PRELIMINARY ASSESSMENT OF THE PROCESSING OF HIGH-ACIDITY FATTY MATERIALS USING SOLID CATALYSTS FOR THE OBTAINMENT OF FATTY ACID METHYL ESTERS

Abstract

This work presents the processing of a high-acidity oil through sequential reactions of esterification using montmorillonite K10 and transesterification using zinc monoglycerolate. Since these solids had not been employed along with this approach beforehand, the objective of this work is to provide a general insight of the proposed process and demonstrate its technical feasibility. In this sense, the processing of a synthetic mixture containing soybean oil and lauric acid provided a reduction of the free fatty acid content from (40.8±0.1) % to (3.1±0.4) % after the esterification reaction and a fatty acid methyl ester yield of (95.4±0.2) % was obtained after the transesterification reaction. As compared to traditional homogeneous catalysts, the solid catalysts employed in this work require higher reaction times to achieve satisfactory ester yields but, on the other hand, they are less sensitive to the presence of both water and free fatty acids in the raw materials and can be easily recovered and reused. Therefore, the results accomplished may help the development of a technology for processing high-acidity fatty materials in order to obtain biodiesel, although its economic feasibility still needs a further assessment.

Keywords:
Biodiesel; Acid oil; Esterification; Montmorillonite K10; Transesterification; Zinc monglycerolate

INTRODUCTION

Biodiesel is often more expensive than diesel fuel and the main reason is the high cost of the raw materials, which may correspond to up to 88 % of the biodiesel cost (Haas, 2005). Furthermore, there is an increasing concern about food security, since the commonly used raw materials can generate a competition with the food industry (Koizumi, 2015). In this scenario, residual fatty materials draw attention due to their low cost and also because their processing might result in an environmental gain, even though these materials may contain high amounts of free fatty acids (FFA).

Throughout the refining processes of vegetable oils, several streams with different FFA contents are generated, and these values also depend on the vegetable source. Piloto-Rodriguez et al. (2014) reported the content of both FFA and triacylglycerol present in each of these fractions, named distilled fatty acids, soapstock and acid oil. In what concerns the refining of soybean oil, the FFA contents of these streams are around 40 % for the distilled fatty acids (Piloto-Rodríguez et al., 2014), while ranging between 35 % and 50 % for the soapstock, and are up to 60 % for the acid oil obtained through the acidification of the soapstock (Piloto-Rodríguez et al., 2014; Wang et al., 2007). Other interesting residual fatty materials are waste cooking oils, whose FFA contents are around 3.5 % (Otadi et al., 2011), and a lipid-rich waste material obtained from sewage sludge, whose FFA contents vary from around 15 % (Kwon et al., 2012) to values between 60 % and 70 % (Boocock et al., 1992; Olkiewicz et al., 2016).

For the use of conventional transesterification reaction catalysts, such as metal hydroxides or alkoxides, it is preferable that the FFA contents of raw materials are lower than 0.5 % (or 1 mg KOH·g^-1), although it is possible to achieve the processing of raw materials whose FFA contents are up to 5 % (Canakci and Gerpen, 2001; Mittelbach and Remschmidt, 2005). Nevertheless, it may be necessary to perform the neutralization of FFA, either by the addition of a glycerol-rich phase of a previous batch (which contains the alkaline catalyst), or by the FFA removal by distillation at high temperatures (Mittelbach and Remschmidt, 2005). Another option is to perform an esterification reaction, in which the FFA are converted to esters, but in this case the proper catalyst is sulfuric acid (Almeida et al., 2015; Encinar et al., 2011; Marchetti et al., 2011).

The aforementioned catalysts (metal hydroxides or alkoxides for transesterification reactions and sulfuric acid for esterification reactions) allow the obtainment of high ester yields, under mild reaction conditions, and require relatively low reaction times. However, the main disadvantage of their use is the difficulty of recovery for further reuse, in such a way that they must be removed from the final product through several washing steps, which also increase production costs and generate more liquid wastes (Mittelbach and Remschmidt, 2005).

On the other hand, solid catalysts have as an advantage the possibility of being easily recovered and reused in the process, while the main disadvantage is the slower reaction rate, thus requiring higher temperatures to achieve satisfactory ester yields. Moreover, solid catalysts are not as sensitive to the characteristics of poor quality raw materials as metal alkoxides or hydroxides and are not as corrosive as sulfuric acid (Mittelbach and Remschmidt, 2005). Therefore, research on alternative solid catalysts capable of processing poor-quality raw materials for biodiesel production could enable the reduction of costs of both raw materials and process operations, whilst the final product still meets the specifications required (Mendow et al., 2011).

In this context, mixed oxides, other mixed compounds (Jindapon et al., 2016), sulfated oxides (Istadi et al., 2015), zincates (Rubio-Caballero et al., 2009), and magnetic catalysts (Dantas et al., 2017) have been reported for the processing of vegetable oils and animal fats with low acid contents (Dias et al., 2012; Pasupulety et al., 2015). Other authors employed solid catalysts for the processing of raw materials with high FFA contents, such as sulfonated solids, used in reactions with materials containing FFA contents of 10 % (Fadhil et al., 2016), 15 % (Dawodu et al., 2014) and up to 43.73 % (Konwar et al., 2014), and bifunctional catalysts with both Brönsted and Lewis acid sites, used for the processing of materials with FFA contents of 1.78 % (Pan et al., 2018) and from 8.6 % to 60 % (Wang et al., 2017). Other solid catalysts such as zeolites, heteropolyacids and metal oxides have also been used, as mentioned in the review presented by Mansir et al. (2017). Finally, zinc monoglycerolate (ZnMGly), used in this work as catalyst for transesterification reactions, also presented catalytic activity regarding the processing of raw materials containing 10 % of FFA (Kwong and Yung, 2016) or even the esterification of oleic acid until a certain extent (Reinoso et al., 2014).

Hence, the main objective of this work was to provide a primary assessment of the processing of high-acidity oils using solid catalysts to obtain high contents of fatty acid methyl esters (FAME). Therefore, an approach consisting of two units with different main reactions (esterification and transesterification), represented by the block diagram shown in Fig. 1, was chosen and its technical feasibility was evaluated. Each unit has unique features, concerning the catalysts, raw materials, reactional conditions (temperature, pressure, density, viscosity, etc) and purification operations. For the development of this strategy, two solid catalysts with known catalytic activity were selected and re-tested under reaction conditions which were different than those already presented in the literature (Lisboa et al., 2014; Lisboa et al., 2013; Reinoso et al., 2014; Zatta et al., 2013).

