Temperature-Dependent Hydrogenation, Hydrodeoxygenation, and Hydrogenolysis of Anisole on Nickel Catalysts

: Hydrogenation stands out as one of the most promising techniques for converting biomass-derived molecules into valuable products. The expected products of upgrading biomass molecules include hydrocarbon, oxygenate, and methane. Ni-based catalysts have attracted considerable interest owing to their unique properties and relatively low cost. In this work, NiO prepared by the calcination and urea precipitation methods, namely NiO–C and NiO–U, is investigated for the hydrogenation of anisole. It is found that reaction temperature exerts a signiﬁcant inﬂuence on the hydrogenation pathways. At 150 ◦ C, C–reduced NiO proves more inclined towards hydrogenation, while U–reduced NiO demonstrates a tendency for hydrodeoxygenation (HDO). Moreover, as the temperature rises, both nickel catalysts change the reaction route to hydrogenolysis and eventually only produce methane at 300 ◦ C, whereas metallic Ni is formed as the catalytic active phase. In situ FTIR experiments suggest the hydrogenolysis pathway and the formation of methane. This work investigates a route to produce methane from biomass molecules.


Introduction
Searching for alternative renewable energy sources has become essential due to the recent depletion in the oil supply available worldwide [1][2][3].Biomass is potentially the world's largest sustainable energy source, with 220 billion dry tons available annually.It is currently the only sustainable source of organic carbon and biofuels [4,5].Thermochemical processes such as pyrolysis can convert biomass directly into bio-oil.However, its low calorific value, thermal instability, and the presence of sulfur, nitrogen, and oxygen heteroatoms hinder its application [6][7][8][9][10].Therefore, an upgrading process is necessary to increase the value of pyrolysis oil.
Apart from enhancing pyrolysis reactors and processes to boost the fast pyrolysis oil production rate, upgrading procedures can be accomplished via emulsification, hydrotreating, zeolite upgrading, and supercritical reforming [11,12].Bio-oil upgrading is most commonly achieved through hydrotreating, which involves hydrodesulfurization (HDS), hydrodenitrogenation (HDN), and hydrodeoxygenation (HDO) reactions [13].Among these reactions, HDO is an effective method to depolymerize and upgrade lignin and bio-oil, improving the C/O ratio and drawing greater attention [14].Pyrolysis oil contains a large number of phenolic derivatives, such as phenol, cresol, anisole, and guaiacol, which are used as model compounds in the HDO studies [15,16].In the HDO reaction, the C-O bond of the model molecule is cleaved to produce saturated or aromatic hydrocarbons [17,18].In general, HDO of phenolic compounds occurs through two pathways: direct deoxygenation (DDO) and hydrogenation-deoxygenation (HYD) [19].DDO breaks the C Ar -O bond of phenolic compounds, generating aromatic hydrocarbons.HYD is a continuous process that involves several steps, including a hydrogenation-dehydration-hydrogenation reaction [20,21].Furthermore hydrogenolysis, transalkylation, and methanation of the C-C bond can occur simultaneously in the HDO process [22,23].
Methane is a promising clean energy source and can be used as a basic material for advanced chemicals [24][25][26].Hydrogenolysis of biomass to methane is a potential energy conversion method.Currently, there are two primary methods of converting biomass to methane-rich gas: biological fermentation and chemical pyrolysis/gasification [27,28].Biological fermentation typically produces methane with a selectivity of around 45-70%, but it takes a long time and may contain unused lignin residue.In contrast, pyrolysis/gasification is usually carried out at high temperatures (600-1000 • C) and produces a mixture of CH 4 , CO 2 , etc., with a relatively low CH 4 content [25,29,30].Therefore, it is essential to design catalysts for converting biomass to methane under mild conditions.
Nickel-based catalysts are promising candidates for converting biomass into biomethane due to their excellent hydrogen dissociation and chemisorption capabilities [31][32][33].As an example, in HDO of guaiacol, it is catalyzed using nickel catalysts supported on Al-MCM-41, with lower temperatures favoring the hydrogenation of the aromatic ring and extensive C-C hydrogenolysis occurring at 400 • C [34,35].In addition, there is a significant increase in methanation activity.The aromatic/cyclohexane hydrogenation and dehydrogenation reactions are thermodynamically sensitive to reaction temperature and pressure due to the complexity of the reaction mechanism.Zhu et al. compare the HDO performances of Ni, Pd, and Pt catalysts without the influence of the solvent and supports [36,37].Although the HDO activities of Ni are lower than those of Pd and Pt catalysts, the C-C hydrogenolysis reaction of Ni catalysts is more favorable and a large amount of methane is generated [38,39].This progress demonstrates that Ni-based catalysts are active in C-C hydrogenolysis, methanation, and other reactions in HDO reactions.
This work investigates the influence of temperature on the hydrogenation reaction pathway of nickel catalysts.Anisole was chosen as a representative molecule because it contains a phenyl ring connecting the methoxyl group (-OCH 3 ), one of the major functional groups of the lignin phenolic.Two NiO catalysts are synthesized through the calcination and precipitation methods.The hydrogenation reaction of anisole is examined under identical conditions in a fixed-bed flow reactor at varying temperatures.The selectivity of the catalysts' hydrogenation reactions is significantly different at low temperatures (150 • C), while at 300 • C or higher temperatures, methane is the main product of the hydrogenation of anisole.This finding is important for directly utilizing biomass resources and showing the possibility of producing clean energy.

