Materials

Sodium borohydride powder (> 98%) was purchased from Acros Organics (Geel, Belgium); cobalt(II) chloride hexahydrate (> 97%) and sodium hydroxide pellets (> 98%) were supplied by Sigma-Aldrich (Taufkirchen, Germany). Halloysite clay powder (>97%), 30–70 nm × 1–3 μm, with 1.26–1.34 mL/g pore volume was obtained from Sigma-Aldrich (Taufkirchen, Germany).

Catalyst Synthesis

Halloysite was used as the supporting material for the synthesis of Co-B catalysts using the impregnation and reduction method. An appropriate (according to Co loading ratio) amount of CoCl₂ solution was prepared with a stoichiometric ratio using distilled water. The Co content in the supported catalysts was adjusted to 5, 10, and 15 wt.%. After impregnation of Co onto halloysite at 75°C for 60 min at 700 rpm, NaBH₄ solution was added dropwise to reduce to Co²⁺ any Co that was oxidized during the preparation. Excess borohydride was used in order to provide complete reduction with a molar ratio of NaBH₄:CoCl₂ of 3:1 and the reduced solution was stirred at room temperature for 60 min at 400 rpm. The sediment was centrifuged (Nuve NF 200, Ankara, Turkey) at 2000 rpm (447 × g) for 5 min. Then the sample was collected and washed with an ethanol-water mixture (volume ratio 1:1) in order to remove insoluble, non-clay inorganic material from the catalyst. The sample was placed in the oven at 105°C for 24 h. The powder obtained was black and kept in a dark bottle for use in hydrolysis reactions.

Catalyst Characterization

The morphological structure, crystallinity, and surface composition of the catalysts were characterized by various methods. N₂ sorption isotherms were measured at 77 K using a Tristar 3020 instrument (Micromeritics, Norcross, Georgia, USA). All samples were degassed first at 90°C for 1 h and then at 300°C for 24 h under vacuum before measurement. The specific surface areas of the samples were calculated using the Brunauer-Emmett-Teller (BET) method.

X-ray diffraction (XRD) patterns were obtained using an XRD D8 Advance (Bruker AXS, Karlsruhe, Germany) powder diffractometer. The samples were scanned over the range 20–80°2θ at a scanning rate of 0.5°2θ min⁻¹.

The morphology and surface compositions of the catalysts and halloysite were analyzed using a Regulus 8230 Scanning Electron Microscope (FE-SEM) (Hitachi, Tokyo, Japan) with energy dispersive spectroscopy analysis (EDX).

The Co-based catalysts were dissolved using a microwave-assisted (Milestone, Sorisole, Bergamo, Italy) acid digestion method and analyzed using an inductively coupled plasma mass spectrometer (ICP-MS) (Thermo Scientific iCAP RQ, Waltham, Massachusetts, USA) to determine Co and B.

The surface electronic state was analyzed by X-ray photoelectron spectroscopy (XPS) using a Versaprobe II (PHI5000, ULVAC-PHI, Osaka, Japan) with AlKα (1486.6 eV) as the X-ray source.

The Catalytic Performance of Halloysite-based Catalyst in the Hydrolysis of NaBH ₄

Hydrogen-production rates from the hydrolysis of NaBH₄ were evaluated to determine the catalytic activity of halloysite-supported catalysts. Initially, an appropriate amount of catalyst (10–50 mg) and NaBH₄ (0.1–0.5 M) was placed in a 150 mL water-jacketed reactor which maintained the temperature by controlling the circulating water temperature.

The reactor content was mixed using a magnetic stirrer at 400 rpm. During the experiment, the volume of hydrogen generated was recorded using the water-displacement method. Hydrogen-generation rates (HGR, mL min⁻¹ g⁻¹ catalyst) were calculated from the hydrogen volume as a function of time and the amount of catalyst used.

To determine the optimal reaction conditions of the hydrolysis reaction via NaBH₄ using halloysite-supported CoB catalysts, the effects of the amount of catalyst (10–50 mg), NaBH₄ initial concentration (0.1–0.50 M), Co loading by weight (5–15%), and temperature (30–50ºC) were studied with a set of values determined by the Design Expert 7.0 software. The experiments were performed at least twice and the results were given as mean values.

