CC BY
19
22. Alkaline leaching of nickel bearing ammonium jarosite precipitate using KOH, NaOH and NH4OH in the presence of EDTA and Na2S / Ntumba Malenga E., Mulaba-Bafubiandi A. F., Nheta W. // Hydrometallurgy. 2015. Vol. 155. P. 69-78. doi: 10.1016/ j.hydromet.2015.04.004
23. Magnetically Recoverable Nanocatalysts / Polshettiwar V., Luque R., Fihri A., Zhu H., Bouhrara M., Basset J.-M. // Chemical Reviews. Vol. 111, Issue 5. P. 3036-3075. doi: 10.1021/cr100230z
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Дослiдження ктетики процесу Фшера-Тропша e досить важливим завданням, так як даний процес дуже чутливий до температурного режиму, та характеристик каталiзатору. Також даний процес супроводжуеть-ся багатьма побiчними реакциями, як негативно впли-вають на швидтсть та селективтсть реакцп. Синтез Фшера-Тропша е альтернативним джерелом отриман-ня яксного палива не з нафти, а з вугЫля або бюма-си. Тому до^дження ктетики реакцп Фшера-Тропша спрямоват на тдвищення селективностi i активностi каталiзаторiв, визначення констант швидкостi хiмiчних реакцш е актуальними.
Вибiр каталiзатору е одним з основних факторiв, що впливають на ятсть i вихiд продукту по синтезу Фшера-Тропша. Для дослiдiв виготовлено два зразка кобальто-вих каталiзаторiв. Перший зразок каталiзатору Со/ J-AI2O3 метить наночистинки кобальту одного розмiру. Другий зразок каталiзатору (Со)/у-А120^ отриманий методом просочення нойя розчином ттрату кобальту. Каталiзатор отриманий методом просочення (Со)/ J-AI2O3 виявив на порядок вищу активтсть в порiвняннi з монодисперсним. Однак монодисперсний каталiзатор показав високу селективтсть за нижчими вуглеводнями.
Для розрахунку ктетики процесу Фшера-Тропша та для знаходження констант швидкостiреакцш, було створено програмний модуль, який розроблявся в середовищi MS Visual Studio 2017 на мовi C# з використанням тех-нологш .NET Framework v4.6. За допомогою розробленого програмного модуля було розраховано константи швид-костi реакцп процесу Фшера-Тропша. Проаналiзувавши отримаш дат, видно, що вiдносна похибка лежить в межах 2...3 %, що свiдчить про адекваттсть запропо-новано1 моделi розв'язку зворотно1 задачi хiмiчноï ктетики. Тому можна засвiдчити, що дану модель розрахунку констант швидкостi можна використовувати для до^дження процесу Фшера-Тропша
Ключовi слова: реакщя Фшера-Тропша, кобальто-вий каталiзатор, зворотна задача ктетики, константа швидкостi
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UDC 66.04:665.7:541.12
|DOI: 10.15587/1729-4061.2018.134165|
MATHEMATICAL MODEL OF OBTAINING A HYDROCARBON FUEL BASED ON THE FISCHER-TROPSCH PATHWAY IN A STATIONARY LAYER OF THE COBALT-BASED CATALYST
Yu. Zakharchuk*
E-mail: zakharchuk.yu@gmail.com Yu. Beznosyk
PhD, Associate Professor* E-mail: yu_beznosyk@ukr.net L. Bugaieva
PhD, Associate Professor* E-mail: bugaeva_l@ukr.net *Department of Cybernetics Chemical Technology Processes National Technical University of Ukraine "Igor Sikorsky Kyiv Polytechnic Institute" Permohy ave., 37, Kyiv, Ukraine, 03056
1. Introduction
At present, the processes for obtaining a synthetic liquid fuel from gases that contain a mixture of carbon monoxide and hydrogen include the Fischer-Tropsch process (FT-syn-thesis) [14]. The FT-synthesis is an alternative source for obtaining high-quality fuel from coal or biomass, rather than petroleum.
Given a decrease in the oil stocks in the world, mankind has begun to look for alternative sources in order to obtain fuel whose production volumes grow every year. Conversion
of synthesis-gas to liquid hydrocarbons using the Fisch-er-Tropsch process (FT-synthesis) [1-4] is an alternative technique for obtaining the motor fuel.
The Fischer-Tropsch synthesis is an important technology, aimed at converting coal, natural gas, or biomass, into valuable products, such as motor fuels or raw materials for petrochemicals [1, 3]. The process is named after Franz Fischer and Hans Tropsch [3, 4], who showed the possibility of this reaction in 1923, by converting a mixture of carbon monoxide and hydrogen into hydrocarbons using an iron catalyst.
©
Even though almost hundred years have passed since the discovery, a given method of production of synthetic hydrocarbons has been attracting the attention of researchers and engineers due to the possibility of obtaining motor fuels and valuable petrochemical products.
