Catalytic Deoxygenation of Hexadecyl Palmitate as a Model Compound of Euglena Oil in H 2 and N 2 Atmospheres

: Hexadecyl palmitate (C 15 H 31 COOC 16 H 33 , used as a model compound for Euglena oil) was deoxygenated to hydrocarbons over various solid catalysts in autoclave reactors. In a H 2 atmosphere, 1 wt.% of Pd/Mg(Al)O catalyst, derived from a hydrotalcite precursor, yielded a C 15 H 31 COOC 16 H 33 conversion close to 100%, and a C 10 –C 16 (aviation fuel range) hydrocarbon yield of 90.2% for the deoxygenation of C 15 H 31 COOC 16 H 33 at 300 ◦ C for 2 h. In a N 2 atmosphere, 1 wt.% of Pd/Mg(Al)O catalyst yielded a C 10 –C 16 hydrocarbon yield of 63.5%, which was much higher than those obtained with Mg(Al)O (15.1%), H-ZSM-5 (8.3%), and 1 wt.% Pd/C (26.2%) for the deoxygenation of C 15 H 31 COOC 16 H 33 at 300 ◦ C for 2 h. The Pd metal site and the solid base site in Mg(Al)O had a synergetic effect on the deoxygenation of C 15 H 31 COOC 16 H 33 in N 2 atmosphere over the Pd/Mg(Al)O catalyst. By prolonging the reaction time to 5 h for reaction at 300 ◦ C in N 2 atmosphere, the yield of C 10 –C 16 hydrocarbons increased to 80.4% with a C 15 H 31 COOC 16 H 33 conversion of 99.1% over the 1 wt.% Pd/Mg(Al)O catalyst.


Introduction
The production of chemicals and transport fuels from renewable biomass is a sustainable and environment-friendly way to reduce the world's dependence on crude oil. Starch and cellulose in wood can be converted to ethanol by yeast fermentation [1]. Lignin in wood and organic wastes can be converted to motor fuels by a biomass-to-liquid (BTL) process using a syngas platform [2,3]. Vegetable oils can be converted to fatty acid methyl esters (FAME, known as biodiesel) by transesterification with methanol [4]. Recently, the hydrotreatment of vegetable oils to produce hydrocarbon 'drop-in' fuels has attracted global research interest [5][6][7].
Algae oils have recently become a promising alternative feedstock for vegetable oils because the oil yields from algae are significantly higher than those from any other crop [8][9][10][11]. Euglena is a promising algae biomass because it is easily cultivated on a large scale. Most algae produce oils composed of triglycerides and fatty acids [8]. However, Euglena produces an oil wax that contains a mixture of saturated esters with long carbon chains (C m H 2m+1 COOC n H 2n+1 , m = 11-15, n = 12-16) [12,13]. While some studies have been reported on the deoxygenation of triglycerides and fatty acids (vegetable oils and algae oils), very few studies have reported on the deoxygenation of fatty acid esters to date [14].
Metal (NiMo, Pt, etc.)-supported catalysts possess high activities for the deoxygenation of triglycerides and fatty acids in H 2 atmosphere [15][16][17]. However, the deoxygenation of triglycerides in N 2 atmosphere (without H 2 ) is an important subject, because H 2 is expensive and may be difficult to obtain in areas of vegetable and algae cultivation. Solid acids and bases have been reported as to obtain in areas of vegetable and algae cultivation. Solid acids and bases have been reported as catalysts for the deoxygenation of triglycerides in N2 atmosphere [18][19][20]. Solid acid catalysts possess relatively high activities; however, hydrocarbons with long carbon chains (heavy hydrocarbons) crack on the acid sites [18]. This is unfortunate, because, in general, heavy hydrocarbons have a high value as chemicals and transport fuels. In contrast, the activities of solid base catalysts are relatively low; moreover, they exhibit relatively high selectivity for heavy hydrocarbons [19,20]. Pd supported on active carbon (Pd/C) has been reported as an effective catalyst for the catalytic deoxygenation of fatty acids and their esters in He atmosphere [14,21].