Results and Discussion
In this work, NiO-C is synthesized directly through calcination, and NiO-U is prepared by urea precipitation.The catalytic activity of the catalysts is evaluated through the HDO reaction of anisole.After pretreatment, both nickel catalysts exhibit high conversion under similar reaction conditions, but their selectivity is very different.As shown in Figure 1a, the conversion for C-reduced NiO is approximately 96% at 150 • C, and all of it converts to the hydrogenation product, methoxycyclohexane.Meanwhile, the yield of methoxycyclohexane decreases as temperature increases.The yield of methane gradually rises, suggesting that the hydrogenation of anisole tends to follow the hydrogenolysis route.As displayed in Figure 1b, the products of the reaction of U-reduced NiO are mostly cyclohexane at 150 • C, and the selectivity of methane reaches 100% at 300 • C.
As shown in Figure 1c,d, reaction temperature has a different effect on the three different types of reactions: hydrogenation, HDO, and C-C hydrogenolysis.Firstly, at a low temperature (150 • C), their selectivity is completely different: C-reduced NiO is prone to following the hydrogenation route, while U-reduced NiO is more likely to undergo the HDO reaction.As temperature increases, the hydrogenation reaction of C-reduced NiO and the HDO reaction of U-reduced NiO are obviously inhibited; the reactions of The particle size and morphology of the catalysts after the reactions were studied using scanning electron microscopy (SEM) and transmission electron microscopy (TEM).As shown in Figure 2, a significant difference in particle size and shape between NiO−C catalyst and NiO−U catalyst after the reaction is observed.The morphology results of NiO−C after the reaction (Figure 2a-d) indicate that the spent NiO−C catalyst exists in the form of larger particles compared to those of the spent NiO−U catalyst.As exhibited in Figure 2e-h, it can be seen that the particles of NiO−U are irregularly distributed after the reaction, and thus generate more stacked pore structures.Furthermore, in the high-resolution TEM image (Figure 2h), the lattice spacing of the spent NiO−U catalyst is 0.20 nm, which corresponds to the (111) plane of metal Ni.This result matches the XRD patterns, as shown in Figure 3 [40].The particle size and morphology of the catalysts after the reactions were studied using scanning electron microscopy (SEM) and transmission electron microscopy (TEM).As shown in Figure 2, a significant difference in particle size and shape between NiO-C catalyst and NiO-U catalyst after the reaction is observed.The morphology results of NiO-C after the reaction (Figure 2a-d) indicate that the spent NiO-C catalyst exists in the form of larger particles compared to those of the spent NiO-U catalyst.As exhibited in Figure 2e-h, it can be seen that the particles of NiO-U are irregularly distributed after the reaction, and thus generate more stacked pore structures.Furthermore, in the highresolution TEM image (Figure 2h), the lattice spacing of the spent NiO-U catalyst is 0.20 nm, which corresponds to the (111) plane of metal Ni.This result matches the XRD patterns, as shown in Figure 3 [40].
The crystalline structures of fresh catalysts were examined.The fresh catalysts both exhibit the same diffraction peaks, which are assigned to NiO (PDF#47-1049), as shown in Figure 3a [32].Moreover, the XRD pattern of NiO-C has a narrower peak width and higher peak intensity compared to NiO-U, indicating significant differences in the degree of crystallization and particle size between the two catalysts.NiO-C exhibits better crystallinity as compared to NiO-U.The particle sizes of the catalysts were calculated by the Scherrer formula and are shown in Table 1 [41].It can be inferred that the crystal size of NiO-C is larger than that of NiO-U.The structure of the catalysts after pretreatment and reaction are further evaluated (Figure 3b), reveals that both catalysts are reduced to nickel (PDF#04-0850).The reduced and spent catalysts exhibit similar crystallinity and particle size [42].The crystalline structures of fresh catalysts were examined.The fresh catalysts both exhibit the same diffraction peaks, which are assigned to NiO (PDF#47-1049), as shown in Figure 3a [32].Moreover, the XRD pattern of NiO−C has a narrower peak width and higher peak intensity compared to NiO−U, indicating significant differences in the degree of crystallization and particle size between the two catalysts.NiO−C exhibits better crystallinity as compared to NiO−U.The particle sizes of the catalysts were calculated by the Scherrer formula and are shown in Table 1 [41].It can be inferred that the crystal size of NiO−C is larger than that of NiO−U.The structure of the catalysts after pretreatment and reaction are further evaluated (Figure 3b), reveals that both catalysts are reduced to nickel (PDF#04-0850).The reduced and spent catalysts exhibit similar crystallinity and particle size [42].The crystalline structures of fresh catalysts were examined.The fresh catalysts both exhibit the same diffraction peaks, which are assigned to NiO (PDF#47-1049), as shown in Figure 3a [32].Moreover, the XRD pattern of NiO−C has a narrower peak width and higher peak intensity compared to NiO−U, indicating significant differences in the degree of crystallization and particle size between the two catalysts.NiO−C exhibits better crystallinity as compared to NiO−U.The particle sizes of the catalysts were calculated by the Scherrer formula and are shown in Table 1 [41].It can be inferred that the crystal size of NiO−C is larger than that of NiO−U.The structure of the catalysts after pretreatment and reaction are further evaluated (Figure 3b), reveals that both catalysts are reduced to nickel (PDF#04-0850).The reduced and spent catalysts exhibit similar crystallinity and particle size [42].Raman spectra were used to investigate the metal state and structures of the fresh catalysts.As presented in Figure 4, it was