Studying the kinetics of the Fischer-Tropsch process is a very important task, as a given process is very sensitive to a temperature mode, as well as characteristics of the catalyst. In addition, this process is accompanied by many side reactions that negatively affect the rate and selectivity of the reaction. Therefore, studies into FT-synthesis, aimed at enhancing the selectivity and activity of catalysts, determining the rate constants of chemical reactions, are relevant.
2. Literature review and problem statement
The Fischer-Tropsch synthesis is a chemical process in which carbon monoxide CO and hydrogen H2 are converted into different liquid hydrocarbons in the presence of a catalyst. The most commonly used catalysts contain iron and cobalt [5, 6]. The FT-synthesis is a heterogeneous-catalytic process that proceeds with a release of huge amount of heat. The reactions proceed, depending on the catalyst used in the process, at atmospheric or high pressure in the temperature range of 160...375 °C [3, 6, 7]. The FT-synthesis is an important industrial process for converting the synthetic gas (H2/CO) derived from carbon sources, such as coal, peat, biomass, and natural gas, into the oxygen-saturated hydrocarbons [1, 2].
The product of the FT-synthesis is a complex multi-component mixture of linear and branched hydrocarbons and oxygen-containing compounds. The fuel, which is produced by the synthesis, is of high quality and it contains no sulfur. Significant progress has been made over the past two decades in the development of more active and selective catalysts of cobalt, iron, and many other effective technologies, modernizing the reactor and the process.
The choice of the catalyst is one of the main factors that affect the quality and output of the product obtained using the FT-synthesis. The issue of the selection of the optimal catalyst for conducting the process is fundamental in the study of the Fischer-Tropsch process.
It is shown that the best catalysts for the FT-synthesis are those catalysts that are based on ferrum and cobalt [6, 8-12, 15]. Paper [10] compares these catalysts. Cobalt catalysts are used at lower temperatures than the catalysts based on iron. Using other metals as catalysts, such as nickel, leads to the formation of toxic compounds. Cobalt catalysts slow down side reactions in the FT-synthesis, while using the catalysts based on ferrum leads to that there is always a reaction that forms water vapor. The activity of the catalysts is affected by the chemical nature of the substance (a carrier), upon which the catalyst is applied, surface and porous structure of the carrier.
In paper [13], authors conducted a kinetic study into and modeling of the Fischer-Tropsch process on a ferrum-cat-alyst. They investigated the mechanisms of formation of products from CH4 to CnH2n+2. However, as noted, the Fischer-Tropsch process on the ferrum-containing catalysts proceeds at higher temperatures, by 50...150 degrees. In addition, in parallel to the main reaction, there is an intensive side reaction that converts water vapor. That leads to inhibiting the primary reaction of the FT-synthesis.
Cobalt is one of the most active metals for the FT synthesis. However, the activity of the cobalt catalyst is influenced
by many factors related to both the preparation of the catalyst and the process parameters.
Papers [7, 14, 16, 18] described mathematical models for the kinetic studies into the FT-synthesis without solving a problem on finding the kinetic constants.
The implementation of the FT-synthesis process is carried out in chemical reactors with a motionless or condensed layer of a catalyst [1, 8, 14]. However, the papers cited lack the mathematical models applicable for calculating or controlling these reactors.
Special attention should be paid to paper [14], which employs a microreactor for the FT-synthesis.
The papers reviewed [8-15] lack solutions to the problems on calculating the kinetic constants for the Fischer-Tropsch synthesis. Finding the rate constants for chemical reactions or solving the inverse problem of chemical kinetics is a non-trivial task [19, 20]. And since the Fischer-Tropsch process is a complex process, which lacks a model to search for the reaction rate constants, it was decided to find and suggest a solution to searching for the reaction rate constants of a given process.
3. The aim and objectives of the study
The aim of this work is to calculate rate constants for a system of the Fischer-Tropsch reactions in the presence of heterogeneous catalysts based on the obtained experimental data. That would make it possible to pass over to modeling and calculation of industrial reactors with both a stationary layer of catalyst and reactors of more sophisticated designs. For the already existing reactors, the constructed mathematical models could enable the optimal control.
To accomplish the aim, the following tasks have been set:
- to analyze theoretically a mathematical model of the kinetics of the Fischer-Tropsch reaction;
- to study experimentally the Fischer-Tropsch process;
- to construct a mathematical model for the kinetics of the heterogeneous catalytic Fischer-Tropsch process and a build a calculation scheme of the reaction rate constants;
- to process the obtained experimental data using the developed software and to calculate reaction rate constants for the Fischer-Tropsch process.
4. Theoretical analysis of the mathematical model for the kinetics of the Fischer-Tropsch reaction
The Fischer-Tropsch process on cobalt catalysts in the general case is described by the following summarizing equation:
nCO+(2n + 1)H2 CnH(2n+2) + nH2O, (1)
where kn is the rate constant of the n-th reaction, n=1, 2, 3,..., 7 is the number of the examined reactions.