In this study, we chose hexadecyl palmitate (C15H31COOC16H33) as a model compound of Euglena oil. We developed a highly active Pd/Mg(Al)O catalyst (derived from Pd-containing MgAltype hydrotalcite) for the deoxygenation of C15H31COOC16H33 to hydrocarbons in H2 and N2 atmospheres.  [22]. The metal cations are distributed in brucite-like layers, and the interlayer anions are fixed between the brucite-like layers by electric charge interaction. The M 2+ cation is usually Mg 2+ and the M 3+ cation is usually Al 3+ . The noble metal Pd 2+ cation can be introduced into the M 2+ position when Pd 2+ /(M 2+ + M 3+ ) < 5 mol % [23][24][25]. Basic MgAltype hydrotalcite is the most common hydrotalcite, and has been used as an effective catalyst for some industrially important reactions [22][23][24][25][26][27][28][29].  Figure 2 shows X-ray diffraction (XRD) patterns of Pd0.016Mg3Al(OH)16CO3•xH2O after drying at 100 °C. By using a JICST database (from The Crystallographic Society of Japan) for identification, only the well-crystallized Mg3Al(OH)16CO3 phase was observed in the XRD pattern of Pd0.016Mg3Al(OH)16CO3•xH2O. The peaks of Pd(OH)2 and PdO phases could not be observed in the XRD pattern, probably because they formed amorphous phases. It is also possible that the Pd 2+ ions entered the Mg 2+ position in Pd0.016Mg3Al(OH)16CO3•xH2O at a low Pd content [25]. The d (001) (basal d) spacing at the lowest angle in the XRD pattern was 9.0 Å for Pd0.016Mg3Al(OH)16CO3•xH2O. As shown in Figure 1, the thickness of the MgAl-type brucite-like layer was 4.7 Å [22]. The gallery height was 4.3 Å in Pd0.016Mg3Al(OH)16CO3•xH2O after subtracting the thickness of the MgAl-type hydrotalcite layer (4.7 Å) from the basal d spacing (9.0 Å). This gallery height (4.3 Å) coincides with the size of the CO3 2− anion [22].   Mg 3 Al(OH) 16 CO 3 ·xH 2 O after drying at 100 • C. By using a JICST database (from The Crystallographic Society of Japan) for identification, only the well-crystallized Mg 3 Al(OH) 16 CO 3 phase was observed in the XRD pattern of Pd 0.016 Mg 3 Al(OH) 16 CO 3 ·xH 2 O. The peaks of Pd(OH) 2 and PdO phases could not be observed in the XRD pattern, probably because they formed amorphous phases. It is also possible that the Pd 2+ ions entered the Mg 2+ position in Pd 0.016 Mg 3 Al(OH) 16 CO 3 ·xH 2 O at a low Pd content [25]. The d (001) (basal d) spacing at the lowest angle in the XRD pattern was 9.0 Å for Pd 0.016 Mg 3 Al(OH) 16 CO 3 ·xH 2 O. As shown in Figure 1, the thickness of the MgAl-type brucite-like layer was 4.7 Å [22]. The gallery height was 4.3 Å in Pd 0.016 Mg 3 Al(OH) 16 CO 3 ·xH 2 O after subtracting the thickness of the MgAl-type hydrotalcite layer (4.7 Å) from the basal d spacing (9.0 Å). This gallery height (4.3 Å) coincides with the size of the CO 3 2− anion [22].  Figure 3 shows the thermogravimetric analysis (TGA) and differential thermal analysis (DTA) results for Pd0.016Mg3Al(OH)16CO3•xH2O after drying at 100 °C. Three stages of sudden weight loss can be observed in the TGA curve. The first sudden weight loss, which appears at below 200 °C, was attributed to the loss of physically absorbed water and interlayer water. The second sudden weight loss, at 220-450 °C, was attributed to the removal of CO2 from the interlayer carbonate anions and hydroxyl groups from the brucite-like layers. The third sudden weight loss, at 850-890 °C, can be ascribed to the formation of the spinel-like phase of MgAl2O4 [20,24]. The results of DTA and TGA nearly coincide. The endotherm band at 130 °C in the DTA curve corresponds to the loss of physically absorbed water. After losing physically absorbed water, Pd0.016Mg3Al(OH)16CO3•xH2O was converted to Pd0.016Mg3Al(OH)16CO3•4H2O. The endotherm band at 190 °C in the DTA curve corresponds to the loss of interlayer water. After losing interlayer water, Pd0.016Mg3Al(OH)16CO3•4H2O was converted to Pd0.016Mg3Al(OH)16CO3. The endotherm band at 420 °C in the DTA curve corresponds to the loss of interlayer carbonate anions and hydroxyl groups in the brucite-like layers. The layered structure of hydrotalcite was destroyed upon calcination at 420 °C, following which Pd0.016Mg3Al(OH)16CO3 was converted to a metal-oxide mixture Pd0.016Mg3AlOx, in which Pd 2+ and Al 3+ ions entered the MgO cubic lattices [22]. The small endotherm band at 860 °C in the DTA curve corresponds to the solid phase change of the metal-oxide mixture to a spinel-like phase of MgAl2O4 and crystalline MgO [22].  