# Green Biodiesel Synthesis Using Waste Shells as Sustainable Catalysts withCamelina sativa Oil

Authors: Yelda Hangun-Balkir
Journal: Journal of Chemistry
 (2016)

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## Abstract

Waste utilization is an essential component of sustainable development and waste shells are rarely used to generate practical products and processes. Most waste shells are CaCO3 rich, which are converted to CaO once calcined and can be employed as inexpensive and green catalysts for the synthesis of biodiesel. Herein, we utilized lobster and eggshells as green catalysts for the transesterification ofCamelina sativa oil as feedstock into biodiesel.Camelina sativa oil is an appealing crop option as feedstock for biodiesel production because it has high tolerance of cold weather, drought, and low-quality soils and contains approximately 40% oil content. The catalysts from waste shells were characterized by X-ray powder diffraction, Fourier Transform Infrared Spectroscopy, and Scanning Electron Microscope. The product, biodiesel, was studied by 1H NMR and FTIR spectroscopy. The effects of methanol to oil ratio, reaction time, reaction temperature, and catalyst concentration were investigated. Optimum biodiesel yields were attained at a 12 : 1 (alcohol : oil) molar ratio with 1 wt.% heterogeneous catalysts in 3 hours at 65°C. The experimental results exhibited a first-order kinetics and rate constants and activation energy were calculated for the transesterification reaction at different temperatures. The fuel properties of the biodiesel produced fromCamelina sativa oil and waste shells were compared with those of the petroleum-based diesel by using American Society for Testing and Materials (ASTM) standards.


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## Body

## 1. Introduction

Development of alternative fuels has been widely studied because of the depletion of fossil fuels and increased concerns for environment. One of the most promising areas of renewable fuel development is the production of biodiesel. Biodiesel, which is a renewable, nontoxic, and biodegradable fuel, can be used in diesel engines without engine modifications. Biodiesel burns cleaner than conventional diesel fuel, substantially reduces carbon monoxide, hydrocarbons, particulate matter, and eliminates sulfur dioxide emissions [1]. It contributes no net carbon dioxide to the atmosphere and it reduces greenhouse gas emissions by 41% compared with diesel [2]. In addition, biodiesel has high cetane number, high flash point, and excellent lubricity and miscibility with petroleum diesel at all ratios [3].Biodiesel, fatty acid methyl ester (FAME), is traditionally made by transesterification reaction from various types of oils and either ethanol or methanol in presence of a homogeneous catalyst [4]. Transesterification is a reversible process which requires a strong acid or a strong base. The main product of the transesterification reaction is biodiesel and glycerol is formed as a by-product. The transesterification reaction is shown in Figure 1 [5].Figure 1
Transesterification reaction of triglycerides to biodiesel.Most of the current biodiesel production comes from soybean as edible oil feedstock in the United States; as a result production of biodiesel competes for food. Worldwide demand for food is estimated to double within the fifty years and need for fuel is anticipated to increase even more rapidly [6]. There is a great need for biodiesel that does not cause significant environmental harm and does not compete with food supply. Biodiesel that can be produced from inedible crops on agriculturally marginal lands with minimal fertilizer, pesticide, and fossil energy inputs has potential to provide energy over the longer term [7].Camelina sativa oil offers a valuable substitute for the edible oils, becauseCamelina sativa plant grows quickly in infertile grounds.Camelina sativa oil is high in erucic acid and glucosinolates which limits the usage as food [8]. It contains approximately 35–45% oil content and it has lower fertilizer, water, and pesticide requirements than other traditional oilseed crops such as soybean, canola, or corn [9]. It can be grown on soils reclaimed from mine spoils and abandoned farmlands. The crop can stand of extreme climate conditions and poor soil quality and it might be grown in the cycle of crop rotation. The oil has significantly low production cost compared to other crops compared to soybean or corn oils [10].Traditionally, transesterification is achieved in the presence of a homogeneous catalyst such as KOH or NaOH. These widely used catalysts, KOH and NaOH, are easily soluble in methanol, forming potassium methoxide or sodium methoxide, respectively. Although homogeneous catalyzed biodiesel reactions are comparatively faster and show high conversions, they present numerous drawbacks [11]. The homogeneous catalysts cannot be recovered and reused and they must be neutralized and separated from the biodiesel, which causes a generation of excess waste water. The oil feedstock should have low free fatty acids; otherwise the reaction forms soap. The soap formation consumes the catalyst and decreases the efficiency of the reaction. In addition, the soap prevents glycerol separation from biodiesel. Production cost of utilization of homogeneous catalysts is relatively high as the process involves number of washing and purification steps in order to meet quality standards. On the other hand, heterogeneous catalysts are more environmentally benign alternatives to homogeneous counterparts and they have many advantages [12]. The use of heterogeneous catalysts does not cause the soap formation and there is no need for neutralization. Reactions with heterogeneous catalysts have simpler biodiesel separation and purification steps. Heterogeneous catalysts do not produce waste water and they could be easily separated from liquid products by filtration and can be designed to give higher activity, selectivity, and longer lifetimes [13]. The catalysts are reusable which reduces the environmental impact and process cost. Use of heterogeneous catalysts instead of homogeneous catalysts could potentially lead to cheaper production costs and opportunities to operate in a fixed bed continuous process [14]. Overall, they act as energy efficient, nontoxic, and greener option.The production of biodiesel needs an efficient and low-cost heterogeneous catalyst to make the process economically viable and environmentally friendly. Alkaline earth metal oxides were widely studied as basic heterogeneous catalysts for biodiesel synthesis [15]. Calcium oxide was employed specifically as a transesterification catalyst because of its availability, low cost, and excellent catalytic performance under ambient conditions. The reactivity of CaO can be further improved upon calcination. At the beginning of the process, CaO is converted to Ca(OCH3)2, which is an initiating reagent for transesterification reaction, by mixing with methanol [16]. CaO has high basicity and low environmental impact due to its low solubility in methanol [17]. In addition, CaO is easy to handle, abundant, nontoxic, and economically feasible catalyst compared to its homogeneous counterpart, KOH. Both waste eggshell and lobster shells are composed of approximately 95% of calcium carbonate and the remaining components are magnesium carbonate, calcium phosphate, and organic matter [18, 19]. Since the shells mainly consist of CaCO3, they decompose to CaO via calcination. Waste shells, including avian eggshells and seashells, are excellent raw materials for the preparation of the heterogeneous catalysts. For sustainable development, wastes should be recycled and reused towards the production of other goods. Over the years, it has become very costly to dispose the waste shells in landfills and the landfills are reaching their capacity. Waste shells remain largely unutilized as they are discarded wrongly. The waste shells are made up of calcium carbonate that can be used to produce heterogeneous catalysts for biodiesel synthesis. Figure 2 shows a flow diagram for transesterification process fromCamelina oil and waste shells as heterogeneous catalysts.Figure 2
The flowchart for the biodiesel reaction fromCamelina sativa oil and waste shells.Utilization of waste shells as catalysts will protect the environment by reducing the waste and create cost-effective biodiesel synthesis. In this paper, we utilized waste eggshells, lobster shells, and CaO as exemplary heterogeneous catalysts for the transesterification ofCamelina sativa oil into biodiesel. The parameters such as methanol to oil ratio, reaction time, reaction temperature, and catalyst concentration were studied and a kinetic study was performed by using the data obtained from the optimization experiments. The study demonstrates several fundamental green principles including the use of renewable feedstocks, catalysis, and design for degradation.