Figure 1
Block diagram for the high-acidity fatty material processing.

Montmorillonite K10 was selected as catalyst for esterification reactions, since activated clay minerals, in general, can be very interesting catalysts for esterification reactions, as reported by several authors (Kanda et al., 2017; Neji et al., 2011; Neji et al., 2009; Pires et al., 2013; Rezende et al., 2012; Santos et al., 2016; Zatta et al., 2012a; Zatta et al., 2012b; Zatta et al., 2011). Furthermore, reports in the literature about the use of this catalyst for the processing of high-acidity oils are scarce. This solid is supplied by the manufacturer after acid and thermal activation of the montomorillonite clay mineral, resulting in a high-surface area material containing strong Brönsted and Lewis acid sites.

Additionally, the catalyst chosen for the transesterification reaction was zinc monoglycerolate, mainly because of its thermal stability, which allowed the use of this solid at higher temperatures than those employed by other authors (Lisboa et al., 2013; Reinoso et al., 2014), so as to improve the reaction evolution. The use of glycerolates (also named glyceroxides) has a close relationship with the use of oxides, since they are formed in situ during transesterification reactions due to the presence of glycerol (Kouzu et al., 2009; León-Reina et al., 2013; López Granados et al., 2010). Several authors employed calcium diglycerolate for transesterification reactions, among them Lukic et al. (2016), who also presented a review about the use of this solid (as well as calcium monoglycerolate) as catalyst towards these reactions. Other works reported the use of different metal glycerolates as catalysts for biodiesel production, such as glycerolates of potassium (Pradhan et al., 2017), lithium (Wang et al., 2015), manganese, iron, cobalt (Lau et al., 2016), calcium, strontium, barium (Lisboa et al., 2014) and zinc (Lau et al., 2016; Lisboa et al., 2014; Reinoso et al., 2014).

The reaction conditions chosen to perform this study are slightly different than those reported in previous works (Lisboa et al., 2014; Lisboa et al., 2013; Reinoso et al., 2014; Zatta et al., 2013), mainly considering the temperature range. The first block of experiments is related to the study of each reaction, while the second block is related to the processing of acid oil (FFA contents of nearly 40 %) through the coupled reactions. It is worth mentioning that an industrial process could use buffer tanks to help and adequate the acidity of the raw material to the desired range of values, avoiding oscillation and easing the reactor operation.

MATERIALS AND METHODS

Chemicals

Esterification studies were performed using montmorillonite K10 (Sigma-Aldrich, CAS number 1318-93-0) and lauric acid (Sigma-Aldrich, ≥ 98 %, CAS number 143-07-7), while transesterification reactions used refined soybean oil (Coamo) and zinc monoglycerolate previously synthesized using zinc acetate dihydrate (Sigma-Aldrich, ≥ 98 %, CAS number 5970-45-6) and glycerol (Synth, ≥ 99 %, CAS number 56-81-5), while its further purification was performed through washing steps using decarbonated distilled water and anhydrous ethanol (Neon, ≥ 99.5 %, CAS number 64-17-5). Methanol (Neon, ≥ 99.8 %, CAS number 67-56-1) was employed as the short chain alcohol for both esterification and transesterification reactions and anhydrous sodium sulfate (Vetec, ≥ 99 %, CAS number 7757-82-6) was used in the purification steps of the final products obtained.

Titration analysis was carried out using hydrated ethanol (Neon, ≥ 95.0 %, CAS number 64-17-5), sodium hydroxide (Vetec, ≥ 97 %, CAS number 1310-73-2), potassium biphthalate (Vetec, ≥ 99.5 %, CAS number 877-24-7) and phenolphthalein (Sigma-Aldrich, CAS number 77-09-8) as indicator. The gas chromatography was performed using the derivatization agent MSTFA (N-methyl-N-(trimethylsilyl) trifluoroacetamide, Sigma-Aldrich, ≥ 98.5 %, CAS number 24589-78-4), heptane (Sigma Aldrich, ≥ 99 %, CAS number 142-82-5) and the internal standards ethyl palmitate (Sigma Aldrich, ≥ 98.5 %, CAS number 628-97-7 67107) and tricaprin (Supelco, solution 8 mg mL^-1, CAS number 621-71-6). The calibration curves were obtained using methyl linoleate (Sigma-Aldrich, ≥ 98.5 %, CAS number 112-63-0), monoolein (Supelco, solution 5 mg mL^-1, CAS number 111-03-5), diolein (Supelco, solution 5 mg mL^-1, CAS number 2465-32-9) and triolein (Supelco, solution 5 mg mL^-1, CAS number 122-32-7).

All chemicals were used without any further purification.

Zinc monoglycerolate synthesis and characterization

Zinc monoglycerolate was synthesized following the reaction presented in Eq. (1), using the glycerol reflux method, as employed by Dong and Feldmann (2012). The experimental apparatus was composed of a hot plate stirrer, which provided both the heating and the magnetic stirring, and a three-neck flask as the reactor. The reactor was kept under nitrogen flow along the course of the reaction, so as to remove the other reaction product, acetic acid, and avoid zinc monoglycerolate consumption, since it is a reversible reaction.

$$\begin{array}{ccccccc}1{\left(C{H}_{3}COO\right)}_{2}Zn& +& 1C_3{H}_8{O}_3& \rightleftarrows & 1C_3{H}_6{O}_{3}Zn& +& 2C{H}_{3}COOH\\ \left(\text{zinc aectate}\right)& & \left(\text{glycerol}\right)& & \left(\text{zinc monoglycerolate}\right)& & \left(\text{acetic acid}\right)\end{array}$$ (1)

After the reaction, the solid was purified by a three-step washing procedure, the first using decarbonated distilled water and the two remaining using ethanol. The solids were vigourosly stirred with the solvents and immediatly centrifuged at 4500 rpm (~ 3600 g) for 10 min. Following the washing steps, the solid was dried in a vacuum oven at 60 °C for 24 h and kept under the form of a fine powder for its characterization through the following analyses: X-Ray Diffraction (XRD), Fourier Transform Infrared Spectroscopy (FTIR), Scanning Electron Microscopy (SEM) and Thermogravimetric Analysis (TGA/DTG).