The experimental setup has a reactor of small size, with a very small amount of the catalyst, sprayed on the carrier; the result implies that the reactor produces little hydrocarbon products. Consequently, we can accept following assumptions for our calculations:
- constant temperature was maintained in the reactor, it should be noted that the reactor operates under isothermal mode, that is
T=const;
dT/dt=0;
- pressure in the reactor was 1 atm, it was maintained at a given level, one can note that pressure did not change over time as well, that is
P=const;
dp/dt=0;
- the concentrations of CO and H2 are in great excess and remain nearly unchanged over time, that is,
CCO=const;
dCco/dt=0;
CH2=const;
dCH2/dt=0.
The rate of hydrocarbon formation in the system is expressed by the following formula:
dCC
d t
((2n+2) _ I pn W2n+1) - bnCC0CH, .
W - dCn - b Cn C(2n+1) W = d t- bnCCoCH2 .
dC„ AC„ Cn ~Cn,
d t At t--t-
I 1-1
Cn -Cn,-, +bn*Cnœ*CH2:+1)*(t,-ts-i).
k. — e
k —
ln(W„ )-n*ln(Cc0 )-(2n+1)»ln(CH2)
>(Wn)
To calculate the quantity of reaction products, we shall write down the balance for the amount of substances, which enter the reactor, and which exit the reactor: - entering the reactor:
N°=N°C0+N°H2; -exiting the reactor: N=Nco+Nm+Nmo+SNCn.
(9)
(1°)
Based on the system of equations for reaction (1), we shall record the amount of CO, H2 and H20 substances, following the reaction:
Nco - Ko-£ nncn,
n—1
N«2 -№„2-¿(2n +1)ncn-
n-1
7
NHO -x nNC,.
(11) (12) (13)
Substituting equations (11) to (13) into equation (10), we obtain:
(2)
N - N°o + N«2 -X 2nNCn.
(14)
For convenience, we denote the concentrations of the reaction products based on the number of hydrocarbons in the chain: Ci - Ccha, C2 - Cc2H6; •••; Cn - CcnH(2n+2). Then the reaction rate can be expressed by the following formula:
Next, by substituting (9) and (11) into (14), we obtain:
(15)
N - N° + 2nNC0 - 2nN°O.
(3)
Substitute the derivative from the product concentration over time with the finite differences:
(4)
where Cni, Cni-1 are the values of concentration of hydrocarbon components n at respective time % ti.1.
Thus, we derive a formula to calculate the concentration of components based on the time of reaction:
(5)
Taking into consideration that the concentrations of CO and H2 are taken in great excess, and remain almost unchanged over time, we can calculate the rate constant for each reaction from the following formula:
ln(Wn )=ln(kn ) + n *ln(Cco )+(2n +1) *ln(Ca). (6)
Hence:
The volume of CO, H2 and C after reaction is derived from the experimentally found LHM chromatogram, by finding the area of peaks that correspond to the given substances. Knowing the amounts of these substances, one can find the volumetric concentrations from formulae:
gco = tC°=-TT, (16)
(17)
(18)
where VP is the volume of loop for the sample at the LHM chromatograph; VCO, VH2, VC1 are the volumes of CO, H2 and CH4, respectively.
We find from formulae (16) to (18):
Vco - Nco
Vp N
V«2 _ n«2
Vp N
VC1 NCt
Vp " ' N '
"n emln(Cco ) *e<2n+1)*ln(CH2 ) '
(7)
(8)
NCO - gco * N, Nh2 - g«2 * N -Nc1 - gc1 * N.
(19) (2°) (21)
Substituting equation (19) into equation (15), we obtain: N=N0 + 2n * gCO * N - 2n * №cO,
or
or, after transforms:
N0 - 2n * №°r
1 -2n *i
(22)
Thus, by finding the total amount of a substance after the reaction, one can calculate the amount of formed methane from formula (21).
5. Experimental study of the Fischer-Tropsch process
The purpose of the experimental research was to study the Fischer-Tropsch process and to obtain data for the further research into the kinetics of the process and calculation of rate constants for the process (solving an inverse problem of chemical kinetics).
We studied the reaction at the installation using a reactor of the flow-through type with a fixed layer of the catalyst (Fig. 1). This is a metallic reactor with a volume of 2 ml. Hydrogen was additionally purified from the traces of oxygen on the industrial catalyst Ni/Cr at 7=300 °C, and of water - on zeolite NaA.
Fig. 1. Experimental installation. Feed cylinders: 1 — H2, 2 - CO, 3 - Ar; 4 - reactor; filters: 5 - Ni/Cr, 6 - CaA, 7 - SiO2; 8 - flow regulators El-Flow; 9 - pressure regulator
El-Press; 10 - Selmi, 11 - LHM; feed flows: 12 - Selmi detector, 13 - Selmi carrier; 14 - Selmi blower; 15 - LHM carrier
The supply of gases was controlled by mass controllers: for CO, H2 and Ar - model F-211CV-AAD-22-V (Bronkhorst High-Tech B. V.). Pressure in the installation was controlled and maintained using the digital pressure sensor P-502-C-100A-AAD (Bronkhorst High-Tech B. V.).