Response Surface Methodology

Response Surface Methodology is defined as: “a set of statistical techniques used to design experiments, build models, evaluate the effects of variables, and determine the optimum conditions of variables to predict a targeted response” (Myers et al. Reference Myers, Montgomery and Anderson-Cook2016). The Box-Behnken Design (BBD) and Central Composite Design (CCD) are the main techniques of RSM and offer very efficient and cost effective solutions for optimizing complex processes (Jitrwung & Yargeau Reference Jitrwung and Yargeau2011; Aytar et al. Reference Aytar, Gedikli, Buruk, Cabuk and Burnak2014; Hitit et al. Reference Hitit, Lazaro and Hallenbeck2017; Mishra et al. Reference Mishra, Ameen, Zaid, Singh, Ab Wahid, Islam and Al Nadhari2019; Yin & Wang Reference Yin and Wang2019). By enabling consideration of multiple variables and their interactions, they are superior to single-parameter testing approaches. Compared with CCD, the BBD technique does not include extreme-factor value combinations and so, BBD precludes potentially unsatisfactory experimental results (Box & Behnken Reference Box and Behnken1960). In this study, BBD, as an important part of RSM, was utilized to optimize the parameters for hydrogen production.

Characterization of Halloysite-based Co Catalysts

In order to understand the catalytic activity of synthesized catalysts in the hydrolysis of alkaline NaBH₄, the textural properties of supports and catalysts were characterized by N₂ sorption measurements. According to IUPAC classification, the adsorption-desorption isotherm characteristics (Fig. 1) conformed to the type IV isotherm (Ayodele et al. Reference Ayodele, Ghazali, Yassin and Abdullah2019). This indicated that the adsorption of the liquid N₂ on the mesoporous Co-B/Hly proceeded via multilayers followed by capillary condensation. An H1-type hysteresis cycle was observed in the range of 0.5–0.95 relative pressure. Pore distribution of catalysts showed that the main pore sizes existed at maximum 14.49, 14.50, 14.50, and 14.64 nm for halloysite, 5Co-B/Hly, 10Co-B/Hly, and 15Co-B/Hly, respectively. This indicated a mesoporous structure for the samples because the main pore sizes were between 2 and 20 nm. The pore characteristics of the halloysite and synthesized catalysts were very similar.

Fig. 1

N₂ adsorption/desorption isotherms and pore distribution of the samples: a Halloysite, b 5Co-B/Hly, c 10Co-B/Hly, and d 15Co-B/Hly

The textural properties of halloysite and synthesized catalysts were characterized by N₂ sorption measurements. The BET specific surface areas of the catalysts were ~87, 77, and 72 m²/g for 5Co-B/Hly, 10Co-B/Hly, and 15Co-B/Hly, respectively. As expected, the reason the catalyst surface areas are smaller than the surface area of halloysite, 90 mg²/g, is related to the dispersion of CoB onto/into the support and the increased loading ratio (Table 1). The specific BET surface areas of Co-B/Hly catalysts in this study were greater than those obtained for unsupported Co-B (17 m²/g) (Yang et al. Reference Yang, Chen and Chen2011). The Barrett-Joyner-Halenda adsorption method (BJH) is utilized to define pore area and specific pore volumes through adsorption and desorption techniques (Barrett et al. Reference Elliott, Barrett, Joyner and Halenda1951); the cumulative pore volume of halloysite was 0.205 cm³/g. The cumulative pore volumes of catalysts for 5Co-B/Hly, 10Co-B/Hly, and 15Co-B/Hly were 0.191, 0.203, and 0.206 cm³/g, respectively, and the metal loading did not affect significantly the pore volume of the support. The average pore diameter values for halloysite, 5Co-B/Hly, 10Co-B/Hly, and 15Co-B/Hly were 10.95, 11.338, 13.195, and 15.121 nm, respectively. The change in pore diameter with increasing Co load may also be explained by collapse of the support material wall (Hosgun et al. Reference Hosgun, Ture, Hosgun and Bozan2020).

