Hydrogen Photo-Production from Glycerol Using Nickel-Doped TiO 2 Catalysts: E ﬀ ect of Catalyst Pre-Treatment

: In the present piece of research, hydrogen production via the photo-reforming of glycerol (a byproduct from biodiesel generation) is studied. Catalysts consisted of titania modiﬁed by Ni (0.5% by weight) obtained through deposition–precipitation or impregnation synthetic methods (labelled as Ni-0.5-DP and Ni-0.5-IMP, respectively). Reactions were performed both under UV and solar irradiation. Activity signiﬁcantly improved in the presence of Ni, especially under solar irradiation. Moreover, pre-reduced solids exhibited higher catalytic activities than untreated solids, despite the “in-situ” reduction of nickel species and the elimination of surface chlorides under reaction conditions (as evidenced by XPS). It is possible that the catalyst pretreatment at 400 ◦ C under hydrogen resulted in some strong metal–support interactions. In summary, the highest hydrogen production value (ca. 2600 micromole H 2 · g − 1 ) was achieved with pre-reduced Ni-0.5-DP solid using UV light for an irradiation time of 6 h. This value represents a 15.7-fold increase as compared to Evonik P25.


Introduction
Fossil fuel depletion and environmental concerns have resulted in the search for clean energies, with one alternative being hydrogen [1].Its use has two main advantages [2,3]: i) a high chemical energy per mass (120 KJ/g), superior to that of many fossil fuels, and ii) its combustion only results in water; therefore, it does not emit any toxic substance or greenhouse gas into the atmosphere.
Nevertheless, hydrogen does not exist in nature in its molecular H 2 form but combined to other elements; thus, it requires dedicated methods for its production.Therefore, whether or not the use of hydrogen as an energy vector can be termed as "fully green" is dependent on its method of production.
Currently, the most widespread hydrogen production methodologies are hydrocarbon reforming with water vapor and water electrolysis.Hydrocarbon reforming has the disadvantages of being based on raw materials which are taken from non-renewable fossil sources and, therefore, the co-generated CO 2 directly impacts the environment by the greenhouse effect.An additional drawback of hydrocarbon reforming with water vapor is its high operating temperature.On the other hand, regarding the production of hydrogen through water electrolysis, its main associated problem is the high consumption of electrical energy to carry out the process.Solar thermal energy can be used as an alternative for water electrolysis but, in this case, large and expensive facilities are needed.
Recently, in addition to the mentioned technologies, innovative techniques have been being developed and could be complementary to those already existing in the medium-term future.Some of these hydrogen production techniques are plasma technology [4], biological production methods such Energies 2019, 12, 3351 2 of 14 as dark fermentation [5,6] or the photocatalytic reforming of oxygenated organic compounds [7,8].The photocatalytic reforming of oxygenated organic compounds consists in the treatment of these compounds with light radiation in the presence of water, at room temperature and under anaerobic conditions, to generate gaseous hydrogen and carbon dioxide.The potential of hydrogen production through photocatalytic reforming is fulfilled when biomass residues (bio-glycerol or glucose, among others) are used as oxygenated organic compounds since, in this case, the generated CO 2 was previously consumed by the biomass during its growth, so there is no net emission of CO 2 but a closing of the carbon cycle [9].In the process, light is used to activate a semiconductor, promoting electrons from the valence to the conduction band.The oxygenated organic compound is used as a sacrificial agent to favor the elimination of the positively-charged holes, whereas electrons are used to reduce protons and generate H 2 .As for the sacrificial agents, glycerol is an excellent candidate since it is a by-product of biodiesel production [10].
One of the keys to the success of this emergent technology is the development of suitable catalysts (i.e., semiconductors) which are able to maximize light harvesting and therefore the hydrogen production [11].TiO 2 is the most widely used semiconductor as a result of its high photocatalytic activity and due to the fact that it is inexpensive, not toxic and biologically and chemically inert [12].Its main drawback is its band gap value (ca.3.2 eV), which means that only ca. 5% of solar irradiation is absorbed.Furthermore, it also exhibits a high electron-hole recombination rate, which is detrimental to the photocatalytic activity [13].
