Nickel foam and stainless steel mesh as electrocatalysts for hydrogen evolution reaction, oxygen evolution reaction and overall water splitting in alkaline media.

In this work, several commonly used conductive substrates as electrocatalysts for hydrogen evolution reaction (HER) and oxygen evolution reaction (OER) under alkaline conditions were studied, including nickel foam (Ni foam), copper foam (Cu foam), nickel mesh (Ni mesh) and stainless steel mesh (SS mesh). Ni foam and SS mesh are demonstrated as high-performance and stable electrocatalysts for HER and OER, respectively. For HER, Ni foam exhibited an overpotential of 0.217 V at a current density of 10 mA cm-2 with a Tafel slope of 130 mV dec-1, which were larger than that of the commercial Pt/C catalyst, but smaller than that of the other conductive substrates. Meanwhile, the SS mesh showed the best electrocatalytic performance for OER with an overpotential of 0.277 V at a current density of 10 mA cm-2 and a Tafel slope of 51 mV dec-1. Its electrocatalytic performance not only exceeded those of the other conductive substrates but also the commercial RuO2 catalyst. Moreover, both Ni foam and SS mesh exhibited high stability during HER and OER, respectively. Furthermore, in the two-electrode system with Ni foam used as the cathode and SS mesh used as the anode, they enable a current density of 10 mA cm-2 at a small cell voltage of 1.74 V. This value is comparable to or exceeding the values of previously reported electrocatalysts for overall water splitting. In addition, NiO on the surface of Ni foam may be the real active species for HER, NiO and FeO x on the surface of SS mesh may be the active species for OER. The abundant and commercial availability, long-term stability and low-cost property of nickel foam and stainless steel mesh enable their large-scale practical application in water splitting. This journal is © The Royal Society of Chemistry.

Introduction

The increasing of energy demands and depleting of fossil fuels are vital challenging issues that call for the urgent discovering of alternative energy resources.[1,2] Hydrogen is considered as a promising alternative to traditional fossil fuels in the future due to its high energy density and environmental friendliness.[3] Electrochemical water splitting, which consists of two half-reactions, namely oxygen evolution reaction (OER) and hydrogen evolution reaction (HER), is an appealing technology to obtain high-purity hydrogen.[4,5] The major challenge to accomplish the two half-reactions in electrochemical water splitting is to overcome the intrinsic sluggish kinetics of HER and OER, especially of OER that arise from a complex multistep proton-coupled electron transfer process.[6,7] Currently, the state-of-the-art electrocatalysts for HER and OER are platinum (Pt) and ruthenium/iridium dioxide (RuO2/IrO2) due to their low overpotential and Tafel slope.[2,8] However, these precious electrocatalysts suffer from scarcity and high-cost that limit their large-scale practical application to generate high-purity hydrogen resource economically by water splitting. Therefore, it is important to explore earth-abundant and low-cost alternatives.[2]

In recent years, much effort has been made on the developing of inexpensive electrocatalysts for HER, OER and overall water splitting based on earth-abundant transition metals. For example, a large amount of transition metal oxides,[9-14] hydroxides,[15-18] chalcogenides,[19-22] phosphides,[23-27] sulfides[28-32] and carbides[33,34] have been explored as efficient and potential HER,[19-30,32,34] OER[9-18,25-31,33] and overall water splitting electrocatalysts[25,26,28-30] for the replacement of precious catalysts. To study the electrocatalytic activity of these catalysts, the first step is to load the catalyst on a conductive substrate either by directly grown or by coating via adhesives (such as Nafion). For instance, Li and co-workers prepared 3D urchin-like Co3O4 by directly grown on nickel foam and studied its OER, HER and overall water splitting performance.[35] Telli and co-workers deposited iron and copper electrochemically on nickel mesh and studied its the catalytic performance of HER.[36] Jiang and co-workers coated CoMo@NC on glassy carbon electrode (GCE) to study its HER, OER and the catalytic performance of overall water splitting.[37] Chen and co-workers growned NiS on stainless steel mesh and studied the catalytic performance of OER.[38] Fan and co-workers directly growned single nanocrystalline tungsten carbide (WC) on vertically aligned carbon nanotubes and studied its catalytic performance of HER.[39] Leem and co-workers deposited Ni(cyclam)-BTC on indium tin oxide (ITO) and studied the catalytic performance of OER.[40] Yang and co-workers directly growned CoP nanosheet on carbon cloth and studied its catalytic performance of HER.[41]

