# Environmentally Benign Neem Biodiesel Synthesis Using Nano-Zn-Mg-Al Hydrotalcite as Solid Base Catalysts

Authors: Karthikeyan Chelladurai; Manivannan Rajamanickam
Journal: Journal of Catalysts
 (2014)

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## Abstract

Hydrotalcite, also known as aluminum-magnesium layered double hydroxide (LDH) or anionic clay, is a synthetic compound that was broadly investigated in the past decade due to its many potential applications. In this work, we present an environmentally benign process for the transesterification (methanolysis) of neem oil to fatty acid methyl esters (FAME) using Zn-Mg-Al hydrotalcites as solid base catalysts in a heterogeneous manner. The catalysts were characterized by XRD, FT-IR, TPD-CO2, and the BET surface area analysis. It is well-known that the catalytic performance of hydrotalcite is dramatically increased through the incorporation of Zn into the surface of Mg-Al hydrotalcite material. The optimized parameters, 10 : 1 methanol/oil molar ratio with 7.5 g catalysts reacted under stirring speed 450 rpm at 65°C for 4 h reaction, gave a maximum ester conversion of 90.5% for the sample with Zn-Mg-Al ratio of 3 : 3 : 1.


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## Body

## 1. Introduction

Biodiesel is a promising nontoxic and biodegradable renewable fuel comprised of monoalkyl esters of long chain fatty acids, which are derived from vegetable oils or animal fats [1]. It has attracted attention during the past few years as a renewable and environmental friendly fuel. The transesterification reaction consists of transforming triglycerides into fatty acid alkyl esters, in the presence of an alcohol, such as methanol or ethanol, and a catalyst, such as an alkali or acid, with glycerol as a byproduct [2]. Nearly 60–80% of the total biodiesel production cost is attributed to biodiesel feedstock. Using cheaper feedstock, such as nonedible oil, animal fats, untreated crude edible oil, or waste cooking oil, has been suggested to lower the feedstock cost [3–5]. Neem oil was selected as a nonedible feedstock for biodiesel production.Mixed metal oxides (hydrotalcites) are ones of the base catalysts affording good catalytic activity for the methanolysis of vegetable oil. Because the actual active sites of the hydrotalcites participating in catalysis situated at the edges of crystals, the smaller crystals have a larger number of active sites [6]. The hydrotalcite is a kind of double-layered hydroxides (LDHs) composed of the brucite-like layers, and Mg2+ and Al3+ cations coordinate an octahedral structure. When Al3+ replaces Mg2+, a positive charge is generated in the layer, which is balanced by CO32- or OH− located between the brucite-like cation layers [7, 8]. The interesting property of the oxides obtained by calcination of LDHs around 400°C is the formation of highly active homogenous mixed oxides which are potentially used as basic catalysts and catalyst supports [9, 10]. We have already reported Mg-Al catalysts with neem oil that gave a maximum ester conversion of 84% for the sample with 3 : 1 molar ratio [11]. In this present work, an environmentally benign process for the methanolysis of neem oil to fatty acid methyl esters using Zn-Mg-Al nanohydrotalcite as solid base catalysts in a heterogeneous manner was analyzed.


## 2. Materials and Methods

Neem oil was purchased from local market, chemicals such as Zn(NO3)2·6H2O, Mg(NO3)2·6H2O, and Al(NO3)3·9H2O were purchased from Merck, and methanol, NaOH, and Na2CO3 were purchased from Sigma Aldrich. All chemicals used were of analytical reagent grade.


### 2.1. Catalysts Preparation

Zn-Mg-Al hydrotalcite was prepared from nitrate salts. Solution A contains various molar ratios of Zn(NO3)2·6H2O, Mg(NO3)2·6H2O, and Al(NO3)3·9H2O and solution B contains 2 M NaOH and 0.125 M Na2CO3. Solution B is added to solution A under vigorous stirring at 65°C for 48 h, maintaining the pH between 8 and 10. The resulting white precipitate was filtered and washed to eliminate the alkali metal ions and the nitrate ions and catalysts were dried at 110°C overnight. The samples were then calcined at 500°C in a muffle furnace for 8 h, with a heating rate of 8 K·min−1. For convenience, the hydrotalcites thus obtained with different Zn-Mg-Al molar ratios of 2 : 2 : 1, 2 : 3 : 1, 3 : 3 : 1, and 3 : 5 : 1 were designated as HT-1, HT-2, HT-3, and HT-4.