One alternative to overcome these problems is the incorporation of metals to the semiconductor [14] (Figure 1), which can shift the absorption to the visible light and also act as electron traps, thus preventing electron-hole recombination.Noble metals such as silver [15], gold [16], platinum [17] or palladium [18] have been found to be particularly effective, although there is a need to implement some more cost-effective transition metals such as iron [19], nickel [20,21] and copper [22,23].Recently, in addition to the mentioned technologies, innovative techniques have been being developed and could be complementary to those already existing in the medium-term future.Some of these hydrogen production techniques are plasma technology [4], biological production methods such as dark fermentation [5,6] or the photocatalytic reforming of oxygenated organic compounds [7,8].The photocatalytic reforming of oxygenated organic compounds consists in the treatment of these compounds with light radiation in the presence of water, at room temperature and under anaerobic conditions, to generate gaseous hydrogen and carbon dioxide.The potential of hydrogen production through photocatalytic reforming is fulfilled when biomass residues (bio-glycerol or glucose, among others) are used as oxygenated organic compounds since, in this case, the generated CO2 was previously consumed by the biomass during its growth, so there is no net emission of CO2 but a closing of the carbon cycle [9].In the process, light is used to activate a semiconductor, promoting electrons from the valence to the conduction band.The oxygenated organic compound is used as a sacrificial agent to favor the elimination of the positively-charged holes, whereas electrons are used to reduce protons and generate H2.As for the sacrificial agents, glycerol is an excellent candidate since it is a by-product of biodiesel production [10].
One of the keys to the success of this emergent technology is the development of suitable catalysts (i.e., semiconductors) which are able to maximize light harvesting and therefore the hydrogen production [11].TiO2 is the most widely used semiconductor as a result of its high photocatalytic activity and due to the fact that it is inexpensive, not toxic and biologically and chemically inert [12].Its main drawback is its band gap value (ca.3.2 eV), which means that only ca. 5% of solar irradiation is absorbed.Furthermore, it also exhibits a high electron-hole recombination rate, which is detrimental to the photocatalytic activity [13].
One alternative to overcome these problems is the incorporation of metals to the semiconductor [14] (Figure 1), which can shift the absorption to the visible light and also act as electron traps, thus preventing electron-hole recombination.Noble metals such as silver [15], gold [16], platinum [17] or palladium [18] have been found to be particularly effective, although there is a need to implement some more cost-effective transition metals such as iron [19], nickel [20,21] and copper [22,23] .
. Figure 1.Activation of titania using a metal as a co-catalyst.
In the present piece of research, nickel structural (particle size) and chemical properties (oxidation state) in Ni-modified titania photocatalysts has been addressed, and their influence on hydrogen production from glycerol photo-reforming studied.Two catalyst synthetic methods (impregnation vs. deposition-precipitation) and catalyst pre-reduction treatment were analyzed and their influence on the amount of hydrogen photo-produced revealed under both UV and solar radiation.In the present piece of research, nickel structural (particle size) and chemical properties (oxidation state) in Ni-modified titania photocatalysts has been addressed, and their influence on hydrogen production from glycerol photo-reforming studied.Two catalyst synthetic methods (impregnation vs. deposition-precipitation) and catalyst pre-reduction treatment were analyzed and their influence on the amount of hydrogen photo-produced revealed under both UV and solar radiation.

Deposition-precipitation Method
The deposition-precipiation method was used for incorporation of nickel on P25 Evonik with a nominal weight of 0.5%.The incorporation of Nickel was carried out in a "Contalab" system (Switzerland) enabling careful control of all the variables, i.e., pH, temperature, stirrer speed, reactant feed flow, etc. Firstly in 150 mL distilled water were dispersed 5 g of P25 Evonik using ultrasound.The deposition of the nickel was carried out at 60 • C and a pH of 6.8, keeping it constant with an 0.2 M aqueous solution of K 2 CO 3 (Sigma Aldrich).Next, an aqueous solution of 2 g•L −1 of nickel (using NiCl 2 (Sigma Aldrich)) was added dropwise and the mixture was maintained for 1 h at 60 • C. Then the solid obtained was filtered and washed with distilled water.Then, the solid was dried at 110 • C overnight.Finally, the solids were calcined at 400 • C for 6 h (using a ramp rate of 10 • C•min −1 ).