found that the two NiO catalysts have similar Raman spectra.For NiO-U, the spectra show signal peaks at 345 cm −1 , 500 cm −1 , and 1066 cm −1 , which correspond to the first-order phonon TO, the first-order phonon LO, and the second-order phonon 2LO of NiO crystals [43,44].The existence of 1TO and 1LO modes in the Raman spectra suggests that Ni 2+ and disordered oxygen may be present.This conclusion suggests that the catalysts are NiO materials, which is in agreement with the XRD (Figure 3) results.Similarly, for NiO-C, the peaks at 500 cm −1 and 1066 cm −1 correspond to the 1TO and 2LO signals of nickel oxide crystals.Combined with the above characterization data, the two catalysts are nickel oxide crystals before pretreatment.Raman spectra were used to investigate the metal state and structures of the fresh catalysts.As presented in Figure 4, it was found that the two NiO catalysts have similar Raman spectra.For NiO−U, the spectra show signal peaks at 345 cm −1 , 500 cm −1 , and 1066 cm −1 , which correspond to the first-order phonon TO, the first-order phonon LO, and the second-order phonon 2LO of NiO crystals [43,44].The existence of 1TO and 1LO modes in the Raman spectra suggests that Ni 2+ and disordered oxygen may be present.This conclusion suggests that the catalysts are NiO materials, which is in agreement with the XRD (Figure 3) results.Similarly, for NiO−C, the peaks at 500 cm −1 and 1066 cm −1 correspond to the 1TO and 2LO signals of nickel oxide crystals.Combined with the above characterization data, the two catalysts are nickel oxide crystals before pretreatment.The redox properties of the catalysts were further investigated using temperatureprogrammed reduction (TPR), as shown in Figure 5.It can be observed that the reduction peaks of the two catalysts are both lower than 400 °C, indicating that NiO−C and NiO−U can be fully reduced at 400 °C.NiO−C displays a wide H2 reduction peak at 360 °C, which is assigned to the reduction of NiO [42,45].NiO−U exhibits three narrow H2 reduction peaks at 233 °C, 261 °C, and 283 °C, which are lower than those observed in NiO−C.A temperature of 200-300 °C is related to the phase transition and reduction of NiO.NiO−U can be reduced to nickel monomers at 350 °C [46].According to other research, it has been reported that Ni 2+ in NiO is more likely to generate defects, leading to the loss of an electron by the two neighboring Ni 2+ and the production of Ni 3+ on the NiO surface to preserve the charge balance [49].
The NiO-C catalyst after pretreatment was also evaluated, as shown in Figure 6a.Compared to fresh NiO-C, it can be observed that the intensity of the Ni 2+ peak weakened and a new peak appeared at 852.4 eV, which corresponds to Ni 0 [50,51].This indicates that nickel oxide is partially reduced to nickel monomers.After the HDO reaction, the catalyst also has a high peak at 852.4 eV, suggesting that nickel monomers are present in the catalyst.However, Ni 3+ is still present in spent catalysts, which may be due to the oxidation of the catalysts by exposure to air after the reaction (Figure 6a).[32,52] Combined with the results of the XRD (Figure 3) and H 2 -TPR (Figure 5) data, it can be assumed that metallic nickel is the main active phase in the reaction.Surface elemental composition and valence of elements in NiO catalysts were analyzed through XPS spectra.Figure 6a shows the XPS spectra of NiO−C catalysts, including a fresh catalyst, pretreated catalyst, and spent catalyst.The fresh NiO−C catalyst shows two peaks at 853.7 and 855.3 eV, which are related to Ni 2+ and Ni 3+ ions, respectively.And the peak at 860.7 eV is attributed to a high-spin Ni 2p3/2 satellite [47,48].It is worth noting that the existence of Ni 3+ does not necessarily indicate the presence of Ni2O3 in the sample According to other research, it has been reported that Ni 2+ in NiO is more likely to generate defects, leading to the loss of an electron by the two neighboring Ni 2+ and the production of Ni 3+ on the NiO surface to preserve the charge balance [49].
The NiO−C catalyst after pretreatment was also evaluated, as shown in Figure 6a Compared to fresh NiO−C, it can be observed that the intensity of the Ni 2+ peak weakened and a new peak appeared at 852.4 eV, which corresponds to Ni 0 [50,51].This indicates that nickel oxide is partially reduced to nickel monomers.After the HDO reaction, the catalyst also has a high peak at 852.4 eV, suggesting that nickel monomers are present in the catalyst.However, Ni 3+ is still present in spent catalysts, which may be due to the oxidation of the catalysts by exposure to air after the reaction (Figure 6a).[32,52] Combined with the results of the XRD (Figure 3) and H2-TPR (Figure 5) data, it can be assumed that metallic nickel is the main active phase in the reaction.Figure 7 shows the XPS spectra of O 1s for fresh, reduced and spent the NiO−C and NiO−U catalysts.The peaks at 529, 530.6, and 532 eV in fresh NiO−C are attributed to lattice oxygen, disordered oxygen, and surface-adsorbed hydroxyl group, respectively.According to the changes in the peak positions and peak intensities of O 1s, it can be seen that the fresh catalyst has a higher lattice oxygen content [53].However, as the catalyst is gradually reduced, nickel oxide gradually turns into nickel, reducing lattice oxygen content while gradually increasing the content of disordered oxygen.Table 2 lists the changes and proportions of various oxygen types in NiO.The trends in the positions and intensities of the peaks on the plots of O 1s for NiO−U catalysts are similar to those of NiO−C catalysts, but there is a significant difference in the amount of the various oxygen species present.In U−reduced NiO, disordered oxygen (530.9 eV) increases significantly to 77.5% (531 eV) after the reaction, which is nearly twice as much as that in NiO−C.Therefore, the amount of disordered oxygen may influence catalyst selectivity in low-temperature reactions [51,54].Figure 7 shows the XPS spectra of O 1s