However, the above mentioned studies only employed nickel foam, stainless steel mesh, etc. as conductive substrates, i.e. catalyst support, and the systematic study of the electrocatalytic performance for HER and OER of these commonly used conductive substrates has been rarely reported.[4,42] In this work, several commonly used conductive substrates, including nickel foam, copper foam, nickel mesh and stainless steel mesh were studied as electrocatalysts for hydrogen evolution reaction, oxygen evolution reaction under alkaline conditions. It was demonstrated that Ni foam and Ni mesh showed better HER activity and the SS mesh showed the best OER performance. The Ni foam requires relatively low overpotential of 0.217 V to produce a current density of 10 mA cm−2, and the SS mesh shows a current density of 10 mA cm−2 at a small overpotential of 0.277 V for the OER. At the same time, Ni foam and SS mesh showed long-term stability of the HER and OER, respectively. Furthermore, in the two-electrode system with the SS mesh used as anode and Ni foam used as cathode, they enable a current density of 10 mA cm−2 at a small cell voltage of 1.74 V, which is comparable to or even better than some reported bifunctional water-splitting catalysts. Because Ni foam and SS mesh can be commercially available with low price that conferring their large-scale application in the production of hydrogen economically by electrochemical water splitting.

Experimental section

Materials

Potassium hydroxide (KOH) was purchased from Shanghai Titan Scientific Co., Ltd. Hydrochloric acid (HCl) and absolute ethanol were purchased from Chengdu Kelon Chemical Reagent Factory. Nafion solution (5 wt%) purchased from Suzhou Yilong Energy Technology Co., Ltd. 20 wt% platinum carbon (Pt/C) purchased from Kunshan Yierwei International Trade Co., Ltd. Ruthenium oxide (RuO2) was purchased from Adamas. All chemicals were used as received without further purification. All electrolyte solutions were prepared with distilled water unless otherwise stated. Ni foam, SS mesh and Cu foam were obtained from Changde Liyuan New Materials Co., Ltd. ITO was purchased from Shenzhen Hua Nanxiang Technology Co., Ltd. Ni mesh was purchased from Anping Kangwei Metal Wire Mesh Co., Ltd. Pt electrode, Ag/AgCl electrode and GCE were purchased from Wuhan Gaoshi Ruilian Technology Co., Ltd.

Characterization

The powder X-ray diffraction (XRD) measurements were recorded on a Rigaku Dmax/Ultima IV diffractometer with monochromatized Cu Kα radiation (λ = 1.5418 Å). The morphologies were observed by scanning electron microscopy (JSM-6530LV, Rigaku Japan). The surface composition and electronic structure were examined by X-ray photoelectron spectroscopy (XPS) on a ThermoFisher K-Alpha XPS spectrometer equipped with an Al Kα X-ray source.

Electrochemical measurements

Electrochemical measurements were performed on an electrochemical workstation (CHI 760E, CH Instruments Inc, Shanghai) using a typical three-electrode setup with an electrolyte solution of 1 M KOH, a Pt wire as the counter electrode, a Ag/AgCl electrode as the reference electrode, and a conductive substrate with geometric area of 1 cm2 was employed as the working electrode. The working electrode was prepared as follows: firstly, the conductive substrate (1 cm2) (except ITO and GCE) was completely immersed in 3 M HCl for 15 min to well clean the surface, then washed with distilled water to insure the undefiled surface, and finally dried at room temperature. 5 mg of Pt/C (or RuO2) and 10 μL of Nafion were ultrasonically dispersed in 1 mL of mixture solution of water/alcohol (v/v 3 : 1) for 30 min. 5 μL of the dispersion was deposited on GCE (d = 3 mm) and dried naturally.

All potentials measured were converted to the reversible hydrogen electrode (RHE) based on the following formula: ERHE = EAg/AgCl + 0.197 V + 0.059pH.[43] Linear sweep voltammetry (LSV), cyclic voltammetry (CV), electrochemical impedance spectroscopy (EIS) and chronopotentiometry (CP) were carried out in 1 M KOH solution. Tafel slope was modeled by the empirical Tafel equation: η = a + b × log|j|,[26] where η is the overpotential, j is the measured current density, b is the Tafel slope, and a is the constant. Electrochemical impedance spectroscopy (EIS) was measured with an amplitude of 5 mV. Without specification, all the potentials are referred to the RHE.