Impregnation Method
A total of 5 g of TiO 2 (P25 Evonik) was dispersed in 100 mL of distilled water containing the required amount of NiCl 2 (Sigma Aldrich) aqueous solution in order to have a nickel nominal content of 0.5% by weight.The suspension was stirred for 1 h and then vacuum filtered at 100 • C.Then, the solid was dried overnight (100 • C) and calcined at 400 • C for 6 h (ramp rate 10 • C•min −1 ).
The catalyst nomenclature includes the metal (Ni), the nominal content (0.5% by weight) and a suffix indicating the synthetic method (DP or IMP for deposition-precipitation or impregnation, respectively).

Catalyst Pre-Reduction
The catalysts were used either as synthesized or after a pre-reduction treatment.In the latter case, the solids were treated at room temperature under N 2 flow (20 mL•min −1 ) for 15 min and then submitted to hydrogen (10mL•min −1 ), the temperature being ramped up to 400 • C (rate, 10 • C•min −1 ) and the final temperature being maintained for 1 h.The nomenclature of pre-reduced solids includes the "Red" suffix.

Characterization of the Solids
The determination of the metallic content in the samples was carried out by by inductively coupled plasma mass spectrometry (ICP-MS) using a Perkin Elmer NexionX instrument.Digestion of the samples consisted in dissolution of the sample in an acid solution of 1:1 H 2 O/H 2 SO 4 /HF solution at 80 • C and and after in 1:3 HNO 3 /HCl mixture.The measurements were carried out by the staff at the Central Service for Research Support (SCAI) of the University of Córdoba.
Transmission electron microscopy (TEM) images were obtained with a JEOL JEM 1400 transmission electron microscope.For the measurements were used a 3 mm holey carbon copper grids.Particle sizes were obtained using using the software ImageJ (a public domain Java image processing and analysis program).TEM was carried out at the Central Service for Research Support (SCAI) of the University of Córdoba.
A Cary 1E (Varian) instrument was used for determination of Band Gap values by Diffuse reflectance UV-vis spectra, using as reference material the polytetraethylene (density = 1 g•cm -3 and thickness = 6 mm).The plot of the modified Kubelka-Munk function [F(R)•E] 1/2 versus the energy of the absorbed light E was use to obtain the value of band gap, extrapolating to y = 0 of the linear regression range.X-ray photoelectron spectroscopy (XPS) data were recorded by a Leibold-Heraeus LHS10 spectrometer capable of operating down to less than 2 × 10 −9 Torr, was equipped with an EA-200MCD hemispherical electron analyzer with a dual X-ray source using AlKα(hν = 1486.6eV) at 120 W, at 30 mA, with C (1s) as energy reference (284.6 eV).The sample was prepared in a on 4 mm × 4 mm pellets 0.5 mm thick, and outgassing to a pressure below about 2 × 10 −8 Torr at 150 • C in the instrument pre-chamber.XPS experiments were carried out at the Central Service for Research Support (SCAI) of the University of Córdoba.
In an Autochem 2920 analyser (Micromeritics Instrument Corp., Norcross, GA, USA) was carried out the Temperature-programmed reduction (TPR) measurements, 200 mg of the solids was used to carried out the experiment with a flow of 40 mL•min −1 of a 5% H 2 /Ar stream.The temperature was ramped from room temperature to 500

Photocatalytic Experiments
Photocatalytic experiments were performed in a 30 mL double -mouthed heart-shaped reactor under UV light irradiation (UV Spotlight source Lightningcure TM L8022, Hamamatsu, maximum emission at 365 nm) or solar irradiation (Newport, Xe lamp).Light was focalized on the sample compartment through an optic fiber.In a typical process, 5 mg of catalyst was dispersed into 5 mL of glycerol/water (10% v/v) solution.Reactions were performed under an inert atmosphere, achieved by bubbling a nitrogen flow (20 mL•min −1 ) for 30 min.The catalyst suspension was continuously stirred (800 rpm) and the reactor was thermostated at 20 • C. A picture of the photocatalytic reactor is shown in Figure 2.
Energies 2019, 12, x FOR PEER REVIEW 4 of 14 X-ray photoelectron spectroscopy (XPS) data were recorded by a Leibold-Heraeus LHS10 spectrometer capable of operating down to less than 2 × 10 −9 Torr, was equipped with an EA-200MCD hemispherical electron analyzer with a dual X-ray source using AlKα(hν = 1486.6eV) at 120 W, at 30 mA, with C (1s) as energy reference (284.6 eV).The sample was prepared in a on 4 mm × 4 mm pellets 0.5 mm thick, and outgassing to a pressure below about 2 × 10 −8 Torr at 150 °C in the instrument pre-chamber.XPS experiments were carried out at the Central Service for Research Support (SCAI) of the University of Córdoba.
In an Autochem 2920 analyser (Micromeritics Instrument Corp., Norcross, GA, USA) was carried out the Temperature-programmed reduction (TPR) measurements, 200 mg of the solids was used to carried out the experiment with a flow of 40 mL•min −1 of a 5% H2/Ar stream.The temperature was ramped from room temperature to 500 °C at 10 °C•min −1 .

