Kinetic modeling of the biodiesel production process using neem seed oil: An alternative to petroleum-diesel European Journal of Chemistry 12 (3) (2021) 242-247 European Journal of Chemistry ISSN 2153-2249 (Print) / ISSN 2153-2257 (Online) – Copyright © 2021 The Authors – Atlanta Publishing House LLC – Printed in the USA. This work is published and licensed by Atlanta Publishing House LLC – CC BY NC – Some Rights Reserved. https://dx.doi.org/10.5155/eurjchem.12.3.242-247.2085 European Journal of Chemistry View Journal Online View Article Online Kinetic modeling of the biodiesel production process using neem seed oil: An alternative to petroleum-diesel Toyese Oyegoke * and Kazeem Ajadi Ibraheem Chemical Engineering Department, Faculty of Engineering, Ahmadu Bello University, Zaria 234, Nigeria oyegoketoyese@gmail.com (T.O.), kazeemolawale634@gmail.com (K.A.I.) * Corresponding author at: Chemical Engineering Department, Faculty of Engineering, Ahmadu Bello University, Zaria 234, Nigeria. e-mail: oyegoketoyese@gmail.com (T. Oyegoke). 10.5155/eurjchem.12.3.242-247.2085 Received: 25 January 2021 Received in revised form: 31 March 2021 Accepted: 17 April 2021 Published online: 30 September 2021 Printed: 30 September 2021 Promoting the green technology campaign that would actualize a biorefinery establishment and would promote cleaner fuel production and air in our environment. This study carried out kinetics studies of biodiesel production over a mixed oxide, Ca-Mg-O catalyst, providing relevant kinetics parameters. This study indicated that biodiesel production is a zero-order reaction, a process independent of the concentration. The results obtained from this study confirm the activation energy, Ea, of the reaction to be 406.53 J/mol, while the pre- exponential factor A was found to be 0.01618 1/min (or 0.9 1/h). Other are kinetics models that were developed for the prediction of the reaction kinetics for the production process is also reported in this study. The findings reported in this study would go a long way to facilitate the modeling, simulation, and design of the biodiesel production process. Biofuel Kinetics Catalysis Biodiesel Renewable energy Reaction engineering Cite this: Eur. J. Chem. 2021, 12(3), 242-247 Journal website: www.eurjchem.com 1. Introduction Biodiesel, an example of biofuels [1-7] which is well known as an alternative petroleum diesel fuel [8], which is produced from the use of batteries, that is, renewable biological sources like algae, plant oils (neem seed oil, sunflower, soybeans, and many others) and animal fats [7,9,10]. Edible feedstocks are primarily discouraged in biofuel production, while nonedible oil like jatropha oil, neem seed oil, and others are promoted. This fuel category is well known for being non-toxic and biodegradable, which has been tested and confirmed to environmentally friendly due to its low emissions [7,11-15]. These features of biodiesel have attracted many attentions toward the promotion of fuels while discouraging the use of fossil fuels such as petroleum diesel, which is mainly used presently as a tool of combating the global warming effect [16,17] caused by the carbon monoxides [18-20] release from the incomplete combustion of fossil fuels and other health- related issues [20,21]. Research carried out so far has indicated that in biodiesel production, a heterogeneous catalyst has always been found to be highly preferred in comparison to homogeneous catalysts due to its effectiveness and easy separation steps for both products and catalysts, eliminate quenching process, and offer conditions for the continuous production system [7,9,22]. In recent studies, nanoparticles' use is significantly gaining greater attention in its use as a heterogeneous catalyst for biodiesel production, which has been observed to have been increasing rapidly. Some of the other studies include Zewude [8], obtained 92.8% yield for the use of neem oil and Na2O-CaO; Abbah [23] obtained 