for fresh, reduced and spent the NiO-C and NiO-U catalysts.The peaks at 529, 530.6, and 532 eV in fresh NiO-C are attributed to lattice oxygen, disordered oxygen, and surface-adsorbed hydroxyl group, respectively.According to the changes in the peak positions and peak intensities of O 1s, it can be seen that the fresh catalyst has a higher lattice oxygen content [53].However, as the catalyst is gradually reduced, nickel oxide gradually turns into nickel, reducing lattice oxygen content while gradually increasing the content of disordered oxygen.Table 2 lists the changes and proportions of various oxygen types in NiO.The trends in the positions and intensities of the peaks on the plots of O 1s for NiO-U catalysts are similar to those of NiO-C catalysts, but there is a significant difference in the amount of the various oxygen species present.In U-reduced NiO, disordered oxygen (530.9 eV) increases significantly to 77.5% (531 eV) after the reaction, which is nearly twice as much as that in NiO-C.Therefore, the amount of disordered oxygen may influence catalyst selectivity in low-temperature reactions [51,54].
Figure 7 shows the XPS spectra of O 1s for fresh, reduced and spent the NiO−C and NiO−U catalysts.The peaks at 529, 530.6, and 532 eV in fresh NiO−C are attributed to lattice oxygen, disordered oxygen, and surface-adsorbed hydroxyl group, respectively According to the changes in the peak positions and peak intensities of O 1s, it can be seen that the fresh catalyst has a higher lattice oxygen content [53].However, as the catalyst is gradually reduced, nickel oxide gradually turns into nickel, reducing lattice oxygen con tent while gradually increasing the content of disordered oxygen.Table 2 lists the changes and proportions of various oxygen types in NiO.The trends in the positions and intensi ties of the peaks on the plots of O 1s for NiO−U catalysts are similar to those of NiO−C catalysts, but there is a significant difference in the amount of the various oxygen species present.In U−reduced NiO, disordered oxygen (530.9 eV) increases significantly to 77.5% (531 eV) after the reaction, which is nearly twice as much as that in NiO−C.Therefore, the amount of disordered oxygen may influence catalyst selectivity in low-temperature reac tions [51,54].The surface characteristics of NiO catalysts were investigated and analyzed by DRIFT-CO.Before the tests, two catalysts were pretreated with pure H 2 (16 mL/min) at 350 • C for 1 h in situ cell.For C-reduced NiO, two peaks at 2100-2200 cm −1 , assigned to the gas phase of CO, are observed, as seen in Figure 8a.This indicates that there is no chemical adsorption of CO on the surface of C-reduced NiO.The NiO-U catalyst after pretreatment undergoes the same testing procedure as the NiO-C.In contrast, U-reduced NiO shows two additional peaks at 2050 and 1975 cm −1 , which are related to linear and bridge CO adsorbed on metallic nickel (Figure 8b) [55].Following argon purging, the adsorption peaks' strength gradually decreases, and within 30 min, they completely disappear.
The absorption and desorption of H 2 O on NiO-U were also tested.As shown in Figure 9a, when water vapor is bubbled into the in situ cell at 300 • C, there is a broad absorption band at 3500-4000 cm −1 , which is attributed to the O-H stretching vibration.This could be caused by the water molecules adsorbed on the surface of NiO.When the bubbling stops, the peak of the O-H stretching vibration gradually decreases, indicating that the peak is mainly caused by physically adsorbed H 2 O.In addition, a weak absorption band is produced near 1650 cm −1 due to the effect of adsorbed H 2 O, which is attributed to the H-O-H bending vibration mode [56].The sharp peaks near 1320 and 3015 cm −1 are assigned to gaseous methane, proving that methane is produced.This is a result of the presence of contaminated carbon in the catalyst, which may have reacted with H 2 at 300 • C.This confirms that the C from the C-C cleavage of anisole can react with H 2 to produce methane, suggesting that the HDO reaction of anisole at 300 • C and above is primarily focused on hydrogenolysis.
hydroxyl oxygen (%) 20.9 13.2 9.4 The surface characteristics of NiO catalysts were investigated and analyzed by DRIFT-CO.Before the tests, two catalysts were pretreated with pure H2 (16 mL/min) at 350 °C for 1 h in situ cell.For C−reduced NiO, two peaks at 2100-2200 cm −1 , assigned to the gas phase of CO, are observed, as seen in Figure 8a.This indicates that there is no chemical adsorption of CO on the surface of C−reduced NiO.The NiO−U catalyst after pretreatment undergoes the same testing procedure as the NiO−C.In contrast, U−reduced NiO shows two additional peaks at 2050 and 1975 cm −1 , which are related to linear and bridge CO adsorbed on metallic nickel (Figure 8b) [55].Following argon purging, the adsorption peaks' strength gradually decreases, and within 30 min, they completely disappear.The absorption and desorption of H2O on NiO−U were also tested.As shown in Figure 9a, when water vapor is bubbled into the in situ cell at 300 °C, there is a broad absorption band at 3500-4000 cm −1 , which is attributed to the O-H stretching vibration.This could be caused by the water molecules adsorbed on the surface of NiO.When the bubbling stops, the peak of the O-H stretching vibration gradually decreases, indicating that the peak is mainly caused by physically adsorbed H2O.In addition, a weak absorption band is produced near 1650 cm −1 due to the effect of adsorbed H2O, which is attributed to the H-O-H bending vibration mode [56].The sharp peaks near 1320 and 3015 cm −1 are assigned to gaseous methane, proving that methane is produced.This is a result of the presence of contaminated carbon in the catalyst, which may have reacted with H2 at 300 °C.This confirms that the C from the C-C cleavage of anisole can react with H2 to produce methane, suggesting that the HDO reaction of anisole at 300 °C and above is primarily focused on hydrogenolysis.