### 2.2. Catalysts Characterization

The crystalline characteristic was determined by using the X-ray diffraction instrument Siemens D-diffractometer using CuKα radiation (λ=1.5406°A). Scans were performed over the 2θ range from 5° to 75°. The particle size of the hydrotalcite was calculated using the Scherer equation. A FEI QUANTA200 Fourier transform infrared (FT-IR) spectrum was recorded on a Nicolet 5DX spectrophotometer using KBr pellet technique. Gas chromatography analysis was performed on a GC-2010 (Shimadzu, Japan). The chemical composition of the synthesized samples was determined using a JEOL JCXA 733 EPMA (electron probe microanalysis). The specific surface area was measured by the flow method using Micromeritics Pulse Chemisorb 2700 instrument.


### 2.3. Catalytic Activity

The catalytic activity was evaluated using the transesterification of crude neem oil with methanol. Transesterification experiments were carried out in a four-necked flask. A specified amount of Zn-Mg-Al mixed metal oxide catalyst and the required volume of methanol were added to the reaction mixture of 20.0 g of neem oil. The reactant mixture was then heated to 120°C under maximum agitation (450 rpm of stirring). At the end of the experiment, the catalyst was separated from the product using a centrifuge, and the reaction mixture was then loaded into a rotary evaporator to remove excess methanol. The top layer was the biodiesel phase of the methyl esters and lower phase was glycerin. The chemical analysis was carried out by the gas chromatography.


## 2.1. Catalysts Preparation

Zn-Mg-Al hydrotalcite was prepared from nitrate salts. Solution A contains various molar ratios of Zn(NO3)2·6H2O, Mg(NO3)2·6H2O, and Al(NO3)3·9H2O and solution B contains 2 M NaOH and 0.125 M Na2CO3. Solution B is added to solution A under vigorous stirring at 65°C for 48 h, maintaining the pH between 8 and 10. The resulting white precipitate was filtered and washed to eliminate the alkali metal ions and the nitrate ions and catalysts were dried at 110°C overnight. The samples were then calcined at 500°C in a muffle furnace for 8 h, with a heating rate of 8 K·min−1. For convenience, the hydrotalcites thus obtained with different Zn-Mg-Al molar ratios of 2 : 2 : 1, 2 : 3 : 1, 3 : 3 : 1, and 3 : 5 : 1 were designated as HT-1, HT-2, HT-3, and HT-4.


## 2.2. Catalysts Characterization

The crystalline characteristic was determined by using the X-ray diffraction instrument Siemens D-diffractometer using CuKα radiation (λ=1.5406°A). Scans were performed over the 2θ range from 5° to 75°. The particle size of the hydrotalcite was calculated using the Scherer equation. A FEI QUANTA200 Fourier transform infrared (FT-IR) spectrum was recorded on a Nicolet 5DX spectrophotometer using KBr pellet technique. Gas chromatography analysis was performed on a GC-2010 (Shimadzu, Japan). The chemical composition of the synthesized samples was determined using a JEOL JCXA 733 EPMA (electron probe microanalysis). The specific surface area was measured by the flow method using Micromeritics Pulse Chemisorb 2700 instrument.


## 2.3. Catalytic Activity

The catalytic activity was evaluated using the transesterification of crude neem oil with methanol. Transesterification experiments were carried out in a four-necked flask. A specified amount of Zn-Mg-Al mixed metal oxide catalyst and the required volume of methanol were added to the reaction mixture of 20.0 g of neem oil. The reactant mixture was then heated to 120°C under maximum agitation (450 rpm of stirring). At the end of the experiment, the catalyst was separated from the product using a centrifuge, and the reaction mixture was then loaded into a rotary evaporator to remove excess methanol. The top layer was the biodiesel phase of the methyl esters and lower phase was glycerin. The chemical analysis was carried out by the gas chromatography.