## 2. Materials and Methods

Cold-pressed and unrefinedCamelina sativa oil was obtained from Ole World Oils Company. Calcium oxide was purchased from Alfa Aesar. Waste eggshells and lobster shells were collected from college’s cafeteria and neighborhood restaurants. Anhydrous methanol was purchased from Fischer Scientific.


### 2.1. Catalyst Preparation

Calcium oxide was used as it was received. The eggshells and lobster shells were rinsed with tap water to remove organic materials and impurities and dried at 110°C for 2 hours. The dried waste shells were grinded and calcined at 900°C in air atmosphere with a heating rate of 10°C per minute for 3 hours. All catalysts were kept in a desiccator to avoid the interaction with air. The raw and calcined samples of the shells were analyzed by X-ray powder diffraction (XRD), Fourier Transform Infrared Spectroscopy (FTIR), and Scanning Electron Microscope (SEM). The XRD characterization was studied on Bruker X-Ray D-2 Phaser diffractometer over a 2θ range from 5° to 60° with a step size of 0.01° and FTIR spectroscopy was performed on Thermo Nexus 470 FTIR spectrometer. The spectra were obtained in the 500–4000 cm−1 region and 32 scans were recorded. Surface structure and the morphology of the heterogeneous catalysts were studied by Zeiss LEO Gemini 1550 Scanning Electron Microscope (SEM).


### 2.2. Characteristics ofCamelina sativa Oil

Fatty acid composition ofCamelina sativa oil, which was provided by the manufacturer, indicates 32.4%, 18.4%, 16.0%, and 15.1% as α-Linolenic Acid (18 : 3), Linoleic Acid (18 : 2), Oleic Acid (18 : 1), and cis-Eicosenoic Acid (20 : 1), respectively. The acid value ofCamelina sativa oil was reported as 1.58% of free fatty acid [20]. As stated by the literature, the yield of biodiesel significantly decreases when the free fatty acid level exceeds 3% (w/w), since the soap formation inhibits the separation between the biodiesel and glycerol and decreases the yield of the final product [21]. Table 1 shows the properties ofCamelina sativa oil.Table 1
Properties ofCamelina sativa oil.
Specific gravity Viscosity Caloric value Acid value Cetane number Pour point (°C) 0.92 14.6 44.5 3.20 35.80 −23


### 2.3. Transesterification Reaction

The transesterification reaction was performed using 500 mL round bottom flask with a magnetic stirrer, thermometer, and reflux condenser. 100 mL ofCamelina sativa oil was heated to 100°C for one hour to remove impurities before starting the transesterification reaction. The oil was allowed to cool down to 65°C. The reaction was carried out with a 12 : 1 molar ratio of methanol : oil ratio and 1% (w/w) of the chosen waste shell catalyst. Pulverized, calcined waste shell was stirred with methanol at 65°C for one hour to activate waste shell catalyst. The mixture was added to the oil and vigorously stirred at 65°C for 3 hours to ensure complete conversion of the oil into biodiesel. The waste shell catalyst was recovered through filtration and the reaction mixture transferred to separatory funnel was allowed to settle for 1 hour. The lower layer, which contains glycerol, was removed from the methyl esters. Due to the low solubility of glycerol in the esters, the separation takes place rapidly. The crude biodiesel remained in the top layer. Yellow color biodiesel was dried using anhydrous sodium sulfate. The yield of biodiesel was calculated by using the following equation:(1)%Yield=Weight  of  BiodieselWeigth  of  Camelina  Oil×100.The conversion of oil to biodiesel was analyzed by 1H NMR and FTIR spectroscopies. An Eft-60 NMR spectrometer (Anasazi Instruments, Indianapolis, IN) and a Thermo Nicolet NEXUS 470 FTIR spectrometer (Thermo Scientific, Waltham, MA) were used for the analyses. The FTIR spectra of the samples were obtained in the 500–4000 cm−1 region after 32 scans were recorded for each sample. The quality of biodiesel product was analyzed according to American Society for Testing and Materials (ASTM) specifications designated in D-6751.


## 2.1. Catalyst Preparation

Calcium oxide was used as it was received. The eggshells and lobster shells were rinsed with tap water to remove organic materials and impurities and dried at 110°C for 2 hours. The dried waste shells were grinded and calcined at 900°C in air atmosphere with a heating rate of 10°C per minute for 3 hours. All catalysts were kept in a desiccator to avoid the interaction with air. The raw and calcined samples of the shells were analyzed by X-ray powder diffraction (XRD), Fourier Transform Infrared Spectroscopy (FTIR), and Scanning Electron Microscope (SEM). The XRD characterization was studied on Bruker X-Ray D-2 Phaser diffractometer over a 2θ range from 5° to 60° with a step size of 0.01° and FTIR spectroscopy was performed on Thermo Nexus 470 FTIR spectrometer. The spectra were obtained in the 500–4000 cm−1 region and 32 scans were recorded. Surface structure and the morphology of the heterogeneous catalysts were studied by Zeiss LEO Gemini 1550 Scanning Electron Microscope (SEM).


