Next Article in Journal
Size-Dependent Structural, Magnetic and Magnetothermal Properties of Y3Fe5O12 Fine Particles Obtained by SCS
Next Article in Special Issue
Recent Advances of Transition Metal Chalcogenides as Cathode Materials for Aqueous Zinc-Ion Batteries
Previous Article in Journal
Graphene-Delivered Insecticides against Cotton Bollworm
Previous Article in Special Issue
Bimetallic Pt-Ni Nanoparticles Confined in Porous Titanium Oxide Cage for Hydrogen Generation from NaBH4 Hydrolysis
 
 
Search for Articles:
Title / Keyword
Author / Affiliation / Email
Journal
Article Type
 
 
Advanced Search
 
Section
Special Issue
Volume
Issue
Number
Page
 
Journals
Nanomaterials
Volume 12
Issue 16
10.3390/nano12162732
nanomaterials-logo
Submit to this Journal Review for this Journal Propose a Special Issue
► Article Menu

Article Menu

share Share announcement Help format_quote Cite question_answer Discuss in SciProfiles
first_page
settings
Order Article Reprints
Font Type:
Arial Georgia Verdana
Font Size:
Aa Aa Aa
Line Spacing:
Column Width:
Background:
Article

Graphene-Modified Co-B-P Catalysts for Hydrogen Generation from Sodium Borohydride Hydrolysis

by
Xinlei Jia
1,†,
Zhen Sang
1,†,
Lixian Sun
1,2,*,
Fen Xu
1,*,
Hongge Pan
3,*,
Chenchen Zhang
1,
Riguang Cheng
1,
Yuqian Yu
1,
Haopan Hu
1,
Li Kang
1 and
Yiting Bu
1
1
School of Material Science & Engineering, Guangxi Key Laboratory of Information Materials, Guangxi Collaborative Innovation Center of Structure and Property for New Energy and Materials, Guilin University of Electronic Technology, Guilin 541004, China
2
School of Mechanical & Electrical Engineering, Guilin University of Electronic Technology, Guilin 541004, China
3
School of New Energy Science and Technology, Xi’an Technological University, Xi’an 710021, China
*
Authors to whom correspondence should be addressed.
†
These authors contributed equally to this work.
Nanomaterials 2022, 12(16), 2732; https://doi.org/10.3390/nano12162732
Submission received: 4 July 2022 / Revised: 2 August 2022 / Accepted: 6 August 2022 / Published: 9 August 2022
(This article belongs to the Special Issue Nanostructured Electrodes for High-Performance Supercapacitors and Batteries)
Browse Figures
Versions Notes

Abstract

:
Sodium borohydride (NaBH4) is considered a good candidate for hydrogen generation from hydrolysis because of its high hydrogen storage capacity (10.8 wt%) and environmentally friendly hydrolysis products. However, due to its sluggish hydrogen generation (HG) rate in the water, it usually needs an efficient catalyst to enhance the HG rate. In this work, graphene oxide (GO)-modified Co-B-P catalysts were obtained using a chemical in situ reduction method. The structure and composition of the as-prepared catalysts were characterized, and the catalytic performance for NaBH4 hydrolysis was measured as well. The results show that the as-prepared catalyst with a GO content of 75 mg (Co-B-P/75rGO) exhibited an optimal catalytic efficiency with an HG rate of 12087.8 mL min−1 g−1 at 25 °C, far better than majority of the findings that have been reported. The catalyst had a good stability with 88.9% of the initial catalytic efficiency following 10 cycles. In addition, Co-, B-, and P-modified graphene showed a synergistic effect improving the kinetics and thermodynamics of NaBH4 hydrolysis with a lower activation energy of 28.64 kJ mol−1. These results reveal that the GO-modified Co-B-P catalyst has good potential for borohydride hydrolysis applications.

1. Introduction

Since the first industrial revolution, the overconsumption of fossil energy has created issues of air pollution and energy storage [1]. Therefore, the development of new renewable green and efficient energy has become an urgent matter for the future development of society and the economy. Hydrogen is expected to be a fossil energy alternative, which relies on its outstanding features of the nonemission of pollutants and high efficiency [2]. In general, there are several ways, such as photocatalysis, biomass decomposition, chemical hydrides hydrolysis, to produce hydrogen [3,4]. In the method described above, hydrogen-rich compound hydrolysis, such as NaBH4 [5] and ammonia borane (NH3BH3) [6], has been considered as a convenient, economical, and efficient way to produce hydrogen.
NaBH4 is rich in hydrogen (10.8 wt%), environmentally friendly, safe, and non-flammable, which can be employed for producing hydrogen through hydrolysis reactions [7]. The hydrolysis reaction occurs through the following reactions:
NaBH4 + 2H2O → NaBO2 + 4H2 + heat (217 kJ mol−1)
During this process, four moles of H2 can be produced by one mole of NaBH4. In particular, NaBH4 and water each provide 50% of the hydrogen. [8]. In addition, the byproduct NaBO2 can be collected to reproduce NaBH4, which shows a sustainable development value. However, the NaBH4 hydrolysis reaction exhibits sluggish kinetics in the solutions. Previous reports have proved that selecting an appropriate catalyst can significantly improve the HG rate. Noble metal-based catalysts (Pt [9,10], Ru [11,12], and Pd [13,14]) have shown positive catalytic performance. However, their scarce storage and high price limit the related practical applications. Transition metal catalysts (Co [15,16], Ni [17], and Co-Ni [18]) with inferior cost and relatively good catalytic activity have been broadly investigated for hydrogen production from NaBH4. In addition, transition metals combined with heteroatoms, such as boron (B) and phosphorus (P), could further enhance the catalytic activity [19,20]. For example, Patel et al. reported that the transition-metal borides (e.g., CoB, NiB) exhibited superior catalytic activities due to the mutual electronic interaction between boron and transition metals (Co or Ni), thus preventing them from oxidation and protecting the active metal center. [21]. Chen et al. prepared cobalt–phosphorus (Co-P) catalysts and investigated their catalytic efficiency in alkaline sodium borohydride solutions. The Co-P catalyst showed favorable hydrolysis performance with a low activation energy, which was attributed to the improvement of the catalytic performance by the appropriate amount of P doping [22]. So far, catalysts including Co-P [22], Ni-B [23], Co-W-B [24], Co-Ni-B [25], Co-B-P [26], etc., have been extensively researched and have shown good catalytic performance. Although these catalysts possess preferable catalytic activity, they usually show a low cycle stability. To address the above issue, selecting a suitable matrix, such as MOFs [27], porous carbon [28], MWCNTs [29], SiO2 [30], and γ-Al2O3 [31], which possesses a high specific surface area to support the active metals, can effectively improve the catalytic performance. Recently, graphene with excellent physical and chemical characteristics has been researched, making it an ideal carrier material to support metal clusters [32,33]. The large specific surface area can not only improve the distribution of metal clusters, thereby exposing more catalytically active sites for catalysis reaction, but it can also suppress the aggregation issue during the catalytic process, thus presenting a superior catalytic performance.
In this study, we successfully prepared the graphene modified Co-B-P catalysts through chemical in situ reduction. The structural characteristics and catalytic efficiency of the Co-B-P/xrGO (x = 25, 50, 75, 100) catalysts were studied. The Co-B-P/75rGO catalyst exhibited an optimal catalytic performance with an average HG rate of 12,087.8 mL min−1 g−1. In addition, the effects of the GO content and heteroatom types on the catalytic activity of NaBH4 hydrolysis were also studied. The excellent hydrogen generation performance is attributed to the fact that the large specific surface area of graphene oxide can better disperse Co-B-P clusters and thus expose more active sites. Meanwhile the elemental B and P doping exhibits a synergistic catalytic effect. This is because the presence of GO increases the specific surface area for uniform dispersion of Co-B-P clusters on the surface of the GO, thus exposing more catalytically active sites for the hydrolysis reaction.