Results and discussion

Characterization of materials

The crystalline phases of these conductive substrate samples were analyzed by XRD. The Ni foam and Ni mesh have similar peaks that centered at about 44.5°, 51.9° and 76.4° (Fig. 1, curves a and b), which can be indexed to the (111), (200) and (220) planes of nickel (PDF #04-0850). The Cu foam shows three peaks at 43.3°, 50.4° and 74.1° (Fig. 1, curve c), which are attributed to the (111), (200) and (220) planes of copper (PDF #04-0836). The distinctive diffraction peaks at 43.6°, 50.9° and 74.7° (Fig. 1, curve d) are corresponding to the (111), (200) and (220) planes of austenite (PDF #33-0397).

Fig. 1

The XRD patterns of Ni foam, Ni mesh, Cu foam and SS mesh before use.

The morphologies of these conductive substrate samples were measured by scanning electron microscopy (SEM). The low magnification SEM images show that the Ni foam and SS mesh have 3D skeleton morphology and 2D structure, respectively (Fig. 2A and C). Both of which possess rough surfaces (Fig. 2B and D). The morphologies of Cu foam and Ni mesh are similar to that of Ni foam and SS mesh, respectively (Fig. S1†).

Fig. 2

The SEM images of Ni foam (A and B) and SS mesh (C and D) before use at low and high magnification.

The chemical binding state and elemental composition of the Ni foam and SS mesh were investigated by XPS. The survey XPS spectrum of Ni foam contains Ni, C and O elements (Fig. S2A†), and the SS mesh mainly contains Fe, Cr, C and O elements (Fig. S2B†). Fig. 3A shows the high resolution Ni 2p XPS of Ni foam. The peaks at binding energies of 873.6 and 855.6 eV can be assigned to Ni 2p1/2 and Ni 2p3/2 of NiO, respectively.[44] The satellite peak at around 879.5 eV and 861.2 eV are two shake-up type peaks of nickel at the high binding energy side of the Ni 2p1/2 and Ni 2p3/2 edge.[45] The small peak at about 852.1 eV is ascribed to Ni 2p3/2 of the metallic Ni.[46] It is worth pointing out that the XPS peak for metallic Ni is much weaker than that of NiO, similar phenomenon was also observed in previous publications.[47] This indicated that the surface of Ni foam was oxidized before XPS measurement. Fig. 3B shows the high resolution Fe 2p XPS spectrum of SS mesh. It can be seen that there are five peaks at binding energies of 706.4, 709.9, 712.1, 722.9 and 724.8 eV, which can be assigned to Fe 2p3/2 and Fe 2p1/2, respectively. The position of these primary peaks is consistent with that of the core-level XPS spectrum of metallic Fe, FeO and Fe2O3. The peaks at 706.4 is Fe0 2p3/2, the peaks at 709.9 and 722.9 eV are assigned to the Fe 2p3/2 and Fe 2p1/2 of FeO.[48] While the peaks at 712.1 and 724.8 eV are assigned to the Fe 2p3/2 and Fe 2p1/2 of Fe2O3.[48,49] The other elements, such as Cr, Si and Mn were not displayed obviously in the survey spectrum, but clearly observed in the high resolution XPS spectra (Fig. S2†).

Fig. 3

The high resolution XPS spectra of (A) Ni 2p of Ni foam; (B) Fe 2p of SS mesh before use.

HER performances

The electrocatalytic activity of these conductive substrates for HER was evaluated by linear sweep voltammetry (LSV) in a standard three-electrode system. The HER polarization curves were recorded by LSV at the slow scan rate of 2 mV s−1 to minimize the diffusion limitations and capacitive current interference. For comparison, the electrocatalytic performances of commercial Pt/C, commonly used GCE and ITO were also measured under the same conditions. Fig. 4A shows the polarization curves of all these materials. The commercial Pt/C catalyst has the best HER activity and provided a near zero onset potential, while the current density of GCE and ITO do not show obvious increase in the potential range of 0 to −500 mV, indicating their low electrocatalytic activity towards HER. The Ni foam exhibits an onset potential of about −120 mV, and achieves the overpotential of 217 mV at the current density of 10 mA cm−2, 292 mV at 30 mA cm−2 and 341 mV at 50 mA cm−2. Although the Ni mesh gave a similar onset potential to Ni foam, it needed a higher overpotential of 275 mV to obtain a current density of 10 mA cm−2. Whereas, the Cu foam and SS mesh required an even higher overpotential of 372 and 420 mV, respectively, to achieve the current density of 10 mA cm−2. Even though the electrocatalytic performance of Ni foam is not as good as that of Pt/C catalyst, it was substantially comparable to or even better than some reported electrocatalysts that prepared in laboratory by researchers (Table S1†). Tafel slope was determined by fitting the linear regions of Tafel plots to the Tafel equation. The Tafel slope of Ni foam was 130 mV dec−1, smaller than that of Ni mesh, Cu foam and SS mesh, suggesting its fast kinetic process.

