Journal of Hazardous Materials B124 (2005) 119–124
OPA oxidation rates in supercritical water
Bambang Veriansyah a,1 , Jae-Duck Kim a,1 , Jong-Chol Lee b,2 ,
Youn-Woo Lee c,∗
a
Supercritical Fluid Research Laboratory, Clean Technology Research Center, Korea Institute of Science and Technology (KIST),
39-1 Hawolgok-dong, Seongbuk-gu, Seoul 136-791, Republic of Korea
b Agency for Defense Development (ADD), P.O. Box 35-1, Yuseong, Daejon, Republic of Korea
c School of Chemical & Biological Engineering and Institute of Chemical Process, Seoul National University (SNU),
San 56-1 Sillim-dong, Gwanak-gu, Seoul 151-744, Republic of Korea
Received 28 December 2004; received in revised form 15 April 2005; accepted 16 April 2005
Available online 6 June 2005
Abstract
Supercritical water oxidation can effectively destroy a large variety of high-risk wastes resulting from munitions demilitarization and
complex industrial chemical. An important design consideration in the development of supercritical water oxidation is the information on the
oxidation rate. In this paper, the oxidation rate of isopropyl amine (OPA), one of high-risk wastes resulting from munitions demilitarization,
was investigated under supercritical water oxidation (SCWO) conditions in an isothermal tubular reactor. H2 O2 was used as the oxidant.
The reaction temperatures were ranged from 684 to 891 K and the residence times varied from 9 to 18 s at a fixed pressure of 25 MPa. The
conversion of OPA was monitored by analyzing total organic carbon (TOC) on the liquid effluent samples. The initial TOC concentrations
of OPA varied from 7.21 to 143.78 mmol/ℓ at the conversion efficiencies from 88.94 to 99.98%. By taking into account the dependence of
reaction rate on oxidant and TOC concentration, a global power-law rate expression was regressed from 38 OPA experimental data. The
resulting pre-exponential factor was 2.46(±0.65) × 103 ℓ1.37 mmol−0.37 s−1 ; the activation energy was 64.12 ± 1.94 kJ/mol; and the reaction
orders for OPA (based on TOC) and oxidant were 1.13 ± 0.02 and 0.24 ± 0.01, respectively.
© 2005 Elsevier B.V. All rights reserved.
Keywords: Kinetics; OPA; Oxidation; Supercritical water; CWA
1. Introduction
Under the provisions of the 1993 International Chemical
Weapon Convention, all stockpiled chemical warfare agents
(CWAs) are to be irreversibly destroyed [1]. Studies of
supercritical water oxidation (SCWO) for treating and destroying CWAs are underway in support of an international
program for the destruction of these CWAs stockpiles.
SCWO has been drawing much attention due to effectively
destroy a large variety of high-risk wastes resulting from
∗
Corresponding author. Tel.: +82 2 880 1883; fax: +82 2 888 1604.
E-mail addresses: vaveri@kist.re.kr (B. Veriansyah), jdkim@kist.re.kr
(J.-D. Kim), jclee@hanafos.com (J.-C. Lee), ywlee@snu.ac.kr (Y.-W. Lee).
1 Tel.: +82 2 958 5881; fax: +82 2 958 5879.
2 Tel.: +82 42 821 4091; fax: +82 42 821 2221.
0304-3894/$ – see front matter © 2005 Elsevier B.V. All rights reserved.
doi:10.1016/j.jhazmat.2005.04.019
munitions demilitarization and complex industrial chemical
and regarded as one of the promising technologies for
alternative to incineration [2–16]. SCWO uses water above
its critical point (674 K, 22.1 MPa) as a reaction medium
where both gas and liquid form a homogeneous single phase,
thus avoiding interfacial mass transfer limitations. At supercritical operation conditions, oxidation proceeds quickly
and completely for most H–C–N compounds with water,
carbon dioxide, and molecular nitrogen as the main products
[17,18].
One of the classes of CWAs stockpiles is a ‘binary chemical weapons’, which includes isopropyl alcohol and isopropyl
amine (OPA), methylphosphonic difluoride (DF), and ethyl
2-diisopropylaminoethyl methylphosphonite (QL) [19,20].
