Open Access Article
This Open Access Article is licensed under a Creative Commons Attribution-Non Commercial 3.0 Unported Licence

Inexpensive electrochemical synthesis of nickel iron sulphides on nickel foam: super active and ultra-durable electrocatalysts for alkaline electrolyte membrane water electrolysis

Pandian Ganesan , Arumugam Sivanantham and Sangaraju Shanmugam *
Department of Energy Systems and Engineering, Daegu Gyeongbuk Institute of Science & Technology (DGIST), 50-1 Sang-Ri, Hyeongpung-Myeon, Dalseong-gun, Daegu, 42988, Republic of Korea. E-mail:

Received 30th May 2016 , Accepted 15th September 2016

First published on the web 16th September 2016

Efficient and durable electrocatalysts for water splitting (both the oxygen evolution reaction (OER) and hydrogen evolution reaction (HER)) are required for the replacement of expensive noble metal-based catalysts used in water electrolysis devices. Herein, we describe the inexpensive synthesis of electrochemically deposited nickel iron sulphides on nickel foam (NiFeS/NF) and their use as highly efficient bi-functional water splitting catalysts that can meet the current energy demands. The NiFeS/NF electrocatalysts exhibited low overpotentials of approximately 231 mV for the OER and 180 mV for the HER in 1 M KOH. Moreover, the NiFeS/NF electrocatalysts exhibited a turnover frequency of one order of magnitude higher than those of state-of-the-art noble metal catalysts (RuO2 and Pt/C) for the OER and HER. In addition to this excellent activity, the bi-functional catalyst also exhibited an outstanding OER and HER electrode stability for over 200 h with minimal loss in activity. Further, it can be directly used in the practical application of alkaline electrolyte membrane water electrolysis. The high performance, prolonged electrode stability, and facile synthesis as an adherent coating on nickel foam suggest that NiFeS/NF electrocatalysts might be suitable for use as alternative commercially viable catalysts.


The production of clean hydrogen through water splitting is a sustainable way of generating renewable energy.1–5 Hydrogen production through polymer electrolyte membrane (PEM) water splitting does not produce CO2 emissions if the electricity is derived from a renewable source (e.g., wind, solar), but it must be sufficiently efficient and inexpensive to compete with hydrogen production from steam reforming of fossil fuel sources.4,6–8 The efficiency of a water electrolyzer system is limited, in part, by the kinetic overpotential losses associated with driving the oxygen evolution reaction (OER) at the anode and the hydrogen evolution reaction (HER) at the cathode under both acidic and basic environments.9–12 Solar water splitting also provides the ability to integrate a photovoltaic device (for energy conversion) and an electrolyzer (for energy storage) within a single device, thereby further lowering the cost of hydrogen production.3

The Department of Energy has stated that the levelized hydrogen plant production cost using green energy, in terms of gallon gas per equivalent (gge) of H2, must decrease from $3 in 2015 to $2 in 2020. Of the total cost of constructing a water electrolyzer, 41% of the expense in MEA assembly arises from making a better stack of the PEM water electrolyzer.13,14 Hence, a cost-effective way of preparing a catalyst that is supported directly on the MEA without an additional current collector would decrease the contact resistance and improve the performance. Nickel current collectors are used widely in PEM water electrolyzers because of their high activity and stability in alkaline media.7,8,15 Although many OER and HER catalysts have been reported, nickel and iron alloys are among the most highly active in alkaline environments and also exhibit good stability with high current densities (up to 100–500 mA cm−2).9,10,15 The role of iron in a NiFe alloy is to prevent the nickel from electrode corrosion during prolonged electrochemical operation in alkaline environments.8,16 Several nickel and iron-based materials (e.g., NiFe/NF, Fe–Ni3S2/NF, Ni3S2/NF, NiFeO2, nickel iron oxyhydroxide and cobalt phosphides) have been reported recently for use as water splitting catalysts.9,10,15,17–27 Although nickel sulphides and selenides on nickel foams (NFs) have been prepared as OER and HER catalysts, they require high overpotentials to afford high current densities and exhibit very poor long-term durability.15,20,25–28 To the best of our knowledge, nickel iron sulphides grown directly on NF for both the OER and HER with long-term durability in alkaline media have not been reported previously.

Herein, we describe the inexpensive synthesis of electrochemically deposited nickel iron sulphides (NiFeS/NF) supported on NF (Fig. 1). Our NiFeS/NF electrocatalyst is highly stable in alkaline environments for a long time, functions with low overpotentials of 231 and 180 mV for the OER and HER, respectively and affords very high current densities for long-term OER and HER activity. Its performance is much better than that of the metal sulphides (e.g., Fe11.8%Ni3S2/NF, NiS/Ni foam, NiFe LDH/NF) reported previously; in addition, the synthesized NiFeS/NF is practically applicable to alkaline membrane full water splitting devices. The NiFeS/NF catalyst also exhibits performance close to that of state-of-the-art noble catalysts (e.g., Pt/C, RuO2).

image file: c6ta04499a-f1.tif
Fig. 1 Schematic illustration of electrochemical deposition of nickel iron sulphides on nickel foam: (a) nickel iron deposition on nickel foam and (b) sulphide deposition on nickel iron foam.