Fig. 4

(A) LSV curves measured at 2 mV s−1 in 1 M KOH solution for HER and (B) the corresponding Tafel slopes; (C) Nyquist plots of EIS of samples from 105 Hz to 0.1 Hz with an amplitude of 5 mV; (D) chronopotentiometric curves at different current density; (E) LSV curves obtained with Ni foam before and after 2000 cycles of an accelerated stability test.

EIS was measured to gain further insight in the kinetics at the interface of the catalyst and electrolyte. Rct is well-correlated to electrocatalytic kinetics, arising from the charge transfer resistance at the interface between the catalyst and the electrolyte. It is generally accepted that small Rct values give rise to rapid charge transfer kinetics.[26]Fig. 4C shows the Nyquist plots of Ni foam, Ni mesh, Cu foam and SS mesh. The Rct of Ni foam was estimated to be about 25 Ω from the diameter of semicircle, which was smaller than that of Ni mesh, Cu foam and SS mesh. The small Rct of Ni foam suggested the fast kinetics in HER, which is in accordance with the Tafel slope and LSV results.

Since the long-term cycling stability is also an important factor in assessing an electrocatalyst, the stability of Ni foam was first evaluated by chronopotentiometry (CP) in 1 M KOH solution at constant current density of −10, −30 and −50 mA cm−2 for 20 h, respectively. As shown in Fig. 4D, the potential increase is negligible, indicating that Ni foam has excellent stability in alkaline conditions. To further confirm the excellent stability of Ni foam, continuous CV measurement was performed in the range of −0.3 to 0 V at 100 mV s−1 for 2000 cycles. As can be seen in Fig. 4E, the LSV curve of Ni foam after 2000 cycles of CV measurement was still similar to the first cycle. These results undoubtedly indicated that the Ni foam has excellent catalytic activity and stability for HER. In addition, after the stability test, the XRD pattern (Fig. S4†), SEM images (Fig. S1E and F†) and XPS spectrum (Fig. S5†) of Ni foam was conducted, a comparative XRD and SEM study of Ni foam indicates no obvious change before and after the HER process. The XPS data after the stability test showed that the metallic nickel on the surface of the Ni foam was oxidized to NiO, indicating that NiO is the active substance of hydrogen evolution reaction.

OER performances

To study the bifunctional catalytic activity of all substrates, we also tested their OER activity by LSV with a standard three-electrode system. Fig. 5A shows the LSV curves for OER at a scan rate of 2 mV s−1 in 1 M KOH solution. The polarization curve of Ni foam has a distinct oxidative peak at 1.37 V versus RHE, which is attributed to the oxidation of Ni species.[50] Different from the activity order of HER, the Ni foam presents the relatively poor OER activity, it achieved the overpotential of 337 mV at the current density of 10 mA cm−2. At the same time, the current density of GCE and ITO did not show obvious increase in the potential range of 1.23 to 1.8 V, the Cu foam and Ni mesh required a even higher overpotential of 464 and 491 mV, respectively, to achieve the current density of 10 mA cm−2, indicating their low electrocatalytic activity towards OER. Contrary to HER, the SS mesh exhibits the highest OER activity among these substrates studied. It achieved the current density of 10, 30 and 50 mA cm−2 at potential of 1.507, 1.556 and 1.597 V, respectively. Note that the OER activity of SS mesh is even better than that of RuO2. RuO2 achieved the overpotential of 303 mV at the current density of 10 mA cm−2, while the SS mesh producing a current density of 10 mA cm−2 at an overpotential of 277 mV. The overpotential values compare favorably with the behavior of most previously reported materials for OER (Table S2†). Since the electrocatalytic reaction current is directly proportional to the oxygen yield, the higher current density here indicates prominent oxygen evolution behavior of SS mesh, highlighting its excellent performance for OER. Fig. 5B shows the Tafel plots of various substrates. The Tafel slope of SS mesh is 51 mV dec−1, which is the smallest among these catalysts, implying its best catalytic performance in OER.