94% yield from the use of neem seed oil and KOH (homogenous catalyst); Dianursanti et al. [24] obtained a yield of 36.8% for the use of CuO/Zeolite and Chlorella Vulgaris oil; Ribwar [25] obtained 83% for the use of waste cooking oil/chicken fat and KOH (homogenous catalyst); Jabiver et al. [26] work which obtained 73% yield for the use of soybean and CaO-ZnO; Ajala et al. [27] obtained 98.7% yield for the use of palm kernel oil and dolomite as the oil and catalyst (or reaction enhancer) respectively. Other works that employed biocatalysts like Istiningrum et al. [28] obtained 81.2% yield in biodiesel production via waste cooking oil and lipase. To further investigate the production of biodiesel, a recent report by Ibraheem et al. [19] unveiled the effect of reaction time and temperature on a biodiesel yield in presences of Ca-Mg-O, where the highest yield (96.4%) was obtained at 70 °C, 60 min, 500 rpm, 6:1 g methanol-to-oil ratio, and 1% w:w catalyst. ABSTRACT RESEARCH ARTICLE KEYWORDS https://dx.doi.org/10.5155/eurjchem.12.3.242-247.2085 https://www.eurjchem.com/ https://dx.doi.org/10.5155/eurjchem.12.3.242-247.2085 mailto:oyegoketoyese@gmail.com mailto:kazeemolawale634@gmail.com mailto:oyegoketoyese@gmail.com http://www.eurjchem.com/ https://crossmark.crossref.org/dialog/?doi=10.5155/eurjchem.12.3.242-247.2085&domain=pdf&date_stamp=2021-09-30 Oyegoke and Ibraheem / European Journal of Chemistry 12 (3) (2021) 242-247 243 2021 – European Journal of Chemistry – CC BY NC – DOI: 10.5155/eurjchem.12.3.242-247.2085 Table 1. Several orders of reaction kinetics models [31]. Kinetic model Rate constant, ko (1/min) Reaction order, n 𝐶𝐶𝑎𝑎𝑎𝑎𝑋𝑋 = 𝑘𝑘𝑘𝑘 𝑘𝑘 𝐶𝐶𝑎𝑎𝑎𝑎 Zeroth 𝑙𝑙𝑙𝑙 � 1 1 − 𝑋𝑋 � = 𝑘𝑘𝑘𝑘 𝑘𝑘 First 1 𝐶𝐶𝑎𝑎𝑎𝑎 � 𝑋𝑋 1 − 𝑋𝑋 � = 𝑘𝑘𝑘𝑘 𝑘𝑘(𝐶𝐶𝑎𝑎𝑎𝑎) Second A number of the previous studies have focused mainly on production optimization or effect/parametric studies, and only a few studies give attention to the study of reaction kinetics and the modeling of the kinetics involved in biodiesel production. This understanding has motivated this present study to explore the use of reaction kinetics principles in providing a better insight into biodiesel production from neem-seed oil in the presence of mixed oxide (Ca-Mg-O) through the provision of relevant kinetic parameters and models. In this study, production was accounted for the yield obtainable across different time intervals (50 to 80 minutes) and different reaction temperatures (50 to 80 °C). 2. Experimental 2.1. Materials and reagents Methanol (99.5%, analytical grade BDH), isopropyl alcohol (99.5%, analytical grade, BDH), hydrochloric acid (95%, analytical grade BDH), potassium hydroxide (analytical grade M&B), phenolphthalein (indicator), calcium carbonate (catalyst component) and magnesium carbonate (catalyst component) were the reagents and materials employed in this study. 2.2. Synthesis of biodiesel 2.2.1. Catalyst synthesis method The mixed metal oxide catalyst was prepared by first mixing 75% (22.5 g) calcium carbonate with 25% (7.5 g) magnesium carbonate and then dissolved in 100 mL of water in a 250 mL beaker and stirred on a magnetic stirrer for 30 min without heating. The solution was filtered to remove the water and was dried in an oven at 120 °C overnight to constant weight, then calcined in a furnace at 900 °C for 90 min. The calcination temperature causes the carbonate compounds to decompose into an oxide compound, as presented in Equations (1) and (2). CaCO3 → CaO + CO2 (1) MgCO3 → MgO + CO2 (2) The mixed metal oxide catalyst was synthesized in like way. Such in situ synthesis result in an intimate contact of the CaO with the MgO during the calcination, in agreement with Javier et al. [26] report for the synthesis for CaO-ZnO. The catalyst was placed in a desiccator to avoid moisture absorption. Details on the characterization of the prepared catalyst employed in this study can find in our previous report [19]. 