Table 1

Texture properties of the halloysite and synthesized catalysts

The SEM images (Fig. 2) of the halloysite showed the multilayer plate and empty spherical layers. With Co loading, the empty spaces were covered with a slight agglomeration. Condensed structures were found with increasing loading ratio of Co. To determine the chemical composition of the surface of synthesized catalysts, EDS analysis was conducted. From EDS spectra, analysis in three randomly selected regions showed that Co loadings were 7.39, 11.11, and 14.96 wt.% for the 5Co-B/Hly, 10Co-B/Hly, and 15Co-B/Hly catalysts, respectively.

Fig. 2

SEM images and EDX micrographs of: a halloysite, b 5Co-B/Hly, c 10Co-B/Hly, and d 15Co-B/Hly

The XRD pattern of halloysite (Fig. 3) showed typical peaks at 11.7, 20.0, 34.9, and 62.3º2θ. The XRD patterns of Co-B/Hly catalysts demonstrated halloysite peaks with intensities varying according to the different loading ratio of catalyst and slight CoOx peaks (33.0, 37.9, and 42.3º2θ) (Fig. 3) (Vinokurov et al. Reference Vinokurov, Sitavitskaya, Gulatov, Ostudin, Sosna, Gushchin, Darrat and Lvov2018). The absence of peaks at 44.1°2θ and 51.3º2θ confirmed the precipitation of amorphous Co₂B (Wang et al. Reference Wang, Li, Bai, Qi, Cao, Zhang, Wu and Wang2016).

Fig. 3

XRD of CoB halloysite catalysts: 5Co-B/Hly, 10Co-B/Hly, and 15Co-B/Hly

The ICP-MS analysis was performed to determine the chemical composition of catalysts and the existence of Co and B in the catalysts. The catalyst samples were analyzed after dissolution in nitric acid and pretreatment with microwaves. Cobalt loadings were obtained as 4.8, 9.4, and 14.2 wt.% for the 5Co-B/Hly, 10Co-B/Hly, and 15Co-B/Hly catalysts, respectively (Table 2). The weight percent of B was less than that required to meet stoichiometric needs. Boron loadings were obtained as 1.8, 1.2, and 0.9 wt.% for the 5Co-B/Hly, 10Co-B/Hly, and 15Co-B/Hly catalysts, respectively. A smaller weight percent of B than the stoichiometrically required amount was also found by Xu et al. (Reference Xu, Wang, Guo and Ji2011), which suggested that the Co metal is adsorbed simultaneously and more easily than B during preparation of the catalyst. The reduction of Co precursors by NaBH₄ is a complex process and the product composition depends on the Co:NaBH₄ ratio, mixing rate, presence/absence of oxygen, etc. Rapid reaction of the precursors led to the exclusive formation of Co₂B; slower reaction led to side products being formed (Krishnan et al. Reference Krishnan, Advani and Prasad2008).

Table 2

Composition of Co-B/Hly catalysts

The oxidation states of elements and the surface interaction between atoms in catalysts were analyzed using XPS analysis. The Co_2p electron energy levels (Fig. 4a) demonstrated that the Co species in the catalyst samples were present in both elemental and oxidized states, corresponding to binding energies (BE) of ~777.9 eV (Co_2p3/2) and 794 eV (Co_2p1/2), respectively (Manna et al. Reference Manna, Ror, Vasthistha and Sharma2014; Wang et al. Reference Wang, Li, Zhang, Zhang and Xie2017). The characteristic peak of Co_2p3/2 for elemental Co of the synthesized catalysts was 777.9 eV. A negative shift of 0.3 eV was observed when the BE of metal Co was compared to the BE of pure Co (778.2 eV). The binding energies of Co for 5Co-B/Hly (793.8 eV), 10Co-B/Hly (794.1 eV), and 15Co-B/Hly (794.3 eV) corresponded to the Co_2p1/2 peaks of Co²⁺ (Wang et al. Reference Wang, Li, Bai, Qi, Cao, Zhang, Wu and Wang2016).