## 2.2. Characteristics ofCamelina sativa Oil

Fatty acid composition ofCamelina sativa oil, which was provided by the manufacturer, indicates 32.4%, 18.4%, 16.0%, and 15.1% as α-Linolenic Acid (18 : 3), Linoleic Acid (18 : 2), Oleic Acid (18 : 1), and cis-Eicosenoic Acid (20 : 1), respectively. The acid value ofCamelina sativa oil was reported as 1.58% of free fatty acid [20]. As stated by the literature, the yield of biodiesel significantly decreases when the free fatty acid level exceeds 3% (w/w), since the soap formation inhibits the separation between the biodiesel and glycerol and decreases the yield of the final product [21]. Table 1 shows the properties ofCamelina sativa oil.Table 1
Properties ofCamelina sativa oil.
Specific gravity Viscosity Caloric value Acid value Cetane number Pour point (°C) 0.92 14.6 44.5 3.20 35.80 −23


## 2.3. Transesterification Reaction

The transesterification reaction was performed using 500 mL round bottom flask with a magnetic stirrer, thermometer, and reflux condenser. 100 mL ofCamelina sativa oil was heated to 100°C for one hour to remove impurities before starting the transesterification reaction. The oil was allowed to cool down to 65°C. The reaction was carried out with a 12 : 1 molar ratio of methanol : oil ratio and 1% (w/w) of the chosen waste shell catalyst. Pulverized, calcined waste shell was stirred with methanol at 65°C for one hour to activate waste shell catalyst. The mixture was added to the oil and vigorously stirred at 65°C for 3 hours to ensure complete conversion of the oil into biodiesel. The waste shell catalyst was recovered through filtration and the reaction mixture transferred to separatory funnel was allowed to settle for 1 hour. The lower layer, which contains glycerol, was removed from the methyl esters. Due to the low solubility of glycerol in the esters, the separation takes place rapidly. The crude biodiesel remained in the top layer. Yellow color biodiesel was dried using anhydrous sodium sulfate. The yield of biodiesel was calculated by using the following equation:(1)%Yield=Weight  of  BiodieselWeigth  of  Camelina  Oil×100.The conversion of oil to biodiesel was analyzed by 1H NMR and FTIR spectroscopies. An Eft-60 NMR spectrometer (Anasazi Instruments, Indianapolis, IN) and a Thermo Nicolet NEXUS 470 FTIR spectrometer (Thermo Scientific, Waltham, MA) were used for the analyses. The FTIR spectra of the samples were obtained in the 500–4000 cm−1 region after 32 scans were recorded for each sample. The quality of biodiesel product was analyzed according to American Society for Testing and Materials (ASTM) specifications designated in D-6751.


## 3. Results and Discussion

The percent conversions ofCamelina oil with CaO, waste eggshell, and lobster shell catalysts to biodiesel are 99.1%, 97.2%, and 90.0%, for the given reaction conditions, respectively.


### 3.1. Catalyst Characterization

#### 3.1.1. X-Ray Diffraction Analysis

The XRD patterns of raw and calcined lobster shell are given in Figure3. The calcination at 900°C causes the removal of CO2 from CaCO3 in the natural waste lobster shell and results in CaO [22]. Narrow and high intense peaks of the calcined catalyst define the well-crystallized structure of the CaO. Figure 4 shows the XRD patterns for calcined eggshell, lobster shell, and commercial CaO. The waste shell catalysts showed clear and sharp peaks which match the crystalline phase of CaO. The peaks for both calcined eggshell and lobster shell at 900°C show 2θ values of 32.40, 37.50, and 54.10 which are the characteristic peaks for CaO [23].Figure 3
XRD pattern of raw and calcined lobster shell.Figure 4
XRD pattern of calcined CaO, eggshell, and lobster shell.


#### 3.1.2. FTIR Analysis

FTIR spectroscopy with Smart Diffuse Reflectance, which was used for characterization of the uncalcined (raw) and calcined lobster shells, is shown in Figure5. KBr was used as infrared transparent matrix for characterization. The broad absorption band at around 3420 cm−1 is most likely due to O-H vibrations in water molecules. The absorption bands of uncalcined lobster shell at 1425 cm−1, 878 cm−1, and 710 cm−1 were attributed to asymmetric stretch, out-of-plane bend, and in-plane bend, respectively, of CO32- ions. The broad absorption band around 3420 cm−1 disappears upon calcination at 900°C. Calcination causes the lobster shell to lose carbonate since CaCO3 decomposes into CaO. While the intensity of CaCO3 peaks decreases, a new sharp stretching band appears at 3630 cm−1 which is corresponding to O-H stretching vibration. The peaks around 1450 cm−1 correspond to the bending vibration of O-Ca-O group. A detailed study about temperature effects on shells was published by Engin et al. and our results agree with the literature findings [24]. Figure 6 shows the FTIR spectra of calcined CaO, lobster, and eggshell. Both waste shells have the same absorption bands as the bands of CaO.Figure 5
Infrared spectrum of uncalcined and calcined lobster shell.Figure 6
Infrared spectrum of calcined CaO, eggshell, and lobster shell.


#### 3.1.3. SEM Analysis

The surface morphology of uncalcined and calcined lobster shell catalysts is shown in Figure7. The uncalcined shells display a typical layered architecture [25]. Both uncalcined and calcined shells contain various sized and shaped particles. The morphology of CaO, waste lobster, and waste eggshell calcined at 900°C is shown in Figure 8. Calcined lobster shell shows regular morphology of sphere particles with the size range from 1.20 to 5.0 μm of width. Upon calcination, the microstructures of the shells are changed from layered architecture to porous structure. The particle shape became more regular with smaller particles as a result of release of gaseous molecules. Calcination of the catalyst derived from the waste shells causes an increase in surface area, leading to better catalytic activity [26]. The small particles were combined together to yield agglomerates because of CaO formation from calcium carbonate decomposition during the calcination process.Figure 7
SEM images of uncalcined and calcined lobster shell.
(a)
Uncalcined lobster shell (b)
Calcined lobster shellFigure 8
SEM images of calcined CaO, lobster, and eggshell.
(a)
Calcined CaO (b)
Calcined lobster shell (c)
Calcined eggshell


### 3.2. Analysis of Biodiesel

#### 3.2.1. NMR Analysis

The conversion ofCamelina sativa oil to biodiesel catalyzed by waste shells was analyzed by using 1H NMR spectroscopy. The spectra for startingCamelina sativa oil and biodiesel are shown in Figure 9. Starting oil has a 4.35 ppm signal which was lost during the transesterification reaction. The biodiesel spectra showed the characteristic peak of methoxy protons that was prominently indicated by a strong singlet at 3.68 ppm and α-CH2 protons as a triplet at 2.30 ppm. These two peaks confirm the presence of fatty acid methyl ester formation from starting oil. The other peaks were observed at 0.8 ppm due to terminal methyl protons; a strong peak at 1.3 ppm is related to the methylene protons of carbon chain, and multiplet at 2.1 ppm is due to β-carbonyl methylene protons, respectively. The peak at 5.4 ppm is solely due to olefinic protons on the carbon chain.Figure 9
1H NMR spectra ofCamelina oil and synthesized biodiesel catalyzed by waste lobster shells.