Figure 3 shows the thermogravimetric analysis (TGA) and differential thermal analysis (DTA) results for Pd 0.016 Mg 3 Al(OH) 16 CO 3 ·xH 2 O after drying at 100 • C. Three stages of sudden weight loss can be observed in the TGA curve. The first sudden weight loss, which appears at below 200 • C, was attributed to the loss of physically absorbed water and interlayer water. The second sudden weight loss, at 220-450 • C, was attributed to the removal of CO 2 from the interlayer carbonate anions and hydroxyl groups from the brucite-like layers. The third sudden weight loss, at 850-890 • C, can be ascribed to the formation of the spinel-like phase of MgAl 2 O 4 [20,24]. The results of DTA and TGA nearly coincide. The endotherm band at 130 • C in the DTA curve corresponds to the loss of physically absorbed water. After losing physically absorbed water, Pd 0.016 Mg 3 Al(OH) 16 Mg 3 Al(OH) 16 CO 3 . The endotherm band at 420 • C in the DTA curve corresponds to the loss of interlayer carbonate anions and hydroxyl groups in the brucite-like layers. The layered structure of hydrotalcite was destroyed upon calcination at 420 • C, following which Pd 0.016 Mg 3 Al(OH) 16 CO 3 was converted to a metal-oxide mixture Pd 0.016 Mg 3 AlO x , in which Pd 2+ and Al 3+ ions entered the MgO cubic lattices [22]. The small endotherm band at 860 • C in the DTA curve corresponds to the solid phase change of the metal-oxide mixture to a spinel-like phase of MgAl 2 O 4 and crystalline MgO [22]. Figure 4 shows the dependence of the Brunauer-Emmett-Teller (BET) surface area of Pd 0.016 Mg 3 Al(OH) 16 CO 3 ·xH 2 O on calcination temperature from 100 • C to 1000 • C. Calcination was carried out at each temperature for 3 h in air. Pd 0.016 Mg 3 Al(OH) 16 CO 3 ·xH 2 O showed a BET surface area of 73 m 2 /g after calcination at 100 • C. The BET surface area increased with an increasing calcination temperature from 100 • C to 450 • C, and then decreased with increasing calcination temperature from 450 • C to 1000 • C. The layered structure of Pd 0.016 Mg 3 Al(OH) 16 CO 3 hydrotalcite was destroyed, and a PdO-Mg(Al)O metal-oxide mixture was formed upon calcination at 450 • C. In the process of destruction, the removal of CO 2 (from the interlayer carbonate anions) and hydroxyl groups (from the brucite-like layers) created pores in the PdO-Mg(Al)O metal-oxide mixture formed. These pores increased the BET surface area. Calcination at a temperature that was higher than 450 • C caused sintering of the metal-oxide mixture particles, which decreased the BET surface area. Moreover, an obvious decrease in the BET surface area was observed at 800-850 • C. The formation of spinel-like phases of MgAl 2 O 4 from the PdO-Mg(Al)O metal-oxide mixture resulted in a decrease in the BET surface area upon calcination at 800-850 • C [25]. Because the highest BET surface area (143 m 2 /g) was obtained for calcination at 450 • C, we calcined Pd 0.016 Mg 3 Al(OH) 16 Figure 4 shows the dependence of the Brunauer-Emmett-Teller (BET) surface area of Pd0.016Mg3Al(OH)16CO3•xH2O on calcination temperature from 100 °C to 1000 °C. Calcination was carried out at each temperature for 3 h in air. Pd0.016Mg3Al(OH)16CO3•xH2O showed a BET surface area of 73 m 2 /g after calcination at 100 °C. The BET surface area increased with an increasing calcination temperature from 100 °C to 450 °C, and then decreased with increasing calcination temperature from 450 °C to 1000 °C. The layered structure of Pd0.016Mg3Al(OH)16CO3 hydrotalcite was destroyed, and a PdO-Mg(Al)O metal-oxide mixture was formed upon calcination at 450 °C. In the process of destruction, the removal of CO2 (from the interlayer carbonate anions) and hydroxyl groups (from the brucite-like layers) created pores in the PdO-Mg(Al)O metal-oxide mixture formed. These pores increased the BET surface area. Calcination at a temperature that was higher than 450 °C caused sintering of the metal-oxide mixture particles, which decreased the BET surface area. Moreover, an obvious decrease in the BET surface area was observed at 800-850 °C. The formation of spinel-like phases of MgAl2O4 from the PdO-Mg(Al)O metal-oxide mixture resulted in a decrease in the BET surface area upon calcination at 800-850 °C [25]. Because the highest BET surface area (143 m 2 /g) was obtained for calcination at 450 °C, we calcined Pd0.016Mg3Al(OH)16CO3•xH2O at 450 °C for 3 h in air before use in this study.  