Fig. 4

XPS spectra of: a Co_2p and b B_1s level for the Co-B/Hly catalysts

For B_1s XPS peaks (Fig. 4b) at 188.6 eV and 192.5 eV corresponded to the elemental and oxidized B_1s levels, respectively. The elemental boron in all the catalyst samples showed a positive shift of 1.5 eV when compared with the BE of pure boron (187.1 eV) (Watts & Wolstenholme Reference Watts and Wolstenholme2003; Fernandes et al. Reference Fernandes, Patel, Miotello and Filippi2009). This shift indicated an electron transfer from elemental B to a vacant d-orbital of metallic Co. This created a lack of electrons in elemental boron, while Co metal became enriched with electrons. The presence of high electron density at the catalytically active sites is important for catalytic activity (Fernandes et al. Reference Fernandes, Patel, Miotello and Filippi2009; Wu et al. Reference Wu, Bai, Liu, Wu, Pang and Yi2011; Guo et al. Reference Guo, Hou, Li and Liu2018).

According to the results above and similar studies (Fernandes et al. Reference Fernandes, Patel, Miotello and Filippi2009; Li et al. Reference Li, Wang, Zhang and Xie2017), a possible mechanism of the production of H₂ from Co-catalyzed hydrolysis of NaBH₄ is proposed that works by following three kinetics steps. In the first step, BH₄ ⁻ ions are chemisorbed on the Co atoms; then the hydride ion, H⁻, is transferred from BH₄ ⁻ ions to adjacent, empty Co atoms. In the last step, this hydrogen atom receives a negative charge in the form of an electron from the Co and leaves the site in hydridic form (H⁻) which reacts with the water molecule to produce H₂ and OH⁻ ions. The OH⁻ reacts with B in BH₃ to produce BH₃(OH)⁻ ions. The cycle of hydrogen adsorption on the Co sites lasts until BH₃(OH)⁻ forms B(OH)₄ ⁻. Molecular hydrogen is formed during the full cycle. On the basis of the possible mechanism mentioned, the electron-enriched active Co sites were able to facilitate the catalytic hydrolysis reaction by providing the negative charge electron needed by the hydrogen atom in the last step. As discussed under XPS results, these electrons are supplied by the elemental B to the active Co sites, resulting in Co₂B with high catalytic activity.

Box Behnken Design

In the present study, BBD was applied to determine the effect of four independent variables. The statistical analysis was conducted using Design Expert 7.0 software. According to BBD, having conducted 27 experiments and collecting the responses, Y denotes the generation rate and A, B, C, and D represent NaBH₄ concentration, catalyst amount, temperature, and metal loading, respectively (Table 3). The factor levels for the hydrogen-generation rate are 0.1, 0.3, and 0.5 M for NaBH₄ concentration; 10, 30, and 50 mg for the amount of catalyst; 30, 40, and 50°C for temperature; 5, 10, and 15 wt.% for metal loading.

Table 3

BBD with response of independent variables

To determine the effect of synthesized, supported, cobalt-based catalysts on hydrogen generation by NaBH₄ hydrolysis, pristine halloysite was tested without any metal loading or modification. The reaction was performed using 50 mg of pristine halloysite, 0.70 M NaBH₄, 0.50 g of NaOH at 50°C reaction temperature, and at a 400 rpm stirring rate for the medium, in accord with a previous study (Erol & Özdemir Reference Erol and Özdemir2017). To compare the halloysite activity, a control experiment was performed under the same reaction conditions without a catalyst. Self-hydrolysis of NaBH₄ and hydrolysis using pristine halloysite produced the same amount of H₂ with very close reaction rates. Less than 20 mL of hydrogen generation was seen after 24 h for both studies and conversion of the reaction was not completed. The catalytic activity of pristine halloysite reached a higher reaction rate with any surface modification or any reaction medium optimization.

The most appropriate mathematical models were determined by considering statistical parameters determined by ANOVA and the regression coefficient of the quadratic model was the most appropriate with the Response Surface Reduced Quadratic Model (Table 4).