To analyze reaction products, the reaction mixture after the reactor was throttled using a heated valve to the atmospheric pressure; next, through two consistently connected six-way valve-dispensers, the gas samples were taken for chromatographic analysis.
Analysis of a gas mixture at the inlet to the laboratory reactor was run at LHM chromatograph. Analysis of the organic products of the vapor-gas phase reaction was performed at the chromatograph SelmiKhrom-1.
The purpose of the first experiment was to study the influence of the method for preparing the cobalt catalysts of carbon monoxide hydrogenation in the process of FS-synthesis for activity and selectivity of catalysts at elevated pressures. We used the industrial sample of y-Al2O3 as carriers.
Two samples of cobalt catalysts were fabricated for the experiments. The first sample of the catalyst Co/y-Al2O3 contains cobalt nanoparticles of the same size. The second sample of the catalyst (Co)/y-Al2O3 was obtained by applying the method of impregnating the carrier with the solution of cobalt nitrate.
Monodispersed cobalt nanoparticles (a diameter of particles of 6.5 nm) were obtained by decomposing cobalt (II) oleate in dibenzyl ether. Photographs of the catalyst and the size distribution of Co particles are shown in Fig. 2, 3.
Fig. 2. Photographs of cobalt particles from a microscope
Fig. 3. Size distribution of Co particles depending on size
All catalysts contained cobalt in the amount of 3 % by weight.
Preparation of catalyst.
1. The synthesis of cobalt nanoparticles. We first synthesize cobalt (II) oleate. To this end, the three-headed reactor with a capacity of 1 l, installed in a water bath, is connected to the cylinder with argon and is equipped with a stirrer with a top drive and an air refrigerator. Water bath is used for heating. We first dissolve in 100 ml of the deionized water 8.7 g of cobalt (II) nitrate; 4.8 g (5.45 ml) of 25 % ammonia solution are separately dissolved in 100 ml of the deionized water. The resulting solutions are placed into the reactor with the agitation switched on; a suspension of cobalt (II) hydroxide is obtained. The resulting suspension of cobalt (II) hydroxide is added with 2 g (2.23 ml) of oleic acid and 200 ml of octadecene. Next, we open the flow of argon and heat the water bath to the boiling point of water. Under such conditions, the reaction mixture is aged for 30 min. Thus,
200
150
M
"¡a
50
190
the cobalt oleate forms, which passes into the organic phase of octadecene.
Upon completion of the reaction, the contents of the flask are transferred to a separating funnel; we select the organic phase, washing it with distilled water.
2. Obtaining Co nanoparticles. The installation for obtaining the nanoparticles of cobalt oleate consists of the reactor with a capacity of 500 ml, a flask heater, a cylinder for argon, two consistently connected air coolers and a stirrer with a top drive.
The resulting solution of cobalt oleate is taken to the reactor with a capacity of 500 ml. The reactor is mounted onto the heater; a cylinder with argon is connected; two consistently connected air coolers and a stirrer with a top drive are added. We heat the flask to 100 °C and age at such a temperature for 60 min in order to evaporate residues of the water phase. Next, we intensify the heating and bring oct-adecene to a boiling point (270 °C). The reaction mixture is aged for 5 hours under such a temperature.
After five hours from the start of octadecene boiling, the heating is switched off to allow the reaction mixture to cool. Then the contents of the flask, where cobalt nanoparticles have already formed, are taken to the centrifuge tubes (2 ml per a tube), adding the excessive ethanol as an extractant. The mixture is agitated and centrifuged until the nanopar-ticles are deposited. Next, the supernatant is decanted while the solid residue in each tube is dispersed into hexane (2 ml of hexane per each tube). The hexane is again added with an excess of alcohol, we agitate and centrifuge it. The top layer of the solvent is decanted; this operation is repeated three times. After that, the solid residue is dispersed into hexane, it is taken to the measuring beaker, then we add hexane to the volume of 100 ml.
3. Obtaining 3 % Co on aluminum oxide. First, we prepare 10 g of the carrier with a fraction size of 1-2 mm by shredding the granules and sifting at the sieves.
To prepare 10 g of the catalyst containing Co in the amount of 3 % by weight, granules in the amount of 9.7 g are put into a weighing bottle; we add, in parts, the prepared suspension of nanoparticles, or a solution of salt depending on the moisture capacity of the carrier. The catalyst is shaken periodically and kept in a closed weighing bottle for 24 hours. Next, the catalyst is dried for 16 hours at 40 °C. These operations are repeated until the content of Co on the carrier reaches 0.3 g. The resulting catalyst is placed in a porcelain cup, put in a muffle, and baked for 6 hours at 320 °C.
Conditions for conducting the experiment.
The batch of catalysts was 0.5 g. Prior to the experiment, the catalysts were reduced in two stages.
Reduction conditions for the first stage: temperature -280 °C; time2 - 60 min.; gas flow rate - 30 cm3/min; gas mixture - H2 (5 % by volume) + Ar (95 % by volume); pressure -atmospheric.