2.2.2. Transesterification A two-step transesterification was adopted for this study where the oil was first pretreated with the use of sulphuric acid to have the free fatty acid (FFA) reduced to 1.6±0.05 %FFA in line with the report of Bello et al. [29], Yusuf [30], and Ibraheem et al. [19] which indicates that low-FFA oil would give a relative higher biodiesel yield in a later step. In the latter method, 12 g of the pretreated oil was heated to 50 °C, and 6:1 g methanol to oil ratio with 1% w:w of the catalyst was added. The oil was pretreated to reduce the FFA present in the oil to improve the yield, in agreement with our previous study [19], where the neem oil FFA and density were reported. The stirring speed was kept at 500 rpm. The process was repeated at 60-80 °C, and time varied from 50-70 min for each temperature, leaving other parameters constant. The maximum yield of biodiesel using the expression is presented in Equation (3). X = Nb No (3) Nb is the amount of biodiesel produced, and No is the amount of oil used. The results obtained were recorded and tabulated. 2.3. Kinetic modeling for the biodiesel production In modeling the kinetics of the biodiesel reaction, the experimentally collected data were fitted into several set of kinetic models, which include the zeroth, first, and second- order models, which were adopted from literature reports about the different order of reaction kinetic models and the summary of the details regarding the kinetic models are presented in Table 1. With the use of computational tools, the experimental data were fitted using a linear regression analysis approach alongside the assessment of the models' fitness accuracy were investigated via the use of scattered plots and R- square values. 2.3.1. Reaction order and rate constant determination The reaction order and rate constants were determined for different temperature ranges using the linear regression model (presented in Equation (4)) to fit the experimental data into the respective kinetic model to assess its fitness for the biodiesel production kinetics. 𝑦𝑦 = m𝑥𝑥 + c (4) To be specific, for the reaction studied, m denoted the slope or gradient, while c denotes the intercept that is constrained to be zero since the set of reaction kinetic models lacks intercepts. Summary of the respective parameters employed in the study for the regression analysis for the reaction kinetic models is presented in Table 2, where the axes (i.e., y and x) and slope (i.e., m) notations were presented. 2.3.2. Determination of activation energy and kinetic rate model The set of slopes, temperature, and R-square values collected were used in the computation of the reaction activation, Ea energy, using the Arrhenius equation (in Equation (5)). The model was linearly (as presented in Equation (4)) fitted using regression analysis where the c intercept of the model was taken to be a nonzero value. According to the literature [32-34]: 𝑘𝑘 = A exp �− 𝐸𝐸a RT � (5) 244 Oyegoke and Ibraheem / European Journal of Chemistry 12 (3) (2021) 242-247 2021 – European Journal of Chemistry – CC BY NC – DOI: 10.5155/eurjchem.12.3.242-247.2085 Table 2. Regression model parameter relation with the reaction kinetics models. Reaction order, n Model y x m c Zeroth 𝑋𝑋 = 𝑘𝑘 𝐶𝐶𝑎𝑎𝑎𝑎 𝑘𝑘 𝑋𝑋 𝑘𝑘 𝑘𝑘 𝐶𝐶𝑎𝑎𝑎𝑎 0 First 𝑙𝑙𝑙𝑙 � 1 1 − 𝑋𝑋 � = 𝑘𝑘𝑘𝑘 𝑙𝑙𝑙𝑙 � 1 1 − 𝑋𝑋 � 𝑘𝑘 𝑘𝑘 0 Second � 𝑋𝑋 1 − 𝑋𝑋 � = 𝑘𝑘𝑘𝑘(𝐶𝐶𝑎𝑎𝑎𝑎) � 𝑋𝑋 1 − 𝑋𝑋 � 𝑘𝑘 𝑘𝑘(𝐶𝐶𝑎𝑎𝑎𝑎) 0 Table 3. Results of biodiesel yield obtained from the experiment. t (min) X (T = 50 °C) X (T = 60 °C) X (T = 70 °C) X (T = 80 °C) 50 0.9180 0.8875 0.9250 0.9530 60 0.9380 0.9400 0.9640 0.9450 70 0.9380 0.9540 0.9150 0.9380 80 0.9170 0.9570 0.9420 0.9460 Table 4. Kinetic modeling via the use of a fitting model. T (°C) t (min) 1st Order, X 2nd Order, ln[1/(1-X)] 3rd Order, X/(1-X) T1 = 50 50 0.9180 2.5010 11.1951 T1 = 50 60 0.9380 2.7806 15.1290 T1 = 50 70 0.9380 2.7806 15.1290 T1 = 50 80 0.9170 2.4889 11.0482 T2 = 60 50 0.8875 2.1848 7.8889 T2 = 60 60 0.9400 2.8134 15.6667 T2 = 60 70 0.9540 3.0791 20.7391 T2 = 