## 3. Result and Discussion

### 3.1. X-Ray Diffraction Analysis

The XRD pattern of Zn-Mg/Al catalyst (Figure1) is corresponding to a typical hydrotalcite structure with strong, sharp, and symmetric peaks for the (003), (006), (110), and (113) planes as well as broad and symmetric peaks for the (015) and (018) planes, which could be attributed to the overlapping MgO and/or ZnO diffraction lines [12, 13]. The three strong peaks at 2θ values of about 11.46°, 23.28°, and 33.57° are characteristic of a layered structure. The difference in the intensities of the reflections from one sample to another indicates different degrees of crystallinity when the cationic composition varies. The peaks of Al2O3 phase were very small, indicating that Al3+ cations were dispersed in the structure of MgO without the formation of spinel species [14].Figure 1
XRD patterns of HT-1, HT-2, HT-3, and HT-4.The cationic ratio in the synthesized hydrotalcites was in good agreement with the theoretical one, as the EPMA results showed no major changing in the final composition. The unit cell parameters were done by the peaks indexing in the hexagonal crystal system which was presented in Table1. The values obtained here are close to previously reported data for similar materials [15, 16]. It can be noticed that the value “a” is not influenced by the nature of divalent cations incorporated in the brucite-like layers and do not lead to distortions in the octahedral planes. [17] The a and c parameters decreased with increasing aluminum content, which can be explained by the substitution of larger Mg2+ ions by smaller Al3+ ions [15]. It also indicates that the incorporation of Zn leads to an increase in stress in the octahedral hydroxide layer in the hydrotalcite crystal structure, due to the difference in ionic radii between Mg2+ and Zn2+ as there are no differences in the bond lengths around a single octahedral site. The average particle size was calculated as 20 nm by the Scherer equation [Dc = k(λ/β)·(cosθ)] where Dc is the average particle size, k is the Scherer constant (0.89), λ is the X-ray wavelength, (CuKα) = 0.1541 nm, β is the FWHM (full-width at half-maximum), and θ is the diffraction angle in the XRD (003) reflection [18].Table 1
Chemical composition analysis and physicochemical properties of Zn-Mg-Al hydrotalcites.
Catalysts
Theoretical ratioZn/Mg/Al
Experimental ratioa  Zn/Mg/Al
Unit cell parameters (Å)
BET surface area (m2/g)b
a
c
c
′
HT-1
2 : 2 : 1
1.96/1.89/1
3.042
22.73
7.31
166.4
HT-2
2 : 3 : 1
1.93/1.98/1
3.058
22.89
7.57
188.6
HT-3
3 : 3 : 1
3.02/2.98/1
3.063
22.95
7.72
220.8
HT-4
3 : 4 : 1
2.85/4.08/1
3.088
23.59
7.94
208.4
aExperimental Mg-Zn-Al atomic ratios in the synthesized catalyst determined by EPMA.
bBET surface area calcined at 500°C/8 h.


### 3.2. FT-IR Analysis

FT-IR spectroscopy showed characteristic frequencies associated with the presence of intercalated anions. In all samples, a broad band between 3600 and 3400 cm−1 was observed (Figure 2) and represents the stretching vibrations of the O–H groups of the inorganic and interlayer water. If the various metals in the hydrotalcites (Mg, Zn, Al) are distributed at random, in most cases one hydroxyl group will be coordinated by at least two different metal cations [9]. Another common frequency for LDH-like materials is the presence of the bending vibrations of water molecules at 1600 cm−1 [10]. Two bands very close together assigned to the ν3 have been observed around 1360 and 1370 cm−1 in HT-3, while in the literature one band is described around 1400 cm−1 [19]. This may indicate that two different types of CO32- are present in the interlayer of the hydrotalcite, possibly associated with the location near octahedral either containing Mg or Zn. In the case of HT-4, the absorption centered at 1380 cm−1 is assigned to the presence of nitrate anions within the structure. The bond located around 780 cm−1 identified in the FTIR spectra may be due to the Al–O, Zn–Al–O, or Mg–Al–O bond vibration in the brucite-like layer [20]. The relatively broad bands at 950 and 1030 cm−1 have not been reported before for hydrotalcite. These bands, which were also observed in the Zn/Al-hydrotalcite, are absent in the spectrum of brucite, Mg(OH)2, the structure from which hydrotalcite can be derived [10]. Therefore, the FTIR characterization of the hydrotalcite structure reflects the coexistence of a strong band with a weak band. In all the samples the main characteristic peaks are quite similar and comparable to previously published data [21, 22].Figure 2
FT-IR spectra of HT-1, HT-2, HT-3, and HT-4.


### 3.3. TPD-CO2 Analysis

The TPD-CO2 measurements were carried out for the series of Zn–Mg–Al catalysts to determine the total basicity and basic strength distribution of the catalyst. The CO2 desorption shows that the main peaks were found at Tmax⁡ ranging from 100 to 150°C is attributed to the interaction of CO2 with the weak basic sites present in the catalyst, while the others found at varying from 200 to 500°C are due to the interaction of CO2 with the medium basic sites of the catalysts system, which were generated from the Mg2+–O2− ion pairs. The Al3+ cations in MgO lattice created a defect in order to compensate the positive charge generated and the adjacent oxygen anions became coordinatively unsaturated. The final basicity of these catalysts and the electronic state of the metallic phase depend on parameters such as M(II)/M(III) ratio, the nature of compensating anions, and thermal treatment [23]. The basicity of HT-1, HT-2, HT-3, and HT-4 is 82, 93.5, 220.8, and 228.7, respectively. The basicity of a catalyst was raised from HT-1 to HT-4 because the synergetic effect between Mg and Zn increased the catalyst basicity.