Experimental section

Materials and methods

Nickel foam (NF, thickness: 1.6 mm) and stainless steel (304 grade, thickness, 0.25 mm) were purchased from MTI Korea Ltd. Nickel chloride, iron chloride nonahydrate, and thiourea were purchased from Alfa Aesar. The nickel iron sulphides were characterized using X-ray diffraction (XRD) for phase confirmation. XRD measurements were carried out using the X-ray diffractometer (Rigaku, MiniFlex 600) with CuKα radiation (1.5418 Å). The morphology of the samples was examined by using a field-emission scanning electron microscope (FE-SEM, Hitachi, S-4800II, 3.0 kV). Before the SEM observation, the samples were sputtered with osmium coating. The transmission electron microscopy (TEM) measurements were made using a Hitachi HF-3300, 300 kV instrument. The nickel iron sulphides were dispersed in isopropanol by sonication in an ultrasonic agitator for 30 min to peel off the deposited nickel iron sulphide film from the Ni foam; a drop of the solution was dispersed on a copper grid, dried under an UV lamp and subjected to TEM measurements. X-ray photoelectron spectroscopy (XPS) measurements were performed using a Thermo-scientific, ESCALAB 250Xi model in an ultrahigh vacuum of 10−9 mbar.

Synthesis of NiFe/NF

First, the NF was sonicated in 3 M HCl solution for 10 min to remove any NiOx layer present on the surface, subsequently washed thoroughly with water and ethanol, and then dried in air. The electrodeposition was carried out using NF as the working electrode, a platinum wire as the auxiliary electrode and Ag/AgCl (3 M KCl) as the reference electrode. The analyte solution consists of 3 mM Ni(NO3)2·6H2O and 3 mM Fe(NO3)3·9H2O. Chronoamperometry was then carried out at −1.0 V at 10 °C. The deposition was varied for 2.5 and 5 min, and the deposited samples were labelled as NiFe-1 and NiFe-2, respectively (Fig. 1a). The optimized deposition time of NiFe on NF was found to be 2.5 min. After deposition, the nickel foams were carefully withdrawn from the electrolyte, rinsed with water and ethanol, then sonicated in ethanol and left to dry in air.29 The iron deposited on the nickel foam was heat treated to 500 °C in an argon atmosphere for 5 h (Fig. S1a).

Synthesis of NiFeS/NF

The deposition of nickel and sulphide on the NiFe/NF, nickel foam, and for a control sample, the deposition also made on stainless steel electrodes were performed through cyclic voltammetry (CV) using the analyte of 50 mM NiCl2·6H2O and 1 M thiourea (TU). The three-electrode setup featured NF or the NiFe/NF substrate as the working electrode, saturated Ag/AgCl as the reference electrode, and a Pt wire as the counter electrode and was monitored using a computer-controlled potentiostat (Bio-Logic) electrochemical analyzer. CV was performed by sweeping between −1.2 V and +0.2 V at a scan rate of 5 mV s−1 for 15 sweep cycles (Fig. 1b). After electrodeposition, the as-deposited electrodes were rinsed with deionized water and dried for 12 h in a vacuum oven at 60 °C.30 During the cyclic voltammetric deposition of sulphide on the NiFe-1/NF electrode, the Ni(Thiourea)22+ intermediate is formed during the oxidative potential sweep (eqn (1)) and Ni(Thiourea)22+ reduces and forms nickel iron sulphide (Ni2FeS4) on the NiFe-1/NF electrode surface (eqn (2)) as previously reported for cobalt sulphide31 (Fig. S1b). Hence, the coating thickness was due to the total coating of the nickel iron sulphide (Fig. S3a).
Ni2+ + 2thiourea → Ni(Thiourea)22+(1)
Ni(Thiourea)22+ + NiFe → Ni2FeS4(2)

The products from the deposition of sulphide on NiFe-1/NF, NiFe-2/NF, and NF are named herein NiFeS-1/NF, NiFeS-2/NF, and Ni3S2/NF, respectively. The thickness of the film coating of NiFeS-1 on NF was measured to be 2.71 μm (Fig. 1b). The NiFeS-1/NF heat treated to 500 °C in an Ar atmosphere exhibited a clear phase of Ni2FeS4 (Fig. S1b) and also the cyclic voltammetric deposition of nickel and sulphide on the stainless steel foil was achieved (Fig. S1c).