Photocatalytic Experiments
Photocatalytic experiments were performed in a 30 mL double -mouthed heart-shaped reactor under UV light irradiation (UV Spotlight source Lightningcure TM L8022, Hamamatsu, maximum emission at 365 nm) or solar irradiation (Newport, Xe lamp).Light was focalized on the sample compartment through an optic fiber.In a typical process, 5 mg of catalyst was dispersed into 5 mL of glycerol/water (10% v/v) solution.Reactions were performed under an inert atmosphere, achieved by bubbling a nitrogen flow (20 mL•min −1 ) for 30 min.The catalyst suspension was continuously stirred (800 rpm) and the reactor was thermostated at 20 °C.A picture of the photocatalytic reactor is shown in Figure 2. Hydrogen was analyzed by sampling with a pressure-lock precision analytical syringe (Valco VICI Precision Syringes, 1 mL, leak-tight to 250 psi) from the head space after 3 and 6 hours of irradiation.Analyses were performed on an Agilent Technologies 7890A gas chromatograph equipped with a Supelco Carboxen TM 1010 Plot column with TCD detector.The separation was performed at 70 °C for 2 min, followed by heating to 120 °C (ramp of 10 °C•min −1 ), and was left for 8 minutes (total analysis time, 15 min).All reactions were performed in duplicate, with the standard deviation being below 3%.The calibration plot (Figure S1) and a typical chromatogram for hydrogen quantification (Figure S2) are given in the Supplementary Materials.

Results and Discussion
The synthesized catalysts were characterized from the structural and chemical point of view with a wide variety of techniques.The chemical composition was determined by ICP-MS and the Picture of the photocatalytic reactor used in the hydrogen production from glycerol photo-reforming.
Hydrogen was analyzed by sampling with a pressure-lock precision analytical syringe (Valco VICI Precision Syringes, 1 mL, leak-tight to 250 psi) from the head space after 3 and 6 h of irradiation.Analyses were performed on an Agilent Technologies 7890A gas chromatograph equipped with a Supelco Carboxen TM 1010 Plot column with TCD detector.The separation was performed at 70 • C for 2 min, followed by heating to 120 • C (ramp of 10 • C•min −1 ), and was left for 8 min (total analysis time, 15 min).All reactions were performed in duplicate, with the standard deviation being below 3%.The calibration plot (Figure S1) and a typical chromatogram for hydrogen quantification (Figure S2) are given in the Supplementary Materials.