Synthesis of Catalysts
NiO−C was obtained by calcinating 3 g Ni(NO3)2•6H2O (AR, Aladdin, Shanghai, China) in a muffle furnace at 350 °C for 3 h at a heating rate of 5 °C/min.NiO−U was prepared by the precipitation method.First of all, 7.793 g of Ni(NO3)2•6H2O (AR, Aladdin, Shanghai, China) and 19.31 g of urea (AR, Aladdin, Shanghai, China ) were dissolved in 200 mL of deionized water, then heated to 80 °C and stirred for 3 h with a rate of 400 r/min.Then, the solution was cooled to room temperature and filtered.Finally, the product of the precipitate was filtered and dried at 80 °C for 12 h.Then, the catalyst was calcined at

Synthesis of Catalysts
NiO-C was obtained by calcinating 3 g Ni(NO 3 ) 2 •6H 2 O (AR, Aladdin, Shanghai, China) in a muffle furnace at 350 • C for 3 h at a heating rate of 5 • C/min.NiO-U was prepared by the precipitation method.First of all, 7.793 g of Ni(NO 3 ) 2 •6H 2 O (AR, Aladdin, Shanghai, China) and 19.31 g of urea (AR, Aladdin, Shanghai, China ) were dissolved in 200 mL of deionized water, then heated to 80 • C and stirred for 3 h with a rate of 400 r/min.Then, the solution was cooled to room temperature and filtered.Finally, the product of the precipitate was filtered and dried at 80 • C for 12 h.Then, the catalyst was calcined at 350 • C in air for 3 h, and NiO-U was obtained.