#### 3.2.2. FTIR Analysis

FTIR spectroscopy was used to analyze biodiesel and the spectrum is shown in Figure10. The most intense peak at 1745 cm−1 is the characteristic of the ester carbonyl stretch, ester -C=O. The absorption bands at 1248, 1198, and 1176 cm−1 can be used to identify the methyl ester C-O-C stretching vibrations in the biodiesel. The absorption bands at 2850 and 2925 indicate the axial deformation of CH2 bond. While the stretching vibrations of CH appear at 3050 cm−1; a weak absorption band at 3445 cm−1 indicates OH stretching vibration. The bands at 1465 and 1448 cm−1 are the indication of CH2 and CH3 bending vibrations.Figure 10
FTIR spectra of biodiesel catalyzed by waste lobster shells.


### 3.3. Effect of Parameters on Biodiesel Synthesis

#### 3.3.1. Effect of Methanol toCamelina sativa Oil Molar Ratio on Biodiesel Yield

Methanol to oil molar ratio was varied from 6 : 1 to 18 : 1 while catalyst concentration and temperature were kept constant at 1% (w/w) and 65°C, respectively. Figure11(a) shows the effect of methanol to oil molar ratio on biodiesel yield for CaO, eggshell, and lobster shell catalyzed transesterification reaction. While the transesterification ofCamelina oil requires three moles of methanol for each mole of oil, excess methanol is required to shift the equilibrium towards the direction of biodiesel formation. The high amount of methanol promotes the formation of methoxy species which leads to higher yields. The biodiesel yield sharply increased while the molar ratio was increased from 6 : 1 to 12 : 1 and slightly decreased exceeding 12 : 1 methanol to oil ratio. According to literature, excess methanol inhibits the separation of glycerol since there is an increase in solubility [27]. Higher amount of glycerol drives the equilibrium back to the left and lowering the yield of biodiesel. The maximum yield was achieved at 12 : 1 molar ratio.Figure 11
Effects of the (a) methanol to oil molar ratio, (b) reaction time, (c) reaction temperature, and (d) catalyst concentration on the biodiesel yield.
(a) (b) (c) (d)


#### 3.3.2. Effect of Reaction Time on Biodiesel Yield

The biodiesel yield was significantly affected by reaction time which was varied from 1 hour to 6 hours for experiments with three heterogeneous catalysts. During the trials, the methanol to oil molar ratio, catalyst concentration, and temperature were kept at 12 : 1 and 1% (w/w) and 65°C, respectively. As shown in Figure11(b), as reaction time was increased from 1 to 3 hours, the yield increased for all catalysts. Longer reaction time may enhance the probability of contact between methanol andCamelina oil with catalysts’ basic sites which improve the biodiesel yield. The yield slightly decreased after 3 hours which may be attributed to hydrolysis of methyl esters.


#### 3.3.3. Effect of Reaction Temperature on Biodiesel Yield

The effect of the reaction temperature on the product yield is shown in Figure11(c). Throughout the experiments, the methanol to oil molar ratio and catalyst concentration were kept at 12 : 1 and 1% (w/w), respectively. Reaction temperature was a significant factor in biodiesel synthesis as the yield increased significantly for all three catalysts between 25°C and 65°C. Addition of heterogeneous catalysts to reaction creates a triple phase system, oil-methanol-catalyst, and the interface of the triple phase probably accommodates the transesterification process [28]. Increasing reaction temperature reduces the viscosity ofCamelina oil and enhances the product yield because of the inhibition of mass transfer resistance. For all catalysts, biodiesel yields were low at low temperatures. Optimum yields (99%, 97%, and 90% for CaO, eggshell, and lobster shell, resp.) were achieved when the reactions’ temperature was held at 65°C. Further increase in temperature caused a decrease in biodiesel yield for all three catalysts which may be attributed to evaporation of methanol.


#### 3.3.4. Effect of Catalyst Concentration on Biodiesel Yield

The yield of biodiesel was greatly dependent on the catalyst concentration. Reactions were carried out with different concentrations of catalysts, ranging from 0.25 to 2 weight%, and the results are illustrated in Figure11(d). The reactions were carried out at 65°C for 3 hours with a methanol to oil ratio of 12 : 1. There was a significant increase in yield for all catalysts from 0.25% to 1.0% and optimum conversion was obtained for 1.0 wt.% catalyst concentration. Pretreating catalysts with methanol, a small amount of CaO was converted into Ca(OCH3)2, which acted as the initiating reagent for transesterification. The catalysts provide active basic sites that transform the methanol into methoxide which attacks the carbonyl carbon structure of oil. As the concentration of catalyst increases, the available active sites also increase leading to the improvement of biodiesel yield [29]. Beyond 1%, the yield was not greatly affected by catalysts’ concentration because the reaction mixture became more viscous and all active sites are loaded.


