 | 21 |
E average | 210 | 173 | 309 | 207 |
Because the Ozawa equation is a model-free kinetic equation, the value of Eo is considered reasonable, implying that the value of Es2 in Table 3 is also reasonable. Furthermore, it can be determined from Table 3 that the reaction mechanism function for PA6 degradation is f(1 − α) = (α)L−1[1 + (L − 1) × (1 − α)], the reaction order is L = 2, while the activation energy is about 207 KJmol−1. Apparently, both Ek and Es1 have larger deviations.
This journal is © The Royal Society of Chemistry 2010 |