Characterization Method
Scanning electron microscopy (SEM): Surface morphology of the samples was analyzed using a Regulus 8100 Scanning electron microscope made by Hitachi Company (Tokyo, Japan).The scan acceleration voltage was 0.5-30 kV.Before the test, a small amount of the sample was smeared on a conductive adhesive, and the unattached catalyst powder was blown off by a rubber suction bulb.
Transmission electron microscopy (TEM): TEM studies of the samples were performed using a TALOS F200s G2 field emission TEM (FEI, Hillsboro, OR, USA, accelerating voltage of 200 kV) to determine the morphology, metal distribution, particle size, and lattice fringes of the catalysts.In a typical TEM sample preparation, 10 mg of the sample was ground to a fine powder and dispersed in 5 mL of anhydrous ethanol by ultrasound.After dispersing the sample, the ethanol solution was added dropwise to the copper grid with a carbon lacey film.The sample was sent to be tested after being dried naturally.The morphologies of the samples were obtained in TEM and HRTEM modes.
X-ray powder diffraction (XRD): XRD patterns were measured by a Rigaku Smart Lab SE diffractometer (Rigaku, Tokyo, Japan) with copper Kα irradiation (λ = 0.1540 nm).The scan range was 30-85 • .The scan rate was 10 • /min.H 2 temperature-programmed reduction (H 2 -TPR): The reducibility of the catalysts was tested by H 2 -TPR.Temperature programming curves were recorded in an Auto-Chem II instrument (Micromeritics Instrument Corporation, Norcross, GA, USA) equipped with a TCD detector.During the test, 0.1 g fresh catalyst was loaded into a quartz tube reactor and then pretreated at 300 • C in a He gas environment for 60 min before cooling to 30 • C. In the temperature-programmed test, the temperature was raised to 500 • C at a heating rate of 10 • C/min in 10% H 2 /Ar gas mixture.
X-ray photoelectron spectroscopy (XPS): XPS spectra were measured with an ES-CALAB 250XI spectrometer (Thermo-Fisher, Waltham, MA, USA).Al target (1486.6eV) was used as the source of X-ray excitation, and C1 at 284.6 eV was used for charge correction.The XPS spectra were analyzed and fitted using Advantage software.
Diffuse reflectance infrared Fourier transform spectra of CO/H 2 O (DRIFT-CO/H 2 O): CO and H 2 O adsorption on the catalyst surface was detected by DRIFT-CO and DRIFT -H 2 O. Experiments were performed on a Nicolet IS50 FTIR spectrometer (Thermo Fisher Scientific, Waltham, MA, USA) with a ZnSe window and an MCT detector.A certain amount of NiO catalyst was reduced with 10% H 2 /Ar (20 mL/min) and pure Ar (20 mL/min) for 1 h at 350 • C.Then, it was naturally cooled to room temperature or 300 • C in a reduced atmosphere and swept with pure Ar (20 mL/min) until there was no H 2 in the pipe.When the OMNIC spectra software detected that the baseline was stable, 10% CO/Ar or H 2 O was introduced to the sample cell and the spectra for testing.When CO or H 2 O was saturated, the gas path was closed, and infrared desorption spectra were recorded.
Raman: Raman spectroscopy (Raman) was used to measure the state and structure of catalyst metals.Tests were performed on a DXR2xi Micro Raman Spectrometer (Thermo Fisher Scientific, Waltham, MA, USA) with a 532 nm laser source.During the test, laser intensity and exposure time were adjusted to look for a better signal-to-noise ratio and obtain clear Raman images.