Results and Discussion
The synthesized catalysts were characterized from the structural and chemical point of view with a wide variety of techniques.The chemical composition was determined by ICP-MS and the results, presented in Table 1, evidenced a good incorporation of nickel, with values being quite close to the nominal content (0.5% by weight).X-ray diffraction patterns were obtained and used to obtain structural information of the catalysts, and the results are presented in Figure S3.The Evonik P25 support clearly shows the diffraction lines corresponding to anatase (80%) and rutile (20%) phases, which are not affected by nickel incorporation, independent of the synthetic method or reduction treatment.In addition, consistent with the small metal loading and the homogeneous nickel dispersion evidenced by TEM micrographs, no signals associated to nickel species are observed.
Temperature-programmed reduction (TPR) measurements were carried out for both Ni-0.5-DP and Ni-0.5-IMP catalysts, and the results are presented in Figure 3 (right).These results showed that the reduction peaks associated with nickel species begin at temperatures below 200 • C but extend to 400 • C.  6, and the particle size distribution is shown in Figure S5.Ni particle sizes were determined using ImageJ software.The deposition-precipitation method resulted in particles with an average size of 2 nm, whereas the impregnation method led to more heterogeneously-distributed sizes (Figure S5), with the average particle size being 4-5 nm.Particle sizes did not vary significantly after the pre-reduction treatment.It is well known that NiO is usually the main surface species when nickel is deposited in high loads on metal oxide-type supports.However, certain species from the Ni-support interaction can be observed depending on the physicochemical properties of the support.It has been reported that the reduction of certain nickel species is difficult in supported nickel catalysts, with this difficulty being proportional to the strength of the Ni-support interaction [24].In general, the Ni-support interaction falls into three categories: i) an absence of interaction, which occurs when the support acts as a mere dispersing agent, ii) a weak interaction, usually associated with the presence of small nickel nanoparticles deposited on the support; and iii) a very strong interaction, involving the formation of a Energies 2019, 12, 3351 6 of 14 new surface species (creation of new chemical bonds).The degree of interaction depends on the nickel charge (particle size) and the calcination temperature of the catalyst [24].
It has been reported that the reduction of unsupported NiO takes place at temperatures of around 220 • C [24], while the presence of metal-support interactions extend the nickel reduction process to higher temperatures.However, Petrik et al. associated the observed reduction peak at 200 • C to the reduction of Ni 2 O 3 (ions with formal oxidation state higher than +2) to NiO [25].In this sense, Carley et al. demonstrated, through XPS studies, the massive formation of surface Ni 3+ species after the calcination of the solid at temperatures above 300 • C [26].Finally, the reduction peaks observed at higher temperatures (300-600 • C) were associated with the reduction of the previously formed NiO species or to the reduction of small nanoparticles interacting with the TiO 2 support [25].
Based on the above considerations, the observed reduction peak at about 200 • C could be associated with either the reduction of bulk NiO or with the reduction of Ni +3 species (nickel ions with a formal oxidation state higher than +2) [25,26].Given the low nickel loading (0.5%) as well as the small particle sizes reported by TEM (2 and 4 nm for Ni-0.5-DP and Ni-0.5-IMP, respectively), it is more feasible to associate the reduction peak at 200 • C with the reduction of Ni +3 species present in the catalyst.Reduction peaks observed at higher temperatures would be associated with small NiO particles interacting with the titania support.According to these results, the temperature chosen for catalyst reduction was set to 400 • C.
Band-gap energy values of the semiconductors were determined from UV-Vis spectra.The method for the determination of band gap values is shown in Figure S4 using the example of Ni-0.5-IMP-Red.As can be seen, the modification of the reference titania material (Evonik P25) by nickel incorporation resulted in a slight decrease in the band gap (Table 2), with the absorption being shifted to the visible spectrum (Figure 3, left)  TEM micrographs of the different solids are shown in Figures 4-6, and the particle size distribution is shown in Figure S5.Ni particle sizes were determined using ImageJ software.The deposition-precipitation method resulted in particles with an average size of 2 nm, whereas the impregnation method led to more heterogeneously-distributed sizes (Figure S5), with the average particle size being 4-5 nm.Particle sizes did not vary significantly after the pre-reduction treatment.Furthermore, the Ni particle size did not vary significantly after the first use.In the case of the utilization of UV light, there were no changes either after the second use.On the contrary, when solar irradiation was applied, the Ni particle size in the Ni-0.5-DPsample increased up to 5 nm (Figure 6).