The use of uniform multicomponent precursors results in well-dispersed metal particles on the surface of supports after calcination and reduction. This method, known as "solid phase crystallization" (SPC), is important in the preparation of highly active metal-supported catalysts [27][28][29][30][31][32][33][34][35]. In this study, Pd 2+ could enter the Mg 2+ position in Pd0.016Mg3Al(OH)16CO3•xH2O hydrotalcite after drying at 100 °C in air. As a result, a well-distributed mixed oxide, PdO-Mg(Al)O, could be formed after calcining Pd0.016Mg3Al(OH)16CO3•xH2O at 450 °C in air. Finally, a Pd/Mg(Al)O catalyst with highly dispersed Pd metal particles and strong interaction between the metal and support could be obtained after the pretreatment process of H2 flow reduction. Figure 5 shows the flame ionization detector-gas chromatography (FID-GC) charts of C15H31COOC16H33 and the liquid product formed upon deoxygenation of C15H31COOC16H33 in H2 atmosphere, at 300 °C, for 2 h, over 1 wt.% Pd/Mg(Al)O catalyst. As shown in Figure 5B, the reactant (C15H31COOC16H33) peak is not observed in the GC chart after reaction at 300 °C for 2 h. The liquid products were almost saturated hydrocarbons n-C16H34 and n-C15H32. By calculating the amount of each component in the product using the GC chart, the molar ratio of n-C16H34 to n-C15H32 in the liquid product was found to be 4.3. The use of uniform multicomponent precursors results in well-dispersed metal particles on the surface of supports after calcination and reduction. This method, known as "solid phase crystallization" (SPC), is important in the preparation of highly active metal-supported catalysts [27][28][29][30][31][32][33][34][35]. In this study, Pd 2+ could enter the Mg 2+ position in Pd 0.016 Mg 3 Al(OH) 16 Figure 5B, the reactant (C 15 H 31 COOC 16 H 33 ) peak is not observed in the GC chart after reaction at 300 • C for 2 h. The liquid products were almost saturated hydrocarbons n-C 16 H 34 and n-C 15 H 32 . By calculating the amount of each component in the product using the GC chart, the molar ratio of n-C 16 H 34 to n-C 15 H 32 in the liquid product was found to be 4.3. As shown in Reactions (1)-(3), deoxygenation of saturated fatty acids (such as stearic acid C17H35COOH) involves three parallel reactions: reduction, decarbonylation, and decarboxylation [7]. For a fatty acid having an even number of carbons, reduction produces a normal paraffin having an even number of carbons plus water; decarbonylation produces a normal paraffin having an odd number of carbons plus water and CO; and, decarboxylation produces a normal paraffin having an odd number of carbons plus CO2.
C15H31COOC16H33 + 2H2 = C15H32 + C16H34 + CO + H2O Decarbonylation C15H31COOC16H33 + H2 = C15H32 + C16H34 + CO2 Decarboxylation (6) As shown in Reactions (4)- (6), the reduction of one C15H31COOC16H33 molecule produces two C16H34 molecules. On the other hand, either decarbonylation or decarboxylation of one C15H31COOC16H33 molecule produces one C16H34 molecule and one C15H32 molecule. The decarbonylation of C15H31COOC16H33 produces CO, whereas the decarboxylation of C15H31COOC16H33 produces CO2. Both CO and CO2 were detected in the gas product from the reaction As shown in Reactions (1)-(3), deoxygenation of saturated fatty acids (such as stearic acid C 17 H 35 COOH) involves three parallel reactions: reduction, decarbonylation, and decarboxylation [7]. For a fatty acid having an even number of carbons, reduction produces a normal paraffin having an even number of carbons plus water; decarbonylation produces a normal paraffin having an odd number of carbons plus water and CO; and, decarboxylation produces a normal paraffin having an odd number of carbons plus CO 2 .  (6)) occurred during the reaction. Moreover, among Reactions (4)-(6), the reduction of C 15 H 31 COOC 16 H 33 (Reaction (4)) was the main reaction, because the quantity of n-C 16 H 34 in the liquid product was much more than that of n-C 15 H 32 ( Figure 5B).