Electrochemical measurements

The electrochemical activities of all nickel foams were evaluated using linear sweep voltammetry (LSV) in an Ar-saturated atmosphere for the hydrogen evolution reaction (HER) and without saturation for the oxygen evolution reaction (OER) at a scan rate of 10 mV s−1 using a computer controlled potentiostat (Bio-Logic) with a typical three-electrode system. The working electrode was immersed in a glass cell containing 1 M KOH aqueous electrolyte. A platinum coil and saturated calomel electrode (SCE) served as counter and reference electrodes, respectively. In order to compare the OER and HER activities, the commercial Pt/C (40%) and RuO2 catalysts were used. The catalyst ink was prepared using five milligrams of the catalyst dispersed in a mixture consisting of 160 μL of isopropanol, 30 μL of DI water and 10 μL of Nafion solution and the contents were dispersed by ultrasonication for approximately 30 min to obtain a homogeneous suspension. The catalyst ink (1.5 μL) was drop cast onto the surface of a glassy carbon disk (working electrode, 0.07 cm2) and dried at room temperature. All potentials reported in this work were converted from the SCE to the RHE scale using ((RHE) = E(SCE) + 1.030 V) in 1 M KOH. The LSV of all nickel foam electrodes was characterized by electrochemical impedance spectroscopy (EIS) in the frequency range of 200 to 100 mHz at 0 V to calculate iR correction, transfer resistance, and double layer capacitance. The iR correction was calculated based on the solution resistance and is about 2.25 ohm, obtained from the EIS. The sulphide coating thickness and weight of NiFeS-1/NF were calculated using a Mitutoya screw gauge (5477300) and an OHAUS microbalance (PAG214C model), respectively.

Preparation of MEA

NiFeS-1/NF is used as the anode and cathode prepared by the electrochemical deposition with 1.5 cm2 nickel foams (Fig. S2a & b). The assembly was made with stainless steel electrodes (Fig. S2c & d) and the Fump Sep alkaline membrane (Tokuyama, A201) which was pre-treated with 1 M KOH for 24 h and then washed with DI water and then used for MEA assembly. The fuel cell equipment from the Heliocentric device (Germany) was used as the PEM water electrolyzer.

Results and discussion

Structure and morphology analysis

Fig. 2 displays XRD patterns for the NF, NiFe-1/NF and NiFeS-1/NF electrocatalysts. In the low-intensity region, NiFe-1/NF appeared to be amorphous with a peak shift of only 0.26° for the nickel substrate peak. The XRD patterns were analysed before and after heat treatment of NiFe-1/NF. Unlike the as-deposited, the heat treated NiFe-1/NF exhibits the NiFe phase (PDF no. 00-012-0736) with a nickel to iron ratio of ∼1[thin space (1/6-em)]:[thin space (1/6-em)]1 (Fig. S1a). This behaviour explains the effect of iron on nickel in NiFe-1/NF. In contrast, the XRD pattern of NiFeS-1/NF featured (220), (533), (400), and (800) diffraction patterns indicative of the formation of a Ni2FeS4 phase (PDF no. 00-047-1747). These peaks were, however, less intense than those of the NF substrate, due to the deposition only on the nickel surface (Fig. 1b). The remaining peaks were less prominent than those of the nickel substrate, due to the minimum diffraction of X-rays and amorphous nature of the iron deposited in the first deposition step (Fig. 1a).29 Further, the NiFeS-1/NF heat treated to 500 °C in an Ar atmosphere shows the clear phase of Ni2FeS4 compared to the as-synthesised NiFeS-1/NF which evidences that the iron was not present in the bottom layer or separate coating, instead the iron exists as a nickel iron sulphide composite (Fig. S1b). In addition, we have carried out a control experiment to understand the influence of the substrate, and cyclic voltammetric deposition of nickel and sulphide on the stainless steel (SS304) foil was also performed. The XRD analysis (Fig. S1c) of this product exhibits a NiS phase (PDF no. 01-075-0612). This observation clearly explains the involvement of iron in the sulphide deposition exclusively. And also the cyclic voltammetric deposition on NiFe-1/NF without thiourea in the analyte was also performed and the XRD phase analysis reveals (Fig. S3b) the peaks of NiO (PDF no. 03-0652865). This clearly confirms that in the presence of thiourea, the metal oxide formation is least probable. In addition, we indexed the XRD pattern of the electrodeposited nickel sulphide to Ni3S2 (PDF no. 01-074-1336) in the absence of the iron impurity,30,32,33 as displayed in Fig. S4; it was entirely different from the Ni2FeS4 phase observed for the NiFeS-1/NF sample. In Fig. 3a, the SEM image reveals the film thickness of NiFeS-1 to be about 2.71 μm on NF; Fig. 3b reveals the nano-honeycomb structure of NiFeS-1 on NF. The NiFeS-2/NF sample possessed a morphology similar to that of NiFeS-1/NF (Fig. S5a and b). The elemental SEM-EDS analysis was carried out on the upper, middle and bottom region of the NiFeS-1 layer on NF as shown in Fig. S6a and the corresponding ratio of nickel, iron, and sulphur is listed in Table S1. The nickel, iron and sulphur in the upper coating (Fig. S6b) is about 96.06, 2.29 and 1.65%, respectively, the middle coating contains (Fig. S6c) about 96.24, 2.70 and 1.06% of nickel, iron, and sulphur, respectively and the bottom coating (Fig. S6d) contains about 96.60, 2.44 and 1.10% of nickel, iron, and sulphur, respectively. From Table S1, it was obvious that throughout the coating of NiFeS-1/NF, the ratio of nickel, iron, and sulphur content was almost equal. This observation reveals the fact that iron exists uniformly throughout the catalyst layer. The TEM image in Fig. 3c confirmed the honeycomb structure of NiFeS-1/NF with vein-like projections on the surface of the catalyst. The high-resolution TEM image in Fig. 3d reveals fringe widths of approximately 2.36 and 1.44 nm that correspond to the (400) and (533) planes, respectively, of the Ni2FeS4 phase in NiFeS-1/NF, confirming the presence of nickel, iron, and sulfur atoms as a composite. The TEM elemental mapping (Fig. S7) confirmed the presence of nickel, sulfur, and iron atoms in the NiFeS-1/NF honeycomb with surface-adsorbed oxygen (Fig. S7a–f).
image file: c6ta04499a-f2.tif
Fig. 2 XRD patterns of NiFeS-1/NF, NiFe-1/NF and NF electrodes.