60 80 0.9570 3.1466 22.2558 T3 = 70 50 0.9250 2.5903 12.3333 T3 = 70 60 0.9640 3.3242 26.7778 T3 = 70 70 0.9150 2.4651 10.7647 T3 = 70 80 0.9420 2.8473 16.2414 T4 = 80 50 0.9530 3.0576 20.2766 T4 = 80 60 0.9450 2.9004 17.1818 T4 = 80 70 0.9380 2.7806 15.1290 T4 = 80 80 0.9460 2.9188 17.5185 ln 𝑘𝑘 = ln𝐴𝐴 – 𝐸𝐸a R �1 T � (6) 𝐸𝐸a = −d(ln 𝑘𝑘) d� 1 RT� = −Rd(ln 𝑘𝑘) d�1T� = −𝑅𝑅(𝑠𝑠𝑙𝑙𝑠𝑠𝑠𝑠𝑠𝑠) (7) 𝐴𝐴 = exp(intercept) (8) where k = Rate constant, T = Reaction temperature, A = Pre- exponential factor, and R = Gas constant (8.3142 J/mol/K). In the regression analysis, the ln k and 1/T were modeled as the vertical and horizontal axis, respectively, where the slope, m represents -Ea/R, while the intercept, c represents ln A in the analysis. The R-square values for the model were also assessed. A kinetic rate model is later modeled after using the results obtained for the rate constant model, k, and the reaction activation energy, Ea. 3. Results and discussions 3.1. Reaction order and rate constants analysis The biodiesel yield results across different time and temperature ranges are presented in Table 3, while the other relevant expressions for the computation of the rate constants and the determination of reaction orders were presented in Table 4. Table 4 presents the relevant parameters used to represent the scattered plot used to investigate the zeroth, first, and second-order reactions in the search for order that best fit the experiment phenomena. In all orders, the horizontal axis was presented as reaction time (t), while the vertical axis was presented as X, ln[1/(1-X)], and X/(1-X) for the zeroth, first and second-order models, respectively in line with the method presented in Table 2. 3.2. Rate constants for different temperature ranges The rate constant for different temperatures from 50 to 80 °C using the scattered plot as presented in Table 5, where the slope (m) was used to compute the rate constant for each temperature, was collected alongside the R-square values. Findings from the results obtained for the rate constant at the different reaction temperatures ranging from 323 to 353 K indicated that all model orders showed a good R-square value, where the average R-square values were reported to be 97.3, 97.1, and 92.5 % for the zeroth, first, and second-order model indicating the zeroth-order displayed a better agreement with the experiment data employed in the modeling of the reaction. Moreover, the rate constant (i.e., ko = slope) was seen to generally increases as the reaction temperature rises, showing that there exists a direct relationship between the rate constant (i.e., ko = slope) and reaction temperature for the zeroth reac- tion order, unlike other higher reaction order (first and second) which indicated a rise and fall at a specific temperature (333 and 343 K) across the range employed in this study evident in Tables 5 and 6. In a nutshell, the analysis of temperature effects confirms the use of zeroth reaction order for the biodiesel production studied to use neem seed oil and Ca-Mg-O catalyst. The order obtained for this process was found to be similar to the report of Mamat [35] and Valenga et al. [36] for the use of Waste- Cooking-Oil/CaO and Moringa-Leave-Waste/KOH (homoge- neous), respectively, following a zeroth-order reaction. However, the results were different from those reported in other literature [37,38] for the use of cottonseed oil/CaO and Aegyptiaca Oil/NaOH (homogeneous catalyst) as second order and first order, respectively. 