For deoxygenation of C 15 H 31 COOC 16 H 33 in H 2 atmosphere, the metal site alone could achieve a high activity, because deoxygenation was carried out via three routes: reduction, decarbonylation, and decarboxylation. We used an acid support for the metal in order to adjust the selectivity of the hydrocarbon products during deoxygenation in H 2 atmosphere [6,7]. In this study, we used a base support (Mg(Al)O) for the metal (Pd) in order to suppress the hydrocracking of n-C 15 H 32 and n-C 16 H 34 products (to light hydrocarbons) during deoxygenation of C 15 H 31 COOC 16 H 33 in H 2 atmosphere. Figure 6 shows X-ray diffraction (XRD) patterns of 1 wt.% Pd/Mg(Al)O catalyst before reaction and after reaction (for deoxygenation of C 15 H 31 COOC 16 H 33 in H 2 atmosphere at 300 • C for 2 h). The sample before reaction was obtained by calcining Pd 0.016 Mg 3 Al(OH) 16 (5)) and decarboxylation of C15H31COOC16H33 (Reaction (6)) occurred during the reaction. Moreover, among Reactions (4)-(6), the reduction of C15H31COOC16H33 (Reaction (4)) was the main reaction, because the quantity of n-C16H34 in the liquid product was much more than that of n-C15H32 ( Figure  5B). For deoxygenation of C15H31COOC16H33 in H2 atmosphere, the metal site alone could achieve a high activity, because deoxygenation was carried out via three routes: reduction, decarbonylation, and decarboxylation. We used an acid support for the metal in order to adjust the selectivity of the hydrocarbon products during deoxygenation in H2 atmosphere [6,7]. In this study, we used a base support (Mg(Al)O) for the metal (Pd) in order to suppress the hydrocracking of n-C15H32 and n-C16H34 products (to light hydrocarbons) during deoxygenation of C15H31COOC16H33 in H2 atmosphere. Figure 6 shows X-ray diffraction (XRD) patterns of 1 wt.% Pd/Mg(Al)O catalyst before reaction and after reaction (for deoxygenation of C15H31COOC16H33 in H2 atmosphere at 300 °C for 2 h). The sample before reaction was obtained by calcining Pd0.016Mg3Al(OH)16CO3•xH2O in air at 450 °C for 3 h, and then reducing in H2 at 300 °C for 1 h. The XRD pattern of the sample before reaction proved the formation of mixed Mg-Al oxides phases, indicating that the decomposition of the layered structure occurred after calcination and reduction. The reflections in XRD pattern at about 43° and 63° corresponded to MgO-like phase (periclase), or rather MgO-Al2O3 solid solution Mg(Al)O [22]. The reflection of Al2O3 phase at 23° was very small, indicating that Al 3+ cations were dispersed in the structure of MgO without the formation of spinel species. Because the Pd loading was low (1 wt.%) in the Pd/Mg(Al)O catalyst, the metal Pd crystals certainly formed in very small sizes, and thus the metal Pd phase could not be detected in the XRD pattern. The sample after reaction was obtained by filtrating out liquid products, and then drying in vacuum at room temperature for 10 h.     Figure 7 shows the dependence of C 15 H 31 COOC 16 H 33 conversion and C 10 -C 16 hydrocarbon yield on the reaction time for the catalytic deoxygenation of C 15 H 31 COOC 16 H 33 in H 2 atmosphere, at 300 • C, over 1 wt.% Pd/Mg(Al)O catalyst. Four autoclave reactors were charged with the same reactant gases and the same amount of catalyst, and then operated at the same temperature (300 • C). The reaction in each autoclave reactor was finished in an hour. The products were analysed to determine the C 15 H 31 COOC 16 H 33 conversion and the C 10 -C 16 hydrocarbon yield at that reaction time. The yield of C 10 -C 16 hydrocarbons is important as they can be used as aviation fuel [16]. As shown in Figure 7, C 15 H 31 COOC 16 H 33 conversion increased with the reaction time, and approached 100% after reaction for 2 h in H 2 atmosphere. CO and CO 2 , which formed from decarbonylation and decarboxylation of C 15 H 31 COOC 16 H 33 (Reactions (5) and (6)) were the main by-products in the deoxygenation of C 15 H 31 COOC 16 H 33 in H 2 atmosphere [6,7]. The amounts of formed CO and CO 2 almost kept constant after reaction for 2 h. A small amount of C 1 -C 4 gaseous hydrocarbons was also formed during the reaction in H 2 atmosphere, and the amount of C 1 -C 4 gaseous hydrocarbons increased with prolonging the reaction time. As shown in Figure 7, the yield of C 1 -C 16 hydrocarbons increased to 90.2% after reaction for 2 h, and then decreased slightly with prolonging reaction time due to the formation of light hydrocarbons (<C 9  in each autoclave reactor was finished in an hour. The products were analysed to determine the C15H31COOC16H33 conversion and the C10-C16 hydrocarbon yield at that reaction time. The yield of C10-C16 hydrocarbons is important as they can be used as aviation fuel [16]. As shown in Figure 7, C15H31COOC16H33 conversion increased with the reaction time, and