Information of binary chemical weapons oxidation rate is
an important design consideration in the development of
120
B. Veriansyah et al. / Journal of Hazardous Materials B124 (2005) 119–124
SCWO process. Knowledge of the reaction kinetics allows
one to calculate the residence times required for desire destruction and removal efficiency in a commercial SCWO reactor [4,5,21,22]. Several researchers have studied oxidation
kinetics of CWAs and chemical agent simulant in SCWO
[4,5,15,16,21]. However, there are no references in the literature about kinetic reaction rate of OPA. Thus, in this study
we report experimental oxidation result of OPA designed to
identify kinetic oxidation rate in supercritical water oxidation.
2. Experimental
2.1. Apparatus and procedure
The experiments were conducted in a laboratory-scale,
continuous-flow SCWO reactor system. The experimental
set-up is similar to previous published works [3]. The system
involved two parallel sets of equipment that are almost
identical, one for delivering the OPA solution and the other
for the oxidant. OPA and oxidant solution were pumped
separately into the system by high pressure pumps (Thermo
Separation Product Company). All hot sections of the system
were insulated in boxes of ceramic board and the temperature
was monitored directly using thermocouple. The temperature
of the system was controlled by a temperature controller
(Hanyoung DX 7). Oxygen, the oxidant used in these
experiments, was prepared by dissolving hydrogen peroxide
with deionized water in a feed tank. In order to assure all
of H2 O2 is decomposed to give H2 O and O2 , the oxidant
was pre-heated by flowing through 6 m coiled 1/8 in. o.d.
SS 316 tubing at 873.15 K and residence time of more than
14 s. Based on the studies of Phenix et al. [23] and Croiset
et al. [24], it has been evidenced that H2 O2 completely
decomposed in the pre-heater even in those experiments
carried out at high flow rate and low temperature. OPA
solution was pre-heated by flowing through 0.5 m 1/8-in. o.d.
SS 316 tubing. The solutions mixed at the reactor entrance
in a SS 316 cross and then entered the reactor, which was
constructed from a 280 mm length of 18 mm o.d. and 9.5 mm
i.d. SS 304 tubing. Upon leaving the reactor, the effluent
was cooled rapidly in a shell and tube heat exchanger and
then depressurized to ambient condition by a back-pressure
regulator (Tescom Co. 26-1721-24). The product stream
was then separated into liquid and vapor phases. The liquid
products were collected in a graduated cylinder, and their
volumetric flow rates were measured at ambient laboratory
conditions.
of oxygen. Diluted oxidant solutions were prepared using
deionized water.
Gas samples were analyzed using a Hewlett-Packard 5890
gas chromatography with a thermal conductivity detector
(TCD). A Rheodyne single mode injection valve provided
on-line sample injection into a 3 m length × 0.318 cm o.d. Supelco Carbosieves-II gas chromatograph column. The system
was calibrated with a standard gas mixture containing H2 , O2 ,
N2 , CO, CO2 , and CH4 .
The concentration of OPA and the liquid-phase reactor effluents were analyzed by total organic carbon (TOC) analyzer
(Shimadzu TOC-VCPN), which is based on combustion catalytic oxidation method and highly sensitive non-dispersive
infrared (NDIR) gas analysis, respectively. In order to provide
precision date, samples were analyzed in duplicate. The relative standard deviation (R.S.D.) for the TOC measurement
falls between 0.2 and 4.5% and the averages are reported as
result.
2.3. Calculations
2.3.1. Residence times
The residence time is calculating using the following equation:
t=
VR
ρ(P, T )
Mtotal
(1)
where VR is the reactor volume, ρ(P, T) the density of fluid
at reaction pressure and temperature, and Mtotal is the total feed mass flow rate including both the waste–water mixture and the oxidant fed into the system. The density of the
fluid is taken from steam tables for pure water [25] since
the kinetic investigations performed with dilute solutions
of OPA in water and no data were available for density
of water–OPA–oxygen mixtures at supercritical condition.
Koda et al. [26] have estimated the influence of 4.86 mol%
O2 on the mixture density. At 683.15 K and 24.7 MPa, the
ratio of the steam table density to the value calculated was
1.20. Therefore, in more diluted systems the error in density
and consequently in the residence time is thus smaller than
20%.
2.3.2. TOC decomposition
Destruction efficiency of OPA, X, based on TOC decomposition was defined as follows:
[TOC]f
(2)
TOC decomposition X = 1 −
[TOC]i
2.2. Materials and analytical methods
where [TOC]i and [TOC]f are the OPA concentrations at the
reactor inlet and outlet based on TOC, respectively.