### 3.4. Kinetic Studies

Kinetic studies of the transesterification reaction ofCamelina sativa oil were performed by lobster waste shell heterogeneous catalyst at three different temperatures, 50°C, 65°C, and 70°C, while the methanol to oil molar ratio and catalyst concentration were kept at 12 : 1 and 1% (w/w). As expected, decrease in temperature from 70°C to 50°C causes decrease in reaction rates. Rate expression of the reaction is shown as follows [30]:(2)-Rate=-dCS  Oildt=kCS  Oil.[CS Oil] represents the concentration ofCamelina sativa oil. Excess methanol was used in the reaction in order to shift the equilibrium towards the product side. Since methanol does not affect the overall order, the transesterification reaction was assumed to follow first-order kinetics [31]. The integration of (2) results as(3)ln⁡CS  Oil0-ln⁡CS  Oilt=kt.The initial concentration ofCamelina oil and the concentration ofCamelina oil at time, t, are shown as CS  Oil0 and ln⁡CS  Oilt, respectively. The fraction conversion ofCamelina biodiesel, XFAME, can be cooperated into (3) as (4)dXFAMEdt=k1-XFAMEand the integration of the equation becomes(5)-ln⁡1-XFAME=kt.Figure 12 shows the graph between ln⁡1-XFAME and time at the three temperatures to obtain rate constant values. The plots are linear plots at three temperatures which indicate that the transesterification reaction obeys first-order kinetics.Figure 12
Plot ofln⁡(1-XFAME) versus time of the transesterification reaction catalyzed by waste lobster shells.Arrhenius equation was utilized to calculate the activation energy and preexponential factor for the transesterification reaction ofCamelina oil catalyzed by waste lobster shells. The activation energy and preexponential factor were determined as 62.5 kJ mol−1 and 7.62 × 107 min−1, respectively, by Arrhenius plot shown in Figure 13.Figure 13
Arrhenius plot ofln⁡k and 1/T of the transesterification reaction catalyzed by waste lobster shells.


### 3.5. Fuel Properties ofCamelina Biodiesel

Biodiesel was characterized for its fuel properties by ASTM D287, 445, 240, 613, and 97 methods. Table2 shows the properties of the synthesized biodiesel and petroleum biodiesel. The comparison showed that most of the fuel properties of theCamelina biodiesel are quite comparable to those of ASTM petroleum diesel standards [32]. The kinematic viscosity ofCamelina based biodiesel was similar to regular diesel fuel viscosity so no modifications of engine are required. The cetane number was found higher than regular diesel standards. Cetane number is a measure of a fuel’s autoignition quality characteristics. Since biodiesel is largely composed of aliphatic hydrocarbons, it usually has a higher cetane number than petroleum diesel [33]. Higher cetane number indicates more complete combustion of the fuel, better fuel efficiency, and quick ignition delay time of fuel. The pour point ofCamelina biodiesel shows a good compatibility for places with cold climate.Table 2
Fuel properties ofCamelina, petroleum diesel and the ASTM biodiesel standards.
Properties Petroleum diesel Camelina biodiesel Biodiesel standards (ASTM D6751) ASTM testing method Unit Kinematic viscosity (40°C) 2.6 3.1 1.9–6.0 D4451 mm2/s Specific gravity 0.85 0.88 0.87–0.90 D287 Calorific value 42 46  D240 MJ/kg Pour point −20 −10 −5 to 10 D97 °C Cetane number 46 49 47–65 D613 min


## 3.1. Catalyst Characterization

### 3.1.1. X-Ray Diffraction Analysis

The XRD patterns of raw and calcined lobster shell are given in Figure3. The calcination at 900°C causes the removal of CO2 from CaCO3 in the natural waste lobster shell and results in CaO [22]. Narrow and high intense peaks of the calcined catalyst define the well-crystallized structure of the CaO. Figure 4 shows the XRD patterns for calcined eggshell, lobster shell, and commercial CaO. The waste shell catalysts showed clear and sharp peaks which match the crystalline phase of CaO. The peaks for both calcined eggshell and lobster shell at 900°C show 2θ values of 32.40, 37.50, and 54.10 which are the characteristic peaks for CaO [23].Figure 3
XRD pattern of raw and calcined lobster shell.Figure 4
XRD pattern of calcined CaO, eggshell, and lobster shell.


### 3.1.2. FTIR Analysis

FTIR spectroscopy with Smart Diffuse Reflectance, which was used for characterization of the uncalcined (raw) and calcined lobster shells, is shown in Figure5. KBr was used as infrared transparent matrix for characterization. The broad absorption band at around 3420 cm−1 is most likely due to O-H vibrations in water molecules. The absorption bands of uncalcined lobster shell at 1425 cm−1, 878 cm−1, and 710 cm−1 were attributed to asymmetric stretch, out-of-plane bend, and in-plane bend, respectively, of CO32- ions. The broad absorption band around 3420 cm−1 disappears upon calcination at 900°C. Calcination causes the lobster shell to lose carbonate since CaCO3 decomposes into CaO. While the intensity of CaCO3 peaks decreases, a new sharp stretching band appears at 3630 cm−1 which is corresponding to O-H stretching vibration. The peaks around 1450 cm−1 correspond to the bending vibration of O-Ca-O group. A detailed study about temperature effects on shells was published by Engin et al. and our results agree with the literature findings [24]. Figure 6 shows the FTIR spectra of calcined CaO, lobster, and eggshell. Both waste shells have the same absorption bands as the bands of CaO.Figure 5
Infrared spectrum of uncalcined and calcined lobster shell.Figure 6
Infrared spectrum of calcined CaO, eggshell, and lobster shell.


### 3.1.3. SEM Analysis

The surface morphology of uncalcined and calcined lobster shell catalysts is shown in Figure7. The uncalcined shells display a typical layered architecture [25]. Both uncalcined and calcined shells contain various sized and shaped particles. The morphology of CaO, waste lobster, and waste eggshell calcined at 900°C is shown in Figure 8. Calcined lobster shell shows regular morphology of sphere particles with the size range from 1.20 to 5.0 μm of width. Upon calcination, the microstructures of the shells are changed from layered architecture to porous structure. The particle shape became more regular with smaller particles as a result of release of gaseous molecules. Calcination of the catalyst derived from the waste shells causes an increase in surface area, leading to better catalytic activity [26]. The small particles were combined together to yield agglomerates because of CaO formation from calcium carbonate decomposition during the calcination process.Figure 7
SEM images of uncalcined and calcined lobster shell.
(a)
Uncalcined lobster shell (b)
Calcined lobster shellFigure 8
SEM images of calcined CaO, lobster, and eggshell.
(a)
Calcined CaO (b)
Calcined lobster shell (c)
Calcined eggshell


## 3.1.1. X-Ray Diffraction Analysis

The XRD patterns of raw and calcined lobster shell are given in Figure3. The calcination at 900°C causes the removal of CO2 from CaCO3 in the natural waste lobster shell and results in CaO [22]. Narrow and high intense peaks of the calcined catalyst define the well-crystallized structure of the CaO. Figure 4 shows the XRD patterns for calcined eggshell, lobster shell, and commercial CaO. The waste shell catalysts showed clear and sharp peaks which match the crystalline phase of CaO. The peaks for both calcined eggshell and lobster shell at 900°C show 2θ values of 32.40, 37.50, and 54.10 which are the characteristic peaks for CaO [23].Figure 3
XRD pattern of raw and calcined lobster shell.Figure 4
XRD pattern of calcined CaO, eggshell, and lobster shell.