XRD analyses were performed using a Shimadzu, XRD-7000, X-Ray diffractometer, which uses Cu_kα radiation (1.5418 Å), in the range from 3° to 40° (2θ), step of 0.02°, scanning speed of 2° min^-1, voltage of 40 kV and current of 20 mA. FTIR analyses were performed using a Bomem spectrometer, model MB100, ranging from 4000 cm^-1 to 400 cm^-1, with 4 cm^-1 of resolution, using transmission mode with accumulation of 32 scans. SEM analysis was performed using a Tescan microscope, model Vega LMU, with resolution of 3 nm. TGA/DTG analysis was performed using a Perkin-Elmer equipment, model TGA 4000, using circa 10 mg of sample, synthetic air flowing at 50 mL min^-1 and using a heating rate of 10 °C min^-1, from 30 °C to 1000 °C.

Catalytic tests

The catalytic tests were performed using a 300 mL Parr bench top mini reactor (series 4560), whose scheme is presented in Fig. 2, equipped with an electrical heater attached to a controller, in order to keep the temperature of the reaction media at the desired value. The controller also permitted setting the stirring speed and a pressure gauge attached to the reactor helped to monitor the pressure. A sampling system allowed the withdrawal of samples from inside of the reactor and the procedure was explained in details in a previous work of our research group (Kanda et al., 2017). In summary, it consisted of a tube extending near to the bottom of the reaction vessel, which allowed the sampling at chosen times of the reaction using a manually operated needle valve.

Figure 2
Experimental set-up used in this work.

As for the reaction conditions, the ranges of values were set in agreement with those of previous works (Kanda et al., 2017; Lisboa et al., 2013; Zatta et al., 2013) (even though the study by Kanda et al. (2017) was performed using ethanol, which is less reactive than methanol). The stirring speed was fixed at 500 rpm for all the reactions, since this was demonstrated to be the optimum value (Lisboa et al., 2013; Zatta et al., 2013). Both esterification and transesterification reactions were also performed in the absence of catalysts, in order to assess the effective contribution of the catalysts.

The initial time of reaction (t = 0) was set as the moment when the reaction heating was turned on. The first sample was withdrawn from the reactor as soon as the temperature reached the desired value, while the other samples were withdrawn at times of reaction that were chosen according to the type of reaction. The maximum number of samples was 6, so the amount removed from the reactor did not have an impact on the reaction evolution.

After sampling, the catalysts were separated by centrifugation at 3500 rpm for 10 min and the alcohol was removed by evaporation at 50 °C using an air-circulation oven at atmospheric pressure inside of which the samples were left for 24 h. After this treatment, the samples were analyzed properly, by titration with NaOH for the determination of FFA content and/or by gas chromatography to evaluate the contents of fatty acid methyl esters (FAME), monoacylglycerols (MAG), diacylglycerols (DAG), and triacylglycerols (TAG).

Since zinc monoglycerolate undergoes a series of transformations in the presence of a considerable amount of free fatty acids, resulting in the formation of zinc carboxylate (Reinoso et al., 2014), it was decided that this catalyst would not be tested for high values of FFA contents. Nevertheless, it was still necessary to determine the integrity of this solid after the reactions, which was achieved through XRD, FTIR and TGA analyses of the recovered solids. The degradation of zinc monoglycerolate could be verified by the presence of either zinc oxide, as a result of oxidation reactions, or zinc carboxylates, as a result of the reaction between zinc monoglycerolate and FFA.

Purification steps

The samples obtained during the reactions for the acid oil processing were prepared prior to the analyses as described earlier. However, after the last sampling of each reaction, the whole content of the reactor was subjected to purification steps which were performed according to the type of reaction, in order to remove not only the catalysts, but also by-products and, consequently, the alcohol.

At the end of the esterification reaction, the reaction medium was cooled down by the flow of fresh water through a cooling coil positioned inside the reactor, which did not allow direct contact between the hot and cold fluids, in a process that lasted around 25 min. Then, the whole content was withdrawn from the reactor and left to rest for at least 12 h to enable the catalyst to settle down. After the catalyst removal, methanol was separated by vacuum distillation and the non-volatile phase was again left to rest to assure that an insignificant amount of montmorillonite K10 would be present during the transesterification step.

As for the transesterification reaction, the same procedure for the cooling of the reaction medium was followed after the reaction was over, but the methanol removal was performed prior to the catalyst separation, since its presence appeared to limit the settling of the catalyst. After methanol removal, the occurrence of a liquid-liquid phase separation was possible, in which both glycerol and zinc monoglycerolate remained in the bottom phase. The upper phase, composed mainly of the methyl esters formed, was separated and washed three times with warm distilled water (60 °C) to ensure glycerol traces were removed and then filtered using anhydrous sodium sulfate.

FFA content analysis

The FFA content was obtained using a method presented by Rukunudin et al. (1998), adapted from the AOCS 5a-40 method. This method shows good agreement with results obtained by high-performance liquid chromatography (HPLC) (Cordeiro et al., 2012) and nuclear magnetic resonance (NMR) (Zatta et al., 2012a) and was used in several works (Cordeiro et al., 2012; Kanda et al., 2017; Santos et al., 2016; Zatta et al., 2012a). The procedure consists of the titration of the samples with a sodium hydroxide solution (0.1 mol L^-1), previously standardized with potassium biphthalate. The FFA content was determined in duplicate using Eq. (2), adapted from the literature (Rukunudin et al., 1998):

$$\text{FFA Content (\%)}=\text{100}\cdot \frac{\text{M}\cdot \text{V}\cdot \text{f}\cdot \text{C}}{\text{m}}$$ (2)

where M is the molar mass of the free fatty acid (g mol^-1), V is the volume of the NaOH solution used in the procedure (L), f is a correction factor for the NaOH solution (dimensionless), C is the molar concentration of the NaOH solution (mol L^-1), and m is the mass of the sample (g).

The conversions were calculated by the comparison of the FFA content of the raw material before the esterification reaction and that of the samples analyzed, according to Eq. (3):

$${\text{X}}_{\text{FFA}}\text{(\%)}=\text{100}\cdot \frac{\left({\text{FFA}}_0-{\text{FFA}}_{\text{i}}\right)}{{\text{FFA}}_0}$$ (3)

where X_FFA is the FFA conversion (%), FFA₀ is the FFA content before the esterification reaction (%) and FFA_i is the FFA content of the samples analyzed (%).

Gas chromatography analysis

For this analysis a Shimadzu gas chromatograph (model GC 2010 Plus) with a flame ionization detector (FID) was used. The chromatograph was equipped with a Select Biodiesel column (Agilent, 15 m x 0.32 mm x 0.10 μm) with split injection mode (1:10). Temperatures of the injector and the detector were set to 380 °C and 400 °C, respectively. The initial oven temperature was set to 50 °C and the temperature heating rate was programmed at 15 °C min^-1 until 180 °C, 7 °C min^-1 until 230 °C and 10 °C min^-1 until 380 °C, remaining at this temperature for 6 min. Helium was used as carrier gas at a flow rate of 29.2 cm³ min^-1.