OPA was prepared by mixing isopropylalcohol (Daejung,
99% purity) with isopropylamine (Acros, 99% purity) by
weight percentage of 71.7:28.3 in water. Hydrogen peroxide (Junsei, 35%, w/v aqueous solution) was used as a source
2.3.3. Initial concentration
The initial concentration of reactants used to determine
the global reaction rates were calculated from the measured
feed stock concentrations and flow rates of the feed streams
B. Veriansyah et al. / Journal of Hazardous Materials B124 (2005) 119–124
with the process condition, assuming that the fluid has the
density of water [27]. For initial concentration of TOC:
NTOC
CTOC
MTOC
=
×
× ρ(P, T )
12
Mtotal
where NTOC is the initial concentration of TOC in mol/ℓ,
CTOC the TOC concentration in the feed stock in g/ℓ, MTOC
the TOC feed flow rate to reactor in g/min, Mtotal the total
feed mass flow rate including both the waste–water mixture
and the oxidant fed into the system in g/min, and ρ(P, T) is
the density of water at reaction pressure and temperature. For
initial concentration of oxidant:
NH2 O2
MH2 O2
= [H2 O2 ] ×
× ρ(P, T )
Mtotal
law reaction rate can be described as follows:
rate = −
(3)
(4)
where NH2 O2 is the initial concentration of H2 O2 in mol/ℓ,
[H2 O2 ] the H2 O2 concentration in the feed stock in mol/ℓ,
MH2 O2 the H2 O2 feed flow rate to reactor in g/min, Mtotal
the total feed mass flow rate including both the waste–water
mixture and the oxidant fed into the system in g/min and ρ(P,
T) is the density of water at reaction pressure and temperature.
Thirty-eight supercritical water oxidation experiments
were conducted at temperatures ranging from 684 to 891 K
and a pressure of 25 MPa, with residence times of 9–18 s.
The initial concentration of OPA based on TOC was ranged
from 7.21 to 143.78 mmol/ℓ and the initial oxygen concentration ranged from 122 to 1685% of stoichiometrically required
amount for complete oxidation of the reactant. A summary of
each experimental condition and the measured conversions
are shown in Table 1.
3.1. OPA decomposition
d [Cn ]
= k[Cn ]a [O2 ]b [H2 O]c
dt
(7)
where [Cn ] is the concentration of reactant (mmol/ℓ); [O2 ] the
concentration of oxidant (mmol/ℓ); [H2 O] the concentration
of water; t the reaction time; a–c are the reaction orders of
Cn , O2 , and H2 O, respectively. k is the rate constant, which
can be expressed in Arrhenius form in equation as follows:
−Ea
(8)
k = A exp
RT
where A and Ea are the pre-exponential factor and activation
energy, respectively.
In this study, we assumed the global oxidation of OPA
depends only on the temperature, the reactant concentration, and the oxidant concentration. The water concentration was assumed to have no explicit effect on the reaction
rate, as is the case in many reported SCWO kinetic studies
[3,5,7–9,14,21,27–31], so the global power-law reaction rate
can be expressed as:
rate = −
3. Results and discussion
121
d [Cn ]
= k[Cn ]a [O2 ]b
dt
(9)
Substituting Cn with [TOC] and rearranging the equation
with respect to the TOC decomposition, X, defined by Eq.
(2), the relationship obtained is,
−
d(1 − X)
= k[TOC]a−1
(1 − X)a [O2 ]b
i
dt
(10)
In order to investigate the effect of the concentrations of
TOC and oxidant one by one on the decomposition rate of
TOC, a series of experiments were carried out in which one
concentration was changed while the other remained constant
during the experiment.
Fig. 1 shows that decomposition of TOC at a given oxidant concentration was increased with higher TOC concentration in the reactor feed. This is the indication of the fact
Decomposition of OPA in the SCWO can be expected to
follow the reactions for complete oxidation of isopropylalcohol and isopropylamine:
C3 H8 O + 29 O2 → 3CO2 + 4H2 O
C3 H9 N +
21
4 O2
→ 21 N2 + 3CO2 + 29 H2 O
(5)
(6)
The gas analysis indicated the absence of hydrogen, carbon monoxide, and methane in the gaseous reactor effluent.
Oxygen, nitrogen, and carbon dioxide were the only reaction
products detected. As can be seen in Table 1, OPA was easily
oxidized in the supercritical water oxidation; up to 99.98%
of TOC decomposition.