The surface chemical composition of the solids was studied by XPS, and the main results are summarized in Table 3.As far as the Ti (2p3/2) signal is concerned, there were no significant changes after the incorporation of nickel, with the signal appearing at ca. 458.5 eV, which is a typical value for Ti 4+ in TiO 2 .Regarding the Ni 2p3/2 signal, it has been reported that binding energies at 852.6, 854.6, and 856.1 eV correspond to Ni 0 , Ni +2 , and Ni +3 , respectively [25,27]  Furthermore, the Ni particle size did not vary significantly after the first use.In the case of the utilization of UV light, there were no changes either after the second use.On the contrary, when solar irradiation was applied, the Ni particle size in the Ni-0.5-DPsample increased up to 5 nm (Figure 6).Furthermore, the Ni particle size did not vary significantly after the first use.In the case of the utilization of UV light, there were no changes either after the second use.On the contrary, when solar irradiation was applied, the Ni particle size in the Ni-0.5-DPsample increased up to 5 nm (Figure 6).The surface chemical composition of the solids was studied by XPS, and the main results are summarized in Table 3.As far as the Ti (2p3/2) signal is concerned, there were no significant changes after the incorporation of nickel, with the signal appearing at ca. 458.5 eV, which is a typical value for Ti 4+ in TiO2.Regarding the Ni 2p3/2 signal, it has been reported that binding energies at 852.6, 854.6, and 856.1 eV correspond to Ni 0 , Ni +2 , and Ni +3 , respectively [25,27].As we have commented  rather than with NiO, whose signal appeared at around 855 eV.The authors thus speculated the existence of Ti-Ni-O interactions that were reflected as Ni +3 species in the XPS spectra [25].
In this work, the XPS data associated with Ni (2p3/2) signals are presented in Table 3 and Figure S6.The spectra showed a signal at ca. 856 eV for fresh unreduced solids which was assigned to Ni +3 species, whereas, after the reduction treatment, the signal shifts to 855 eV as a result of the reduction of Ni +3 to Ni +2 species.This is in agreement with the reduction peak observed in the TPR profile at around 200 • C.Moreover, in the XPS analysis of the non-reduced catalysts used in a photo-reforming process (both UV and solar), the Ni (2p3/2) signal appears at ca. 855 eV, indicating that during the photocatalytic process, the in-situ reduction of Ni +3 to Ni +2 species takes place (Figure S6).No signal associated to Ni metal was detected in XPS profiles, even for the reduced solids, and so the catalyst reduction at 400 • C would not be strong enough to carry out the NiO reduction to Ni 0 , or else the hypothetically formed Ni 0 would re-oxidize in contact with air.In this sense, Ju et al. have already reported the absence of the Ni (0) peak at 852 eV after the reductive treatment of nickel-containing absorbents, were was associated with the difficulty of reducing NiO to metallic nickel [28].
It is also interesting to note that XPS revealed the presence of chlorine from the precursor in fresh unreduced solids (0.56 and 0.80 atomic % for Ni-0.5-IMP and Ni-0.5-DP, respectively).Such chlorine atoms were eliminated either during pre-reduction treatment as HCl or during the photocatalytic reaction.
H 2 production from glycerol photo-reforming on fresh unreduced catalysts after 3 and 6 h of UV (A) or solar (B) irradiation are given in Figure 7.For the sake of comparison, results obtained for the reference material (Evonik P25) have also been included.
A first conclusion from Figure 7 is that hydrogen production using UV light is always higher than that achieved with solar light.This is hardly surprising, considering that the former irradiation source is more energetic.Moreover, Ni incorporation to TiO 2 (irrespective of the method) led to an increase in hydrogen production.For instance, when UV light was used, hydrogen production increased from 166 micromole•g −1 (Evonik P25) up to 534 (Ni-0.5-DP)or 551 (Ni-0.5-IMP)after t = 6 h.Such an increase is even more significant when visible light was used.The observed shift of UV-Vis absorption to the visible region on the introduction of Ni could account for this effect.
A comparison of hydrogen production on pre-reduced (Figure 8) and untreated systems (Figure 7) allows us to conclude that catalyst pre-reduction treatment significantly increases catalytic activity (3-5 fold or 8-9 fold for experiments under UV or solar irradiation, respectively).As with the untreated systems, there are no large differences in their catalytic behavior depending on the synthesis procedure (DP or IMP).In the pre-reduced systems, those synthesized by DP have 39% greater activity, which could be due to the more homogeneous particle size distribution of Ni.
Energies 2019, 12, 3351 9 of 14 Ni-0.5-DP 2 using UV 855.2 458.4 -Ni-0.5-DP 2 using solar 854.9 458.4 -H2 production from glycerol photo-reforming on fresh unreduced catalysts after 3 and 6 hours of UV (A) or solar (B) irradiation are given in Figure 7.For the sake of comparison, results obtained for the reference material (Evonik P25) have also been included.A first conclusion from Figure 7 is that hydrogen production using UV light is always higher than that achieved with solar light.This is hardly surprising, considering that the former irradiation source is more energetic.Moreover, Ni incorporation to TiO2 (irrespective of the method) led to an increase in hydrogen production.For instance, when UV light was used, hydrogen production increased from 166 micromole•g −1 (Evonik P25) up to 534 (Ni-0.5-DP)or 551 (Ni-0.5-IMP)after t = 6 h.Such an increase is even more significant when visible light was used.The observed shift of UV-Vis absorption to the visible region on the introduction of Ni could account for this effect.
A comparison of hydrogen production on pre-reduced (Figure 8) and untreated systems (Figure 7) allows us to conclude that catalyst pre-reduction treatment significantly increases catalytic activity (3-5 fold or 8-9 fold for experiments under UV or solar irradiation, respectively).As with the untreated systems, there are no large differences in their catalytic behavior depending on the synthesis procedure (DP or IMP).In the pre-reduced systems, those synthesized by DP have 39% greater activity, which could be due to the more homogeneous particle size distribution of Ni.
The highest hydrogen production values (2606 H2 micromole•g −1 ) corresponded to Ni-0.5-DP-Red for t = 6 h.This value is similar to that achieved in previous studies on 0.2% Pt [29], which is quite promising considering that Pt is ca.2000 times more expensive than Ni.
Some authors, such as Bahruji et al. [30], have described the influence of the metal oxidation state on the photocatalytic process.As can be seen in Figure 9B, the electron transfer from titania to NiO is thermodinamically impeded.On the contrary, the pre-reduction of the solid (Figure 9A) results in electron transfer from titania to Ni(0) being favored, with the metal thus acting as an electron trap and preventing electron-hole recombination.