The samples to be analyzed were first diluted in appropriate amounts of heptane or ethanol and a small amount of this solution was added to a vial, as well as the solution containing the internal standards (ethyl palmitate and tricaprine) and the derivatization reagent MSTFA. The final required volume was reached by the addition of heptane so that the solutions analyzed by GC had concentrations near to 1 mg mL^-1. Despite both the injection mode and the injector temperature, this procedure was based in the recommendations of the standards for quantification of FAME (EN 14103) and acylglycerols (EN 14105), in which calibration curves for the species were provided using methyl linoleate, monoolein, diolein and triolein.

The results are presented as content (mass fractions) of compounds versus time of reaction, but for comparison purposes, the processing of acid oils was evaluated through TAG conversion (X_TAG) and FAME yield (y_FAME), calculated using Eqs. (4) and (5), along with the FFA conversion (X_FFA), defined previously by Eq. (3):

$${\text{X}}_{\text{TAG}}\text{(\%)}=\text{100}\cdot \frac{\left({\text{TAG}}_{\text{0}}-{\text{TAG}}_{\text{i}}\right)}{{\text{TAG}}_0}$$ (4)

$${\text{y}}_{\text{FAME}}\text{(\%)}=\text{100}\cdot \frac{{\text{FAME}}_{\text{i}}}{\left(\text{3}\cdot {\text{TAG}}_0+\text{2}\cdot {\text{DAG}}_0+{\text{MAG}}_0+{\text{FFA}}_0\right)}$$ (5)

where X_TAG is the TAG conversion (%), y_FAME is the FAME yield (%), TAG₀, DAG₀, MAG₀ and FFA₀ are the initial number of moles of TAG, DAG, MAG and FFA, respectively, and TAG_i and FAME_i are the number of moles of TAG and FAME, respectively, of the samples analyzed.

RESULTS AND DISCUSSION

Catalyst characterization

An extensive characterization of the as-received montmorillonite K10 was reported in a previous work from our research group (Kanda et al., 2017), including XRD and FTIR analyses, as well as information regarding the acidic sites and textural properties. The material was not analyzed after the reactions performed in this work, since acid activated clay minerals tend to be stable compounds that can be reused for several reaction cycles (Santos et al., 2016; Zatta et al., 2013; Zatta et al., 2012a).

As for the zinc monoglycerolate, Lisboa et al. (2013) reported the possibility that this catalyst could be reused three times, while Reinoso et al. (2014) performed five catalytic cycles with this solid without its deactivation. In this work, three different batches were prepared and after the X-Ray Diffraction (XRD) analysis confirmed the formation of the desired compound, as shown in Fig. A.1 (Appendix), the batches were mixed together. The reaction conditions are presented in Table 1 and the time of reaction was fixed at 2 h. Therefore, the zinc glycerolate used for the transesterification reactions was composed of the solids of these three batches, whose mass percentages were 85.5 % of batch #1, 7.7 % of batch #2 and 6.8 % of batch #3.

Table 1
Reaction conditions used for the synthesis of zinc monoglycerolate.

Batch #	MR	T (°C)
1	46	109 - 119
2	29a	85 - 93
3	30a	97 - 101
4b	-	-

• MR = Molar Ratio glycerol:zinc acetate.
• a Theoretical values. The pore volume of the silica supports might have restricted the access of glycerol to the zinc acetate impregnated inside the pores.
• b Obtained by blending batches #1, #2 and #3

The Bragg’s Law equation was used to determine the basal distance, which for batch #1 was 8.10 Å, as identified by the basal peak around 10.92° (2θ), while these values for batch #2 were 8.05 Å and 10.99° (2θ) and, for batch #3, 8.03 Å and 11.01° (2θ), respectively. These results are nearly identical to the values reported by Lisboa et al. (2013). The main peaks observed for the XRD pattern of zinc monoglycerolate crystals are around 10° (100), 17° (011), 20° (111) and 28° (211) (2θ, Cu_kα radiation).

Batches #2 and #3 were obtained after an attempt to perform the synthesis of supported zinc monoglycerolate using different types of silica supports (these solids were obtained as a residue, outside the supports). SEM analysis, presented in Figs. 3.A-D, confirmed the platelet-like morphology of the zinc monoglycerolate particles obtained, which is typical of layered materials and was also observed by Reinoso et al. (2014). However, the dimensions varied according to the conditions used during each synthesis and, as a result of the mixture of different batches, the SEM image of batch #4 (Fig. 3.D) indicated the presence of heterogeneous particle sizes. As long as this batch was used for all the transesterification reactions, including those performed for the acid oil processing, the comparison of the obtained results was not affected by this feature.

Figure 3
SEM images of zinc monoglycerolate: (A) batch #1, (B) batch #2, (C) batch #3, and (D) batch #4.

Moreover, batch #1 was analyzed by FTIR (this analysis will be further presented) and batch #4 was analyzed by TGA (Fig. A.2 - Appendix), confirming the formation of the desired compound. According to the thermal analysis, the first thermal event, related to water removal (dehydration), presented an onset temperature of 110 °C and 1^st derivative peak temperature of 135 °C, resulting in a mass loss of 6.0 % (which can be attributed to the humidity of the material). The second thermal event, related to the zinc monoglycerolate oxidation to zinc oxide, presented an onset temperature of 360 °C and 1^st derivative peak temperature of 375 °C. The amount of zinc oxide obtained at the end of the analysis corresponded to 50.3 % of the initial mass, on a dry basis. This result is very close to the theoretical value expected for zinc monoglycerolate (Zn(C₃H₆O₃)), which is 52.3 % (deviation of 3.8 %).

Methyl esterification of lauric acid

The reaction conditions employed in the assessment of lauric acid esterification using methanol and montmorillonite K10 as catalyst are presented in Table 2 and were chosen as such due to the achievement of the best results, as reported by Kanda et al. (2017) for the ethylic route. In this study, 6 esterification reactions were performed and each reaction provided 6 samples, resulting in a total of 36 experimental data. In this case, the molar ratio (MR) is referred to the number of moles of methanol for each mole of FFA, while the catalyst load (Cat.) represents the mass of montmorillonite K10 used for each 100 g of FFA.

Table 2
Experimental conditions employed in the methyl esterification of lauric acid catalyzed by montmorillonite K10.