### 3.4. BET Surface Area Measurement

The BET surface area of calcined samples having different composition is given in Table1. Thermal decomposition of hydrotalcite precursors led to the formation of high surface area. Also creation of large surface area is an important characteristic needed for catalysis. Surface areas of calcined hydrotalcite were significantly higher than in uncalcined hydrotalcite samples [24]. The increase in surface area during calcination at 500°C can be attributed to the formation of mesopores due to expulsion of CO2 and H2O from the hydrotalcite precursors [25]. The higher surface area in case of 3 : 3 : 1 in Zn–Mg–Al ratio compared to other catalyst composition may be due to the presence of equal amount of Zn metal-support interaction in the Mg–O lattice that modifies the atomic and electronic structure of catalyst [26].


### 3.5. Methanolysis of Neem Oil

This transesterification reaction could be mainly influenced by the following factors: amount of catalysts, reaction time, methanol/oil molar ratio, reaction temperature, and molar ratio of Zn-Mg-Al. The effect of catalyst amount on FAME yield was studied; when increasing the amount of catalyst, the slurry (mixture of catalyst and reactants) becomes too viscous giving rise to a problem of mixing and a demand of higher power consumption for adequate stirring. On the other hand, when the catalyst amount is not sufficient, maximum conversion cannot be reached. The maximum yield is obtained when the catalyst amount is 7.5 g, due to increasing the contact between catalyst and reactants. The rate of methanolysis reaction is strongly influenced by the reaction time. The conversion increased progressively with increasing reaction time and then reached a plateau value representative of a nearly equilibrium conversion. The maximum conversion of 90.5% is obtained at 4 h reaction time; after 4 h reaction time yield was decreased probably due to reverse reaction (formation of triglycerides).The conversion and the viscosity of produced ester depended on the molar ratio of methanol to vegetable oil which was one of the most important variables. But when mass transfer is limited due to problems of mixing, the mass transfer rate seems to be much slower than the reaction rate, so the conversion can be elevated by introducing excess amount of the reactant methanol to shift the equilibrium to the right-hand side. Higher molar ratios result in greater ester conversions in a shorter time [27]. The maximum yield was reached when the molar ratio was 10 : 1; higher molar ratio of methanol results in higher rate of esters formation and could ensure complete reaction. Excessive methanol had no significant effect on the yield.


#### 3.5.1. Effect of Reaction Temperature

The effect of reaction temperature on the ester conversion was studied with the catalyst at various temperatures in Figure3. The transesterification proceeded slowly at 45°C; at lower temperatures it resulted in a drop of the ester conversion because only a small amount of molecules was able to get over the required energy barrier. The ester conversion increased up to 92.5% when reaction temperature close to 65°C. Thus, the optimum temperature for the preparation of the ester was found to be 65°C, which was near the boiling point of anhydrous methanol. The conversion fell to about 60% in the temperature range of 75°C, probably because the molar ratio of methanol to oil decreased when methanol reactant volatilized into gas phase above 65°C, the boiling point of pure methanol.Figure 3
Effect of reaction temperature of HT-3 on conversion of FAME (%).


#### 3.5.2. Effect of Molar Ratio of Zn/Mg/Al and Catalytic Studies

The effect of molar ratio of Zn/Mg/Al and the catalytic activity studied at 65°C were illustrated in Figure4, which indicates that the catalytic activity was improved with the increase in Zn and Mg content in Zn/Mg/Al molar ratio at 3 : 3 : 1; but increase in the Mg content in Zn/Mg/Al molar ratio at 3 : 5 : 1, the catalytic activity dropped. The activity decreased in samples due to the formation of surface amorphous Al–O structure that partially covered Mg–O pairs and decreased the concentration surface O2− [15]. The increased catalytic activity of the tertiary oxide system was due to the modification of the electronic properties between the oxides [26]. Table 2 showed various molar ratios of Zn/Mg/Al with product selectivity. The high activity of LDHS is due to the surface site of low (OH− group), medium (Mg–O pairs), and strong (O2− anions) basicity [9]. The catalytic activity of the catalyst is also monitored through the percentage extent of formation of fatty acid methyl ester and glycerol conversion.Table 2
Effect of Zn/Mg/Al molar ratio on product distribution and conversion.
Catalysts
Zn/Mg/Almolar ratio
ConversionWt (%)
Product selectivity Wt (%)
FAME
Glycerol
HT-1
2 : 2 : 1
32
43.49
23.51
HT-2
2 : 3 : 1
43
65.12
19.88
HT-3
3 : 3 : 1
56
92.5
10.02
HT-4
3 : 5 : 1
49
88.3
6.35
Note: FAME: fatty acid methyl ester.
Temperature: 65°C.
Neem oil: methanol: 10 : 1.
Catalyst weight: 7.5 g.Figure 4
Effect of molar ratio of Zn/Mg/Al on conversion of FAME (%) at 65°C.The higher catalytic activity HT-3 indicates the higher acidity of this catalyst which can be attributed to the dissolution of more amount of Al3+ in the M(II)-O lattice introducing Lewis acidity. Also the Zn2+ ions in Mg2+ lattice, the acidic centers submerged in the basic matrix, may be resulting in concomitant acidic-basic centers and more in the presence of considerable amount of Lewis acidity in these compounds [10]. According to literature study, the main factor to influence transesterification activity is the alkalinity and the type of basic strength of the catalysts [28, 29]. The linearity between FAME yield and total basicity was lightly deviated. HT-1 with lower number of basicity was found; this indicated that medium basic strength is less influencing in transesterification rate. In case of HT-3 and HT-4 with highest number of basicity, the FAME yield was higher than the latter. The author previously reported that the M(II)/Al3+ hydrotalcites at ratio 3.0 showed higher acidity of this catalyst which can be attributed to the dissolution of more amount of Al3+ in the M(II)-O lattice introducing Lewis acidity and also contain high density of Al–O pairs; lower and medium strength basic sites Al3+–O2− pairs do not contribute much to the surface basicity. In contrast, both M(II) and M(III) cations provide Lewis acidic sites [9]. Biodiesel produced from the neem oil was analyzed by gas chromatography. The reaction studied with HT-3 at 65°C and the results indicate neem biodiesel compositions like palmitic acid (C16:0) 13.79%, palmitoleic acid (C16:1) 0.95%, stearic acid (C18:0) 6.33%, oleic acid (C18:1) 42.61%, linoleic acid (C18:2) 26.34%, and linolenic acid (C18:3) 0.06%. The identified composition is compared with standard compounds. From the analysis data confirmed, the product is biodiesel phase of the methyl esters.