Furthermore, Caravaca et al. [31], studying hydrogen photo-production from sugars on Ni-based catalysts, observed an induction period (in their case, 60 min) required for in-situ reduction of NiO to Ni.After that period of time, the hydrogen production rate of both the untreated and pre-reduced solid was the same.According to these reports, we asume the in-situ reduction of our catalysts during reactions, and so the electron transfer from titania to Ni(0) is favored [30].Another possible explanation for the observed better catalytic performance of pre-reduced solids as compared to untreated systems is the presence in the latter solids of surface chlorides (a well-known poison for metals arising from the precursor and evidenced by XPS analyses).As mentioned above, those chloride species were not observed in pre-reduced systems as they were eliminated as HCl during hydrogen pretreatment.The highest hydrogen production values (2606 H 2 micromole•g −1 ) corresponded to Ni-0.5-DP-Red for t = 6 h.This value is similar to that achieved in previous studies on 0.2% Pt [29], which is quite promising considering that Pt is ca.2000 times more expensive than Ni.
Some authors, such as Bahruji et al. [30], have described the influence of the metal oxidation state on the photocatalytic process.As can be seen in Figure 9B, the electron transfer from titania to NiO is thermodinamically impeded.On the contrary, the pre-reduction of the solid (Figure 9A) results in electron transfer from titania to Ni(0) being favored, with the metal thus acting as an electron trap and preventing electron-hole recombination. .Energy levels of (A) TiO2/metal and (B) TiO2/NiO, adapted from Bahruji et al [30].
In order to cast further light on the effect of Ni oxidation states and the presence of chloride species on catalytic performance, some reutilisation studies were carried out on the Ni-0.5-DPcatalyst both under UV and solar irradiation.Therefore, after 6 h irradiation, the solid was recovered by filtration, washed with methanol and acetone and dried at 110 °C.The catalyst was labelled as Ni-0.5-DP 1 using UV and Ni-0.5-DP 1 using solar, depending on the irradiation source.The solids were tested in another reaction, and the catalytic results are shown in Figure 10.As can be seen, hydrogen production dropped from 503 to 212 micromole per gram of catalyst after 6 h of UV irradiation, whereas no significant deactivation was observed under visible light.In any case, catalytic results were far below those achieved with fresh, pre-reduced catalysts.
TEM micrographs (Figure 5) did not evidence any significant increase in Ni particle size with the first use.After the second use, the metal particle size only slightly increased for solar irradiation studies.
XPS experiments (Table 3) showed that surface chlorides had already been eliminated after the first use, and it is assumed that there had been an in-situ reduction of nickel species.Thus, neither the presence of chlorides nor the in-situ reduction of NiO can account for the possitive effect of pre-reduction treatment at 400 °C on catalytic performance.It is possible that such a pre-treatment induced a strong metal-support interaction (SMSI) [32,33] which somehow favored the subsequent catalytic performance.This SMSI would be favored on homogeneously-distributed particles achieved by the deposition-precipitation method, which could explain the above-mentioned better catalytic performance of Ni-0.5-DP-Red as compared to Ni-0.5-IMP-Red.Nevertheless, these hypothetical Ni-support interactions were not detected by XPS measurements and therefore require further studies.Furthermore, Caravaca et al. [31], studying hydrogen photo-production from sugars on Ni-based catalysts, observed an induction period (in their case, 60 min) required for in-situ reduction of NiO to Ni.After that period of time, the hydrogen production rate of both the untreated and pre-reduced solid was the same.According to these reports, we asume the in-situ reduction of our catalysts during reactions, and so the electron transfer from titania to Ni(0) is favored [30].
Another possible explanation for the observed better catalytic performance of pre-reduced solids as compared to untreated systems is the presence in the latter solids of surface chlorides (a well-known poison for metals arising from the precursor and evidenced by XPS analyses).As mentioned above, those chloride species were not observed in pre-reduced systems as they were eliminated as HCl during hydrogen pretreatment.
In order to cast further light on the effect of Ni oxidation states and the presence of chloride species on catalytic performance, some reutilisation studies were carried out on the Ni-0.5-DPcatalyst both under UV and solar irradiation.Therefore, after 6 h irradiation, the solid was recovered by filtration, washed with methanol and acetone and dried at 110 • C. The catalyst was labelled as Ni-0.5-DP 1 using UV and Ni-0.5-DP 1 using solar, depending on the irradiation source.The solids were tested in another reaction, and the catalytic results are shown in Figure 10.As can be seen, hydrogen production dropped from 503 to 212 micromole per gram of catalyst after 6 h of UV irradiation, whereas no significant deactivation was observed under visible light.In any case, catalytic results were far below those achieved with fresh, pre-reduced catalysts.method as compared to the IMP method.This would be consistent with the observed higher activities of Ni-0.5-DPRed as compared to Ni-0.5-IMP Red.In summary, the addition of a small percentage (0.5% by weight) of a transition metal such as Ni (ca.2000 times cheaper than Pt) resulted in a 15.5-fold increase in the catalytic activity of Evonik P25, producing 2.6 mmol H 2 •g −1 after 6 h of UV irradiation.Thus, Ni proved to be a promising metal for use in photo-reforming processes of biomass-derived oxygenated compounds.