Reaction	T (°C)	MR	Cat. (%)
E1	140	6.06:1	12.03
E2	160	6.18:1	12.01
E3	180	5.97:1	11.75
E4	140	6.01:1	0
E5	160	6.10:1	0
E6	180	6.01:1	0

• MR = Molar Ratio methanol:lauric acid; Cat. = Catalyst load expressed as g of catalyst per 100 g of lauric acid.

The results obtained are presented in terms of FFA conversion versus time of reaction in Fig. 4. It is possible to infer that the reaction may occur if enough heat is provided to the system, although the catalyst was responsible for improving the reaction rates. For all cases, the maximum time of reaction evaluated was 6 h and the higher conversion obtained for reactions performed without catalyst was 90.6 % at 180 °C. As for the montmorillonite K10-catalyzed reactions, at 140 °C the FFA conversion was 95.0 % after 6 h, while at 160 °C the conversion reached 95.4 % after 90 min and at 180 °C, the conversion reached 95.0 % after 60 min. These values around 95 % seem to refer to the equilibrium conversion, since it was not possible to achieve higher conversions, even for longer reaction times.

Figure 4
Comparison of the results obtained for the methyl esterification of lauric acid (Cat. ≈ 12 % and MR ≈ 6:1). Symbols represent experimental data obtained for reactions without catalyst (empty symbols) and using montmorillonite K10 (full symbols and asterisk), at T = 140 °C (triangles, E1 and E4), T = 160 °C (squares, E2 and E5) and T = 180 °C (asterisks and circles, E3 and E6). Dotted lines are a guide for the eye.

The effect of molar ratio on the methyl esterification of lauric acid catalyzed by montmorillonite K10 was evaluated for reactions performed at 180 °C. The amount of catalyst is usually reported as the relation between the mass of catalyst and the mass of FFA. However, since the volume of the reaction medium was required to be kept in a certain range (so that the samples withdrawn from the reaction vessel did not interfere in the results), when different molar ratios are tested, the amount of FFA also varies, which affects the amount of catalyst. Therefore, to avoid the catalyst dilution, its concentration was kept constant and is reported as g of catalyst per L of reaction media.

The reaction conditions are presented in Table 3, while the results obtained, presented in Fig. 5, allowed the observation of the equilibrium conversion displacement due to the use of excess alcohol. Using a MR methanol:FFA near to 3:1, the conversion could not exceed 91.8 %, while for MR near to 6:1 and higher (the other values tested in this work were around 12:1 and 50:1), maximum values are around 95 % and cannot be surpassed. On the other hand, the equilibrium was reached faster when higher amounts of methanol were used. Under the conditions tested in this work (T = 180°C and Cat. ≈ 40 g L^-1), all MR except near 3:1 provided nearly the same values of conversion after 30 min of reaction (or around 75 min, if the heating of the reaction media is considered).

Table 3
Experimental conditions employed to evaluate the effect of molar ratio on the methyl esterification of lauric acid catalyzed by montmorillonite K10.

Reaction	T (°C)	MR	Cat. (g L-1)
E7	180	3.05	39.7
E8	180	5.97	40.7
E9	180	11.94	40.3
E10	180	49.79	39.8

• MR = Molar Ratio methanol:lauric acid; Cat. = Catalyst load expressed as g of catalyst per liter of reaction media.

Figure 5
Comparison of results obtained for the methyl esterification of lauric acid using different molar ratios at T = 180 °C and Cat. ≈ 40 g L^-1. Symbols represent experimental data obtained for reactions using MR = 3.05:1 (squares, E7), MR ≈ 5.97:1 (diamonds, E8), MR ≈ 11.94:1 (squares, E9) and MR ≈ 49.79:1 (triangles, E10). Dotted lines are a guide for the eye.

Due to the experimental set-up, the reagents must be loaded into the reaction vessel at room temperatures and the reaction media is heated to the desired temperature using a heating mantle (electrical heater) attached to a controller. The heating of the reaction medium is a function of the controller and, since esterification reactions are affected well by the temperature, this factor plays a major role in the reaction conversions (as confirmed by the comparison between reactions E3 and E8, performed using the same reaction conditions). Therefore, heating ramps were obtained for each reaction and are shown in Fig. A.3 (see Appendix).

Transesterification of soybean oil

The composition of the refined soybean oil used for transesterification reactions, as determined by GC, was 98.8 % of TAG, 1.1 % of DAG and 0.1 % of MAG. Previous GC analyses performed for samples with known composition provided relative errors of 3.72 % and 4.72 % for the contents of FAME and TAG, respectively, while absolute errors for the contents of MAG and DAG were 2.31 % and 6.19 %, respectively. The FFA content of the soybean oil was neglected, since titration analysis provided a value of (0.13±0.02) %.

Methyl transesterification reactions catalyzed by zinc monoglycerolate were performed using the conditions presented in Table 4, which corresponded to 5 reactions with 6 samples each, resulting in a total of 30 experimental data. The temperature range tested in this work, from 140 °C to 180 °C, is higher than the maximum temperatures tested in the works of Lisboa et al. (2013) (120 °C) and Reinoso et al. (2014) (140 °C). This temperature range was chosen in an attempt to achieve better results in less time of reaction and was possible due to the fact that this solid is stable until nearly 360 °C (as determined by TGA analysis).

Table 4
Experimental conditions for the transesterification of soybean oil with methanol using zinc monoglycerolate as catalyst.

Reaction	T (°C)	MR	Cat. (%)
T1	140	50.18:1	2.02
T2	160	49.88:1	2.00
T3	180	50.64:1	2.02
T4	140	49.22:1	0
T5	180	48.55:1	0

• MR = Molar Ratio alcohol:acylglycerols; Cat. = Catalyst load expressed as g of catalyst per 100 g of soybean oil.

The molar ratios of these reactions were determined by comparing the number of moles of methanol to the total number of moles of acylglycerols (MAG, DAG and TAG), while the catalyst amount is presented as the mass of solids for each 100 g of soybean oil. Thus, the molar masses of the acylglycerols were achieved based on the FFA profile of soybean oil obtained by gas chromatography. This procedure was employed by Voll et al. (2013) and considers that the acylglycerols are composed of one, two or three alkyl groups derived from the FFAs that are bonded to the glycerol backbone. Therefore, because the FFA profile was obtained (C16:0 = (10.14±0.87) %, C18:0 = (0.0414±0.62) %, C18:1 = (25.96±2.26) %, C18:2 = (51.77±3.30) % and C18:3 = (8.00±2.26) %), it was also possible to achieve the mean molar mass of the alkyl group (235.32 g·mol^-1), so as the mean molar masses of MAG (354.42 g mol^-1), DAG (616.74 g mol^-1) and TAG (879.06 g mol^-1).