## 3.1.2. FTIR Analysis

FTIR spectroscopy with Smart Diffuse Reflectance, which was used for characterization of the uncalcined (raw) and calcined lobster shells, is shown in Figure5. KBr was used as infrared transparent matrix for characterization. The broad absorption band at around 3420 cm−1 is most likely due to O-H vibrations in water molecules. The absorption bands of uncalcined lobster shell at 1425 cm−1, 878 cm−1, and 710 cm−1 were attributed to asymmetric stretch, out-of-plane bend, and in-plane bend, respectively, of CO32- ions. The broad absorption band around 3420 cm−1 disappears upon calcination at 900°C. Calcination causes the lobster shell to lose carbonate since CaCO3 decomposes into CaO. While the intensity of CaCO3 peaks decreases, a new sharp stretching band appears at 3630 cm−1 which is corresponding to O-H stretching vibration. The peaks around 1450 cm−1 correspond to the bending vibration of O-Ca-O group. A detailed study about temperature effects on shells was published by Engin et al. and our results agree with the literature findings [24]. Figure 6 shows the FTIR spectra of calcined CaO, lobster, and eggshell. Both waste shells have the same absorption bands as the bands of CaO.Figure 5
Infrared spectrum of uncalcined and calcined lobster shell.Figure 6
Infrared spectrum of calcined CaO, eggshell, and lobster shell.


## 3.1.3. SEM Analysis

The surface morphology of uncalcined and calcined lobster shell catalysts is shown in Figure7. The uncalcined shells display a typical layered architecture [25]. Both uncalcined and calcined shells contain various sized and shaped particles. The morphology of CaO, waste lobster, and waste eggshell calcined at 900°C is shown in Figure 8. Calcined lobster shell shows regular morphology of sphere particles with the size range from 1.20 to 5.0 μm of width. Upon calcination, the microstructures of the shells are changed from layered architecture to porous structure. The particle shape became more regular with smaller particles as a result of release of gaseous molecules. Calcination of the catalyst derived from the waste shells causes an increase in surface area, leading to better catalytic activity [26]. The small particles were combined together to yield agglomerates because of CaO formation from calcium carbonate decomposition during the calcination process.Figure 7
SEM images of uncalcined and calcined lobster shell.
(a)
Uncalcined lobster shell (b)
Calcined lobster shellFigure 8
SEM images of calcined CaO, lobster, and eggshell.
(a)
Calcined CaO (b)
Calcined lobster shell (c)
Calcined eggshell


## 3.2. Analysis of Biodiesel

### 3.2.1. NMR Analysis

The conversion ofCamelina sativa oil to biodiesel catalyzed by waste shells was analyzed by using 1H NMR spectroscopy. The spectra for startingCamelina sativa oil and biodiesel are shown in Figure 9. Starting oil has a 4.35 ppm signal which was lost during the transesterification reaction. The biodiesel spectra showed the characteristic peak of methoxy protons that was prominently indicated by a strong singlet at 3.68 ppm and α-CH2 protons as a triplet at 2.30 ppm. These two peaks confirm the presence of fatty acid methyl ester formation from starting oil. The other peaks were observed at 0.8 ppm due to terminal methyl protons; a strong peak at 1.3 ppm is related to the methylene protons of carbon chain, and multiplet at 2.1 ppm is due to β-carbonyl methylene protons, respectively. The peak at 5.4 ppm is solely due to olefinic protons on the carbon chain.Figure 9
1H NMR spectra ofCamelina oil and synthesized biodiesel catalyzed by waste lobster shells.


### 3.2.2. FTIR Analysis

FTIR spectroscopy was used to analyze biodiesel and the spectrum is shown in Figure10. The most intense peak at 1745 cm−1 is the characteristic of the ester carbonyl stretch, ester -C=O. The absorption bands at 1248, 1198, and 1176 cm−1 can be used to identify the methyl ester C-O-C stretching vibrations in the biodiesel. The absorption bands at 2850 and 2925 indicate the axial deformation of CH2 bond. While the stretching vibrations of CH appear at 3050 cm−1; a weak absorption band at 3445 cm−1 indicates OH stretching vibration. The bands at 1465 and 1448 cm−1 are the indication of CH2 and CH3 bending vibrations.Figure 10
FTIR spectra of biodiesel catalyzed by waste lobster shells.


## 3.2.1. NMR Analysis

The conversion ofCamelina sativa oil to biodiesel catalyzed by waste shells was analyzed by using 1H NMR spectroscopy. The spectra for startingCamelina sativa oil and biodiesel are shown in Figure 9. Starting oil has a 4.35 ppm signal which was lost during the transesterification reaction. The biodiesel spectra showed the characteristic peak of methoxy protons that was prominently indicated by a strong singlet at 3.68 ppm and α-CH2 protons as a triplet at 2.30 ppm. These two peaks confirm the presence of fatty acid methyl ester formation from starting oil. The other peaks were observed at 0.8 ppm due to terminal methyl protons; a strong peak at 1.3 ppm is related to the methylene protons of carbon chain, and multiplet at 2.1 ppm is due to β-carbonyl methylene protons, respectively. The peak at 5.4 ppm is solely due to olefinic protons on the carbon chain.Figure 9
1H NMR spectra ofCamelina oil and synthesized biodiesel catalyzed by waste lobster shells.