## 3.1. X-Ray Diffraction Analysis

The XRD pattern of Zn-Mg/Al catalyst (Figure1) is corresponding to a typical hydrotalcite structure with strong, sharp, and symmetric peaks for the (003), (006), (110), and (113) planes as well as broad and symmetric peaks for the (015) and (018) planes, which could be attributed to the overlapping MgO and/or ZnO diffraction lines [12, 13]. The three strong peaks at 2θ values of about 11.46°, 23.28°, and 33.57° are characteristic of a layered structure. The difference in the intensities of the reflections from one sample to another indicates different degrees of crystallinity when the cationic composition varies. The peaks of Al2O3 phase were very small, indicating that Al3+ cations were dispersed in the structure of MgO without the formation of spinel species [14].Figure 1
XRD patterns of HT-1, HT-2, HT-3, and HT-4.The cationic ratio in the synthesized hydrotalcites was in good agreement with the theoretical one, as the EPMA results showed no major changing in the final composition. The unit cell parameters were done by the peaks indexing in the hexagonal crystal system which was presented in Table1. The values obtained here are close to previously reported data for similar materials [15, 16]. It can be noticed that the value “a” is not influenced by the nature of divalent cations incorporated in the brucite-like layers and do not lead to distortions in the octahedral planes. [17] The a and c parameters decreased with increasing aluminum content, which can be explained by the substitution of larger Mg2+ ions by smaller Al3+ ions [15]. It also indicates that the incorporation of Zn leads to an increase in stress in the octahedral hydroxide layer in the hydrotalcite crystal structure, due to the difference in ionic radii between Mg2+ and Zn2+ as there are no differences in the bond lengths around a single octahedral site. The average particle size was calculated as 20 nm by the Scherer equation [Dc = k(λ/β)·(cosθ)] where Dc is the average particle size, k is the Scherer constant (0.89), λ is the X-ray wavelength, (CuKα) = 0.1541 nm, β is the FWHM (full-width at half-maximum), and θ is the diffraction angle in the XRD (003) reflection [18].Table 1
Chemical composition analysis and physicochemical properties of Zn-Mg-Al hydrotalcites.
Catalysts
Theoretical ratioZn/Mg/Al
Experimental ratioa  Zn/Mg/Al
Unit cell parameters (Å)
BET surface area (m2/g)b
a
c
c
′
HT-1
2 : 2 : 1
1.96/1.89/1
3.042
22.73
7.31
166.4
HT-2
2 : 3 : 1
1.93/1.98/1
3.058
22.89
7.57
188.6
HT-3
3 : 3 : 1
3.02/2.98/1
3.063
22.95
7.72
220.8
HT-4
3 : 4 : 1
2.85/4.08/1
3.088
23.59
7.94
208.4
aExperimental Mg-Zn-Al atomic ratios in the synthesized catalyst determined by EPMA.
bBET surface area calcined at 500°C/8 h.