The compositions obtained for reactions T1 to T5 were plotted in Figs. A.4.A-E (Appendix). The comparison of the contents of both FAME and TAG obtained for reactions performed either in the absence or in the presence of ZnMGly are presented in Figs. 6.A-D. From Fig. 6.C, it is possible to note a considerable amount of FAME after 6 h of reaction, performed in the absence of catalyst, at 180 °C and molar ratio of nearly 50:1. Therefore, it is clear that zinc monoglycerolate presents catalytic activity for this kind of reactions, as confirmed by both the higher initial reaction rate and also by the final content of FAME (91.9 %), which is higher, and of TAG (0.89 %), which is lower, as compared to the contents obtained for the reaction performed without catalyst (68.5 % and 10.5 %, respectively). However, it is also clear that the thermal effects could not be neglected if the kinetics modeling of these data were performed.

Figure 6
Comparison of (A, C) FAME and (B, D) TAG contents obtained for the methyl transesterification of soybean oil using zinc monoglycerolate as catalyst. The symbols represent experimental data obtained for reactions without catalyst (empty symbols) and using zinc monoglycerolate (full symbols). Reaction conditions were: T1 (Cat. = 2.02 %, MR = 50.18:1 and T = 140 °C), T3 (Cat. = 2.02 %, MR = 50.64:1 and T = 180 °C), T4 (Cat. = 0 %, MR = 49.22:1 and T = 140 °C) and T5 (Cat. = 0 %, MR = 48.55:1 and T = 180 °C). Dotted lines are a guide for the eye.

Figs. 7.A-B present the effect of temperature on the zinc monoglycerolate-catalyzed reactions and the results indicated that this parameter has a positive effect in the reaction rates of both FAME formation (Fig. 7.A) and TAG consumption (Fig. 7.B). Furthermore, after 6 h of reaction, at 140 °C the TAG conversion was 78.3 % and the FAME yield was 53.2 %, while these values were, respectively, 88.1 % and 71.4 % at 160 °C and 99.1 % and 92.7% at 180 °C.

Figure 7
Temperature effect in the contents of both (A) FAME and (B) TAG obtained for the methyl transesterification of soybean oil using zinc monoglycerolate (Cat. ≈ 2 % and MR ≈ 50:1). The symbols represent experimental data obtained for reactions T1 (triangles, T = 140 °C), T2 (diamonds, T = 160 ºC), and T3 (squares, T = 180 °C). Dotted lines are a guide for the eye.

Processing of high-acidity oils

The processing of high-acidity oils was carried out in duplicate through sequential reactions of esterification and transesterification, using a mixture containing soybean oil and lauric acid, whose content was nearly 40 %, on a mass basis. This FFA was chosen due to its absence in the fatty acid profile of soybean oil, which could help the monitoring of each reaction. Table 5 presents the reaction conditions, in which molar ratios represent the relationship between the amounts of methanol and fatty materials that could produce FAME (both free fatty acids and acylglycerols). The initial contents of each compound in the second step (transesterification reaction) were considered to be the same as the contents of samples obtained after 1 h of esterification reaction. The reaction conditions for the processing of high-acidity oils were slightly different from those employed for both esterification and transesterification reactions presented previously, especially concerning the molar ratios and catalyst loads.

Table 5
Experimental conditions employed for the simulation of the processing of acid oils using the methanol route.

Reaction	t (h)	T (°C)	MR	Cat. (g L-1)	FFA0 (%)	FAME0 (%)
E11	1	160	5.93:1	35.8	40.7	0
T6	2	180	43.30:1	3.87	2.7	42.9
E12	1	160	5.95:1	35.9	40.8	0
T7	2	180	39.31:1	3.83	3.4	38.1

• t = Time of reaction; T = Temperature; MR = Molar Ratio alcohol:fatty materials (FFA + acylglycerols); Cat. = Catalyst load expressed as g of catalyst per liter of reaction media; FFA0 = Initial FFA content; FAME0 = Initial FAME content.

As for the catalyst loads, the conventional manner is to represent the mass of catalyst used for each 100 g of the fatty material (Lisboa et al., 2014; Zatta et al., 2014). However, for the processing of high-acidity oil, the most proper form to present this variable is probably in terms of the concentration of catalyst (g L^-1). In order to assess the volume of the reaction medium, the same strategy used by Kanda et al. (2017) was employed in this work, using experimental data available in the literature (Huber et al., 2009; Ndiaye et al., 2006; Nogueira et al., 2010; Noureddini and Zhu, 1997) to fit the parameters for equations that related densities of pure components to the temperature. In the case of methanol, the equation and respective parameters were taken from the DIPPR database. The density values used in this work are presented in Table A.1 (Appendix).

This particular study ended up providing 15 samples and the results of analyses performed by GC and titration are shown in Figs. 8.A-B. The esterification of high-acidity oils using montmorillonite K10 under the conditions employed in this work allowed the reduction of FFA contents from 40.7 % to 2.7 % and from 40.8 % to 3.4 %. Hence, FFA conversions of 84.3 % and 78.1 % were obtained, while the esterification of lauric acid without the presence of soybean oil (reaction E2) provided a conversion of 94.5 % after 1 h of reaction. This difference might be due to the fact that the catalyst concentration in the latter reaction was of 42.4 g L^-1, while for the processing of acid oil this value was around 36 g L^-1. Moreover, TAG conversions obtained after the esterification reaction using montmorillonite K10, performed in duplicate, were 7.5 % and 4.1 %, while after 1 h in the transesterification reaction T2, using zinc monoglycerolate, performed at the same temperature (160 °C), this value was 70.3 %. This result indicates that montmorillonite K10 does not present a good catalytic activity towards the transesterification of acylglycerols.

Figure 8
Monitoring of composition of the samples obtained from the processing of acid oil using the methanol route, performed in duplicate (A) and (B). The symbols represent experimental data obtained for esterification reactions using montmorillonite K10 (reactions E11 and E12, Cat. ≈ 36 g L^-1, FFA₀ ≈ 40 %, MR ≈ 6:1 and T = 160 °C) and for transesterification reactions using zinc monoglycerolate (reactions T6 and T7, Cat. ≈ 4 g L^-1, MR ≈ 40:1 and T = 180 °C). Lines are a guide for the eye.