approached 100% after reaction for 2 h in H2 atmosphere. CO and CO2, which formed from decarbonylation and decarboxylation of C15H31COOC16H33 (Reactions (5) and (6)) were the main by-products in the deoxygenation of C15H31COOC16H33 in H2 atmosphere [6,7]. The amounts of formed CO and CO2 almost kept constant after reaction for 2 h. A small amount of C1-C4 gaseous hydrocarbons was also formed during the reaction in H2 atmosphere, and the amount of C1-C4 gaseous hydrocarbons increased with prolonging the reaction time. As shown in Figure 7, the yield of C1-C16 hydrocarbons increased to 90.2% after reaction for 2 h, and then decreased slightly with prolonging reaction time due to the formation of light hydrocarbons (<C9). On the whole, the Pd/Mg(Al)O catalyst provided a high catalytic performance for the catalytic deoxygenation of C15H31COOC16H33 to hydrocarbons in H2 atmosphere.  Table 1 shows the C15H31COOC16H33 conversion and C10-C16 hydrocarbons yield of the deoxygenation of C15H31COOC16H33 in N2 atmosphere at 300 °C for 2 h over various catalysts. The 1 wt.% Pd/Mg(Al)O catalyst resulted in a C15H31COOC16H33 conversion of 76.4% and a C10-C16 yield of 63.5% for the reaction at 300 °C for 2 h in N2 atmosphere. Both, C15H31COOC16H33 conversion and the C10-C16 yield obtained in N2 atmosphere, were much lower than those obtained in H2 atmosphere ( Figure 6) over Pd/Mg(Al)O after reaction at 300 °C for 2 h. This indicates that H2 greatly improves the deoxygenation of C15H31COOC16H33, and that it is difficult to produce hydrocarbons from C15H31COOC16H33 in N2 atmosphere. The use of basic hydrotalcite, acidic H-ZSM-5, and Pd/C has been reported for the deoxygenation of triglycerides or fatty acids in N2 or Ar atmospheres [14,17,18]. As shown in Table 1, the basic catalyst Mg(Al)O without Pd gave low conversion (23.3%) and a low yield of C10-C16 hydrocarbons (15.1%) for the reaction in N2 atmosphere. In contrast, the conversion was relatively high (55.6%), but the yield of C10-C16 hydrocarbons was very low (8.3%) over the acidic   16 H 33 in N 2 atmosphere. The use of basic hydrotalcite, acidic H-ZSM-5, and Pd/C has been reported for the deoxygenation of triglycerides or fatty acids in N 2 or Ar atmospheres [14,17,18]. As shown in Table 1, the basic catalyst Mg(Al)O without Pd gave low conversion (23.3%) and a low yield of C 10 -C 16 hydrocarbons (15.1%) for the reaction in N 2 atmosphere. In contrast, the conversion was relatively high (55.6%), but the yield of C 10 -C 16 hydrocarbons was very low (8.3%) over the acidic catalyst H-ZSM-5. Heavy hydrocarbons formed in the reaction cracked to light hydrocarbons on the acidic sites of H-ZSM-5 during the reaction. The use of Pd/C resulted in a C 15 H 31 COOC 16 H 33 conversion of 41.7% and a C 10 -C 16 hydrocarbons yield of 26.2% for the reaction at 300 • C for 2 h in N 2 atmosphere. Therefore, Pd/Mg(Al)O shows a much higher catalytic performance than these catalysts that are reported in the literature, for the deoxygenation of C 15 H 31 COOC 16 H 33 in N 2 atmosphere. The development of multi-functional catalysts to improve catalyst performance is an important challenge in the catalyst field. The catalyst containing Pt metal and basic hydrotalcite has been reported as excellent for the aromatization of n-hexane [26]. We had developed some multi-functional catalysts containing metal and solid acid for some industrially important reactions [36][37][38][39][40][41][42] Figures 5B and 8A shows that the peak of the C 15 H 31 COOC 16 H 33 reactant still appears in the GC chart after reaction in N 2 atmosphere. For the deoxygenation of C 15 H 31 COOC 16 H 33 over the Pd/Mg(Al)O catalyst, the reaction rate in N 2 atmosphere was slow in comparison with that in the H 2 atmosphere. The reaction in N 2 atmosphere formed some compounds with a retention time ranging from 14 to 22 min in the GC chart (fatty acid, alcohol, and ketones). These compounds decreased the yield of hydrocarbons from the deoxygenation of C 15 H 31 COOC 16 H 33 . Moreover, peaks of C 5 -C 14 hydrocarbons appear in the GC chart of the 2 h reaction in N 2 atmosphere ( Figure 8A). Figure 8B shows the magnified area from 11.1 to 14.1 min in Figure 8A; this enables us to observe the composition of C 15 and C 16 hydrocarbons that are formed by the reaction in N 2 atmosphere. As shown in Figure 5B, deoxygenation of C 15 H 31 COOC 16 H 33 in H 2 atmosphere only formed normal paraffin hydrocarbons. As shown in Figure 8B, the hydrocarbon products that are formed by the deoxygenation of C 15 H 31 COOC 16 H 33 in N 2 atmosphere contained n-paraffin and several kinds of olefins. A comparison of the GC-MS results with values in the NIST-11 database indicates that the peaks around n-paraffin were olefins with the same number of carbon chains. The initially formed