## 3.2. FT-IR Analysis

FT-IR spectroscopy showed characteristic frequencies associated with the presence of intercalated anions. In all samples, a broad band between 3600 and 3400 cm−1 was observed (Figure 2) and represents the stretching vibrations of the O–H groups of the inorganic and interlayer water. If the various metals in the hydrotalcites (Mg, Zn, Al) are distributed at random, in most cases one hydroxyl group will be coordinated by at least two different metal cations [9]. Another common frequency for LDH-like materials is the presence of the bending vibrations of water molecules at 1600 cm−1 [10]. Two bands very close together assigned to the ν3 have been observed around 1360 and 1370 cm−1 in HT-3, while in the literature one band is described around 1400 cm−1 [19]. This may indicate that two different types of CO32- are present in the interlayer of the hydrotalcite, possibly associated with the location near octahedral either containing Mg or Zn. In the case of HT-4, the absorption centered at 1380 cm−1 is assigned to the presence of nitrate anions within the structure. The bond located around 780 cm−1 identified in the FTIR spectra may be due to the Al–O, Zn–Al–O, or Mg–Al–O bond vibration in the brucite-like layer [20]. The relatively broad bands at 950 and 1030 cm−1 have not been reported before for hydrotalcite. These bands, which were also observed in the Zn/Al-hydrotalcite, are absent in the spectrum of brucite, Mg(OH)2, the structure from which hydrotalcite can be derived [10]. Therefore, the FTIR characterization of the hydrotalcite structure reflects the coexistence of a strong band with a weak band. In all the samples the main characteristic peaks are quite similar and comparable to previously published data [21, 22].Figure 2
FT-IR spectra of HT-1, HT-2, HT-3, and HT-4.


## 3.3. TPD-CO2 Analysis

The TPD-CO2 measurements were carried out for the series of Zn–Mg–Al catalysts to determine the total basicity and basic strength distribution of the catalyst. The CO2 desorption shows that the main peaks were found at Tmax⁡ ranging from 100 to 150°C is attributed to the interaction of CO2 with the weak basic sites present in the catalyst, while the others found at varying from 200 to 500°C are due to the interaction of CO2 with the medium basic sites of the catalysts system, which were generated from the Mg2+–O2− ion pairs. The Al3+ cations in MgO lattice created a defect in order to compensate the positive charge generated and the adjacent oxygen anions became coordinatively unsaturated. The final basicity of these catalysts and the electronic state of the metallic phase depend on parameters such as M(II)/M(III) ratio, the nature of compensating anions, and thermal treatment [23]. The basicity of HT-1, HT-2, HT-3, and HT-4 is 82, 93.5, 220.8, and 228.7, respectively. The basicity of a catalyst was raised from HT-1 to HT-4 because the synergetic effect between Mg and Zn increased the catalyst basicity.


## 3.4. BET Surface Area Measurement

The BET surface area of calcined samples having different composition is given in Table1. Thermal decomposition of hydrotalcite precursors led to the formation of high surface area. Also creation of large surface area is an important characteristic needed for catalysis. Surface areas of calcined hydrotalcite were significantly higher than in uncalcined hydrotalcite samples [24]. The increase in surface area during calcination at 500°C can be attributed to the formation of mesopores due to expulsion of CO2 and H2O from the hydrotalcite precursors [25]. The higher surface area in case of 3 : 3 : 1 in Zn–Mg–Al ratio compared to other catalyst composition may be due to the presence of equal amount of Zn metal-support interaction in the Mg–O lattice that modifies the atomic and electronic structure of catalyst [26].


## 3.5. Methanolysis of Neem Oil

This transesterification reaction could be mainly influenced by the following factors: amount of catalysts, reaction time, methanol/oil molar ratio, reaction temperature, and molar ratio of Zn-Mg-Al. The effect of catalyst amount on FAME yield was studied; when increasing the amount of catalyst, the slurry (mixture of catalyst and reactants) becomes too viscous giving rise to a problem of mixing and a demand of higher power consumption for adequate stirring. On the other hand, when the catalyst amount is not sufficient, maximum conversion cannot be reached. The maximum yield is obtained when the catalyst amount is 7.5 g, due to increasing the contact between catalyst and reactants. The rate of methanolysis reaction is strongly influenced by the reaction time. The conversion increased progressively with increasing reaction time and then reached a plateau value representative of a nearly equilibrium conversion. The maximum conversion of 90.5% is obtained at 4 h reaction time; after 4 h reaction time yield was decreased probably due to reverse reaction (formation of triglycerides).The conversion and the viscosity of produced ester depended on the molar ratio of methanol to vegetable oil which was one of the most important variables. But when mass transfer is limited due to problems of mixing, the mass transfer rate seems to be much slower than the reaction rate, so the conversion can be elevated by introducing excess amount of the reactant methanol to shift the equilibrium to the right-hand side. Higher molar ratios result in greater ester conversions in a shorter time [27]. The maximum yield was reached when the molar ratio was 10 : 1; higher molar ratio of methanol results in higher rate of esters formation and could ensure complete reaction. Excessive methanol had no significant effect on the yield.