Fig. 5

(A) The LSV curves measured at 2 mV s−1 in 1 M KOH solution for OER and (B) the corresponding Tafel slopes; (C) chronopotentiometric curves at different current density; (D) LSV curves obtained with SS mesh before and after 2000 cycles of an accelerated stability test.

The long-term stability of the electrocatalyst is another important criterion for practical applications. In order to detect the durability of the SS mesh in an alkaline environment, we tested the cycling stability of SS mesh in 1 M KOH solution. The stability test was performed by chronopotentiometry at a series of constant current density of 10, 30 and 50 mA cm−2. As shown in Fig. 5C, the operating potentials of SS mesh are nearly constant, the potential increase of was only about 10 mV with 20 h chronopotentiometry test, indicating the excellent stability of SS mesh. Then, the stability was further estimated by the continuous CV measurements, which were performed at a scan rate of 100 mV s−1 in the range from 1.4 to 1.6 V for 2000 cycles, its attenuation is negligible, verifying its excellent stability. The XRD patterns (Fig. S4†) and SEM images (Fig. S1G and H†) after the stability test were consistent with the original crystal phases and morphologies. The XPS (Fig. S6†) measurement after the OER stability test showed that the surface of the SS mesh changed to some degree after OER performance. Both Fe and Ni elements were existed as FeO and NiO (Fig. S6 and ESI for details†). According to the experimental results and the earlier studies,[51,52] the FeO, Fe2O3 and NiO on the surface of SS mesh was proposed to be the active species for oxygen evolution reaction.

Moreover, EIS investigations were conducted to further explore the OER kinetics in catalysis. As shown in Fig. S3B,† the SS mesh has relatively lower charge transfer resistance for OER, indicating its faster electron transfer rate during the OER process. This further suggests that SS mesh is more advantageous for OER.

On the basis of the excellent HER performance of Ni foam and the OER performance of SS mesh in alkaline solution, we further studied their catalytic performance for overall water splitting in a two-electrode system by using Ni foam as cathode and SS mesh as anode. As shown in Fig. 6A, the obvious hydrogen and oxygen bubbles are formed on Ni foam and SS mesh, respectively, in 1 M KOH solution. Fig. 6B shows the LSV polarization curve of SS mesh (+)‖Ni foam (−). A current density of 10 mA cm−2 can be achieved with a cell potential of 1.74 V, which is comparable to or even better than many other reported bifunctional water-splitting catalysts (Table S3†). Furthermore, as shown in Fig. 6C, the potential difference (ΔV) at 10, 30 and 50 mA cm−2 between HER and OER was 1.73, 1.85 and 1.94 V, respectively, which are very close to the actual measured values of 1.74, 1.86 and 1.93 V (Fig. 6B), indicating the steady-state performance of the HER, OER and overall water splitting process.

Fig. 6

(A) Optical photograph of the generation of hydrogen and oxygen bubbles on Ni foam and SS mesh; (B) polarization curve in a two-electrode system with SS mesh (+)‖Ni foam (−); (C) polarization curves of SS mesh for OER and Ni foam for HER.

Conclusions

In summary, we investigated several commonly used conductive substrates as electrocatalysts for HER and OER under alkaline conditions. The electrochemical measurements revealed that Ni foam shows the best catalytic activity for HER and SS mesh shows the best catalytic activity for OER. The OER activity of SS mesh is even better than that of commercial RuO2 catalyst. Both Ni foam and SS mesh showed excellent stability as tested by chronopotentiometry. Furthermore, the assembled SS mesh (+)‖Ni foam (−) system for water splitting afforded a current density of 10 mA cm−2 at a small cell voltage of 1.74 V. This work provides a feasible way for the production of hydrogen economically by electrochemical water splitting with inexpensive and commercial available Ni foam and SS mesh as cathode and anode electrocatalysts.

Conflicts of interest

There are no conflicts of interest to declare.