Catalyst Evaluation
The catalytic reaction was carried out in a fixed-bed reactor with 100 mg NiO-C or 100 mg NiO-U catalyst and a certain amount of quartz sand in a quartz tube.The catalysts were pretreated with H 2 (16 mL/min) at 350 • C for 1 h.After pretreatment, the reactor was cooled to room temperature naturally, and then the gas path was changed so that H 2 (4 mL/min) passed through the anisole bubbling bottle and the anisole vapor was carried into the reactor.The reactor heating rate was 10 mL/min, and the catalytic performance of the catalysts was evaluated at temperatures from 150 to 400 • C.During the reaction, the gas flowing out of the reactor was detected by online GC in real time, and the conversion and selectivity for each product were calculated as follows.
Selectivity X (%) = N X ∑ N All, products × 100% Selectivity X -selectivity of X product; N X -mol of product X; ∑N All,products -sum mol of all products.

Conclusions
In summary, two NiO catalysts were prepared by different methods and used for the reaction of anisole hydrodeoxygenation.After pretreatment, it was found that the two catalysts have completely different selectivity for HDO under low temperature conditions (150 • C).The two catalysts were characterized by XRD, TEM, and Raman, which found that fresh catalysts are nickel oxides.After the HDO reaction, nickel catalysts transform into metallic nickel, which was confirmed by XRD, TEM and XPS analysis.According to the H 2 -TPR results, NiO-U is completely reduced at a lower temperature.In addition, the DRIFT-H 2 O results revealed that the HDO reaction of anisole with U-reduced NiO catalyst tends to follow the hydrogenolysis pathway at 300 • C, and its selectivity to methane is nearly 100%.The catalytic performance and characterization results indicate that the three different types of route-anisole hydrogenation, HDO, and C-C hydrogenolysis-are all affected by temperature.As shown in Scheme 1, at 150 • C, C-reduced NiO is prone to following the hydrogenation route, and U-reduced NiO is more likely to undergo the HDO reaction.When temperature increases to 300 • C, the reaction will undergo C-C hydrogenolysis.This work provides a new insight into the hydrodeoxygenation of anisole.

Figure 1 .
Figure 1.Hydrogenation activity patterns of NiO−C and NiO−U after pretreatment.Conversion of anisole and distribution of products during the reaction as a function of temperature for (a) C−reduced NiO and (b) U−reduced NiO.Selectivity of hydrogenation products, hydrodeoxygenation products, and hydrocracking products at different temperatures for (c) C−reduced NiO and (d) U−reduced NiO.

Figure 1 .
Figure 1.Hydrogenation activity patterns of NiO-C and NiO-U after pretreatment.Conversion of anisole and distribution of products during the reaction as a function of temperature for (a) C-reduced NiO and (b) U-reduced NiO.Selectivity of hydrogenation products, hydrodeoxygenation products, and hydrocracking products at different temperatures for (c) C-reduced NiO and (d) U-reduced NiO.

Figure 2 .
Figure 2. Scanning electron microscope (SEM) and transmission electron microscope (TEM) images of NiO−C and NiO−U: SEM images of (a,b) NiO−C and (e,f) NiO−U; TEM images of (c,d) NiO−C and (g,h) NiO−U.

Figure 2 .
Figure 2. Scanning electron microscope (SEM) and transmission electron microscope (TEM) images of NiO-C and NiO-U: SEM images of (a,b) NiO-C and (e,f) NiO-U; TEM images of (c,d) NiO-C and (g,h) NiO-U.

Figure 2 .
Figure 2. Scanning electron microscope (SEM) and transmission electron microscope (TEM) images of NiO−C and NiO−U: SEM images of (a,b) NiO−C and (e,f) NiO−U; TEM images of (c,d) NiO−C and (g,h) NiO−U.

Figure 4 .
Figure 4. Raman spectra of fresh NiO−C and NiO−U catalysts.