### 3.5.1. Effect of Reaction Temperature

The effect of reaction temperature on the ester conversion was studied with the catalyst at various temperatures in Figure3. The transesterification proceeded slowly at 45°C; at lower temperatures it resulted in a drop of the ester conversion because only a small amount of molecules was able to get over the required energy barrier. The ester conversion increased up to 92.5% when reaction temperature close to 65°C. Thus, the optimum temperature for the preparation of the ester was found to be 65°C, which was near the boiling point of anhydrous methanol. The conversion fell to about 60% in the temperature range of 75°C, probably because the molar ratio of methanol to oil decreased when methanol reactant volatilized into gas phase above 65°C, the boiling point of pure methanol.Figure 3
Effect of reaction temperature of HT-3 on conversion of FAME (%).


### 3.5.2. Effect of Molar Ratio of Zn/Mg/Al and Catalytic Studies

The effect of molar ratio of Zn/Mg/Al and the catalytic activity studied at 65°C were illustrated in Figure4, which indicates that the catalytic activity was improved with the increase in Zn and Mg content in Zn/Mg/Al molar ratio at 3 : 3 : 1; but increase in the Mg content in Zn/Mg/Al molar ratio at 3 : 5 : 1, the catalytic activity dropped. The activity decreased in samples due to the formation of surface amorphous Al–O structure that partially covered Mg–O pairs and decreased the concentration surface O2− [15]. The increased catalytic activity of the tertiary oxide system was due to the modification of the electronic properties between the oxides [26]. Table 2 showed various molar ratios of Zn/Mg/Al with product selectivity. The high activity of LDHS is due to the surface site of low (OH− group), medium (Mg–O pairs), and strong (O2− anions) basicity [9]. The catalytic activity of the catalyst is also monitored through the percentage extent of formation of fatty acid methyl ester and glycerol conversion.Table 2
Effect of Zn/Mg/Al molar ratio on product distribution and conversion.
Catalysts
Zn/Mg/Almolar ratio
ConversionWt (%)
Product selectivity Wt (%)
FAME
Glycerol
HT-1
2 : 2 : 1
32
43.49
23.51
HT-2
2 : 3 : 1
43
65.12
19.88
HT-3
3 : 3 : 1
56
92.5
10.02
HT-4
3 : 5 : 1
49
88.3
6.35
Note: FAME: fatty acid methyl ester.
Temperature: 65°C.
Neem oil: methanol: 10 : 1.
Catalyst weight: 7.5 g.Figure 4
Effect of molar ratio of Zn/Mg/Al on conversion of FAME (%) at 65°C.The higher catalytic activity HT-3 indicates the higher acidity of this catalyst which can be attributed to the dissolution of more amount of Al3+ in the M(II)-O lattice introducing Lewis acidity. Also the Zn2+ ions in Mg2+ lattice, the acidic centers submerged in the basic matrix, may be resulting in concomitant acidic-basic centers and more in the presence of considerable amount of Lewis acidity in these compounds [10]. According to literature study, the main factor to influence transesterification activity is the alkalinity and the type of basic strength of the catalysts [28, 29]. The linearity between FAME yield and total basicity was lightly deviated. HT-1 with lower number of basicity was found; this indicated that medium basic strength is less influencing in transesterification rate. In case of HT-3 and HT-4 with highest number of basicity, the FAME yield was higher than the latter. The author previously reported that the M(II)/Al3+ hydrotalcites at ratio 3.0 showed higher acidity of this catalyst which can be attributed to the dissolution of more amount of Al3+ in the M(II)-O lattice introducing Lewis acidity and also contain high density of Al–O pairs; lower and medium strength basic sites Al3+–O2− pairs do not contribute much to the surface basicity. In contrast, both M(II) and M(III) cations provide Lewis acidic sites [9]. Biodiesel produced from the neem oil was analyzed by gas chromatography. The reaction studied with HT-3 at 65°C and the results indicate neem biodiesel compositions like palmitic acid (C16:0) 13.79%, palmitoleic acid (C16:1) 0.95%, stearic acid (C18:0) 6.33%, oleic acid (C18:1) 42.61%, linoleic acid (C18:2) 26.34%, and linolenic acid (C18:3) 0.06%. The identified composition is compared with standard compounds. From the analysis data confirmed, the product is biodiesel phase of the methyl esters.