olefins were converted into other olefins by double bond migration on the basic sites of Mg(Al)O. Solid base catalysts (such as MgO) have the catalytic ability for double bond migration of olefins [43]. By calculating the amount of each component in the product using the GC chart, the amount of total C 16 hydrocarbons and the amount of total C 15 hydrocarbons was found to be almost the same in the liquid product that was formed from the catalytic deoxygenation of C 15 H 31 COOC 16 H 33 in N 2 atmosphere, at 300 • C, for 2 h, over the Pd/Mg(Al)O catalyst. Reactions (7) and (8) show the reactions for the deoxygenation of C15H31COOC16H33 in N2 (without H2) atmosphere. CO could not be detected in the gas products of the reaction in N2 atmosphere, thus, decarboxylation was deduced to be the only reaction in the deoxygenation of C15H31COOC16H33 in N2 atmosphere. C15H31COOC16H33 = C15H32 + C16H32 + CO2 Decarboxylation (7) C15H31COOC16H33 = C15H30 + C16H34 + CO2 Decarboxylation (8) In N2 atmosphere, the number of H atoms in the C15H31COOC16H33 molecule was not enough to obtain the saturated hydrocarbons C16H34 and C15H32 in the decarboxylation of C15H31COOC16H33. One C15H31COOC16H33 molecule must form one paraffin and one olefin by decarboxylation without H2. The high reactivity of the olefin molecules formed resulted in the formation of light hydrocarbons. A few heavy hydrocarbons larger than C16 were also formed by the polymerization of light olefins. Because both Reactions (7) and (8) form the same amount of C15 and C16 hydrocarbons, the molar ratio of total C16 hydrocarbons to total C15 hydrocarbons was 1.0, as shown in Figure 8B. Moreover, the ratio of n-C15H32 in the total C15 hydrocarbons was much higher than the ratio of n-C16H34 in the total C16 hydrocarbons ( Figure 8B). Thus, Reaction (7) was the main decarboxylation reaction (as compared to Reaction (8)) in the catalytic deoxygenation of C15H31COOC16H33 in N2 atmosphere.

Catalytic Deoxygenation of C15H31COOC16H33 in N2 Atmosphere
For deoxygenation of C15H31COOC16H33 in N2 atmosphere, the metal site alone could not achieve enough activity, because deoxygenation was carried out via a single route, namely decarboxylation. In this study, we used a base support (Mg(Al)O) for the metal (Pd) in order to enhance the catalytic activity during deoxygenation of C15H31COOC16H33 in N2 atmosphere. Figure 9 shows the dependence of C15H31COOC16H33 conversion and C10-C16 hydrocarbons yield on reaction time for the catalytic deoxygenation of C15H31COOC16H33 in N2 atmosphere, at 300 °C, Reactions (7) and (8) 16 were also formed by the polymerization of light olefins. Because both Reactions (7) and (8) form the same amount of C 15 and C 16 hydrocarbons, the molar ratio of total C 16 hydrocarbons to total C 15 hydrocarbons was 1.0, as shown in Figure 8B. Moreover, the ratio of n-C 15 H 32 in the total C 15 hydrocarbons was much higher than the ratio of n-C 16 H 34 in the total C 16 hydrocarbons ( Figure 8B). Thus, Reaction (7) was the main decarboxylation reaction (as compared to Reaction (8)) in the catalytic deoxygenation of C 15 H 31 COOC 16 H 33 in N 2 atmosphere.
For deoxygenation of C 15 H 31 COOC 16 H 33 in N 2 atmosphere, the metal site alone could not achieve enough activity, because deoxygenation was carried out via a single route, namely decarboxylation. In this study, we used a base support (Mg(Al)O) for the metal (Pd) in order to enhance the catalytic activity during deoxygenation of C 15 H 31 COOC 16 H 33 in N 2 atmosphere. Figure 9 shows the dependence of C 15 Figure 10 shows the dependence of C15H31COOC16H33 conversion and C10-C16 hydrocarbon yield on reaction temperature for the catalytic deoxygenation of C15H31COOC16H33 in N2 atmosphere, for 2 h, over the 1 wt.% Pd/Mg(Al)O catalyst. C15H31COOC16H33 conversion increased with an increasing reaction temperature from 275 to 375 °C, and achieved a conversion of over 99% for the reaction at 375 °C for 2 h. The yield of C10-C16 hydrocarbons increased with an increasing reaction temperature from 275 to 325 °C. At a reaction temperature higher than 325 °C, the yield of C10-C16 hydrocarbons could not be improved by increasing the reaction temperature because the number of light hydrocarbons (<C9) in the product increased at high reaction temperatures.  conversion increased with an increasing reaction temperature from 275 to 375 • C, and achieved a conversion of over 99% for the reaction at 375 • C for 2 h. The yield of C 10 -C 16 hydrocarbons increased with an increasing reaction temperature from 275 to 325 • C. At a reaction temperature higher than 325 • C, the yield of C 10 -C 16 hydrocarbons could not be improved by increasing the reaction temperature because the number of light hydrocarbons (<C 9 ) in the product increased at high reaction temperatures.