Table 4

ANOVA for Response Surface Reduced Quadratic Model

R-squared: 0.8324; Adj R-squared: 0.7706

The relationship between variables and responses was determined by the second-order polynomial model. The ANOVA table indicates that the main effects of NaBH₄ concentration, catalyst amount, temperature, and metal loading and the second-order effects of catalyst amount×temperature, catalyst amount×metal loading, and metal loading² are significant model terms. The reduced quadratic model is presented in Eq. 2:

(2) $\begin{array}{cc}\mathrm{Log}10\left(Y\right)=3.96& +0.25\ast A-0.18\ast B+0.12\ast C\\ & -0.11\ast D+0.25\ast B\ast C\\ & -0.16\ast B\ast D+0.26D^2\end{array}$

Using Design Expert 7.0 software, log transformation was found to provide the best fit. The large F value (13.48) and the very low probability (p < 0.0001) in ANOVA indicate that the model fits the experimental results adequately (Table 4). The normal probability plot of studentized residuals (Fig. 5) is close to a straight line, which validates the significance of the model (Mishra et al. Reference Mishra, Ameen, Zaid, Singh, Ab Wahid, Islam and Al Nadhari2019).

Fig. 5

Normal probability versus internally studentized residuals for the hydrogen generation rate

The three-dimensional surface plots represent graphically the regression equations. These plots present the main and interaction effects of two factors, while the other two factors are maintained at fixed levels (Sarac et al. Reference Sarac, Uğur, Simsek, Aytar, Toptas, Buruk, Cabuk and Burnak2017).

The effects of metal loading and amount of catalyst (Fig. 6a) were that the hydrogen-generation rate increased with a decrease in the amount of catalyst from 50 to 10 mg, at a NaBH₄ concentration of 0.3 M and temperature of 40°C. The rate of hydrogen generation was calculated using the generated hydrogen volume per reaction total time and catalyst amount. In order to obtain a large hydrogen-generation rate by the hydrolysis reaction, the appropriate amount of catalyst should be used according to the cobalt content of the catalyst. The increase in the amount of catalyst led to an increase in the viscosity of the reaction medium, thereby causing mass transfer limitations. Hydrogen production increased at low metal loading and high NaBH₄ concentration (Fig. 6b). With a concentration of 0.3 M NaBH₄ and 30 mg of catalyst, when temperature varied from 30 to 50°C and metal loading decreased from 15 to 5 wt.%, the maximum hydrogen-generation rate was obtained (Fig. 6c). The hydrogen-generation rate increased with increasing NaBH₄ concentration, but the rate decreased with an increasing amount of catalyst due to mass-transfer limitations (Fig. 6d). The effect of NaBH₄ concentration on the hydrogen generation rate was seen more effectively with small amounts of catalyst. Similar studies in the literature show that the hydrogen-generation rate increases to an optimum value, and then decreases (Tian et al. Reference Tian, Guo and Xu2010; Li et al. Reference Li, Wang, Zhang and Xie2017). The reason is that the mass transfer restrictions observed are due to the increase in NaBO₂ in the solution phase and also to increased viscosity. The maximum temperature and NaBH₄ concentration reveal a maximum hydrogen-generation rate (Fig. 6e). As expected, the reaction rate was faster at high temperatures and showed a linear relationship with reaction time (Sahin et al. Reference Sahin, Kιlιnc and Saka2016). Due to strong binary interactions between catalyst amount and temperature, high temperature increased the hydrogen generation rate with the optimum amount of catalyst (Fig. 6f).

Fig. 6

Response surface curves for hydrogen-generation rate

Determination of Optimal Conditions

The optimal levels of variables and maximum hydrogen production were estimated by desirability function (Ayodele et al. Reference Ayodele, Ghazali, Yassin and Abdullah2019; Derringer & Suich Reference Derringer and Suich1980; Wang & Wan Reference Wang and Wan2009). By setting the constraints at predetermined levels, Design Expert 7.0 software was used to generate a set of solutions ranked according to the desirability values that aimed to maximize hydrogen-generation rate (Table 5).

Table 5

Optimum conditions based on desirability

Ten solutions were obtained with a desirability range from 0.83 to 1.00. Among the solutions, the optimum conditions of 0.44 M, 10.66 mg, 39.96°C, and 5.01 wt.% were selected for NaBH₄ concentration, catalyst amount, temperature, and metal loading, respectively. At these levels, the predicted hydrogen production was 33,185.2 mL min⁻¹ g_Co ⁻¹. To validate the accuracy of the model, an additional, confirmatory experiment was carried out. The objective was to decide whether the conclusions obtained from the analyses were valid. “A useful confirmation is to determine whether the new observation falls within the predicted response interval at that point” according to Montgomery (Reference Montgomery2017). Three additional experimental runs were employed with the proposed optimal conditions. Repetitive performance tests resulted in hydrogen generation rates of 33,945, 33,873, and 33,744 mL min⁻¹ g_Co ⁻¹ which were consistent with the RSM optimization. The fact that the results fell into the prediction interval confirmed the validity and adequacy of the predicted models.