Reduction conditions for the second stage, which took place directly after the first: temperature - 320 °C; time -90 min.; gas flow rate - 30 cm3/min; gas mixture - H2 (5 % by volume) + Ar (95 % by volume).
Conditions for conducting the experiment: the temperature varied (190 °C, 215 °C, 240 °C); time - 60 min.;
gas flow rate - 30 cm3/min; gas mixture - H2/CO=2.5; pressure - 30 bars.
The result of our study is the obtained dependence of the catalyst activity (per a gram of the product formed per a gram of the catalyst per second) on temperature of the course of the reaction (Fig. 4) [21].
(Co)/y-Al O —Co/y-Al O
____I
--1 — -
200
230
240
Fig
210 220 T, c
4. The catalyst activity dependence on temperature
Fig. 4 shows that the catalyst that was obtained using the method of impregnating (Co)/Y-Al2O3 demonstrated the activity higher by an order of magnitude compared with the monodispersed one. However, the monodispersed catalyst showed higher selectivity for the lower hydrocarbons.
Compared with the monodispersed catalyst, the catalyst that was obtained using the method of impregnation, demonstrates in the CO hydrogenation reaction the formation of a broad spectrum of hydrocarbons - from C1 to C8. At the same time, the main product of the CO hydrogenation on the monodispersed catalysts was methane.
The purpose of the second experiment was to study the influence of the surface modification of catalyst based on cobalt with the ions of metals, specifically magnesium.
The carrier used was the industrial sample of silica gel KSKG (Coarse Silica gel, Large porosity, Granulated, xSiO2nH2O). The catalyst was obtained using a standard method of impregnating the carrier with a water solution of cobalt nitrate in which the active phase are the particles of polydispersed cobalt.
Preparation of the catalyst.
Spherical KSKG (balls the size of 3-5 mm) with a weight of 590 g is baked in the air at 250 °C for 3 hours. Next, the cooled silica gel is impregnated to a full moisture capacity with a water solution of magnesium nitrate (110 g of Mg(NO3)2-6H2O+385 g of distilled H2O). Impregnation was performed at a room temperature at intensive agitation. Next, it was air dried at 150 °C for 8 hours.
The drying was followed by the calcination in the air at 350 °C (10 hours). The cooled baked catalyst was impregnated to a full moisture capacity with a water solution of cobalt nitrate (930 g of Co(NO3)2-6H2O + 380 g of distilled H2O) at a room temperature with intensive agitation over 4 hours. The impregnated contact mass was dried in the air at 150 °C, intensely agitating for 8 hours. It was followed by the calcination in the air at 350 °C for 10 hours and cooling in a flow of inert gas (nitrogen, argon) to 260 °C. The catalyst was then reduced with a mixture of argon + hydrogen with a hydrogen content of 3...5 %.
On baking, the catalyst was cooled in a flow of inert gas (nitrogen, argon) to 260 °C. It was then reduced with the
gas mixture Ar+H2 containing hydrogen in the amount of 3-5 % by volume, increasing the temperature to 350 °C over 14 hours at a volumetric speed of 3-4 thousand h-1 (about 3,500 l/hour for the reducing mixture).
Next, the reduced catalyst was cooled to room temperature, blown with nitrogen, until the oxygen content at the inlet and outlet was the same (approximately 14 hours).
Conditions for conducting the experiment.
We investigate the reaction at the same installation using a reactor of the flow-through type with a fixed layer of the catalyst (Fig. 1).
The batch of catalysts was 0.3 g. Prior to the experiment, the catalyst was also reduced. Conditions for the catalyst reduction: temperature - 350 °C; time - 10 h; gas flow rate -30 ml/min; composition of the gas mixture: Ar+H2 with a hydrogen content of 33 % by volume; pressure - 1 bar.
Conditions for conducting the experiment: the temperature varied within 250...300 °C; time - 30 min.; gas flow rate -40 ml/min; composition of the gas mixture - H2:CO=3:1; pressure - 1 bar.
The result of the experiment is the charts acquired from the chromatographs LHM and Selmi, based on which we calculated the amount of hydrocarbon products of the reaction. An example of chromatograms, at a reaction temperature of 300 °C, is shown in Fig. 5, 6.
S
S3=mc_;.
S. mr
■3 LHM
0.08-
H2
. 1 \ C1
Fig. 5. LHM chromatogram
CI
p
/°C4 C5 li / C6 1 C7 \
Fig. 6. Selmi chromatogram
Fig. 5 and Fig. 6 show that the result of the reaction is the formed series of hydrocarbon products whose molecules have in their chain from 1 to 7 carbon atoms.
Based on the Selmi chromatograph, the ratios between the obtained hydrocarbon products are directly proportional to the ratio of the areas of peaks that correspond to the given substances (Fig. 6). That is, we shall write for the kinetic system:
By finding the mass of Ci from formula (23), one can find masses of other hydrocarbon reaction products using formula (24):
mC. = Nc* Mc,,
S
(23)
(24)
Knowing the masses of hydrocarbons, one can find their amount and concentration:
m
Nc =—"
c M,
Cn
Cc =-
cn
Nc
_cn
VD
(25)
(26)
We shall give an example of calculating the amount of reaction products, using the acquired experimental data (Fig. 4, 6) from formulae (16) to (26).