On the other hand, unlike the transesterification reactions performed using pure soybean oil, the second step of the processing of high-acidity fatty materials occurred almost to completion, since TAG conversions were virtually 100 % (as no TAG was detected by the end of the 2 h transesterification reaction) and small contents of DAG (2.4 % and 2.2 %) and MAG (0.53 % and 0.42 %) were detected in both the reactions performed. As a matter of fact, low contents of the acylglycerols were observed even for the first samples obtained in each reaction (right after the desired temperature for the reactions was reached). The presence of small amounts of FFA may be responsible for the enhancement of the transesterification reaction when zinc monoglycerolate is used as catalyst (Reinoso et al., 2014).

A comparison between the performances of various solid catalysts in esterification and transesterification reactions performed under different conditions, obtained in this work and in previous studies, is shown in Table 6. Results from this work are related to the processing of high-acidity fatty materials, in which sequential esterification and transesterification reactions were performed. Thus, conversions of both TAG and FFA, as well as FAME yields presented for the reactions using zinc monoglycerolate were assessed considering the amounts of the chemical species in the beginning of the processing. From this comparison, it is easy to infer that solid catalysts, in general, require either higher reaction times or higher temperatures, as compared to homogeneous catalysts, so as high FAME yields are obtained.

Table 6
Performance comparison of various solid catalysts used in previous studies and in this work for the production of biodiesel.

Reference	Catalyst	FFA0 (%)	MR	t (h)	T (°C)	Cat. (%)	XTAG (%)	XFFA (%)	yFAME (%)
Kwong & Yung (2016)	Zinc oxide/zinc glycerolate	0	30:1	0.5	140	8	0.8	-	-
		6		2			98.5	-	-
Reinoso et al. (2014)	Zinc glycerolate	10	30:1	2	140	3	99.5	-	93.8
		100		1			-	80	-
Pan et al. (2018)	1,3-disulfonic acid imidazolium chloride	1.78	15:1	8	120	5	-	-	86
	1,3-disulfonic acid imidazolium tetrachloroferrate						-	-	97
Wang et al. (2017)	Bifunctional magnetic acid	60	12:1	8	140	7	-	-	93.07
		8.6		3	90	9	-	95.9	-
Dawodu et al. (2014)	Sulfonated carbon	15	30:1	5	150	6	-	87.2	75
					180	7.6	-	-	99
Fadhil et al. (2016)		10	15:1	6	60	6	-	~ 85	-
					68		-	94.4	-
Konwar et al. (2013)		8.17	43:1	6	100	5	-	~99	-
		14.4	10.8:1		80		-	~97	-
		43.73	10.8:1				-	~99	-
This work	Montmorillonite K10	40.7	5.9:1	1	160	6.63	7.53	84.3	43.4
		40.8	6.0:1	1	160	6.65	4.07	78.1	39.8
	Zinc monoglycerolate	2.7	53.7:1	2	180	2.2	100a	99.2a	95.3a
		3.4	49.7:1	2	180	2.2	100a	98.6a	95.5a

• FFA0 = Initial FFA content; MR = Molar Ratio alcohol:fatty materials (FFA + acylglycerols); t = Time of reaction; T = Temperature; Cat. = Catalyst load expressed as g of catalyst per 100 g of fatty material (FFA + acylglycerols); X TAG = TAG conversion; X FFA = FFA conversion; y FAME = FAME yield. a Results were assessed considering the amounts before esterification reactions using montmorillonite K10.

It worth mentioning that the material obtained after the esterification step could be processed by the traditional means of alkaline transesterification. However, zinc monoglycerolate can be easily recovered and reused in the reaction (Lisboa et al., 2013; Reinoso et al., 2014), which makes its use interesting even though these reactions require more time to achieve high FAME yields. The approach followed in this work for the processing of high-FFA content raw materials can successfully result in high FAME yields (95.3 % and 95.5 %) after reasonable times of reaction.

Zinc monoglycerolate characterization after the reactions

After the catalyst recovery and purification following the procedures described earlier, the solids were analyzed by XRD to determine whether they maintained their integrity. Results obtained for zinc monoglycerolate prior to the reactions and those recovered after the methyl transesterification of soybean oil are presented in Fig.A.5 (Appendix), while the results for the analysis of solids employed in the processing of acid oils are presented in Fig. 9.A. Slightly different diffraction angles were observed, mainly caused by inherent errors of the equipment, meaning that no significant changes were detected in the catalysts recovered after the methyl transesterification of soybean oil, especially since the zinc oxide diffraction pattern was not identified in the samples. Moreover, zinc monoglycerolate recovered after the two-step processing of the high-acidity oil also remained intact, as diffraction patterns of zinc laurate (expected if zinc monoglycerolate reacted with lauric acid) were not identified. The recovered solids were likewise subjected to FTIR and TGA analyses.

Figure 9
Analyses of zinc monoglycerolate recovered after the processing of high-acidity fatty materials, reactions T6 and T7 (Cat. ≈ 4 g·L^-1, MR ≈ 40:1 and T = 180 °C). (A) Comparison of XRD analysis of zinc monoglycerolate before and after reactions (dashed lines are a guide for the eye); (B) Comparison of FTIR spectra of zinc monoglycerolate before and after reactions; thermal analysis curves (TGA/DTG) of zinc monoglycerolate after reactions (C) T6 and (D) T7 (continuous lines indicate thermogravimetric curves and dotted lines refer to the thermogravimetric derivatives).

The FTIR spectra of zinc monoglycerolate recovered after reactions T6 and T7 are presented in Fig. 9.B and show a good agreement with the spectrum of the zinc monoglycerolate before the reactions (batch #1), indicating that the catalyst suffered no significant changes. Despite that, the recovered solids presented noise between 3500 and 4000 cm^-1 and there is evidence for the presence of water in the zinc monoglycerolate before the reactions via the broad band between 3300 and 3400 cm^-1, attributed to O-H stretching. Narrow bands were identified between 2800 and 3000 cm^-1 and are related to the vibrational modes of C-H e H-C-H groups. Vibrations related to the stretching of C-O bonds are identified near 1900 cm^-1 and 1100 cm^-1 (the first of which is related to the hydrogen bond C-O∙∙∙H-O). Finally, a narrow band is observed close to 875 cm^-1 and is related to the Zn-O-C bending modes, while metal-oxygen (Zn-O) stretching bands are observed at 650 cm^-1 and 400 cm^-1, confirming the coordination of the metal to the monoglycerolate anion. These results are consistent with those presented by Lisboa et al. (2013) and Reinoso et al. (2014).