3.2. Rate expression for oxidation of OPA
In order to develop reliable reaction rate expression, 38
data were taken under various conditions. The global power-
Fig. 1. Dependence of TOC decomposition on the initial TOC
concentration.
122
B. Veriansyah et al. / Journal of Hazardous Materials B124 (2005) 119–124
Table 1
Summary of OPA oxidation experiments conducted in the SCWO flow reactor
Reaction temperature (K)
684
684
684
684
684
684
684
711
712
716
718
729
729
730
730
731
732
751
771
771
773
773
775
776
801
807
828
828
828
828
829
829
887
888
888
889
890
891
Residence time (s)
18
18
18
18
18
18
18
14
14
14
14
14
13
13
14
14
14
12
12
13
11
12
12
12
10
10
10
10
10
10
10
10
9
9
9
9
9
9
Initial concentration at reactor inlet∗
TOC (mmol/ℓ)
H2 O2 (mmol/ℓ)
21.2
20.9
20.7
20.7
20.9
20.7
20.7
124.5
28.6
143.8
51.7
15.2
15.0
15.1
15.3
16.2
15.4
120.2
12.1
12.4
11.5
11.8
12.2
12.1
76.6
97.6
10.4
10.3
10.1
10.7
10.5
10.4
7.6
7.5
7.3
7.2
7.3
7.5
217.5
108.9
174.6
87.3
130.4
152.4
196.5
1038.6
1031.2
1020.5
1005.3
95.8
80.1
111.2
126.6
154.0
140.1
853.3
94.2
106.9
67.9
80.8
118.6
131.8
790.8
729.5
58.6
70.6
106.4
115.9
81.6
93.5
92.4
102.8
83.1
62.3
51.7
71.5
Oxygen excess (%)
TOC decomposition (%)
445
175
344
122
228
287
404
307
1686
269
843
233
183
290
338
380
404
244
271
311
183
227
362
421
406
267
180
241
422
437
285
348
380
436
347
239
179
274
92.04
89.87
90.97
88.94
90.10
90.86
91.92
99.94
98.31
99.96
99.27
94.93
94.36
95.44
95.75
96.03
96.08
99.97
98.49
98.70
98.19
98.31
99.01
99.10
99.98
99.98
99.35
99.44
99.58
99.67
99.36
99.57
99.95
99.95
99.92
99.90
99.86
99.91
* TOC and H O concentration at the reactor inlet were calculated from the feed stock concentrations and flow rates of the feed streams with the process
2 2
condition.
that the global reaction order for TOC is greater than zero.
Fig. 2 shows the effect of oxidant concentration on the TOC
decomposition at given TOC concentration. The decomposition of TOC is also enhanced by higher oxidant concentration.
This implies that the global reaction order for oxidant is also
greater than zero.
In this study, all of experiments were performed at a short
contact time, between 9 and 18 s, therefore the method of
initial rates can be used to all data [32,33]. If the method of
initial rate is applied to Eq. (10) with the initial condition
X = 0 at reaction time t = 0, it can be solved analytically to
provide Eq. (11) as the relationship between the TOC removal
efficiency and the experiment variables.
X = 1 − [1 − (1 − a)kt[TOC]a−1
[O2 ]bi ]
i
for a = 1
1/(1−a)
(11)
Fig. 2. Dependence of TOC decomposition on the initial oxidant.
B. Veriansyah et al. / Journal of Hazardous Materials B124 (2005) 119–124
123
7.21 to 143.78 mmol/ℓ and the initial oxygen concentration
ranged from 122 to 1685% of stoichiometrically requirement.
Experimental data showed that TOC decomposition greater
than 99.9% can be obtained within 10 s at temperature 801 K.
By taking into account the dependence of reaction rate
on oxidant and TOC concentration, all experimental data
were used to fit the reaction rate in a non-linear regression analysis, assuming a zero-order dependence on water
concentration. Reaction parameter values were determined
to be 2.46( ± 0.65) × 103 ℓ1.37 mmol−0.37 s−1 for the preexponential factor, 64.12 ± 1.94 kJ/mol for the activation energy, and for the reaction orders, 1.13 ± 0.02 for OPA (based
on TOC), and 0.24 ± 0.01 for oxidant.
Acknowledgements
This work has been supported by the Agency for Defense
Development and National Research Laboratory Program for
Supercritical Fluids.