The calculation is conducted under the following conditions of the experiment:
- CO flow rate - 10 ml/min;
- H2 flow rate - 30 ml/min;
- temperature in the reactor - 300 °C.
Using the LHM chromatogram, we find the amount of CO and CH4 at the outlet from the experimental reactor. To this end, it is necessary to find the areas of the corresponding peaks from the chart, shown in Fig. 5, and multiply them by a ratio coefficient that, shows the connection between a volume of the respective substance and the area of the corresponding peak:
Vco=1.6-0.3846=0.61538 ml; VCi=0.75-0.01646=0.01235 ml.
Knowing the volume of CO and CH4, we shall find their molar concentrations from formulae (16) and (18):
gco=0.61538/4.5=0.13675;
gci=0.01235/4.5=0.00274.
Next, knowing the amount of substance at the inlet to the reactor, from formula (22), we shall determine the total amount of a substance at the outlet to the reactor:
iV=(2.009-10~4-2-5.02-10~5)/(l-2-0.13675)=1.382-10"4.
Next, knowing the total amount of a substance at the outlet from the reactor and the molar concentration of CH4, we find from formulae (21) and (23) the amount and mass of the formed methane:
NC1=2.74-10-M.382-10-4=3.79-10-7,
mC1=3.79-10-716=6.071-10-6.
The concentration of component C1 derived from formula (26) is equal to:
S
m
c
2
CC1=(3.7940-7)/0.0045=8.43240-5.
Based on the Selmi chromatogram (Fig. 6), knowing the mass of methane at the outlet from the reactor, and by defining the areas of peaks for the hydrocarbon substances, we shall determine the mass, quantity, and concentration of each component (formulae (24), (25), (26)). The following calculation is only for component C2H6 (C2):
mC2=6.07140-^(041209/0.46626)=1.45940-6,
NC2=(1.45940-6)/30=4.86540-8,
CC2=(4.86540-8)/0.0045=L08140-5.
Calculations for all components of the reaction mixture are included in the developed software module. Now, knowing the concentration of reaction products, one can proceed to the calculation of reaction rate constants.
ccbhu. - cc6hui-1 +k6 ' Cco'Ca2 ' (ti ti-1),
CC7H16, - CC7H16i-1 + k7 ' CCO ' CH2 ' (ti -ti-1).
In order to calculate the kinetics of the Fischer Tropsch process and to find the reaction rate constants, we created a software module, which was developed in the programming environment MS Visual Studio 2017 in the programming language C# using the .NET Framework v4.6 technologies [21].
A given software module includes the following components:
- files of forms: Form1.cs, Form2.cs, FormGraph.cs, Form-Help.cs;
- project files: Program.cs, Controller.cs, Model.cs, DB.cs. The scheme of interaction between the files and forms is
shown in Fig. 7.
Controller Model DB
6. Calculation of reaction rate constants based on the obtained experimental data
A model of the system of kinetic equations of the Fisch-er-Tropsch reaction for the derived experimental data and for the calculation of kinetic constants based on formulae (2), (5), (8) is summarized in Table 1.
Fig. 7. Scheme of interaction between files and forms of the software module
The Fischer-Tropsch reaction pathway and the calculation of constants
Reaction pathway Reaction rate Calculation of reaction rate constant
CO+3H2^CH4+H2O w = dCcH4 = k Cco CH 1 dt 1 CO H2 k exp(ln(Wi)) 1 exp(ln(Cco ))*exp(3ln(CH2))
2CO+5H2^C2H6+2H2O dCc Hi 2 5 W2 - dt - k2 CCO CH2 k exp(ln(W2))
exp(2ln(Cco ))*exp(5ln(CH2))
3CO+7H2^C3H8+3H2O dCc H i 3 7 W3 - dt - k3 Cco CH2 k exp(ln(W,))
*3 exp(3ln(Cco ))*exp(7ln(CH2))
4CO+9H2^C4H10+4H2O W4 - ^dr - k4 CC0CH2 k exp(ln(Wi))
*4 exp(4ln(Cco ))*exp(9ln(CH2))
5CO+9H2^C5H12+5H2O w - ^dr - ks CC0CH2 k exp(ln(W5))
*5 exp(5ln(Cco))*exp(11ln(CH2))
6CO+13H2^C6H14+6H2O dCc h * 6 13 W6 Ct k6 CCO CH2 k exp(ln(W6))
*6 exp(6ln(Q,o))*exp(13ln(CH2))
7CO+15H2^C7H16+7H2O w7 - dCcf 16 - k7 C7C0CH 7 dt 7 CO H2 k exp(ln(W7))
*7 exp(7ln(Cco))*exp(15ln(CH2))
Knowing the reaction rate constants, one can show the dependence of products concentration on the time of the reaction progress:
Table 1 The main elements of the computational module:
- Form1.cs - the main form that contains two databases of experimental data acquired from the chromato-graphs LHM and Selmi, buttons for graphical representation of the recorded chromatograms, fields for entering the flow rates of incoming gases to the system, and a button to launch calculations;
- Form2.cs - a form to represent the results of calculations; it contains a table with the results of calculations, a chart that shows the distribution of the formed products, and buttons to graphically represent the solution to a direct problem of chemical kinetics;