3.3. Results for the computation of activation energy The parameter employed in determining the reaction activation energy in Table 6, while the results obtained from the analysis were presented in Table 7 and Figure 1. Table 6 shows where k1 = k/Cao, k2 = k, and k3 = kCao is zeroth, first, and second-order rate constants. Oyegoke and Ibraheem / European Journal of Chemistry 12 (3) (2021) 242-247 245 2021 – European Journal of Chemistry – CC BY NC – DOI: 10.5155/eurjchem.12.3.242-247.2085 Table 5. The kinetic plot’s R-square value, slopes, and intercepts at varying temperatures. Temperature Reaction order, n Zeroth - ko = k/Cao = m, n = 0 First - ko = k = m, n = 1 Second - k3 = kCao = m, n = 2 T (°C) T (K) R-square Slope m = k1 R-square Slope m = k2 R-square Slope m = k3 50.00 323.15 0.9710 0.0139 0.9679 0.0394 0.9479 0.1960 60.00 333.15 0.9793 0.0140 0.9954 0.0428 0.9719 0.2625 70.00 343.15 0.9710 0.0140 0.9569 0.0424 0.8415 0.2458 80.00 353.15 0.9701 0.0141 0.9633 0.0434 0.9391 0.2589 Average R-square 0.9729 - 0.9709 - 0.9251 - Table 6. Activation energy and pre-exponential factor analysis where the rate constant, ko in 1/min. T (K) 1/T (1/K) k1 k2 k3 ln k1 ln k2 ln k3 323.15 0.003095 0.0139 0.0394 0.1960 -4.27587 -3.23399 -1.62964 333.15 0.003002 0.0140 0.0428 0.2625 -4.26870 -3.15122 -1.33750 343.15 0.002914 0.0140 0.0424 0.2458 -4.26870 -3.16061 -1.40324 353.15 0.002832 0.0141 0.0434 0.2589 -4.26158 -3.13730 -1.35131 Table 7. Results of activation energy, Ea and preexponential factor, A. Description Reaction order Zeroth, n=0 First, n=1 Second, n=2 Slope = (-Ea/R) -48.896 -324.250 -893.910 Intercept = ln A -4.1240 -2.2108 1.2160 R-square 0.8990 0.7207 0.5548 Ea (J/mol) = (-slope*R) 406.5311 2695.879 7432.147 A (1/min) = exp(intercept) 0.01618 0.109613 3.373666 Figure 1. A plot for the computation of activation energy, Ea, and preexponential factor, A. Moreover, the reaction's activation energy was therefore confirmed to be 406.53 J/mol, while the pre-exponential factor was found to be 0.01618 1/min (or 0.9 1/h). Findings from literature indicated that the results obtained for the activation energy in this study were smaller than that reported as 23.2 kJ/mol for Waste-Cooking-Oil/CaO [35]; 127.7 kJ/mol for cottonseed oil/CaO [37]; and 242.1 kJ/mol for Moringa-Leave- Waste/KOH [36]. Furthermore, the Arrhenius model for the rate constant prediction in line with Equation (5) can be written thus: 𝑘𝑘o = 0.01618exp �− 406.5311 RT � in 1/min (9) Recall that ko (general form) is expressed in per second (Table 2), where k is the specific rate constant for the reaction whose relationship as presented in Table 2 were represented as: 𝑘𝑘o = 𝑘𝑘 Cao (Zeroth order) (10) 𝑘𝑘o = 𝑘𝑘 (First order) (11) 𝑘𝑘o = 𝑘𝑘Cao (Second order) (12) Re-expressing the above expression in Equation (10) to (12) to make the specific rate constant subject of the kinetic rate constant expression result into: 𝑘𝑘 = 𝑘𝑘oCao (Zeroth order) (13) 𝑘𝑘 = 𝑘𝑘o (First order) (14) 𝑘𝑘 = 𝑘𝑘o Cao (Second order) (15) Substituting Equation (9) into Equation (13) (since the zeroth-order fit best with the experimental output) to yield: 𝑘𝑘 = 0.01618Caoexp �−406.5311 RT � in mol/(m3/min) (16) Using Cao = 1 mol/m3, Equation (16) becomes: 𝑘𝑘 = 0.01618exp �−406.5311 RT � in mol/(m3/min) (17) In the rate constant expression, Cao is the initial concentration of the feed (oil), R is 8.3142 J/mol/K, T is the reaction temperature in K, and k is the reaction specific rate constant (zero-order reaction) expressed in mol/(m3.s), which were found to agree with the literature [32-34,36,37]. y = -48.829x - 4.1241 R² = 0.8987 y = -323.88x - 2.2119 R² = 0.7206 y = -892.99x + 1.2135 R² = 0.5548 -4.5 -4.0 -3.5 -3.0 -2.5 -2.0 -1.5 -1.0 -0.5 0.0 0.00280 0.00285 0.00290 0.00295 0.00300 0.00305 0.00310 0.00315 ln (k ) 1/T (1/K) ln k1 ln k2 ln k3 Linear (ln k1) Linear (ln k2) Linear (ln k3) 246 Oyegoke and Ibraheem / European Journal of Chemistry 12 (3) (2021) 242-247 2021 – European Journal of Chemistry – CC BY NC – DOI: 10.5155/eurjchem.12.3.242-247.2085 3.4. Kinetic rate model In modeling the biodiesel production rate model, the rate of biodiesel production can be generally be modeled to be in the form: dCa dt = 𝑘𝑘Can (18) Employing the results obtained for the reaction order, the reaction order (n = 0, 𝐶𝐶𝑎𝑎0 = 1) can be substituted into Equation (18) to give us a zeroth-order reaction rate model: dCa dt = 𝑘𝑘Ca0 = 𝑘𝑘 (19) The above model expression developed