2. Materials and Methods

2.1. Materials

High purity flake graphite (300 mesh), sulfuric acid, hydrochloric acid, hydrogen peroxide, sodium nitrate, potassium permanganate, sodium borohydride, sodium hydroxide, cobalt chloride hexahydrate, and sodium hypophosphite monohydrate were obtained from Alfa Aesar Co., Ltd. (Tianjin, China). The chemicals used were analytical reagent. All experiments used ultrapure water.

2.2. Synthesis of GO

We prepared the GO materials using a modification of the Hummers method [34]. First, concentrated H2SO4 (60 mL), NaNO3 (2 g), and flake graphite (2 g) were mixed at 5 °C to obtain a solution. Subsequently, 12 g of KMnO4 was slowly added to the above solution, and the solution was heated to 35 °C for 7 h with magnetic stirring. Then, 200 mL ice water and 15 mL H2O2 were added in turn to the mixed solution, until the mixed solution changed from brown to bright yellow. Next, the mixed solution was repeatedly washed with hydrochloric acid and deionized water until the pH was 7 to obtain the GO solution. Finally, the GO was obtained after freeze-drying for 72 h.

2.3. Catalyst Preparation

The Co-B-P/75rGO was obtained through chemical in situ reduction synthesis. First, GO (75 mg), CoCl2·6H2O (5 mmol), and NaH2PO2·H2O (30 mmol) were dispersed into 20 mL ultrapure water with sonication for 30 min. Next, 20 mL solution containing an appropriate amount of NaBH4 (30 mmol) was slowly dropped into the reaction solution with intense agitation. After being aged in an ice water bath for 10 h, the Co-B-P/75rGO catalysts were obtained after washing with water, washing with ethanol, and drying. For comparison, a Co-B-P cluster without GO was prepared under the same conditions. In addition, we controlled the addition of GO to be 25, 50, and 100 mg, and the obtained corresponding composites were labeled as Co-B-P/xrGO (x = 25, 50, and 100), respectively. The comparison samples of CoB, CoP, and CoBP without GO were prepared under the same conditions.

2.4. Catalyst Characterization

The Co-B-P/xrGO catalyst structures were analyzed by X-ray diffraction (XRD). The chemical structures of the catalyst were characterized by Fourier transform infrared (FTIR) spectroscopy. The elemental valence states of the Co-B-P/xrGO catalysts were determined by X-ray photoelectron spectroscopy (XPS). The morphologies of the Co-B-P/xrGO catalysts were determined by scanning electron microscopy (SEM). The degree of graphitization of the Co-B-P/xrGO catalysts was analyzed by Raman microscope (Raman spectra). The specific surface areas of the Co-B-P/xrGO catalysts were calculated by the Brunauer–Emmett–Teller (BET) method. The bulk elemental composition of Co, B, and P in the as-prepared Co-B-P/xrGO catalysts was measured via inductive coupled plasma–optical emission spectroscopy (ICP-OES).

2.5. Hydrogen Generation Measurement

The catalytic efficiency of Co-B-P/xrGO in alkaline NaBH4 solution was evaluated by a laboratory fabricated self-assembled drainage device [35]. The amount of hydrogen produced was determined by the volume of water drained, and the hydrogen generation rate was calculated through tracking the volume of water expelled at regular periods. Firstly, 0.1 g of Co-B-P/xrGO was added to a dry 125 mL wide-mouth flask. Then, 10 mL of a solution (1.5 wt% NaBH4 and 5 wt% NaOH) was placed into a wide-mouth flask through a 10 mL capacity syringe, and an appropriate amount of sodium hydroxide solution inhibited the NaBH4 self-hydrolysis reaction. The hydrogen generation efficiency of the catalyst hydrolysis was tested at different temperatures, and the reaction activation energy (Ea) was evaluated by the exponential law of reaction rate. After the hydrolysis test, the catalyst was washed with water and vacuum dried for 10 h. Then, the catalyst was tested for durability by adding 10 mL of fresh NaBH4 solution as described above.