- FormGraph.cs - a form to graphically display the results of calculations;
- FormHelp.cs - a form to display a Help program;
- Program.cs - a file class (a file, simply put), which initiates the program;
- Controller.cs - a file class, which is designed to link the forms and the file "Model.cs" (or the forms and the class
CCH4. - CCHi._l + k1 'CCO 'CH2 '(ti-ti- -l), Model); - Model.cs - a file class, which keeps records of all the
CC2 H6, CC2 H6,■-1 + k2 'CCO 'CH2 '(ti-t, methods, designed for calculations in the program;
- DB.cs - a file class, which is designed to read data
Cc3 H8,' Cc3 H8,-1 + k3 ' CCO ' C72 ' (ti - ti-l), from TXT files. In addition, it contains certain data for
calculations: a volume of the reactor, a loop volume of the
CC4H10 t - CC4H10 . -i + k4 ' CCo ' CH2 ' (ti ~ -ti-l), chromatograph, the time of substance yield at the chro-
matograph LHM, and molar masses of the formed hydro-
CC5 H12i CC5H12j. _1 + k5 ' CCO ' CH2 ' (ti - "ti-l), carbons.
A software module is designed to solve a direct and inverse problems of chemical kinetics for the Fischer Tropsch process using different catalysts. The application requires the following data:
- data from the chromatograph LHM;
- data from the chromatograph Selmi;
- flow rates of CO and H2 at the inlet to the reactor in the dimensionality of ml/min.
Graphical user interface, which opens when downloading the software, is shown in Fig. 8.
Launching the software opens a form that shows the data acquired from the chromatographs LHM and Selmi, tools to change the file with the data acquired from the chromatographs and to display the chromatograms in the graphical form. In addition, this form contains a field for entering the flow rates of CO and H2 at the inlet to the reactor in the dimensionality of ml/min, and a button that enables the calculation operation.
After pressing the button "Start calculation", a software module would calculate the amount of the derived hydrocarbon products, concentration, and would determine the reaction rate constants. Next, the program launches the form "Form2" to display the results of calculations (Fig. 9).
The window that appears in the upper left corner displays the calculated amounts of H2, CO and CH4, at the outlet from the reactor (relative to the loop of the LHM chromatograph, to which, in order to analyze, we take the sample of products formed as a result of the reaction. The total volume of the loop is 4.5 ml). In addition, the window displays molar concentrations of H2, CO and CH4, calculated per a mole of a substance, per a mole of the total amount of substances that exited the reactor.
In addition, the window displays calculation results on the amount, concentration, and constants of the formation rate of hydrocarbon products in the Fischer-Tropsch process.
The right part of the window that contains results of the calculations shows the distribution diagram of the amount of created hydrocarbon products, depending on the number of carbon atoms in molecules.
In addition, the window with the results of calculations has 2 buttons: "Concentration of reaction products dependent on time", which opens a window shown in Fig. 10, and "Concentration of CO and H2 depending on time", which opens a window shown in Fig. 11.
Main Довдоа Вих1д
Додатков! дан для розрахунку Швидк1сть потоку СО на вход! в реактор
Швидкютъ потоку Н2на вход в реактор 30 мл/хв
Запусти ти розрахунки
БД Л ХМ
D:\DB\LHM_t_300_(1).txt Вщкрита
Time
U
0 1E-05
0.531 1E-05
1.063 1E-05
1.594 1E-05
2.125 1E-05
2,656 1E-05
3.188 1E-05
3.719 2E-05
Вщобразити графмно
БД Selmi
| D:\DB\Selmi_t_300J1).txt | В1дкрита
| Time U /s
0 7E-05 V
1.5 7E-05
2.766 0,00011
4.281 0.00011
5.531 4E-05
6.797 0.0001
8.563 0.00017
10,063 0,00016
-
Вщобразити граФ1чно
Fig. 8. Main software window
Fig. 9. Window that displays calculation results
Fig. 10. Dependence of concentration of carbohydrate reaction products on time
Fig. 11. Dependence of the TO and ^ concentration on time
The result of the conducted experiments and calculation is the derived values for rate constants under different conditions of conducting the Fischer-Tropsch reaction. Estimation of the adequacy of the data obtained was performed by calculating the relative error e.
The first experiment: the flow rate of CO is 10 ml/min; the flow rate of H2 is 30 ml/min; temperature in the reactor is 300 °C. The results of calculations are given in Table 2.
The second experiment: the flow rate of CO is 20 ml/min; the flow rate of H2 is 60 ml/min; temperature in the reactor is 300 °C. The results of calculations are given in Table 3.