## 3.2.2. FTIR Analysis

FTIR spectroscopy was used to analyze biodiesel and the spectrum is shown in Figure10. The most intense peak at 1745 cm−1 is the characteristic of the ester carbonyl stretch, ester -C=O. The absorption bands at 1248, 1198, and 1176 cm−1 can be used to identify the methyl ester C-O-C stretching vibrations in the biodiesel. The absorption bands at 2850 and 2925 indicate the axial deformation of CH2 bond. While the stretching vibrations of CH appear at 3050 cm−1; a weak absorption band at 3445 cm−1 indicates OH stretching vibration. The bands at 1465 and 1448 cm−1 are the indication of CH2 and CH3 bending vibrations.Figure 10
FTIR spectra of biodiesel catalyzed by waste lobster shells.


## 3.3. Effect of Parameters on Biodiesel Synthesis

### 3.3.1. Effect of Methanol toCamelina sativa Oil Molar Ratio on Biodiesel Yield

Methanol to oil molar ratio was varied from 6 : 1 to 18 : 1 while catalyst concentration and temperature were kept constant at 1% (w/w) and 65°C, respectively. Figure11(a) shows the effect of methanol to oil molar ratio on biodiesel yield for CaO, eggshell, and lobster shell catalyzed transesterification reaction. While the transesterification ofCamelina oil requires three moles of methanol for each mole of oil, excess methanol is required to shift the equilibrium towards the direction of biodiesel formation. The high amount of methanol promotes the formation of methoxy species which leads to higher yields. The biodiesel yield sharply increased while the molar ratio was increased from 6 : 1 to 12 : 1 and slightly decreased exceeding 12 : 1 methanol to oil ratio. According to literature, excess methanol inhibits the separation of glycerol since there is an increase in solubility [27]. Higher amount of glycerol drives the equilibrium back to the left and lowering the yield of biodiesel. The maximum yield was achieved at 12 : 1 molar ratio.Figure 11
Effects of the (a) methanol to oil molar ratio, (b) reaction time, (c) reaction temperature, and (d) catalyst concentration on the biodiesel yield.
(a) (b) (c) (d)


### 3.3.2. Effect of Reaction Time on Biodiesel Yield

The biodiesel yield was significantly affected by reaction time which was varied from 1 hour to 6 hours for experiments with three heterogeneous catalysts. During the trials, the methanol to oil molar ratio, catalyst concentration, and temperature were kept at 12 : 1 and 1% (w/w) and 65°C, respectively. As shown in Figure11(b), as reaction time was increased from 1 to 3 hours, the yield increased for all catalysts. Longer reaction time may enhance the probability of contact between methanol andCamelina oil with catalysts’ basic sites which improve the biodiesel yield. The yield slightly decreased after 3 hours which may be attributed to hydrolysis of methyl esters.


### 3.3.3. Effect of Reaction Temperature on Biodiesel Yield

The effect of the reaction temperature on the product yield is shown in Figure11(c). Throughout the experiments, the methanol to oil molar ratio and catalyst concentration were kept at 12 : 1 and 1% (w/w), respectively. Reaction temperature was a significant factor in biodiesel synthesis as the yield increased significantly for all three catalysts between 25°C and 65°C. Addition of heterogeneous catalysts to reaction creates a triple phase system, oil-methanol-catalyst, and the interface of the triple phase probably accommodates the transesterification process [28]. Increasing reaction temperature reduces the viscosity ofCamelina oil and enhances the product yield because of the inhibition of mass transfer resistance. For all catalysts, biodiesel yields were low at low temperatures. Optimum yields (99%, 97%, and 90% for CaO, eggshell, and lobster shell, resp.) were achieved when the reactions’ temperature was held at 65°C. Further increase in temperature caused a decrease in biodiesel yield for all three catalysts which may be attributed to evaporation of methanol.


### 3.3.4. Effect of Catalyst Concentration on Biodiesel Yield

The yield of biodiesel was greatly dependent on the catalyst concentration. Reactions were carried out with different concentrations of catalysts, ranging from 0.25 to 2 weight%, and the results are illustrated in Figure11(d). The reactions were carried out at 65°C for 3 hours with a methanol to oil ratio of 12 : 1. There was a significant increase in yield for all catalysts from 0.25% to 1.0% and optimum conversion was obtained for 1.0 wt.% catalyst concentration. Pretreating catalysts with methanol, a small amount of CaO was converted into Ca(OCH3)2, which acted as the initiating reagent for transesterification. The catalysts provide active basic sites that transform the methanol into methoxide which attacks the carbonyl carbon structure of oil. As the concentration of catalyst increases, the available active sites also increase leading to the improvement of biodiesel yield [29]. Beyond 1%, the yield was not greatly affected by catalysts’ concentration because the reaction mixture became more viscous and all active sites are loaded.


## 3.3.1. Effect of Methanol toCamelina sativa Oil Molar Ratio on Biodiesel Yield

Methanol to oil molar ratio was varied from 6 : 1 to 18 : 1 while catalyst concentration and temperature were kept constant at 1% (w/w) and 65°C, respectively. Figure11(a) shows the effect of methanol to oil molar ratio on biodiesel yield for CaO, eggshell, and lobster shell catalyzed transesterification reaction. While the transesterification ofCamelina oil requires three moles of methanol for each mole of oil, excess methanol is required to shift the equilibrium towards the direction of biodiesel formation. The high amount of methanol promotes the formation of methoxy species which leads to higher yields. The biodiesel yield sharply increased while the molar ratio was increased from 6 : 1 to 12 : 1 and slightly decreased exceeding 12 : 1 methanol to oil ratio. According to literature, excess methanol inhibits the separation of glycerol since there is an increase in solubility [27]. Higher amount of glycerol drives the equilibrium back to the left and lowering the yield of biodiesel. The maximum yield was achieved at 12 : 1 molar ratio.Figure 11
Effects of the (a) methanol to oil molar ratio, (b) reaction time, (c) reaction temperature, and (d) catalyst concentration on the biodiesel yield.
(a) (b) (c) (d)


## 3.3.2. Effect of Reaction Time on Biodiesel Yield

The biodiesel yield was significantly affected by reaction time which was varied from 1 hour to 6 hours for experiments with three heterogeneous catalysts. During the trials, the methanol to oil molar ratio, catalyst concentration, and temperature were kept at 12 : 1 and 1% (w/w) and 65°C, respectively. As shown in Figure11(b), as reaction time was increased from 1 to 3 hours, the yield increased for all catalysts. Longer reaction time may enhance the probability of contact between methanol andCamelina oil with catalysts’ basic sites which improve the biodiesel yield. The yield slightly decreased after 3 hours which may be attributed to hydrolysis of methyl esters.