Figure 4 .
Figure 4. Raman spectra of fresh NiO-C and NiO-U catalysts.The redox properties of the catalysts were further investigated using temperatureprogrammed reduction (TPR), as shown in Figure5.It can be observed that the reduction peaks of the two catalysts are both lower than 400 • C, indicating that NiO-C and NiO-U can be fully reduced at 400 • C. NiO-C displays a wide H 2 reduction peak at 360 • C, which is assigned to the reduction of NiO[42,45].NiO-U exhibits three narrow H 2 reduction peaks at 233 • C, 261 • C, and 283 • C, which are lower than those observed in NiO-C.A temperature of 200-300 • C is related to the phase transition and reduction of NiO.NiO-U can be reduced to nickel monomers at 350 • C[46].Surface elemental composition and valence of elements in NiO catalysts were analyzed through XPS spectra.Figure6ashows the XPS spectra of NiO-C catalysts, including a fresh catalyst, pretreated catalyst, and spent catalyst.The fresh NiO-C catalyst shows two peaks at 853.7 and 855.3 eV, which are related to Ni 2+ and Ni 3+ ions, respectively.And the peak at 860.7 eV is attributed to a high-spin Ni 2p3/2 satellite[47,48].It is worth noting that the existence of Ni 3+ does not necessarily indicate the presence of Ni 2 O 3 in the sample.According to other research, it has been reported that Ni 2+ in NiO is more likely to generate defects, leading to the loss of an electron by the two neighboring Ni 2+ and the production of Ni 3+ on the NiO surface to preserve the charge balance[49].The NiO-C catalyst after pretreatment was also evaluated, as shown in Figure6a.Compared to fresh NiO-C, it can be observed that the intensity of the Ni 2+ peak weakened and a new peak appeared at 852.4 eV, which corresponds to Ni 0[50,51].This indicates that nickel oxide is partially reduced to nickel monomers.After the HDO reaction, the catalyst also has a high peak at 852.4 eV, suggesting that nickel monomers are present in the catalyst.However, Ni 3+ is still present in spent catalysts, which may be due to the oxidation of the catalysts by exposure to air after the reaction (Figure6a).[32,52]Combined with the results
NiO−U and NiO−C have remarkably similar profiles and catalyst valence transformations.According to Figure 6b, Ni 2+ and Ni 3+ peaks in the fresh NiO−U catalyst are located at 853.6 eV and 855.3 eV, respectively.The Ni 2p spectra of NiO−U undergo the same changes as those of NiO−C during pretreatment and the reaction.A Ni 0 peak appears suggesting that reduced and spent catalysts are converted to monomeric nickel.Metal Ni undergoes spontaneous oxidation in the atmosphere, and then the presence of Ni 3+ is captured by XPS.

Figure 6 .
Figure 6.X-ray photoelectron spectra of Ni 2p for (a) NiO-C and (b) NiO-U catalysts before the reaction, after pretreatment, and after the reaction.NiO-U and NiO-C have remarkably similar profiles and catalyst valence transformations.According to Figure 6b, Ni 2+ and Ni 3+ peaks in the fresh NiO-U catalyst are located at 853.6 eV and 855.3 eV, respectively.The Ni 2p spectra of NiO-U undergo the same changes as those of NiO-C during pretreatment and the reaction.A Ni 0 peak appears, suggesting that reduced and spent catalysts are converted to monomeric nickel.Metal Ni undergoes spontaneous oxidation in the atmosphere, and then the presence of Ni 3+ is captured by XPS.Figure7shows the XPS spectra of O 1s for fresh, reduced and spent the NiO-C and NiO-U catalysts.The peaks at 529, 530.6, and 532 eV in fresh NiO-C are attributed to lattice oxygen, disordered oxygen, and surface-adsorbed hydroxyl group, respectively.According to the changes in the peak positions and peak intensities of O 1s, it can be seen

Figure 7 .
Figure 7. X-ray photoelectron spectroscopy (XPS) spectra of O 1s for NiO−C and NiO−U catalysts (a before the reaction, (b) after reduction, and (c) after the reaction.The blue line represents lattice oxygen, red line is disordered oxygen and green line is hydroxyl oxygen.

Figure 7 .
Figure 7. X-ray photoelectron spectroscopy (XPS) spectra of O 1s for NiO-C and NiO-U catalysts (a) before the reaction, (b) after reduction, and (c) after the reaction.The blue line represents lattice oxygen, red line is disordered oxygen and green line is hydroxyl oxygen.

Figure 9 .
Figure 9. DRIFT-H2O spectra of NiO−U catalysts.(a) is the adsorption of water by NiO over 190 min, and (b) is the desorption of H2O when NiO−U stops bubbling water vapor and purges with pure Ar (20 mL/min).

Figure 9 .
Figure 9. DRIFT-H 2 O spectra of NiO-U catalysts.(a) is the adsorption of water by NiO over 190 min, and (b) is the desorption of H 2 O when NiO-U stops bubbling water vapor and purges with pure Ar (20 mL/min).

Table 1 .
XRD peak analyses of fresh, reduced, and spent NiO-C and NiO-U catalysts.
a Average sizes were estimated using the Scherrer formula.

Table 2 .
Fresh catalysts, reduced catalysts, and spent NiO-C and NiO-U catalysts with different oxygen ratios.