3. Results and Discussion

3.1. Catalyst Characterization

The Co-B-P/xrGO was prepared through the chemical in situ reduction method (Figure 1) [36]. In a typical procedure, GO material was prepared by a modified Hummers method and distributed in ultrapure water under ultrasonic conditions. Subsequently, Co2+ was anchored on the GO surface by the electrostatic adsorption. After adding the NaH2PO2·H2O and NaBH4 solution, GO was reduced to rGO, and Co-B-P clusters formed on the rGO surface [37].
The microscopic morphology and nanostructure of the catalysts were characterized through SEM. The prepared pure Co-B-P alloy catalyst was agglomerated in a granular morphology (Figure 2a), which was ascribed to the exothermic nature of the catalyst during the preparation process. Figure 2b shows that the GO was successfully synthesized by the modified Hummers method with a typical pleated-sheet morphology. To overcome the aggregation issue, GO with a typical pleated structure can act as a matrix material to disperse the Co-B-P clusters [38]. For exploring the effect of the GO addition on the catalytic performance, catalysts with different contents of GO were prepared. Figure 2c–f show the morphologies of Co-B-P/xrGO (x = 25, 50, 75, and 100), respectively. All the SEM images showed that the metal clusters were tightly anchored to the surface of the reduced graphene. Increasing the content of GO means the larger specific surface area can be used to provide a larger space for the dispersion of Co-B-P clusters. The Co-B-P clusters tended to grow uniformly on the surface of the reduced graphene. However, when the addition content was 100 mg, the redundant reduced graphene wrapped around leading to the aggregation issue of Co-B-P clusters. Among them, Co-B-P/75rGO exhibited an optimal morphology with Co-B-P clusters tightly and uniformly anchored on the surface of the reduced graphene. This structure can expose more active sites for the catalytic reaction, which was verified in subsequent hydrolysis catalysis measurements [29]. In addition, the EDX spectra (Figure 2g–l) showed that the Co, B, P, O, and C elements were uniformly dispersed in the Co-B-P/75rGO catalyst.
The XRD patterns and Raman spectra of Co-B-P/xrGO were measured as shown in Figure 3a. A broad diffraction peak near 2θ = 45° corresponded to the Co-B and Co-P phases, indicating that the as-prepared catalysts were a typical amorphous structure [39,40], and the addition of GO would not affect the amorphous structure of the catalyst. The peaks around 26.0° belonged to the (002) plane of reduced graphene, indicating that the GO was reduced. The short-range ordered and long-range disordered amorphous structures are generally considered to have an unsaturated surface coordination, which has been proved to be beneficial for catalytic hydrolysis [21]. The characteristic peaks of the D-band and G-band were observed near 1350 and 1580 cm−1, as shown in Figure 3b. The ratio of the strength of the D band to the G band represents the disorder of the carbon-based hybrid material [41]. Experimental results showed that with the addition of GO, the ID/IG values of all catalysts were greater than 1.00; in particular, Co-B-P/75rGO (ID/IG) reached 1.28. The ID/IG value indicated that Co-B-P/75rGO had more defects, which can anchor more metal and metal-like clusters to improve the catalytic performance. The following performance test experiments also confirmed this conclusion.
The chemical structures of GO and the Co-B-P/75rGO were characterized by FTIR (Figure 4). For the spectra of GO, the peak of the -OH stretching vibration of water molecules appeared at 3431 cm−1 [42]. The characteristic peaks at 1736, 1630, and 1089 cm−1 were observed for the -COOH stretching vibration, C=C bond skeleton vibration, and C-O-C vibration of GO, respectively [42]. The considerable numbers of oxygen-containing groups contained in the GO were produced during the oxidation of the graphite with a strong oxidizer, which can easily absorb metal ions. The FTIR spectrum of Co-B-P/75rGO was similar to the GO; yet, the peak near 1736 cm−1 disappeared. We ascribed this to the addition of H2PO2− and BH4−, which acted as reducing agents to reduce the GO to reduced graphene (rGO) [39]. These experimental results show that the Co-B-P/75rGO catalyst was successfully synthesized.
The surface interactions and electronic states of the Co-B-P/75rGO catalyst were investigated by XPS. In the XPS spectrum of Co 2p (Figure 5b), the two major peaks at 781.4 and 797.2 eV were Co 2p 3/2 and Co 2p 1/2, respectively [43], while two satellite peaks were observed at 786.5 and 803.1 eV, indicating the presence of elemental Co and the oxidized state of Co in the catalyst [44]. The C 1s spectrum (Figure 5c) showed three peaks located at 284.8, 285.9, and 288.7 eV, which belonged to the C-C/C=C, C-O, and O=C-O groups of rGO, respectively [45]. The peaks of B 1s at 187.7 and 191.2 eV were attributed to boron in the elemental and oxidized states, respectively. The elemental boron was positively shifted by 1.2 eV compared to the pure boron (186.5 eV) binding energy [46]. This was due to the transfer of electrons from boron to cobalt, filling the empty d-orbitals of cobalt (Figure 5d). In the O 1s XPS spectrum, two peaks located at 531.6 and 533.0 eV were ascribed to -C=O and -C-O, respectively (Figure 5e). In addition, two distinctive characteristic peaks near 129.5 and 132.9 eV in the full spectrum of element P (Figure 5f) were attributed to the presence of P0 and P-O, respectively [29]. Due to the high electronegativity of P, the binding energy of P0 was negatively shifted by 0.7 eV compared to pure P (130.2 eV) [47]. Apparently, as shown in Figure 2, the binding energy of cobalt in Co-B-P/75rGO was positively shifted by 0.3 eV compared to that in Co-B/75rGO.These experimental results suggest that there was an interaction between Co, B, and P, which is more favorable for catalysis.
The specific surface area and surface pore characteristics of the catalysts were tested by an Autosorb-iQ analyzer. According to the IUPAC classification, both curves in Figure 6a show hysteresis back loops, which were apparently type IV isotherms, indicating that both catalysts had a mesoporous characteristic [48]. The mesoporous channels are beneficial to the diffusion and contact between catalyst and reactant [49]. In addition, according to Table 1, the specific surface area of the Co-B-P/75rGO catalyst increased from 3 m2/g to 89 m2/g as the GO was added. Compared with pure Co-B-P, the total pore volume of Co-B-P/75rGO was increased, and the average pore diameter of 12.0 nm decreased to 9.0 nm. The addition of GO significantly increased the specific surface area for uniform distribution of Co-B-P clusters; thus, the composite catalyst offered more active sites for catalyzing the hydrolysis.

3.2. Effect of Different Types of Catalysts

In order to evaluate the properties of the catalyst, performance tests with different comparison samples were carried out. Figure 7 shows the hydrogen production per unit time of sodium borohydride hydrolysis catalyzed by the GO, Co-P, Co-B, Co-B-P, and Co-B-P/75rGO catalysts, and the magnitude of the slope represents the different superior and inferior performances. The experimental results showed that pure GO had less catalytic performance when used for NaBH4 hydrolysis. Moreover, the combination of Co elements with heteroatoms (e.g., B and P) presented better catalytic performance than pure Co-based catalysts, which is due to the addition of heteroatoms forming electronic interactions with Co, thereby enhancing the catalytic behavior [21]. Based on the above conclusion, the Co-B-P catalyst with two heteroatoms exhibited a better performance than Co-B and Co-P catalysts because of the synergistic effect between Co, B, and P. Moreover, after combining Co-B-P with GO, the Co-B-P/rGO catalyst presented the optimal catalytic activity and has a higher competitive advantage over previously reported catalysts (Table 2). This is because the presence of GO increased the specific surface area for the uniform dispersion of the Co-B-P clusters on the surface of GO, thus exposing more catalytically active sites for the hydrolysis reaction [38]. Therefore, our further research was based on the Co-B-P/rGO catalyst.

3.3. Effect of GO Amount

The appropriate amount of carrier plays a crucial role in the synthesis of catalysts. The effects on Co-B-P/rGO catalysts with different amounts of GO (25, 50, 75, and 100 mg) for the catalytic activity of NaBH4 were also investigated. The hydrolysis of NaBH4 experiments showed that, with an increase in the amount of GO, the HG rate first increased and then decreased. The Co-B-P/75rGO sample with 75 mg GO presented an optimal catalytic performance with the HG rate of 12,087.8 mL min−1 g−1 (Figure 8a,b). Previous studies have proved that metal clusters play a major role in the hydrolysis NaBH4 reaction. The chemical composition of the prepared catalysts with different amounts of GO were determined by ICP–OES (Table 3). The results showed that the Co-B-P/75rGO catalyst had the highest Co content (61.79%), which also corresponded to the results of the hydrolysis experiment. Combined with the textural and surface morphology analysis, there were two factors for the superior performance of the Co-B-P/75rGO. First, the optimal content of GO supplied sufficient specific surface area for uniform distribution of Co-B-P/75rGO and provided more active sites for catalysis reaction [57]. Meanwhile, B and P heteroatoms doping led to a higher electron density in the active site of the catalyst, thus exhibiting a better catalytic performance.

3.4. Effect of Catalyst Amount

In order to investigate the relationship between the catalyst amount and catalytic performance, four groups of different masses of Co-B-P/75rGO (25, 50, 75, and 100 mg) were tested for hydrolysis performance (Figure 9a). Each test reached the theoretical capacity of hydrogen volume, and the HG rate became increasingly faster with the increase in catalyst dosage. A linear relationship between the two can be seen in Figure 9b. This indicates that the Co-B-P/75rGO catalyst’s catalyzing hydrogen production from NaBH4 was characterized by first-order reaction kinetics.

3.5. Effect of NaBH4 Concentration

The effect of NaBH4 concentration on hydrogen generation was studied under the condition of 0.1 g Co-B-P/75rGO catalyst and 25 °C (Figure 10a). The generated hydrogen volume was gradually increased to the theoretical capacity after increasing the NaBH4 concentration from 0.5 wt% to 2.0 wt%. In addition, Figure 10b shows that the HG rate remained nearly identical as the NaBH4 concentration increased. The insignificant change in HG rate indicated that the concentration of NaBH4 did not affect the HG reaction, showing zero-order reaction kinetics [58].

3.6. Kinetic Studies at Different Temperatures

The HG rate of the Co-B-P/75rGO catalyst was measured under standard conditions. The temperature was controlled from 15 °C to 55 °C with 10 °C as a gradient. Figure 11a shows that high temperature had a significant promotion effect on the rate of hydrogen production. The total HG volume reached theoretical capacity at different temperatures. The formula is shown below:
k = k 0 · exp E a RT
where k0 is the rate constant (mL min−1 g−1), Ea is the activation energy (kJ mol−1), T is the reaction temperature (K), and R is the gas constant (8.314 kJ mol−1 K−1). Figure 11b shows the Arrhenius plot of ln k and the reciprocal of the absolute temperature (1/T). According to the slope of the fitting line, the Ea of the hydrolysis reaction in this study was calculated to be 28.64 kJ mol−1, which is lower than most previous reports in the literature (Table 2). The favorable catalytic activity was ascribed to the presence of GO, which promoted the uniform dispersion of Co-B-P clusters and exposed more catalytically active sites for the hydrolysis. Meanwhile the synergistic effect of the GO and Co-B-P clusters was also conducive to the hydrolysis activity of NaBH4.

3.7. Reusability Performance

The cycle stability of catalysts is critical in practical applications. Therefore, NaBH4 was hydrolyzed 10 times with Co-B-P/75rGO catalyst in the same conditions. Figure 12 shows the variation in the catalytic hydrogen production efficiency of the Co-B-P/75rGO catalyst with the number of cycles. It can be observed that the HG rate decreased slightly as the cycle time increased. The HG rate still maintained 88.9% of the initial rate after 10 cycles, which shows better stability compared to other previously reported cobalt-based catalysts (Table 2). The decline in the catalytic activity may be due to the active clusters being reunited during each cycle. In addition, the produced boride byproducts (such as BαOβ(OH)γ and BxOy·nH2O) were adsorbed on the catalyst surface during the catalysis process, thereby decreasing the HG rate [59].

4. Conclusions

In summary, a series of Co-B-P/xrGO catalysts were achieved using a chemical in situ reduction method and were employed for NaBH4 hydrolysis. The experimental results showed that Co-B-P/xrGO had a strong effect on the catalytic behaviors, in which the Co-B-P/75rGO presented an optimal HG rate (12,087.8 mL min−1 g−1) and lower activation energy (28.64 kJ mol−1). The satisfied catalytic performances were due to the uniform dispersion of clusters and the synergistic catalytic effect between Co, B, and P. In addition, the repeatability test results showed that 88.9% of the initial catalytic efficiency could be maintained following 10 cycles, indicating that the catalyst had a good cycle stability. The above findings suggest that the Co-B-P/75rGO catalyst has great promise for producing hydrogen via chemical hydrate hydrolysis.

Author Contributions

Conceptualization, X.J. and Z.S.; methodology, X.J. and Z.S.; software, X.J., Z.S., H.H., Y.Y. and C.Z.; validation, X.J. and Z.S.; formal analysis, X.J., L.S. and F.X.; investigation, X.J., L.S. and F.X.; resources, L.S. and F.X.; data curation, X.J., Z.S., L.K., R.C. and Y.B.; writing—original draft preparation, X.J. and Z.S.; writing—review and editing, L.S., F.X. and H.P.; visualization, X.J. and Z.S.; supervision, L.S. and F.X.; project administration, L.S. and F.X.; funding acquisition, L.S. and F.X. All authors have read and agreed to the published version of the manuscript.

Funding

This work was supported by the National Key Research and Development Program of China (2018YFB1502103, 2018YFB1502105), the National Natural Science Foundation of China (51971068, U20A20237 and 51871065), the Scientific Research and Technology Development Program of Guangxi (AA19182014, AD17195073, AA17202030-1, 2021AB17045), Guangxi Bagui Scholar Foundation, Guangxi Collaborative Innovation Centre of Structure and Property for New Energy and Materials, Guangxi Advanced Functional Materials Foundation and Application Talents Small Highlands, Chinesisch-Deutsche Kooperationsgruppe (GZ1528), and the Science Research and Technology Development Project of Guilin (20210102-4, 20210216-1).

Data Availability Statement

Not applicable.

Conflicts of Interest

The authors declare no conflict of interest.

References

  1. Liang, Z.Q.; Yao, Z.D.; Li, R.H.; Xiao, X.Z.; Ye, Z.C.; Wang, X.C.; Qi, J.C.; Bi, J.P.; Fan, X.L.; Kou, H.Q.; et al. Regulating local chemistry in ZrCo-based orthorhombic hydrides via increasing atomic interference for ultra-stable hydrogen isotopes storage. J. Energy Chem. 2022, 69, 397–405. [Google Scholar] [CrossRef]
  2. Cai, W.T.; Yang, Y.Z.; Tao, P.J.; Ouyang, L.Z.; Wang, H. Correlation between structural stability of LiBH4 and cation electronegativity in metal borides: An experimental insight for catalyst design. Dalton Trans. 2018, 47, 4987–4993. [Google Scholar] [CrossRef] [PubMed]
  3. Schapbach, L.; Züttel, A. Hydrogen-storage materials for mobile applications. Nature 2001, 414, 265–270. [Google Scholar]
  4. Zhu, Y.Y.; Ouyang, L.Z.; Zhong, H.; Liu, J.W.; Wang, H.; Shao, H.Y.; Huang, Z.G.; Zhu, M. Closing the loop for hydrogen storage: Facile regeneration of NaBH4 from its hydrolytic product. Angew. Chem. Int. Ed. 2020, 132, 8701–8707. [Google Scholar] [CrossRef]
  5. Hashimi, A.S.; Nohan, M.A.N.M.; Chin, S.X.; Zakaria, S.; Chia, C.H. Copper Nanowires as Highly Efficient and Recyclable Catalyst for Rapid Hydrogen Generation from Hydrolysis of Sodium Borohydride. Nanomaterials 2020, 9, 1153. [Google Scholar] [CrossRef]
  6. Wang, Y.; Zou, K.L.; Wang, D.; Meng, W.; Qi, N.; Cao, Z.Q.; Zhang, K.; Chen, H.H.; Li, G.D. Highly efficient hydrogen evolution from the hydrolysis of ammonia borane solution with the Co-Mo-B/NF nanocatalyst. Renew. Energy 2020, 154, 453–460. [Google Scholar] [CrossRef]
  7. Zhong, H.; Ouyang, L.Z.; Ye, J.S.; Liu, J.W.; Wang, H.; Yao, X.D.; Zhu, M. An one-step approach towards hydrogen production and storage through regeneration of NaBH4. Energy Storage Mater. 2017, 7, 222–228. [Google Scholar] [CrossRef]
  8. Lee, J.; Kong, K.Y.; Jung, C.R.; Cho, E.; Yoon, S.P.; Han, J.; Lee, T.G.; Nam, S.W. A structured Co–B catalyst for hydrogen extraction from NaBH4 solution. Catal. Today 2007, 120, 305–310. [Google Scholar] [CrossRef]
  9. Huang, Y.K.; An, C.H.; Zhang, Q.Y.; Zang, L.; Shao, H.X.; Liu, Y.F.; Zhang, Y.; Yuan, H.T.; Wang, C.Y.; Wang, Y.J. Cost-effective mechanochemical synthesis of highly dispersed supported transition metal catalysts for hydrogen storage. Nano Energy 2021, 80, 105535. [Google Scholar] [CrossRef]
  10. Zhang, H.M.; Zhang, L.; Rodriguez-Perez, I.A.; Miao, W.K.; Chen, K.L.; Wang, W.F.; Li, Y.; Han, S.M. Carbon nanospheres supported bimetallic Pt-Co as an efficient catalyst for NaBH4 hydrolysis. Appl. Surf. Sci. 2021, 540, 148296. [Google Scholar] [CrossRef]
  11. Liu, H.Y.; Ning, H.L.; Peng, S.G.; Yu, Y.H.; Ran, C.; Chen, Y.M.; Ma, J.Y.; Xie, J.P. Surface tailored Ru catalyst on magadiite for efficient hydrogen generation. Colloids Surf. A 2021, 631, 127627. [Google Scholar] [CrossRef]
  12. Zou, Y.C.; Nie, M.; Huang, Y.M.; Wang, J.Q.; Liu, H.L. Kinetics of NaBH4 hydrolysis on carbon-supported ruthenium catalysts. Int. J. Hydrogen Energy 2011, 36, 12343–12351. [Google Scholar] [CrossRef]
  13. Zhao, Y.C.; Ning, Z.; Tian, J.N.; Wang, H.W.; Liang, X.Y.; Nie, S.L.; Yu, Y.; Li, X.X. Hydrogen generation by hydrolysis of alkaline NaBH4 solution on Co–Mo–Pd–B amorphous catalyst with efficient catalytic properties. J. Power Sources 2012, 207, 120–126. [Google Scholar] [CrossRef]
  14. Zhang, B.P.; Xia, G.L.; Sun, D.L.; Fang, F.; Yu, X.B. Magnesium hydride nanoparticles self-assembled on graphene as anode material for high-performance lithium-ion batteries. ACS Nano 2018, 12, 3816–3824. [Google Scholar] [CrossRef] [PubMed] [Green Version]
  15. Ma, H.; Ji, W.Q.; Zhao, J.Z.; Liang, J.; Chen, J. Preparation, characterization and catalytic NaBH4 hydrolysis of Co-B hollow spheres. J. Alloys Compd. 2009, 474, 584–589. [Google Scholar] [CrossRef]
  16. Zhang, X.W.; Zhang, Q.; Xu, B.; Liu, X.Q.; Zhang, K.M.; Fan, A.Y.; Jiang, W.D. Efficient Hydrogen Generation from the NaBH4 Hydrolysis by Cobalt-Based Catalysts: Positive Roles of Sulfur-Containing Salts. ACS Appl. Mater. Inter. 2020, 12, 9376–9386. [Google Scholar] [CrossRef]
  17. Lin, H.J.; Xu, C.; Gao, M.; Ma, Z.L.; Meng, Y.Y.; Li, L.Q.; Hu, X.H.; Zhu, Y.F.; Pan, S.P.; Li, W. Hydrogenation properties of five-component Mg60Ce10Ni20Cu5 × 5 (X=Co, Zn) metallic glasses. Intermetallics 2019, 108, 94–99. [Google Scholar] [CrossRef]
  18. Didehban, A.; Zabihi, M.; Shahrouzi, J.R. Experimental studies on the catalytic behavior of alloy and core-shell supported Co-Ni bimetallic nano-catalysts for hydrogen generation by hydrolysis of sodium borohydride. Int. J. Hydrogen Energy 2018, 43, 20645–20660. [Google Scholar] [CrossRef]
  19. Eom, K.S.; Cho, K.W.; Kwon, H.S. Effects of electroless deposition conditions on microstructures of cobalt-phosphorous catalysts and their hydrogen generation properties in alkaline sodium borohydride solution. J. Power Sources 2008, 180, 484–490. [Google Scholar] [CrossRef]
  20. Li, H.; Yang, P.F.; Chu, D.S.; Li, H.X. Selective maltose hydrogenation to maltitol on a ternary Co-P-B amorphous catalyst and the synergistic effects of alloying B and P. Appl. Catal. A-Gen. 2007, 325, 34–40. [Google Scholar] [CrossRef]
  21. Patel, N.; Fernandes, R.; Miotello, A. Hydrogen generation by hydrolysis of NaBH4 with efficient Co-P-B catalyst: A kinetic study. J. Power Sources 2009, 188, 411–420. [Google Scholar] [CrossRef]
  22. Zhang, X.W.; Zhao, J.Z.; Cheng, F.Y.; Liang, J.; Tao, Z.L.; Chen, J. Electroless-deposited Co–P catalysts for hydrogen generation from alkaline NaBH4 solution. Int. J. Hydrogen Energy 2010, 35, 8363–8369. [Google Scholar] [CrossRef]
  23. Ekinci, A.; Cengiz, E.; Kuncan, M.; Sahin, Ö. Hydrolysis of sodium borohydride solutions both in the presence of Ni-B catalyst and in the case of microwave application. Int. J. Hydrogen Energy 2020, 45, 34749–34760. [Google Scholar]
  24. Sun, H.M.; Meng, J.; Jiao, L.F.; Cheng, F.Y.; Chen, J. A review of transition-metal boride/phosphide-based materials for catalytic hydrogen generation from hydrolysis of boron-hydrides. Inorg. Chem. Front. 2018, 5, 760–772. [Google Scholar] [CrossRef]
  25. Li, L.; Wang, Y.J.; Wang, Y.P.; Ren, Q.L.; Jiao, L.F.; Yuan, H.T. Effect of Ni Content in Co1-xNixB Catalysts on Hydrogen Generation during Hydrolysis. Acta Phys.-Chim. Sin. 2010, 26, 1575–1578. [Google Scholar] [CrossRef]
  26. Şahin, Ö.; Karakaş, D.E.; Kaya, M.; Saka, C. The effects of plasma treatment on electrochemical activity of Co-B-P catalyst for hydrogen production by hydrolysis of NaBH4. J. Energy Inst. 2017, 90, 466–475. [Google Scholar] [CrossRef]
  27. Zhang, X.Y.; Sun, X.W.; Xu, D.Y.; Tao, X.M.; Dai, P.; Guo, Q.J.; Liu, X. Synthesis of MOF-derived Co@C composites and application for efficient hydrolysis of sodium borohydride. Appl. Surf. Sci. 2019, 469, 764–769. [Google Scholar] [CrossRef]
  28. Zhang, P.F.; Chen, N.Q.; Chen, D.; Yang, S.Z.; Liu, X.F.; Wang, L.; Wu, P.W.; Phillip, N.; Yang, J.; Dai, S. Ultra-Stable and High-Cobalt-Loaded Cobalt@Ordered Mesoporous Carbon Catalysts: All-in-One Deoxygenation of Ketone into Alkylbenzene. ChemCatChem 2018, 10, 3299–3304. [Google Scholar] [CrossRef]
  29. Shi, L.M.; Chen, Z.; Jian, Z.Y.; Guo, F.H.; Gao, C.L. Carbon nanotubes-promoted Co-B catalysts for rapid hydrogen generation via NaBH4 hydrolysis. Int. J. Hydrogen Energy 2019, 44, 19868–19877. [Google Scholar] [CrossRef]
  30. Yang, C.C.; Chen, M.S.; Chen, Y.W. Hydrogen generation by hydrolysis of sodium borohydride on CoB/SiO2 catalyst. Int. J. Hydrogen Energy 2011, 36, 1418–1423. [Google Scholar] [CrossRef]
  31. Ye, W.; Zhang, H.; Xu, D.; Ma, L.; Yi, B.L. Hydrogen generation utilizing alkaline sodium borohydride solution and supported cobalt catalyst. J. Power Sources 2007, 164, 544–548. [Google Scholar] [CrossRef]
  32. Zhang, R.Z.; Zheng, J.L.; Chen, T.W.; Ma, G.S.; Zhou, W. RGO-wrapped Ni-P hollow octahedrons as noble-metal-free catalysts to boost the hydrolysis of ammonia borane toward hydrogen generation. J. Alloys Compd. 2018, 763, 538–545. [Google Scholar] [CrossRef]
  33. Yao, Q.; Lu, Z.H.; Huang, W.; Chen, X.S.; Zhu, J. Highly Pt-like activity of Ni-Mo/graphene catalyst for hydrogen evolution from hydrolysis of ammonia borane. J. Mater. Chem. A 2016, 4, 8579–8583. [Google Scholar] [CrossRef]
  34. Hummers, W.S.; Offeman, R.E. Preparation of Graphitic Oxide. J. Am. Chem. Soc. 1958, 208, 1334–1339. [Google Scholar] [CrossRef]
  35. Fernandes, R.; Patel, N.; Miotello, A. Efficient catalytic properties of Co-Ni-P-B catalyst powders for hydrogen generation by hydrolysis of alkaline solution of NaBH4. Int. J. Hydrogen Energy 2009, 34, 2893–2900. [Google Scholar] [CrossRef]
  36. Zhao, X.; Xu, D.Y.; Liu, K.; Dai, P.; Gao, J. Remarkable enhancement of PdAg/rGO catalyst activity for formic acid dehydrogenation by facile boron-doping through NaBH4 reduction. Appl. Surf. Sci. 2020, 512, 145746. [Google Scholar] [CrossRef]
  37. Wang, W.Y.; Liu, P.L.; Wu, K.; Tan, S.; Li, W.S.; Yang, Y.Q. Preparation of hydrophobic reduced graphene oxide supported Ni-B-P-O and Co-B-P-O catalysts and their high hydrodeoxygenation activities. Green Chem. 2016, 18, 984–988. [Google Scholar] [CrossRef]
  38. Shi, L.M.; Xie, W.; Jian, Z.Y.; Liao, X.M.; Wang, Y.J. Graphene modified Co-B catalysts for rapid hydrogen production from NaBH4 hydrolysis. Int. J. Hydrogen Energy 2019, 44, 17954–17962. [Google Scholar] [CrossRef]
  39. Wang, Y.; Qi, K.Z.; Wu, S.W.; Cao, Z.Q.; Zhang, K.; Lu, Y.S.; Liu, H.X. Preparation, characterization and catalytic sodium borohydride hydrolysis of nanostructured cobalt-phosphorous catalysts. J. Power Sources 2015, 284, 130–137. [Google Scholar] [CrossRef]
  40. Dai, H.B.; Liang, Y.; Wang, P. Effect of trapped hydrogen on the induction period of cobalt-tungsten-boron/nickel foam catalyst in catalytic hydrolysis reaction of sodium borohydride. Catal. Today 2011, 170, 27–32. [Google Scholar] [CrossRef]
  41. Bharath, G.; Anwer, S.; Mangalaraja, R.V.; Alhseinat, E.; Banat, F.; Ponpandian, N. Sunlight-Induced photochemical synthesis of Au nanodots on α-Fe2O3@Reduced graphene oxide nanocomposite and their enhanced heterogeneous catalytic properties. Sci. Rep. 2018, 8, 5718. [Google Scholar] [CrossRef] [PubMed]
  42. Riahi, K.Z.; Sdiri, N.; Ennigrou, D.J.; Horchani-Naifer, K. Investigations on electrical conductivity and dielectric properties of graphene oxide nanosheets synthetized from modified Hummer’s method. J. Mol. Struct. 2020, 1216, 128304. [Google Scholar] [CrossRef]
  43. Bai, Y.J.; Zhang, H.J.; Liu, L.; Xu, H.T.; Wang, Y. Tunable and Specific Formation of C@NiCoP Peapods with Enhanced HER Activity and Lithium Storage Performance. Chem. Eur. J. 2016, 22, 1021–1029. [Google Scholar] [CrossRef] [PubMed]
  44. Zou, Y.J.; Yin, Y.; Gao, Y.B.; Xiang, C.L.; Chu, H.L.; Qiu, S.J.; Yan, E.H.; Xu, F.; Sun, L.X. Chitosan-mediated Co-Ce-B nanoparticles for catalyzing the hydrolysis of sodium borohydride. Int. J. Hydrogen Energy 2018, 43, 4912–4921. [Google Scholar] [CrossRef]
  45. Fan, G.; Huang, W.; Wang, C. In situ synthesis of Ru/RGO nanocomposites as a highly efficient catalyst for selective hydrogenation of halonitroaromatics. Nanoscale 2013, 5, 6819–6825. [Google Scholar] [CrossRef]
  46. Moddeman, W.E.; Burke, A.R.; Bowling, W.C.; Foose, D.S. Surface oxides of boron and B12O2 as determined by XPS. Surf. Interface Anal. 1989, 14, 224–232. [Google Scholar] [CrossRef]
  47. Guang, H.L.; Zhu, S.L.; Liang, Y.Q.; Wu, S.L.; Li, Z.Y.; Luo, S.Y.; Cui, Z.D.; Inoue, A. Highly efficient nanoporous CoBP electrocatalyst for hydrogen evolution reaction. Rare Metals 2021, 40, 1031–1039. [Google Scholar] [CrossRef]
  48. Shi, L.M.; Zhang, G. Improved Low-Temperature Activity of CuO-CeO2-ZrO2 Catalysts for Preferential Oxidation of CO in H2-Rich Streams. Catal. Lett. 2016, 146, 1449–1456. [Google Scholar] [CrossRef]
  49. Tong, D.G.; Han, X.; Chu, W.; Chen, H.; Ji, X.Y. Preparation of mesoporous Co-B catalyst via self-assembled triblock copolymer templates. Mater. Lett. 2007, 61, 4679–4682. [Google Scholar] [CrossRef]
  50. Wang, J.; Ke, D.D.; Li, Y.; Zhang, H.M.; Wang, C.X.; Zhao, X.; Yuan, Y.J.; Han, S.M. Efficient hydrolysis of alkaline sodium borohydride catalyzed by cobalt nanoparticles supported on three-dimensional graphene oxide. Mater. Res. Bull. 2017, 95, 204–210. [Google Scholar] [CrossRef]
  51. Zhang, H.M.; Feng, X.L.; Cheng, L.; Hou, X.W.; Li, Y.; Han, S.M. Non-noble Co anchored on nanoporous graphene oxide, as an efficient and long-life catalyst for hydrogen generation from sodium borohydride. Colloid Surf. A 2019, 563, 112–119. [Google Scholar] [CrossRef]
  52. Liu, H.Y.; Shi, Q.Y.; Yang, Y.M.; Yu, Y.N.; Zhang, Y.; Zhang, M.S.; Wei, L.; Lu, Y.H. CoO-Co2P composite nanosheets as highly active catalysts for sodium borohydride hydrolysis to generate hydrogen. Funct. Mater. Lett. 2020, 13, 2051025. [Google Scholar] [CrossRef]
  53. Li, J.H.; Hong, X.Y.; Wang, Y.L.; Luo, Y.M.; Huang, P.R.; Li, B.; Zhang, K.X.; Zou, Y.J.; Sun, L.X.; Xu, F.; et al. Encapsulated cobalt nanoparticles as a recoverable catalyst for the hydrolysis of sodium borohydride. Energy Storage Mater. 2020, 27, 187–197. [Google Scholar] [CrossRef]
  54. Li, Z.; Wang, L.N.; Zhang, Y.; Xie, G.W. Properties of Cu-Co-P/γ-Al2O3 catalysts for efficient hydrogen generation by hydrolysis of alkaline NaBH4 solution. Int. J. Hydrogen Energy 2017, 42, 5749–5757. [Google Scholar] [CrossRef]
  55. Wang, F.H.; Zhang, Y.J.; Wang, Y.N.; Luo, Y.M.; Chen, Y.N.; Zhu, H. Co-P nanoparticles supported on dandelion-like CNTs-Ni foam composite carrier as a novel catalyst for hydrogen generation from NaBH4 methanolysis. Int. J. Hydrogen Energy 2018, 43, 8805–8814. [Google Scholar] [CrossRef]
  56. Wei, L.; Dong, X.L.; Yang, Y.M.; Shi, Q.Y.; Lu, Y.H.; Liu, H.Y.; Yu, Y.N.; Zhang, M.H.; Qi, M.; Wang, Q. Co-O-P composite nanocatalysts for hydrogen generation from the hydrolysis of alkaline sodium borohydride solution. Int. J. Hydrogen Energy 2020, 45, 10745–10753. [Google Scholar] [CrossRef]
  57. Cui, Z.; Guo, Y.; Ma, J. In situ synthesis of graphene supported Co-Sn-B alloy as an efficient catalyst for hydrogen generation from sodium borohydride hydrolysis. Int. J. Hydrogen Energy 2016, 41, 1592–1599. [Google Scholar] [CrossRef]
  58. Wang, L.N.; Li, Z.; Zhang, P.P.; Wang, G.X.; Xie, G.W. Hydrogen generation from alkaline NaBH4 solution using Co-Ni-Mo-P/γ-Al2O3 catalysts. Int. J. Hydrogen Energy 2016, 41, 1468–1476. [Google Scholar] [CrossRef]
  59. Li, Z.; Li, H.L.; Wang, L.N.; Liu, T.Y.; Zhang, T.; Wang, G.X.; Xie, G.W. Hydrogen generation from catalytic hydrolysis of sodium borohydride solution using supported amorphous alloy catalysts (Ni-Co-P/γ-Al2O3). Int. J. Hydrogen Energy 2014, 39, 14935–14941. [Google Scholar] [CrossRef]
Nanomaterials 12 02732 g001 550
Figure 1. The illustration of the synthetic route of Co-B-P/xrGO.
Figure 1. The illustration of the synthetic route of Co-B-P/xrGO.
Nanomaterials 12 02732 g001
Nanomaterials 12 02732 g002 550
Figure 2. SEM images of (a) Co-B-P, (b) GO, (c–f) Co-B-P/xrGO (x = 25, 50, 75, and 100), and EDX mapping images of (g) Co-B-P/75rGO, (h) Co, (i) B, (j) P, (k) O, and (l) C in Co-B-P/xrGO.
Figure 2. SEM images of (a) Co-B-P, (b) GO, (c–f) Co-B-P/xrGO (x = 25, 50, 75, and 100), and EDX mapping images of (g) Co-B-P/75rGO, (h) Co, (i) B, (j) P, (k) O, and (l) C in Co-B-P/xrGO.
Nanomaterials 12 02732 g002
Nanomaterials 12 02732 g003 550
Figure 3. (a) XRD patterns of Co-B-P and Co-B-P/xrGO catalysts; (b) Raman spectra of Co-B-P/xrGO catalysts (x = 25, 50, 75, and 100).
Figure 3. (a) XRD patterns of Co-B-P and Co-B-P/xrGO catalysts; (b) Raman spectra of Co-B-P/xrGO catalysts (x = 25, 50, 75, and 100).
Nanomaterials 12 02732 g003
Nanomaterials 12 02732 g004 550
Figure 4. FTIR spectra of GO and CO-B-P/75rGO.
Figure 4. FTIR spectra of GO and CO-B-P/75rGO.
Nanomaterials 12 02732 g004
Nanomaterials 12 02732 g005 550
Figure 5. XPS analysis of Co-B-P/75rGO: (a) full spectrum, (b) Co 2p, (c) C 1s, (d) B 1s, (e) O 1s, and (f) P 2p.
Figure 5. XPS analysis of Co-B-P/75rGO: (a) full spectrum, (b) Co 2p, (c) C 1s, (d) B 1s, (e) O 1s, and (f) P 2p.
Nanomaterials 12 02732 g005
Nanomaterials 12 02732 g006 550
Figure 6. Nitrogen sorption isotherms (a) and pore-size distributions (b) for the Co-B-P and Co-B-P/75rGO catalysts.
Figure 6. Nitrogen sorption isotherms (a) and pore-size distributions (b) for the Co-B-P and Co-B-P/75rGO catalysts.
Nanomaterials 12 02732 g006
Nanomaterials 12 02732 g007 550
Figure 7. Hydrogen volume versus time for GO, Co-P, Co-B, Co-B-P, and Co-B-P/rGO (batch system, 25 °C, 1.5 wt% NaBH4 + 5 wt% NaOH, 0.1 g catalyst).
Figure 7. Hydrogen volume versus time for GO, Co-P, Co-B, Co-B-P, and Co-B-P/rGO (batch system, 25 °C, 1.5 wt% NaBH4 + 5 wt% NaOH, 0.1 g catalyst).
Nanomaterials 12 02732 g007
Nanomaterials 12 02732 g008 550
Figure 8. Hydrogen volume versus reaction time for the as-prepared catalysts (a); the histogram of the H2 generation rate versus the additive amount of GO (b) (batch system, 25 °C, 1.5 wt% NaBH4 + 5 wt% NaOH, 0.1 g catalyst).
Figure 8. Hydrogen volume versus reaction time for the as-prepared catalysts (a); the histogram of the H2 generation rate versus the additive amount of GO (b) (batch system, 25 °C, 1.5 wt% NaBH4 + 5 wt% NaOH, 0.1 g catalyst).
Nanomaterials 12 02732 g008
Nanomaterials 12 02732 g009 550
Figure 9. (a) Effect of catalyst loadings on the HG rate (batch system, 25 °C, 1.5 wt% NaBH4 + 5 wt% NaOH); (b) HG rate versus catalyst dosage.
Figure 9. (a) Effect of catalyst loadings on the HG rate (batch system, 25 °C, 1.5 wt% NaBH4 + 5 wt% NaOH); (b) HG rate versus catalyst dosage.
Nanomaterials 12 02732 g009
Nanomaterials 12 02732 g010 550
Figure 10. (a) Effect of NaBH4 concentrations on the HG rate (batch system, 25 °C, 5 wt% NaOH, 0.1 g of catalyst); (b) HG rate versus NaBH4 concentration.
Figure 10. (a) Effect of NaBH4 concentrations on the HG rate (batch system, 25 °C, 5 wt% NaOH, 0.1 g of catalyst); (b) HG rate versus NaBH4 concentration.
Nanomaterials 12 02732 g010
Nanomaterials 12 02732 g011 550
Figure 11. (a) Hydrogen generation kinetics curves and (b) Arrhenius plot obtained using 1.5 wt% NaBH4 and 1.0 wt% NaOH solution and employing Co-B-P/75rGO as a catalyst at different solution temperatures.
Figure 11. (a) Hydrogen generation kinetics curves and (b) Arrhenius plot obtained using 1.5 wt% NaBH4 and 1.0 wt% NaOH solution and employing Co-B-P/75rGO as a catalyst at different solution temperatures.
Nanomaterials 12 02732 g011
Nanomaterials 12 02732 g012 550
Figure 12. (a) Reusability of Co-B-P/75rGO with 0.1 g catalyst and 1.5 wt% NaBH4 + 5 wt% NaOH solution at 25 °C; (b) HG rate bar chart of catalyst used 10 times.
Figure 12. (a) Reusability of Co-B-P/75rGO with 0.1 g catalyst and 1.5 wt% NaBH4 + 5 wt% NaOH solution at 25 °C; (b) HG rate bar chart of catalyst used 10 times.
Nanomaterials 12 02732 g012
Table
Table 1. Textural parameters of the Co-B-P and Co-B-P/75rGO catalysts.
Table 1. Textural parameters of the Co-B-P and Co-B-P/75rGO catalysts.
CatalystSpecific Surface Area (m2 g−1)Pore Volume (cm3 g−1)Average Pore Diameter (nm)
Co-B-P30.0112.0
Co-B-P/75rGO890.289.0
Table
Table 2. The Co-B-P/75rGO catalyst was compared with those previously reported in the literature.
Table 2. The Co-B-P/75rGO catalyst was compared with those previously reported in the literature.
SampleMaximum HG Rate (mL min−1 g−1)Ea (kJ mol–1)Number
of Cycles		Cyclic
Stability		References
Co@3DGO439437.42554.0%[50]
Co@GO595564.87573.0%[51]
Co-P1647.947.0531.0%[39]
CoO-Co2P394027.4460.0%[52]
Co@N MGC-500357535.22082.5%[53]
Cu-Co-P/γ-Al2O3111547.8666.0%[54]
Co-P/CNTs-Ni foam243049.94874.0%[55]
Co-B-10CNTs12,00023.5564.0%[29]
Co-O-P485063578.0%[56]
Co-B-50GO14,43026.2581.5%[40]
Co-B-P/75rGO12,087.828.641088.9%This work
Table
Table 3. The chemical composition of the prepared catalysts with different amounts of GO were determined by ICP–OES.
Table 3. The chemical composition of the prepared catalysts with different amounts of GO were determined by ICP–OES.
CatalystAmount of Co (wt%)Amount of B (wt%)Amount of P (wt%)
Co-B-P/25GO35.800.0416.48
Co-B-P/50GO40.21.0212.62
Co-B-P/75GO61.792.515.50
Co-B-P/100GO34.650.7214.34
Publisher’s Note: MDPI stays neutral with regard to jurisdictional claims in published maps and institutional affiliations.

Share and Cite

MDPI and ACS Style

Jia, X.; Sang, Z.; Sun, L.; Xu, F.; Pan, H.; Zhang, C.; Cheng, R.; Yu, Y.; Hu, H.; Kang, L.; et al. Graphene-Modified Co-B-P Catalysts for Hydrogen Generation from Sodium Borohydride Hydrolysis. Nanomaterials 2022, 12, 2732. https://doi.org/10.3390/nano12162732

AMA Style

Jia X, Sang Z, Sun L, Xu F, Pan H, Zhang C, Cheng R, Yu Y, Hu H, Kang L, et al. Graphene-Modified Co-B-P Catalysts for Hydrogen Generation from Sodium Borohydride Hydrolysis. Nanomaterials. 2022; 12(16):2732. https://doi.org/10.3390/nano12162732

Chicago/Turabian Style

Jia, Xinlei, Zhen Sang, Lixian Sun, Fen Xu, Hongge Pan, Chenchen Zhang, Riguang Cheng, Yuqian Yu, Haopan Hu, Li Kang, and et al. 2022. "Graphene-Modified Co-B-P Catalysts for Hydrogen Generation from Sodium Borohydride Hydrolysis" Nanomaterials 12, no. 16: 2732. https://doi.org/10.3390/nano12162732

APA Style

Jia, X., Sang, Z., Sun, L., Xu, F., Pan, H., Zhang, C., Cheng, R., Yu, Y., Hu, H., Kang, L., & Bu, Y. (2022). Graphene-Modified Co-B-P Catalysts for Hydrogen Generation from Sodium Borohydride Hydrolysis. Nanomaterials, 12(16), 2732. https://doi.org/10.3390/nano12162732

Note that from the first issue of 2016, this journal uses article numbers instead of page numbers. See further details here.

Article Metrics

Back to TopTop