## 3.5.1. Effect of Reaction Temperature

The effect of reaction temperature on the ester conversion was studied with the catalyst at various temperatures in Figure3. The transesterification proceeded slowly at 45°C; at lower temperatures it resulted in a drop of the ester conversion because only a small amount of molecules was able to get over the required energy barrier. The ester conversion increased up to 92.5% when reaction temperature close to 65°C. Thus, the optimum temperature for the preparation of the ester was found to be 65°C, which was near the boiling point of anhydrous methanol. The conversion fell to about 60% in the temperature range of 75°C, probably because the molar ratio of methanol to oil decreased when methanol reactant volatilized into gas phase above 65°C, the boiling point of pure methanol.Figure 3
Effect of reaction temperature of HT-3 on conversion of FAME (%).


## 3.5.2. Effect of Molar Ratio of Zn/Mg/Al and Catalytic Studies

The effect of molar ratio of Zn/Mg/Al and the catalytic activity studied at 65°C were illustrated in Figure4, which indicates that the catalytic activity was improved with the increase in Zn and Mg content in Zn/Mg/Al molar ratio at 3 : 3 : 1; but increase in the Mg content in Zn/Mg/Al molar ratio at 3 : 5 : 1, the catalytic activity dropped. The activity decreased in samples due to the formation of surface amorphous Al–O structure that partially covered Mg–O pairs and decreased the concentration surface O2− [15]. The increased catalytic activity of the tertiary oxide system was due to the modification of the electronic properties between the oxides [26]. Table 2 showed various molar ratios of Zn/Mg/Al with product selectivity. The high activity of LDHS is due to the surface site of low (OH− group), medium (Mg–O pairs), and strong (O2− anions) basicity [9]. The catalytic activity of the catalyst is also monitored through the percentage extent of formation of fatty acid methyl ester and glycerol conversion.Table 2
Effect of Zn/Mg/Al molar ratio on product distribution and conversion.
Catalysts
Zn/Mg/Almolar ratio
ConversionWt (%)
Product selectivity Wt (%)
FAME
Glycerol
HT-1
2 : 2 : 1
32
43.49
23.51
HT-2
2 : 3 : 1
43
65.12
19.88
HT-3
3 : 3 : 1
56
92.5
10.02
HT-4
3 : 5 : 1
49
88.3
6.35
Note: FAME: fatty acid methyl ester.
Temperature: 65°C.
Neem oil: methanol: 10 : 1.
Catalyst weight: 7.5 g.Figure 4
Effect of molar ratio of Zn/Mg/Al on conversion of FAME (%) at 65°C.The higher catalytic activity HT-3 indicates the higher acidity of this catalyst which can be attributed to the dissolution of more amount of Al3+ in the M(II)-O lattice introducing Lewis acidity. Also the Zn2+ ions in Mg2+ lattice, the acidic centers submerged in the basic matrix, may be resulting in concomitant acidic-basic centers and more in the presence of considerable amount of Lewis acidity in these compounds [10]. According to literature study, the main factor to influence transesterification activity is the alkalinity and the type of basic strength of the catalysts [28, 29]. The linearity between FAME yield and total basicity was lightly deviated. HT-1 with lower number of basicity was found; this indicated that medium basic strength is less influencing in transesterification rate. In case of HT-3 and HT-4 with highest number of basicity, the FAME yield was higher than the latter. The author previously reported that the M(II)/Al3+ hydrotalcites at ratio 3.0 showed higher acidity of this catalyst which can be attributed to the dissolution of more amount of Al3+ in the M(II)-O lattice introducing Lewis acidity and also contain high density of Al–O pairs; lower and medium strength basic sites Al3+–O2− pairs do not contribute much to the surface basicity. In contrast, both M(II) and M(III) cations provide Lewis acidic sites [9]. Biodiesel produced from the neem oil was analyzed by gas chromatography. The reaction studied with HT-3 at 65°C and the results indicate neem biodiesel compositions like palmitic acid (C16:0) 13.79%, palmitoleic acid (C16:1) 0.95%, stearic acid (C18:0) 6.33%, oleic acid (C18:1) 42.61%, linoleic acid (C18:2) 26.34%, and linolenic acid (C18:3) 0.06%. The identified composition is compared with standard compounds. From the analysis data confirmed, the product is biodiesel phase of the methyl esters.


## 4. Conclusions

The present work has dealt with the transesterification of neem oil was studied in a heterogeneous system using calcined Zn-Mg-Al hydrotalcites as solid base catalysts. The effects on biodiesel production of the methanol/oil molar ratio, reaction temperature, and catalysts amount were studied. Catalysts with Zn-Mg-Al molar ratio 3 : 3 : 1 exhibited maximum catalytic activity for transesterification of neem oil with methanol. The highest triglyceride conversion rate of 92.5% was achieved after 4 h of reaction at 65°C, with a 10 : 1 molar ratio of methanol to neem oil and 7.5 g catalysts. It could be concluded that the calcined nanohydrotalcite is an effective catalysts for the synthesis of biodiesel from neem oil.



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*Source: 326575-2014-08-21.xml*