Fig. 3. Parity plot for power-law rate equation on decomposition of TOC.
A multi variable non-linear least squares technique was
used to estimate the kinetic parameters A, Ea , and the reaction
orders. The best-fit values were obtained by minimizing the
sum of squares error
N
exp
s2 =
(Xexp − Xpred )2
(12)
i
where Nexp is the number of experiments, Xexp the experimental conversion, and Xpred is the model predicted OPA
conversion. The quality of data fitting was evaluated by R2
in ANOVA routine [34]. It has algorithms to estimate 95%
confidence interval on each parameter and on the predicted response. Using this procedure and considering all data points,
the best-fit global rate expression for TOC of OPA oxidation
in supercritical water was obtained as
d [TOC]
−64.12 ± 1.94
3
−
= 2.46(±0.65) × 10 exp
dt
RT
× [TOC]1.13±0.02 × [O2 ]0.24±0.01
(13)
Fig. 3 shows a good comparison between the experimental and prediction TOC decomposition with R2 = 0.992. The
dashed line, indicating a deviation of ±1% TOC decomposition from the 45◦ line (perfect match), contain all data points.
This model fits very well with our experimental data.
4. Conclusions
The oxidation kinetics of OPA was examined from 684
to 891 K at 25 MPa, residence times of 9–18 s with the initial concentration of OPA based on TOC was ranged from
References
[1] Organization for the Prohibition of Chemical Weapons, Convention on the Prohibition of the Development, Production, Stockpiling
and Use of Chemical Weapons and on Their Destruction, Chemical Weapons Convention, http://www.opcw.org/html/db/cwc/eng/
cwc frameset.html.
[2] Z. Fang, S.K. Xu, R.L. Smith Jr., K. Arai, J.A. Kozinski, Destruction of deca-chlorobiphenyl in supercritical water under oxidizing
conditions with and without Na2 CO3 , J. Supercrit. Fluids 33 (2005)
247–258.
[3] B. Veriansyah, T.-J. Park, J.S. Lim, Y.-W. Lee, Supercritical water
oxidation of wastewater from LCD manufacturing process: kinetic
and formation of chromium oxide nanoparticles, J. Supercrit. Fluids
34 (2005) 51–61.
[4] P.A. Sullivan, J.W. Tester, Methylphosphonic acid oxidation kinetics
in supercritical water, AIChE J. 50 (3) (2004) 673–683.
[5] S. Bianchetta, L. Li, E.F. Gloyna, Supercritical water oxidation of
methylphosphonic acid, Ind. Eng. Chem. Res. 38 (1999) 2902–2910.
[6] Y. Matsumura, T. Nunoura, T. Urase, K. Yamamoto, Supercritical
water oxidation of high concentrations of phenol, J. Hazard. Mater.
B73 (2000) 245–254.
[7] J.R. Portela, J. López, E. Nebot, E.M. de la Ossa, Elimination of
cutting oil wastes by promoted hydrothermal oxidation, J. Hazard.
Mater. B88 (2001) 95–106.
[8] C.J. Martino, P.E. Savage, Total organic carbon disappearance kinetics for the supercritical water oxidation of monosubstituted phenols,
Environ. Sci. Technol. 33 (1999) 1911–1915.
[9] S.F. Rice, R.R. Steeper, Oxidation rates of common organic compounds in supercritical water, J. Hazard. Mater. 59 (1998) 261–278.
[10] T.-J. Park, J.S. Lim, Y.-W. Lee, S.-H. Lim, Catalytic supercritical
water oxidation of wastewater from terephthalic acid manufacturing
process, J. Supercrit. Fluids 26 (2003) 201–213.
[11] J. Kronholm, J. Kalpala, K. Hartonen, M.-L. Riekkola, Pressurized
hot water extraction coupled with supercritical water oxidation in
remediation of sand and soil containing PAHs, J. Supercrit. Fluids
23 (2002) 123–134.
[12] K.S. Lin, H.P. Wang, Supercritical water oxidation of 2-chlorophenol
catalyzed by Cu2+ cations and copper oxide clusters, Environ. Sci.
Technol. 34 (2000) 4849–4854.
124
B. Veriansyah et al. / Journal of Hazardous Materials B124 (2005) 119–124
[13] C.A. Blaney, L. Li, E.F. Gloyna, S.U. Hossain, Supercritical water
oxidation of pulp and paper mill sludge as an alternative to incineration, ACS Symp. Ser. 608 (1995) 444–455.