## 3.3.3. Effect of Reaction Temperature on Biodiesel Yield

The effect of the reaction temperature on the product yield is shown in Figure11(c). Throughout the experiments, the methanol to oil molar ratio and catalyst concentration were kept at 12 : 1 and 1% (w/w), respectively. Reaction temperature was a significant factor in biodiesel synthesis as the yield increased significantly for all three catalysts between 25°C and 65°C. Addition of heterogeneous catalysts to reaction creates a triple phase system, oil-methanol-catalyst, and the interface of the triple phase probably accommodates the transesterification process [28]. Increasing reaction temperature reduces the viscosity ofCamelina oil and enhances the product yield because of the inhibition of mass transfer resistance. For all catalysts, biodiesel yields were low at low temperatures. Optimum yields (99%, 97%, and 90% for CaO, eggshell, and lobster shell, resp.) were achieved when the reactions’ temperature was held at 65°C. Further increase in temperature caused a decrease in biodiesel yield for all three catalysts which may be attributed to evaporation of methanol.


## 3.3.4. Effect of Catalyst Concentration on Biodiesel Yield

The yield of biodiesel was greatly dependent on the catalyst concentration. Reactions were carried out with different concentrations of catalysts, ranging from 0.25 to 2 weight%, and the results are illustrated in Figure11(d). The reactions were carried out at 65°C for 3 hours with a methanol to oil ratio of 12 : 1. There was a significant increase in yield for all catalysts from 0.25% to 1.0% and optimum conversion was obtained for 1.0 wt.% catalyst concentration. Pretreating catalysts with methanol, a small amount of CaO was converted into Ca(OCH3)2, which acted as the initiating reagent for transesterification. The catalysts provide active basic sites that transform the methanol into methoxide which attacks the carbonyl carbon structure of oil. As the concentration of catalyst increases, the available active sites also increase leading to the improvement of biodiesel yield [29]. Beyond 1%, the yield was not greatly affected by catalysts’ concentration because the reaction mixture became more viscous and all active sites are loaded.


## 3.4. Kinetic Studies

Kinetic studies of the transesterification reaction ofCamelina sativa oil were performed by lobster waste shell heterogeneous catalyst at three different temperatures, 50°C, 65°C, and 70°C, while the methanol to oil molar ratio and catalyst concentration were kept at 12 : 1 and 1% (w/w). As expected, decrease in temperature from 70°C to 50°C causes decrease in reaction rates. Rate expression of the reaction is shown as follows [30]:(2)-Rate=-dCS  Oildt=kCS  Oil.[CS Oil] represents the concentration ofCamelina sativa oil. Excess methanol was used in the reaction in order to shift the equilibrium towards the product side. Since methanol does not affect the overall order, the transesterification reaction was assumed to follow first-order kinetics [31]. The integration of (2) results as(3)ln⁡CS  Oil0-ln⁡CS  Oilt=kt.The initial concentration ofCamelina oil and the concentration ofCamelina oil at time, t, are shown as CS  Oil0 and ln⁡CS  Oilt, respectively. The fraction conversion ofCamelina biodiesel, XFAME, can be cooperated into (3) as (4)dXFAMEdt=k1-XFAMEand the integration of the equation becomes(5)-ln⁡1-XFAME=kt.Figure 12 shows the graph between ln⁡1-XFAME and time at the three temperatures to obtain rate constant values. The plots are linear plots at three temperatures which indicate that the transesterification reaction obeys first-order kinetics.Figure 12
Plot ofln⁡(1-XFAME) versus time of the transesterification reaction catalyzed by waste lobster shells.Arrhenius equation was utilized to calculate the activation energy and preexponential factor for the transesterification reaction ofCamelina oil catalyzed by waste lobster shells. The activation energy and preexponential factor were determined as 62.5 kJ mol−1 and 7.62 × 107 min−1, respectively, by Arrhenius plot shown in Figure 13.Figure 13
Arrhenius plot ofln⁡k and 1/T of the transesterification reaction catalyzed by waste lobster shells.


## 3.5. Fuel Properties ofCamelina Biodiesel

Biodiesel was characterized for its fuel properties by ASTM D287, 445, 240, 613, and 97 methods. Table2 shows the properties of the synthesized biodiesel and petroleum biodiesel. The comparison showed that most of the fuel properties of theCamelina biodiesel are quite comparable to those of ASTM petroleum diesel standards [32]. The kinematic viscosity ofCamelina based biodiesel was similar to regular diesel fuel viscosity so no modifications of engine are required. The cetane number was found higher than regular diesel standards. Cetane number is a measure of a fuel’s autoignition quality characteristics. Since biodiesel is largely composed of aliphatic hydrocarbons, it usually has a higher cetane number than petroleum diesel [33]. Higher cetane number indicates more complete combustion of the fuel, better fuel efficiency, and quick ignition delay time of fuel. The pour point ofCamelina biodiesel shows a good compatibility for places with cold climate.Table 2
Fuel properties ofCamelina, petroleum diesel and the ASTM biodiesel standards.
Properties Petroleum diesel Camelina biodiesel Biodiesel standards (ASTM D6751) ASTM testing method Unit Kinematic viscosity (40°C) 2.6 3.1 1.9–6.0 D4451 mm2/s Specific gravity 0.85 0.88 0.87–0.90 D287 Calorific value 42 46  D240 MJ/kg Pour point −20 −10 −5 to 10 D97 °C Cetane number 46 49 47–65 D613 min


## 4. Conclusion

Every year, enormous amount of waste shells are disposed of in landfills. Waste shells, such as eggshells or seashells, are rarely used to produce practical products and utilization of the waste shells will help sustainable development. Waste shells can be utilized as economical and environmentally benign solid catalysts for the biodiesel synthesis. CaO, lobster, and eggshell catalysts were effectively employed for biodiesel synthesis fromCamelina sativa oil and methanol at 60°C. The fuel properties of the biodiesel favorably match petroleum-based diesel counterparts. Biodiesel synthesis that employs waste shells andCamelina sativa oil will reduce waste disposal problem and cut the price of biodiesel, making biodiesel a viable fuel alternative compared to petroleum-derived biodiesel.



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*Source: 6715232-2016-12-18.xml*