Figure 1 .
Figure 1.Activation of titania using a metal as a co-catalyst.

Figure 2 .
Figure 2. Picture of the photocatalytic reactor used in the hydrogen production from glycerol photo-reforming.

Figure 2 .
Figure 2.Picture of the photocatalytic reactor used in the hydrogen production from glycerol photo-reforming.

Figure 3 .Table 2 .
Figure 3. UV-vis spectra (left) and temperature-programmed reduction profiles (right) obtained for the catalysts prepared in this work.

Figure 3 .
Figure 3. UV-vis spectra (left) and temperature-programmed reduction profiles (right) obtained for the catalysts prepared in this work.

Figure 6 .
Figure 6.TEM micrographs of Ni-0.5-DP solid after the second reutilization using UV (A) or solar (B) irradiation.

Figure 7 .
Figure 7. H 2 production from glycerol photo-reforming on fresh, unreduced solids using UV (A) and solar (B) irradiation.

5 -Figure 8 .
Figure 8. H2 production via glycerol photo-reforming on untreated and pre-reduced solids using UV (A) and solar (B) irradiation.

Figure 8 .
Figure 8. H 2 production via glycerol photo-reforming on untreated and pre-reduced solids using UV (A) and solar (B) irradiation.

Table 2 .
Band-gap energy values of the solids as determined by UV-Vis spectroscopy.

Table 3 .
Ni (2p3/2), Ti (2p3/2) and Cl (2p) binding energies (eV) as determined by XPS.Petriket al., working with nanosized nickel oxides, found that binding energies at 855.3 and 856.7 eV were typical for Ni/TiO 2 systems, with the signal at around 856 eV being preferably associated with Ni 2 O 3