[14] G. Anitescu, L.L. Tavlarides, Oxidation of Aroclor 1248 in supercritical water: a global kinetic study, Ind. Eng. Chem. Res. 39 (2000)
583–591.
[15] R.W. Shaw, N. Dahmen, Destruction of toxic organic materials using supercritical water oxidation: current state of the technology,
in: E. Kiran, P.G. Debenedetti, C.J. Peters (Eds.), Supercritical Fluids: Fundamental and Applications, Kluwer Academic Publishers,
Netherlands, 2000, pp. 425–437.
[16] K.W. Downey, R.H. Snow, D.A. Hazlebeck, A.J. Roberts, Corrosion
and chemical agent destruction: research on supercritical water oxidation of hazardous military wastes, ACS Symp. Ser. 608 (1995)
313–326.
[17] E.F. Gloyna, L. Li, R.N. McBrayer, Engineering aspects of supercritical water oxidation, Water Sci. Technol. 30 (9) (1994) 1–10.
[18] H. Schmieder, J. Abeln, Supercritical water oxidation: state of the
art, Chem. Eng. Technol. 22 (11) (1999) 903–908.
[19] E.J. Hogendoorn, A chemical weapons atlas, Bull. At. Sci. 53 (5)
(1997) 35–39.
[20] Factfile: US Unitary and Binary Chemical Stockpiles, Arms Control
Today, February 1996. p. 34.
[21] R. Lachance, J. Paschkewitz, J. DiNaro, J.W. Tester, Thiodiglycol
hydrolysis and oxidation in sub- and supercritical water, J. Supercrit.
Fluids 16 (1999) 133–147.
[22] H.E. Barner, C.Y. Huang, T. Johnson, G. Jacobs, M.A. Martch, W.R.
Killilea, Supercritical water oxidation: an emerging technology, J.
Hazard. Mater. 31 (1) (1992) 1–17.
[23] B.D. Phenix, J.L. DiNaro, J.W. Tester, J.B. Howard, K.A. Smith,
The effect of mixing and oxidant choice on laboratory-scale mea-
[24]
[25]
[26]
[27]
[28]
[29]
[30]
[31]
[32]
[33]
[34]
surements of supercritical water oxidation kinetics, Ind. Eng. Chem.
Res. 41 (2002) 624–631.
E. Croiset, S.F. Rice, R.G. Hanush, Hydrogen peroxide decomposition in supercritical water, AIChE J. 43 (9) (1997) 2343–2352.
W. Wagner, A. Pru, The IAPWS formulation 1995 for the thermodynamic properties of ordinary water substance for general and
scientific use, J. Phys. Chem. Ref. Data 31 (2) (2002) 387–535.
S. Koda, N. Kanno, H. Fujiwara, Kinetics of supercritical water
oxidation of methanol studied in a CSTR by means of Raman spectroscopy, Ind. Eng. Chem. Res 40 (2001) 3861–3868.
S. Gopalan, Phenol oxidation in supercritical water: from global
kinetics to a detailed mechanistic model, Ph.D. Thesis, Department
of Chemical Engineering, The University of Michigan, MI, 1995.
J. Schanzenbächer, J.D. Taylor, J.W. Tester, Ethanol oxidation and
hydrolysis rates in supercritical water, J. Supercrit. Fluids 22 (2002)
139–147.
M. Krajnc, J. Levec, On the kinetics of phenol oxidation in supercritical water, AIChE J. 42 (7) (1996) 1977–1984.
F.M. Jin, A. Kishita, T. Moriya, H. Enomoto, Kinetics of oxidation
of food wastes with H2 O2 in supercritical water, J. Supercrit. Fluids
19 (2001) 251–262.
S.N.V.K. Aki, M.A. Abraham, Catalytic supercritical water oxidation
of pyridine: kinetics and mass transfer, Chem. Eng. Sci. 54 (1999)
3533–3542.
H.S. Fogler, Elements of Chemical Reaction Engineering, Prentice
Hall International (UK) Limited, London, 1999, pp. 223–269.
J.R. Portela, E. Nebot, E. Martinez de la Ossa, Kinetic comparison between subcritical and supercritical water oxidation of phenol,
Chem. Eng. J. 81 (2001) 287–299.
R.A. Johnson, G.K. Bhattacharyya, Statistics Principles and Methods,
Wiley, New York, 2001, pp. 585–621.