A Box Behnken Design was used by Ayodele et al. (Reference Ayodele, Ghazali, Yassin and Abdullah2019) to optimize hydrogen production with photocatalytic steam methane reforming in order to investigate the combined effects of irridation time, metal loading, methane concentration, and steam concentration; under optimum conditions, a generation rate of 2.35 µmol H₂/min was obtained with 3 wt.% La/TiO₂. The effects of reaction conditions on sodium borohydride-to-hydrogen generation using the Box-Wilson optimization technique was studied by Ozkan et al. (Reference Ozkan, Akkus and Ozkan2019). Optimization of the catalyst loading for the direct borohydride fuel cell (DBFC) was studied by San et al. (Reference San, Karadag, Okur and Okumus2016) with the power density of the fuel cell chosen as a response (dependent) parameter. Catalyst loading is an important factor for DBFC performance. Increasing the catalyst loading was expected to increase fuel cell performance, but increasing the amount of catalyst more than was required affected the power density of the fuel cell adversely. This was because the active centers of the catalyst particles became clogged with increasing viscosity. CoB/SiO₂ was used by Yang et al. (Reference Yang, Chen and Chen2011) to catalyze the hydrolysis reaction of NaBH₄. Those authors found that a SiO₂-supported CoB catalyst showed activity which was four times greater than unsupported CoB catalysts with a rate of 10,586 mL min⁻¹ g⁻¹ at 298 K. A hydrogen generation rate of 2400 mL min⁻¹ g⁻¹ was recorded by Jeong et al. (Reference Jeong, Cho, Nam, Oh, Jung and Kim2007) using a CoB catalyst calcined at 250ºC.

Optimization of a hydrolysis reaction for hydrogen generation using Co-based metal oxide nanocrystals was studied by Kim et al. (Reference Kim, Lee, Li and Fortner2020), who reported a maximum hydrogen-production rate of 10,367 mL min⁻¹ g⁻¹ at 293 K via NaBH₄ hydrolysis with wüsite cobalt oxide nanorods (wz-CoO-NRs). In a study by Zhang et al. (Reference Zhang, Feng, Cheng, Hou, Li and Han2019), a maximum rate of 5955 mL min⁻¹ g⁻¹ hydrogen at 298 K was achieved by NaBH₄ hydrolysis using a non-noble Co-based nanoporous graphene oxide catalyst. A 8333 mL min⁻¹ g⁻¹ rate of H₂ generation at 303 K using CoO nanorods was found by Lu et al. (Reference Lu, Chen, Jin, Yue and Peng2012). A maximum H₂ generation rate (303 K) of 6130 mL min⁻¹ g⁻¹ was reported by Zhang et al. (Reference Zhang, Ling and Du2015) for porous CoO nanorods (length of >500 nm). A maximum hydrogen generation rate of 2218 mL min⁻¹ g⁻¹ with methanolysis of sodium borohydride using various halloysite-supported functionalized amine groups was achieved by Sahiner and Sengel (Reference Sahiner and Sengel2017b). An 18,700 mL min⁻¹ g_Co ⁻¹ hydrogen-production rate with 16 wt.% of a Co-loaded halloysite catalyst was obtained by Vinokurov et al. (Reference Vinokurov, Sitavitskaya, Gulatov, Ostudin, Sosna, Gushchin, Darrat and Lvov2018) using several preparation techniques which included wet impregnation and surface modification of halloysite with ligand assistance. In the present study, however, using a chemical reduction method in addition to wet impregnation to allow better distribution of metal, higher catalytic activity enabled the authors to obtain a hydrogen-generation rate of 33,854 mL min⁻¹ g_Co ⁻¹ using 5.01 wt.% Co metal loading.