for the zeroth order-based reaction was found to be in line with relevant related works in the literature. The kinetic rate model can be represented by substituting the development rate constant expression in Equation (16) into (19) to give us: dCa dt = 0.01618C𝑎𝑎𝑎𝑎exp �− 406.5311 RT � in mol/(m3/min) (20) 1 C𝑎𝑎𝑎𝑎 dC𝑎𝑎 dt = 0.01618exp �− 406.5311 RT � in mol/(m3/min) (21) dX dt = 0.01618exp �− 406.5311 RT � in mol/(m3/min) (22) where the initial concentration (i.e., Cao) is expressed in mol/m3 in the form of Equation (20), while Equation (22) expresses the concentration as a normalized variable (i.e., dCa/Cao = dX) where all concentrations are expressed as a fraction of the initial concentration (i.e., Cao). 4. Conclusions The exploration of reaction kinetics principles towards providing a better insight into biodiesel production from neem- seed oil in the presence of mixed oxide (Ca-Mg-O) through the provision of relevant kinetic parameters and models was successfully carried out. Therefore, the study’s findings indicate that the analysis of temperature effects confirms the use of zeroth reaction order for the biodiesel production studied with the use of neem seed oil and Ca-Mg-O catalyst. Moreover, the activation energy, Ea of the reaction, was therefore confirmed to be 406.53 J/mol, while the preexponential factor, A, was found to be 0.01618 1/min (or 0.9 1/h). The kinetic parameters are computed together with the reaction kinetics models developed, which would fit nicely into prediction provisions and would go a long way to facilitate the modeling, simulation, and design of the biodiesel production process through the relevant kinetic data and model reported in this study. Disclosure statement Conflict of interests: The authors declare that they have no conflict of interest. Author contributions: All authors contributed equally to this work. Ethical approval: All ethical guidelines have been adhered to. 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The full terms of this license are available at http://www.eurjchem.com/index.php/eurjchem/pages/view/terms and incorporate the Creative Commons Attribution-Non Commercial (CC BY NC) (International, v4.0) License (http://creativecommons.org/licenses/by-nc/4.0). By accessing the work, you hereby accept the Terms. This is an open access article distributed under the terms and conditions of the CC BY NC License, which permits unrestricted non-commercial use, distribution, and reproduction in any medium, provided the original work is properly cited without any further permission from Atlanta Publishing House LLC (European Journal of Chemistry). No use, distribution or reproduction is permitted which does not comply with these terms. Permissions for commercial use of this work beyond the scope of the License (http://www.eurjchem.com/index.php/eurjchem/pages/view/terms) are administered by Atlanta Publishing House LLC (European Journal of Chemistry). http://161.139.21.153/index.php/FYP/article/viewFile%20/24/pdf http://161.139.21.153/index.php/FYP/article/viewFile%20/24/pdf http://www.eurjchem.com/index.php/eurjchem/pages/view/terms http://creativecommons.org/licenses/by-nc/4.0 http://www.eurjchem.com/index.php/eurjchem/pages/view/terms 1. Introduction 2. Experimental 2.1. Materials and reagents 2.2. Synthesis of biodiesel 2.2.1. Catalyst synthesis method 2.2.2. Transesterification 2.3. Kinetic modeling for the biodiesel production 2.3.1. Reaction order and rate constant determination 2.3.2. Determination of activation energy and kinetic rate model 3. Results and discussions 3.1. Reaction order and rate constants analysis 3.2. Rate constants for different temperature ranges 3.3. Results for the computation of activation energy 3.4. Kinetic rate model 4. Conclusions Disclosure statement ORCID References PrintField10: PrintField11: PrintField12: PrintField13: PrintField14: PrintField15: PrintField20: PrintField21: PrintField22: PrintField23: PrintField24: PrintField25: