In Situ Preparation of 2D Co-B Nanosheets@1D TiO 2 Nanoﬁbers as a Catalyst for Hydrogen Production from Sodium Borohydride

: In this study, 2D Co-B nanosheet-decorated 1D TiO 2 nanoﬁbers (2D Co-B NS-decorated 1D TiO 2 NFs) are synthesized via electrospinning and an in situ chemical reduction technique. The as-prepared catalyst showed excellent catalytic performance in H 2 generation from sodium borohydride (SBH). When compared to naked Co-B nanoparticles, the catalytic activity of the 2D Co-B NS-decorated 1D TiO 2 NFs catalyst for the hydrolysis of SBH is signiﬁcantly enhanced, as demonstrated by the high hydrogen generation rate (HGR) of 6020 mL min − 1 g − 1 at 25 ◦ C. The activation energy of hydrolysis was measured to be 30.87 kJ mol − 1 , which agreed with the reported values. The catalyst also showed good stability. Moreover, the effects of SBH, catalyst concentration, and temperature on the catalytic performance of 2D Co-B NS-decorated 1D TiO 2 NFs were studied to gain a comprehensive understanding of the dehydrogenation mechanism of SBH. Based on these ﬁndings, we conclude that 2D Co-B NS-decorated 1D TiO 2 NFs are effective catalytic materials for the dehydrogenation of SBH.


Introduction
Hydrogen, due to its wide availability and eco-friendly nature, can serve as a future clean energy carrier [1][2][3]. Hydrogen has gained tremendous popularity as a green fuel option for fuel cells during the past recent years. Metal hydrides are potential solutions to address the challenges of transport and storage. Sodium borohydride (SBH; NaBH 4 ), a metal hydride, has attracted a lot of interest from the researchers because it offers several advantages over other hydrogen storage materials, including greater control over H 2 production rate, purity, safe production method, ability to recycle the by-product NaBO 2 into borohydride, and potentially a lower temperature at which hydrogen releases [4][5][6]. Also, it has superior physicochemical features, such as non-flammability, low molecular weight (37.83 g mol −1 ), high hydrogen capacity (10.8 wt.%), high room-temperature stability in a solid state, high stability in alkaline aqueous solutions, and secure and reliable hydrogen release via hydrolysis. Although it is counterproductive, an alkaline SBH solution frequently undergoes hydrolysis due to the key role NaOH plays in inhibiting SBH self-decomposition.
In addition to NaOH, catalysts are other options to promote a favorable outcome in this reaction. An effective and sturdy catalyst is required to regulate hydrogen generation during the hydrolysis of SBH. Initially, precious metals emerged as prospective catalysts for generating H 2 from dehydrogenation reaction at room temperature [7,8] because of their stability, longevity, outstanding efficiency, and resistance to deactivation [9]. However, due to their scarce availability and high cost, it has become of the utmost importance to investigate their substitute catalysts that are cheap and have the potentials to accelerate reaction rates while simultaneously reducing threshold activation energies. Thus, researchers are now focusing increasingly on abundant earth metals, such as transition metals like copper, cobalt, and nickel that are capable of catalyzing the dehydrogenation process of SBH [10][11][12].
Various studies have shown that catalysts constituting cobalt are most effective in hydrolyzing SBH. Among Co-based catalysts, cobalt-boride (Co-B) catalysts show unique features in the hydrolysis process of SBH. In particular, amorphous Co-B catalysts are superior to crystalline Co-B, Co metal powder forms, and other precious catalysts in terms of H 2 generation rate [9]. Co-B is a distinguished candidate due to a number of unique features, including its isotropic structure, a large concentration of coordinative unsaturated sites, and its stable chemical properties.
Recent research has shown that nanoscale Co-B materials with large surface areas and porosities facilitate the transfer and interaction of reactant molecules, leading to increased catalytic efficiencies as compared to conventional Co-B [9]. Naked nano-Co-B is readily susceptible to oxidization in air. It is particularly prone to aggregation and has a high degree of instability. Furthermore, naked nano-Co-B, being ferromagnetic, adheres themselves to the magnetic stirring rod during the hydrolysis process. Nano-Co-B can be stabilized when placed on the support matrix. Nano-TiO 2 has many useful properties as a catalyst and photocatalyst, including excellent chemical resistance, non-toxicity, and efficiency. H 2 production via AB hydrolysis has been reported by Yousef et al. [13], utilizing nano-TiO 2 as a supporting framework for copper (0) as an effective and recyclable catalyst. It has also been shown that palladium immobilized on TiO 2 nanoparticles is extremely effective, can be isolated, and is recyclable in AB hydrolysis, as demonstrated in the work of Rakap et al. [14]. Our research group has seen encouraging results by employing TiO 2 nanofibers (TiO 2 NFs) as support matrixes. NFs possess a high surface area and less aggregates than other nanostructures because of their high axial ratio and less grain boundaries. In addition, the surface area of NFs is almost twice than that of presently available thin film materials [15].
One-dimensional NFs and two-dimensional nanosheets (NS) stand out among the many different morphologies due to evident improvements in particle performances that they offer during catalysis and various other applications [16]. Due to their unique structures with high specific surface areas, they significantly improve the efficiency of the catalytic process. In this paper, we examine the catalytic activity of 2D Co-B NS-supported on 1D TiO 2 NFs synthesized via electrospinning and an in situ chemical reduction technique. The catalytic activity of the produced catalyst is shown to be superior for the release of H 2 from SBH.

Results and Discussion
It is well known that organic and inorganic nanofibers produced by electrospinning have their own distinctive nanoporous structures. FESEM images of pure TiO 2 nanofibers and CoAc/TiO 2 produced via the in situ chemical reduction of CoAc with SBH are displayed in Figure 1. The continuous, smooth, and beads-free surfaces of the pristine TiO 2 NFs can be observed in the image shown in Figure 1a. The FESEM in Figure 1b clearly reveals very thin horizontal and vertical Co-B NS attached to the surface of the TiO 2 NFs. The average size of the prepared NFs is 221.60 nm (inset in Figure 1b). The formation of the structure that consists of Co-B NS@TiO 2 NFs can be inferred by visual inspection of the surface of the TiO 2 NFs covered with very thin Co-B NS, as shown in Figure 1c,d. These structural features are useful to provide a greater number of catalytic active sites on the surface of the Co-B catalyst, allowing better adsorption of reactants. When CoAc and TiO 2 NFs are mixed, the pores in the TiO 2 NFs are filled with CoAc. When SBH is introduced, the CoAc on the nanoporous surface is converted into Co-B NPs. As the reaction continued, the newly generated nanoparticles acted as nucleation sites, and Co-B NPs grew on the surfaces of the TiO 2 NFs. This process continued until the whole CoAc was successfully converted to Co-B. Finally, the 2D Co-B NS grew on the surfaces of 1D TiO 2 NFs.
Inorganics 2023, 11, x FOR PEER REVIEW 3 of 12 the structure that consists of Co-B NS@TiO2 NFs can be inferred by visual inspection of the surface of the TiO2 NFs covered with very thin Co-B NS, as shown in Figure 1c,d. These structural features are useful to provide a greater number of catalytic active sites on the surface of the Co-B catalyst, allowing better adsorption of reactants. When CoAc and TiO2 NFs are mixed, the pores in the TiO2 NFs are filled with CoAc. When SBH is introduced, the CoAc on the nanoporous surface is converted into Co-B NPs. As the reaction continued, the newly generated nanoparticles acted as nucleation sites, and Co-B NPs grew on the surfaces of the TiO2 NFs. This process continued until the whole CoAc was successfully converted to Co-B. Finally, the 2D Co-B NS grew on the surfaces of 1D TiO2 NFs. XRD studies were performed to assess the phase structures of pristine 1D TiO2 NFs and 2D Co-B NS@1D TiO2 NFs ( Figure 2). Pristine 1D TiO2 NFs exhibited an XRD pattern characteristic of mixed phases of anatase and rutile, as illustrated in Figure 2 Figure 2 that the 2D Co-B NS@1D TiO 2 NFs comprise entirely well-crystallized tetragonal TiO 2 (Anatase; JCPDS # 21-1272) and (Rutile; JCPDS # 21-1276). However, no peak is seen for Co-B, which may be due to its amorphous nature.
Inorganics 2023, 11, x FOR PEER REVIEW 4 of 12 tion peaks of Figure 2 that the 2D Co-B NS@1D TiO2 NFs comprise entirely well-crystallized tetragonal TiO2 (Anatase; JCPDS # 21-1272) and (Rutile; JCPDS # 21-1276). However, no peak is seen for Co-B, which may be due to its amorphous nature.  Figure 3e depicts two peaks corresponding to Co 2p of Co 2+ states occurring at the binding energies of 782.10 eV and 797.80 eV, respectively [17][18][19]. Moreover, three satellite peaks of 788.19, 801.33, and 803.94 eV were observed [2,3]. This suggested that the oxidation of the catalyst's surface may have occurred during the sample preparation for analysis. The presence of B was confirmed through the observation of a peak at a binding energy of 191.2 eV (Figure 3d) associated with the B1s level. This peak was shifted by +3.5 eV in comparison to pure B (187.8 eV) [20], suggesting an electron transfer from B to the vacant d-orbital of metallic Co that may have formed linear chains containing B-B bonds [19]. Furthermore, the presence of borate (B 3+ ) in the formed boron cannot be excluded [21]. This electron transfer results in the surplus of electrons in Co and a deficiency of electrons in B [22,23]. Furthermore, the estimations of elements and compounds in the produced NFs for Titanium Dioxide (TiO2), Boron (B), and Cobalt (Co) were found to be 63.69 wt%, 6.37 wt%, and 29.93 wt%, respectively.
The catalytic performance of the synthesized catalyst was evaluated by adding 5 mg of catalyst to a solution containing 26 mM and 0.25 M NaOH at 25 °C. The volume of H2 that was generated by the dehydrogenation of SBH was continuously monitored. Figure  4a depicts the volume of H2 achieved by the Co-B NPs and 2D Co-B NS@1D TiO2 NFs catalyst. As shown in figure, the 2D Co-B NS@1D TiO2 NFs catalyst generated a higher volume of H2 as compared to Co-B NPs and pristine 1D TiO2 NFs catalyst. Lu et al. [24] studied the hydrolysis of the dehydrogenation of SBH using Co-B supported on different substrates (Al2O3, TiO2, and CeO2) and compared it with naked Co-B. The obtained results indicated that supported Co-B produced a high volume of H2 as compared to the naked Co-B because Co-B was supported four times higher than the naked Co-B catalyst. Furthermore, Co-B-supported TiO2 producing 6738 mL min -1 g -1 of H2, which demonstrated higher catalytic performance as compared to the Co-B-supported Al2O3, which produced 5495 mL min -1 g -1 , and Co-B-supported CeO2, which produced 4717 mL min -1 g -1 . Also, the HGR was found to be 6020 mL min -1 g -1 for 2D Co-B NS@1D TiO2 NFs, which was higher than that of the 2672 mL min -1 g -1 naked Co-B (Figure 4b). This may have been due  Figure 3e depicts two peaks corresponding to Co 2p of Co 2+ states occurring at the binding energies of 782.10 eV and 797.80 eV, respectively [17][18][19]. Moreover, three satellite peaks of 788.19, 801.33, and 803.94 eV were observed [2,3]. This suggested that the oxidation of the catalyst's surface may have occurred during the sample preparation for analysis. The presence of B was confirmed through the observation of a peak at a binding energy of 191.2 eV (Figure 3d) associated with the B1s level. This peak was shifted by +3.5 eV in comparison to pure B (187.8 eV) [20], suggesting an electron transfer from B to the vacant d-orbital of metallic Co that may have formed linear chains containing B-B bonds [19]. Furthermore, the presence of borate (B 3+ ) in the formed boron cannot be excluded [21]. This electron transfer results in the surplus of electrons in Co and a deficiency of electrons in B [22,23]. Furthermore, the estimations of elements and compounds in the produced NFs for Titanium Dioxide (TiO 2 ), Boron (B), and Cobalt (Co) were found to be 63.69 wt%, 6.37 wt%, and 29.93 wt%, respectively.
The catalytic performance of the synthesized catalyst was evaluated by adding 5 mg of catalyst to a solution containing 26 mM and 0.25 M NaOH at 25 • C. The volume of H 2 that was generated by the dehydrogenation of SBH was continuously monitored. Figure 4a depicts the volume of H 2 achieved by the Co-B NPs and 2D Co-B NS@1D TiO 2 NFs catalyst. As shown in figure, the 2D Co-B NS@1D TiO 2 NFs catalyst generated a higher volume of H 2 as compared to Co-B NPs and pristine 1D TiO 2 NFs catalyst. Lu et al. [24] studied the hydrolysis of the dehydrogenation of SBH using Co-B supported on different substrates (Al 2 O 3 , TiO 2 , and CeO 2 ) and compared it with naked Co-B. The obtained results indicated that supported Co-B produced a high volume of H 2 as compared to the naked Co-B because Co-B was supported four times higher than the naked Co-B catalyst. Furthermore, Co-B-supported TiO 2 producing 6738 mL min −1 g −1 of H 2 , which demonstrated higher catalytic performance as compared to the Co-B-supported Al 2 O 3 , which produced 5495 mL min −1 g −1 , and Co-B-supported CeO 2 , which produced 4717 mL min −1 g −1 . Also, the HGR was found to be 6020 mL min −1 g −1 for 2D Co-B NS@1D TiO 2 NFs, which was higher than that of the 2672 mL min −1 g −1 naked Co-B (Figure 4b). This may have been due to the increased number of available active sites on the surfaces of the 2D Co-B NS@1D TiO 2 NFs. to the increased number of available active sites on the surfaces of the 2D Co-B NS@1D TiO2 NFs.   Figure 5 shows the volume of H2 production versus time by varying 2D Co-B NS@1D TiO2 NFs catalyst loading from 5 to 20 mg while maintaining the other parameters (26 mM of SBH, 25 °C, and 1000 rpm) to be constant. The volume of H2 rises rapidly with increased catalyst loading (Figure 5a), which is consistent with the literature [25,26]. Table 1 demonstrates the HGR and yield using different 2D Co-B NS@1D TiO2 NFs catalyst loads. Also, the reaction time decreases with the increased catalyst amount. When the catalyst loading to the increased number of available active sites on the surfaces of the 2D Co-B NS@1D TiO2 NFs.   Figure 5 shows the volume of H2 production versus time by varying 2D Co-B NS@1D TiO2 NFs catalyst loading from 5 to 20 mg while maintaining the other parameters (26 mM of SBH, 25 °C, and 1000 rpm) to be constant. The volume of H2 rises rapidly with increased catalyst loading (Figure 5a), which is consistent with the literature [25,26]. Table 1 demonstrates the HGR and yield using different 2D Co-B NS@1D TiO2 NFs catalyst loads. Also, the reaction time decreases with the increased catalyst amount. When the catalyst loading  Figure 5 shows the volume of H 2 production versus time by varying 2D Co-B NS@1D TiO 2 NFs catalyst loading from 5 to 20 mg while maintaining the other parameters (26 mM of SBH, 25 • C, and 1000 rpm) to be constant. The volume of H 2 rises rapidly with increased catalyst loading (Figure 5a), which is consistent with the literature [25,26]. Table 1 demonstrates the HGR and yield using different 2D Co-B NS@1D TiO 2 NFs catalyst loads. Also, the reaction time decreases with the increased catalyst amount. When the catalyst loading increased from 5 mg to 20 mg, the reaction time decreased from 12 to 3.3 min. H 2 generation tends to be rate-limited by the amount of the catalyst [25,26]. Figure 5b shows a logarithmic relationship between the reaction rate and concentration of catalyst, demonstrating that the dehydrogenation of SBH in the presence of 2D Co-B NS@1D TiO 2 NFs follows first-order reaction kinetics with respect to the catalyst concentration.

Influence of 2D Co-B NS@1D TiO 2 NFs Loading
increased from 5 mg to 20 mg, the reaction time decreased from 12 to 3.3 min. H2 generation tends to be rate-limited by the amount of the catalyst [25,26]. Figure 5b shows a logarithmic relationship between the reaction rate and concentration of catalyst, demonstrating that the dehydrogenation of SBH in the presence of 2D Co-B NS@1D TiO2 NFs follows first-order reaction kinetics with respect to the catalyst concentration.

Influence of SBH Concentration
The effect of changing the initial SBH concentration from 26 to 105 mM on the HGR was examined while maintaining the other parameters to be constant (5 mg of catalyst, 25 °C, and 1000 rpm) throughout the experiments (Figure 6a). As the volume of H2 generation increased with increasing SBH concentration at almost identical HGR, it can be concluded that the dehydrogenation of SBH in the presence of the 2D Co-B NS@1D TiO2 NFs catalyst was independent of the SBH concertation and followed zero-order reaction kinetics with respect to the SBH concentration ( Figure 6b).

Influence of SBH Concentration
The effect of changing the initial SBH concentration from 26 to 105 mM on the HGR was examined while maintaining the other parameters to be constant (5 mg of catalyst, 25 • C, and 1000 rpm) throughout the experiments (Figure 6a). As the volume of H 2 generation increased with increasing SBH concentration at almost identical HGR, it can be concluded that the dehydrogenation of SBH in the presence of the 2D Co-B NS@1D TiO 2 NFs catalyst was independent of the SBH concertation and followed zero-order reaction kinetics with respect to the SBH concentration (Figure 6b).

Influence of Reaction Temperature
As expected, raising the reaction temperature accelerates the reaction rate of H2 (Figure 7). Figure 7a displays the H2 production volume employing 2D Co-B NS@1D TiO2 NFs catalyst at various temperatures. With an increase in temperature, the reaction rate increases rapidly. Table 2 demonstrates the HGR and yield at various reaction temperatures.

Influence of Reaction Temperature
As expected, raising the reaction temperature accelerates the reaction rate of H 2 (Figure 7). Figure 7a displays the H 2 production volume employing 2D Co-B NS@1D TiO 2 NFs catalyst at various temperatures. With an increase in temperature, the reaction rate increases rapidly. Table 2 demonstrates the HGR and yield at various reaction temperatures. The reaction time decreased for producing stoichiometric hydrogen with the increase in the reaction temperature. A plausible explanation to this observation is the ever-increasing mobility of SBH molecules, which leads to a greater number of realistic collisions beyond the energy threshold barrier [26]. Based on these observations, the reaction turned out to be zero order since the volume of H 2 production grows linearly with the reaction time. The rate of a zero-order reaction is given by the following expression: Plotting ln k against 1/T yielded the activation energy (E a ) to be 30.87 kJ mol −1 of the hydrolysis reaction process (Figure 7b). This value was at par with the others that had been achieved and published in the literature (Table 3). Also, plotting ln k D against 1/T yielded the entropy (∆S # ) and enthalpy (∆H # ) of the activations of the hydrolysis reaction as 0.065 kJ mol −1 K −1 and 28.28 kJ mol −1 , respectively. The ∆H # and ∆S # values could now be used to obtain the Gibbs eneregy of activation (∆G # ) using Equation (2)

2D Co-B NS@1D TiO 2 NFs Recyclability
For any practical application, the potential to recycle the catalyst is very crucial. The depreciation that occurs in the hydrogen production rate (Yield and HGR) with the 2D Co-B NS@1D TiO 2 NFs catalyst after going through 10 reuse cycles is depicted in Figure 8. After five repetitions, the yield efficiency of the 2D Co-B NS@1D TiO 2 NFs catalyst was compared with the intra-zeolite Co(0) nanoclusters, which preserved 59% of their activities after the 5th cycle [36], and the cobalt (Co)-based thin-film catalysts preserved 14% of their activities after the 5th cycle [37]. However, after five cycles, the depreciated activity of the Co-B/Ag-TiO 2 was slightly lower than 70% [33], 64% for the Co-B-supported on N 2 -doped carbon [26], and 37.5% for Co-B-supported carbon-derived bacterial cellulose [38]. The loss of cobalt was mostly responsible for the reduction in the H 2 yield [26]. After every run, the catalyst was recovered and cleaned extensively with water to remove residuals from the catalyst's surface, resulting in the loss of some catalyst. The formation of by-products, such as NaBO 2 and B 2 O 3 , is another reason for the reduction in H 2 yield [38]. In addition, the surface oxidation of the Co-B catalyst is also a factor that contributes to the deactivation of the catalyst [26]. However, when the low price of the raw materials and the simple synthesis process of our catalyst are taken into consideration, these disadvantages become insignificant up to come extent. run, the catalyst was recovered and cleaned extensively with water to remove residuals from the catalyst's surface, resulting in the loss of some catalyst. The formation of byproducts, such as NaBO2 and B2O3, is another reason for the reduction in H2 yield [38]. In addition, the surface oxidation of the Co-B catalyst is also a factor that contributes to the deactivation of the catalyst [26]. However, when the low price of the raw materials and the simple synthesis process of our catalyst are taken into consideration, these disadvantages become insignificant up to come extent.

Preparation of 2D Co-B NS-Decorated 1D TiO2 NFs
First, we prepared a TiO2 sol by mixing 2.25 g of Polyvinylpyrrolidone (PVP, average Mw 1,300,000, 98%, Sigma Aldrich, St. Louis, MO, USA) with 8 g of acetic acid (99.5%, Beijing chemical works, Beijing, China) and 8 g of ethanol (99.5%, Beijing Chemical Works, Beijing, China). The solution was then mixed with 1.5 g of titanium isopropoxide (TIIP, 97%, Sigma Aldrich, St. Louis, MO, USA). The solution was stirred continuously overnight. After the precursor solution was stirred thoroughly at room temperature to achieve the homogenous, clear, and light-yellow solution that was needed to perform electrospinning process, the solution was loaded into a plastic syringe. The voltage applied to the syringe was 18 kV, and the tip of the syringe and the paraffin sheet collector were 16 cm apart. After this, the collected mats were separated away from the sheet and calcined at a temperature of 700 °C for a period of 2 h. Then, 1 g of electrospun TiO2 NFs was placed in a 500 mL beaker containing 100 mL of deionized water and 2 g of cobalt acetate tetrahydrate (Co(CH3COO)2, CoAc, 98%, Sigma Aldrich, St. Louis, MO, USA) to produce a cata-

Preparation of 2D Co-B NS-Decorated 1D TiO 2 NFs
First, we prepared a TiO 2 sol by mixing 2.25 g of Polyvinylpyrrolidone (PVP, average Mw 1,300,000, 98%, Sigma Aldrich, St. Louis, MO, USA) with 8 g of acetic acid (99.5%, Beijing chemical works, Beijing, China) and 8 g of ethanol (99.5%, Beijing Chemical Works, Beijing, China). The solution was then mixed with 1.5 g of titanium isopropoxide (TIIP, 97%, Sigma Aldrich, St. Louis, MO, USA). The solution was stirred continuously overnight. After the precursor solution was stirred thoroughly at room temperature to achieve the homogenous, clear, and light-yellow solution that was needed to perform electrospinning process, the solution was loaded into a plastic syringe. The voltage applied to the syringe was 18 kV, and the tip of the syringe and the paraffin sheet collector were 16 cm apart. After this, the collected mats were separated away from the sheet and calcined at a temperature of 700 • C for a period of 2 h. Then, 1 g of electrospun TiO 2 NFs was placed in a 500 mL beaker containing 100 mL of deionized water and 2 g of cobalt acetate tetrahydrate (Co(CH 3 COO) 2 , CoAc, 98%, Sigma Aldrich, St. Louis, MO, USA) to produce a catalyst referred from now onwards as 2D@1D Co-B@TiO 2 NF. To achieve complete dissolution of the CoAc, the solution was sonicated for 30 min. Later, an aqueous solution of sodium borohydride (SBH, NaHB 4 (98%), Sigma Aldrich, St. Louis, MO, USA) was introduced in drops to the aforementioned solution while keeping the molar ratio of Co and B to be 1:5 for the entire reductive reaction of CoAc. As soon as SBH was attached with the solution, a dark gray precipitate was formed. The as-prepared product was then filtered and washed with deionized water and absolute ethanol. The resulting product was then vacuum dried at 60 • C overnight. Under identical conditions, unsupported Co-B NPs were synthesized.

Characterization
Field-emission scanning electron microscopy (FESEM, Hitachi S-7400, Tokyo, Japan) was used to examine the surface morphology of the NFs that had been prepared. By the use of X-ray diffraction (Rigaku Co., Japan), we determined the crystalline structures of the catalysts as well as their crystal sizes (λ = 1.54056 Å). An investigation using X-ray photoelectron spectroscopy (XPS, AXIS-NOVA, Kratos Analytical, Manchester, UK) was carried out with the following measurement parameters: a starting pressure of 6.5 × 10 −9 Torr, a resolution (pass energy) of 20 eV, and a scan step of 0.05 eV/step.

Dehydrogenation of SBH Using 2D@1D Co-B@TiO 2 NFs
The SBH solution and the catalyst were kept in a round-bottomed flask with two necks; one was sealed with a stopper, and the other was connected to a gas burette. This apparatus was submerged in a water bath to control the reaction temperature. A thermocouple was employed to control the reaction temperature. The reactions initiated when 26 mM of alkaline aqueous solution of SBH and 5 mg of catalyst were added to a flask and stirred magnetically at 1000 rpm and 25 • C. Using the water-displacement method, the volume of gas was determined employing a gas burette at NTP. Time was recorded against the amount of evolved hydrogen. The procedure was terminated when hydrogen gas production ceased. For the sake of comparison, we also conducted the same procedure without the inclusion of any catalytic substance. All synthesized catalysts had undergone identical testing. The kinetics of SBH hydrolysis was further investigated by running the process at several concentrations of catalyst, SBH, and temperatures from 298 to 313 K. The synthesized NFs were also tested for recycle efficiency. This procedure was conducted several times using the same set of catalytic NFs to evaluate the catalyst's stability. Once the hydrolysis was complete, the catalyst was rinsed with de-ionized water, filtered, and dried under vacuum. A new 26 mM SBH was added to the regenerated catalyst in the reactor.

Conclusions
In this study, a 2D Co-B NS@1D TiO 2 NFs catalyst was synthesized employing electrospinning and chemical reduction methods. In terms of catalytic activity, the 2D Co-B NS@1D TiO 2 NFs performed well during the dehydrogenation of SBH. At 25 • C, a high HGR of 6020 mL min −1 g −1 was obtained. The kinetic analysis of the dehydrogenation process by the 2D Co-B NS@1D TiO 2 NFs catalyst showed the reaction order to be of zero order and first order with respect to the concentration of the SBH and catalyst, respectively. The activation energy Ea for the hydrolysis process was found to be 30.87 kJ mol −1 , whereas the ∆H and ∆S were calculated to be 28.28 kJ mol −1 and 0.065 kJ mol −1 K −1 , respectively. We demonstrated that the 2D Co-B NS@1D TiO 2 NFs catalyst is a promising candidate for the H 2 production via the selective catalytic dehydrogenation of SBH process because of its ease of fabrication, cheap price of the precursor, and high catalytic activities.

Data Availability Statement:
The data presented in this study are available from the corresponding authors upon reasonable request.