Table 3
Calculated data for the second experiment
Table 2
Calculated data for the first experiment
i ki Ci Error e, %
Experiment Calculation
1 4.070E-6 8.43E-05 8.22E-05 2.51
2 1.950E-7 1.08E-05 1.05E-05 2.47
3 4.470E-8 6.61E-06 6.44E-06 2.55
4 9.250E-9 3.66E-06 3.56E-06 2.74
5 8.340E-10 8.81E-07 8.57E-07 2.68
6 2.770E-10 7.81E-07 7.60E-07 2.75
7 5.280E-11 3.98E-07 3.87E-07 2.84
i ki Ci Error e, %
Experiment Calculation
1 9.02E-07 3.58E-05 3.49E-05 2.38
2 1.66E-08 3.21E-06 3.13E-06 2.52
3 2.18E-09 2.04E-06 1.99E-06 2.29
4 2.37E-10 1.08E-06 1.06E-06 2.15
5 9.61E-12 2.13E-07 2.08E-07 2.39
6 1.56E-12 1.68E-07 1.64E-07 2.50
7 1.61E-13 8.44E-08 8.22E-08 2.61
The third experiment: the flow rate of CO is 10 ml/min; the flow rate of H2 is 20 ml/min; temperature in the reactor is 300 °C. The results of calculations are given in Table 4.
Table 4
Calculated data for the third experiment
i ki Ci Error £, %
Experiment Calculation
1 1.820 E-6 3.72E-05 3.63E-05 2.40
2 7.330 E-8 3.95E-06 3.85E-06 2.43
3 1.860 E-8 2.66E-06 2.59E-06 2.63
4 4.150 E-9 1.56E-06 1.52E-06 2.49
5 3.710 E-10 3.69E-07 3.60E-07 2.47
6 1.460 E-10 3.84E-07 3.74E-07 2.55
7 2.720 E-11 1.89E-07 1.84E-07 2.59
The fourth experiment: the flow rate of CO is 10 ml/min; the flow rate of H2 is 30 ml/min; temperature in the reactor is 250 °C. The results of calculations are given in Table 5.
Table 5
Calculated data for the fourth experiment
i ki Ci Error £, %
Experiment Calculation
1 8.290 E-9 3.08E-07 3.00E-07 2.60
2 2.850 E-10 4.72E-08 4.60E-08 2.54
3 4.410 E-11 3.27E-08 3.19E-08 2.45
4 1.460 E-11 4.84E-08 4.72E-08 2.48
5 6.360 E-13 9.42E-09 9.20E-09 2.34
6 1.260 E-13 8.37E-09 8.20E-09 2.03
7 3.000 E-14 8.87E-09 8.70E-09 1.92
The results of calculations show that the relative error of the calculations is within 2...3 %, indicating the adequacy of the proposed model for calculating the reaction rate constants.
7. Discussion of results of using a mathematical model for calculating the rate constants for a system of the Fischer-Tropsch reactions
Using the developed software module, we calculated reaction rate constants of the Fischer-Tropsch process (that is, we resolved the inverse problem of chemical kinetics for the Fischer-Tropsch process), which proceeded in the reactor
under an isothermal mode. In order to analyze and estimate the data obtained, we also solved a direct problem of chemical kinetics.
After analyzing the data acquired, we can see that the relative error is within 2...3 %, indicating the adequacy of the suggested model for solving the inverse problems of chemical kinetics. Therefore, we can attest that a given model for the calculation of rate constants could be used to study the Fischer-Tropsch process.
However, it should also be noted that the calculated values for rate constants will be different for a different quantity (mass or contact area) of the catalyst, which is why further research and description of the Fischer-Tropsch process should take this factor into consideration.
8. Conclusions
1. We have analyzed a mathematical model of the Fischer-Tropsch reaction kinetics. To find the rate constants of the Fischer-Tropsch chemical reactions, we constructed dependences for the calculation of constants and developed the algorithm for solving the inverse problem of kinetics. The numerical values for constants that we derived make it possible to pass over to modeling the reactor of the FT-syn-thesis. To calculate the rate constants, one should know the concentration of the mixture of reaction gases.
2. We studied experimentally, at the laboratory installation, the Fischer-Tropsch process on cobalt catalysts. We acquired the LHM and Selmi chromatograms for calculating the concentrations of a mixture of gases. It is shown that the catalyst, obtained by the method of impregnation, demonstrated a higher activity, larger by an order of magnitude than the monodispersed catalyst.
3. We have developed a software module in the programming environment MS Visual Studio 2017 in the programming language C# using the .NET Framework v4.6 technologies, for calculating the kinetics and for finding the reaction rate constants for the Fischer-Tropsch process.
4. We have calculated rate constants for the Fischer-Tropsch reactions based on data from four experiments at different flow rates of carbon monoxide and hydrogen and different temperature in the reactor. The relative error of calculations is within 2...3 %, indicating the adequacy of the proposed model.
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