Reagents
Hexadecyl palmitate (C15H31COOC16H33) of purity higher than 95% was purchased from Tokyo Chemical Industry Co., Ltd. (Tokyo, Japan) Na-ZSM-5 zeolite (SiO2/Al2O3 = 50) was purchased from Wako Pure Chemical Industries, Ltd. (Tokyo, Japan) Activated carbon (C), with a particle size of 100 mesh, was purchased from Aldrich Chem. Co. Inc. (Milwaukee, WI, USA); the BET surface area of the C support was 593 m 2 /g by N2 adsorption measurement. Other chemical reagents were purchased from Wako Pure Chemical Industries Ltd. (Tokyo, Japan) with purities higher than 99%. Gas Figure 10. 1000 • C. N 2 adsorption measurements were carried out at −196 • C using a Belsorp 28SA automatic adsorption instrument (MicrotracBEL Corp., Osaka, Japan). The surface areas of the samples were obtained from a Brunauer-Emmett-Teller (BET) plot. Elemental analysis of Pd was measured by an inductive coupled plasma analysis, using a Thermo Jarrell Ash IRIS/AP instrument (SpectraLab Scientific Inc., Markham, ON, Canada).

Reactions
Before reaction, Pd/Mg(Al)O and Pd/C were reduced in a H 2 flow (60 mL/min) at 300 • C for 1 h. The reaction was carried out in a type of 100-mL stainless-steel autoclave reactor with a stirrer. In general, 0.2 g catalyst and 5 g hexadecyl palmitate (C 15 H 31 COOC 16 H 33 ) were introduced into an autoclave reactor. Then, 0.9 MPa H 2 (for the reaction in H 2 atmosphere) or 0.9 MPa N 2 (for the reaction in N 2 atmosphere) was charged into the autoclave at room temperature (25 • C). The autoclave reactor was then heated and was kept at the reaction temperature (275-375 • C) for 1-6 h with vigorous stirring (600 rpm). After the reaction, the reactor was cooled down to room temperature before analysis.

Analyses
The gas products were collected into a plastic bag, from which the air had been taken out by using a pump. The total volume of the total gas was measured using a WS-1 integration flow meter (Shinagawa Corp., Tokyo, Japan). The composition of the gas products was analysed using gas chromatography (Shimadzu Corp., Kyoto, Japan). Inorganic gases (H 2 , N 2 , CO, and CO 2 ) were analysed using a Shimadzu 14B type GC with a thermal conductivity detector (TCD) that was equipped with MS-5A and Porapak-Q columns. Gaseous hydrocarbons (C 1 -C 4 ) were analysed using a Shimadzu GC-2014 type FID-GC equipped with an RT-QPLOT (Agilent Technologies Japan, Ltd, Tokyo, Japan) capillary column. The factors of various gases (H 2 , N 2 , CO, CO 2 , C 1 -C 4 hydrocarbons) were obtained using a standard mixed gas (with known concentration for each component) from a cylinder.
The liquid products were taken out from the autoclave reactor. After filtering out the solid catalyst, a certain amount of dioxane (C 4 H 8 O 2 ) was added to the liquid products as an internal standard. Dichloromethane (CH 2 Cl 2 ) was used as a solvent to wash the reactor and the used catalyst, and then mixed with the liquid products. The liquid products were analysed by a Shimadzu GC-2014 type GC-FID equipped with a UA-DX30 capillary column (Frontier Laboratories Ltd., Koriyama, Fukushima, Japan). Gas chromatography-mass spectrometry (GC-MS) analysis was performed on a Shimadzu GCMS-QP2010 Ultra (Shimadzu Corp., Kyoto, Japan) to confirm the components of the liquid products. Each component in the liquid product was separated on a UA-DX30 capillary column, and was identified by GC-MS analysis, with reference to the NIST-11 database. The amount of each normal paraffin in the product was calculated from the results of GC-FID analysis, and the factor of each normal paraffin was obtained using a pure reagent with a certain amount of dioxane (C 4 H 8 O 2 ) in the GC-FID analysis. Each olefin in the product was identified by GC-MS analysis, and the amount of each olefin was calculated from the results of GC-FID analysis by using the factor of a normal paraffin with the same number of carbon chains.
Using the results of the GC analyses, C 15 H 31 COOC 16 H 33 conversion was calculated from the ratio of the decreased amount to the fed amount of C 15 H 31 COOC 16 H 33 ; the yield of each carbon-containing product was calculated from the ratio of the formed amount of each product to the fed amount of C 15 H 31 COOC 16 H 33 . The carbon mass balance (before and after reaction) had an error less than ±5% for the reaction in H 2 atmosphere, and had an error less than ±10% for the reaction in N 2 atmosphere.

Conclusions
The Pd/Mg(Al)O catalyst derived from Pd 0.016 Mg 3 Al(OH) 16