Finally, Figs. 9.C-D show the thermogravimetric analyses for the solids recovered after the processing of acid oil performed in duplicate, in which the same thermal events are identified and that also present a good agreement with the TGA of zinc monoglycerolate prior to the reactions (Fig. A.2 - Appendix). Very close temperatures of onset and of the 1^st derivative peak were also observed and, by the end of the analysis, the solids recovered after reactions T6 and T7 presented final zinc oxide contents of 49.7 % and 49.1 %, while the solids prior to the reactions presented 50.3 % of this content (as mentioned before). All the calculations were performed on a dry basis.

All the analyses presented indicated that the zinc monoglycerolate retained its integrity and thus can be considered as a stable material under the conditions tested, proving the possibility of using this solid for the processing of acid oil. Even though it was possible that zinc carboxylates were formed during the reaction, according to Reinoso et al. (2014), the formation of glycerol during the course of the reaction contributes to the metal carboxylate to shift it back to the metal monoglycerolate. Furthermore, zinc oxide might be present if the heating mantle temperature reached higher values (according to the thermal analysis, the zinc monoglycerolate oxidation begins at approximately 360 °C).

CONCLUSION

The two-step process using solid catalysts, montmorillonite K10 to reduce the FFA content of acid oils, followed by the use of zinc monoglycelorate to perform the transesterification reaction, had its technical feasibility demonstrated for the prompt usage of oils with high-acidity aiming at biodiesel production. The main results achieved were a reduction of (92.6±1.2) % in the FFA content after the first step and a final FAME content of (96.6±0.2) %. Considering the conditions employed in this work, the industrial use of both solid catalysts seems to be promising, especially considering the possibility of their recovery and further reuse in the process (the latter was not performed in this work). Furthermore, the results obtained may encourage the production of biodiesel from otherwise unusual raw materials, especially regarding higher acidity fatty materials, whose processing result in both environmental and economic gains.

ACKNOWLEDGEMENTS

The authors are thankful to the Brazilian funding agencies (CNPq - Proc. Num. 303846/2014-3 and 40117/2016-9, CAPES - Finance Code 001 and Fundação Araucária) for the financial aid of this work. We are also grateful for the analytical support provided by Laboratório de Óptica de Raios X e Instrumentação (LORXI - UFPR), Laboratório de Espectroscopia de Absorção no Infravermelho (Chemistry Department - UFPR), Centro de Microscopia Eletrônica (CME-UFPR) and Central Analítica (Chemical Engineering Department - UFPR).

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APPENDIX

Figure A.1
XRD analysis of zinc monoglycerolate (batches #1, #2, and #3).

Figure A.2
Thermal analysis curves (TGA/DTG) of zinc monoglycerolate (batch #4) used for transesterification of soybean oil. Continuous lines indicate thermogravimetric curves (black) and thermogravimetric derivatives (red).

Figure A.3
Heating ramps for (A) esterification reactions using FFA, (B) transesterification reactions using soybean oil and (C) esterification and transesterification reactions using acid oil. The symbols represent experimental data obtained for reactions E1: Cat. = 12.03 %, MR = 6.06:1, T = 140 °C; E2: Cat. = 12.01 %, MR = 6.18:1, T = 160 °C; E3: Cat. = 11.75 %, MR = 5.97:1, T = 180 °C; E4: Cat. = 0 %, MR = 6.01:1, T = 140 °C; E5: Cat. = 0 %, MR = 6.10:1, T = 160 °C; E6: Cat. = 0 %, MR = 6.01:1, T = 180 °C; E7: Cat. = 39.7 g L^-1, MR = 3.05:1, T = 180 °C; E8: Cat. = 40.7 g L^-1, MR = 5.97:1, T = 180 °C; E9: Cat. = 40.3 g L^-1, MR = 11.94:1, T = 180 °C; E10: Cat. = 39.8 g L^-1, MR = 49.79:1, T = 180 °C; T1: Cat. = 2.02 %, MR = 50.18:1, T = 140 °C; T2: Cat. = 2.00 %, MR = 49.88:1, T = 160 °C; T3: Cat. = 2.02 %, MR = 50.64:1, T = 180 °C; T4: Cat. = 0 %, MR = 49.22:1, T = 140 °C; T5: Cat. = 0 %, MR = 48.55:1, T = 180 °C; E11 and E12: Cat. ≈ 36 g L^-1, FFA₀ ≈ 40 %, MR ≈ 6:1, T = 160 °C; T6 and T7: Cat. ≈ 4 g L^-1, MR ≈ 40:1 and T = 180 °C. Lines are a guide for the eye.

Figure A.4
Effects of both the presence of zinc monoglycerolate and the temperature in the transesterification of soybean oil with methanol. The symbols represent experimental data obtained for reactions (A) T1 (Cat. = 2.02 %, MR = 50.67:1 and T = 140 °C), (B) T2 (Cat. = 2.00 %, MR = 49.91:1 and T = 160 ºC), (C) T3 (Cat. = 2.02 %, MR = 50.21:1 and T = 180 °C), (D) T4 (Cat. = 0 %, MR = 49.25:1 and T = 140 °C) and (E) T5 (Cat. = 0 %, MR = 48.58:1 and T = 180 °C). Dotted lines are a guide for the eye.

Figure A.5
Comparison of XRD analysis for zinc monoglycerolate before the reactions (batch #1) and recovered after the reactions of methyl transesterification of soybean oil. Reaction conditions were: T1: Cat. = 2.02 %, MR = 50.67:1 and T = 140 °C, T2: Cat. = 2.00, MR = 49.91:1 and T = 160 ºC, and T3: Cat. = 2.02, MR = 50.21:1 and T = 180 °C.

Table A.1
Densities of the compounds used in this work as a function of temperature.

T (°C)	Density (g mL-1)
Compound: methanola
140	0.6584
160	0.6281
180	0.5929
Compound: lauric acidb
140	0.8072
160	0.7941
180	0.7814
Compound: soybean oilb
140	0.8404
160	0.8266
180	0.8127
Compound: FAMEc (obtained from soybean oil)
140	0.7971
160	0.7812
180	0.7650

• ^a DIPPR equation 105.
• ^b Extrapolated data, based in the works of Noureddini et al. (1997) and Ndiaye et al. (2006).
• ^c Extrapolated data, based in the works of Huber et al. (2009) and Nogueira et al. (2010).

Publication Dates

• Publication in this collection
  13 Jan 2020
• Date of issue
  Oct-Dec 2019

History

• Received
  23 Feb 2019
• Reviewed
  24 June 2019
• Accepted
  26 June 2019