image file: c6ta04499a-f3.tif
Fig. 3 SEM images: (a) low magnification of NiFeS-1 coating on NF, (b) high magnification distribution. (c) TEM and (d) HR-TEM images of the NiFeS-1 nanosheet detached from the surface of the NF.

XPS analysis

We recorded XPS spectra to examine the chemical environment of NiFeS-1/NF and NiFe-1/NF. The XPS discussion of NiFe-1/NF (details in ESI section 3) exhibits metallic nickel and iron along with adsorbed hydroxides (Fig. S8). The XPS spectra of fresh NiFeS-1/NF (Fig. 4a) featured a Ni3+ 2p3/2 peak at 858.5 eV, suggesting that nickel atoms may have been bonded to both iron and sulfur atoms.32 Moreover, the signal near 861.8 eV indicated the presence of an oxidation state of Ni2+ relevant to nickel sulphide,1,17,33 but there was a shift of 0.3 eV from the characteristic Ni–S oxidation states, possibly because of the incorporation of iron atoms. The main signal at 856.3 eV, with its satellite peak at 864.3 eV, revealed the presence of surface-adsorbed nickel oxide.7,19,34 Taken together, these features are consistent with the presence of a NiFeS film in the NF. Signals for metallic nickel in the range of 852.0–856.0 eV were absent for NiFeS-1/NF,33 suggesting that all of the nickel atoms on the NiFe-1 surface were completely converted into NiFeS without any impurities. The Fe 2p3/2 spectrum (Fig. 4b) of fresh NiFeS-1/NF featured a signal at 725.2 eV characteristic of the oxidation state of the nickel iron sulphide composite.19 Signals at 706.7 and 719.2 eV revealed that some of the iron atoms in this structure were in the Fe(0) oxidation state;8,20 signals at 710.3 and 715.4 eV revealed that some of the iron atoms also existed as FeO in the +2 oxidation state.10,35Fig. 4c displays the S 2p spectra, the characteristic signal appeared at 169.9 eV (ref. 19) for the oxidation state of nickel iron sulphide and also the characteristic oxidation state of a metal disulphide peak at 162.5 eV, suggesting that existence of nickel, iron and sulfur atoms may have been bonded together as Ni2FeS4.35,36 The signal at 164.2 eV confirmed the presence of surface oxygen adsorbed Ni–S on the nickel surface; the presence of surface oxygen was further evidenced by the sulfoxide peak at 165.6 eV.35–37 Although sulfate and sulfite peaks were present at 168.8 and 171.5 eV, respectively, the intensity of the sulfur oxidation peak at 169.9 eV, relevant to the nickel iron sulphide composite, was much higher than those of the others, consistent with the composite having the Ni2FeS4 phase, as determined from the XRD pattern.19,35,36
image file: c6ta04499a-f4.tif
Fig. 4 XPS spectra of (a) nickel (Ni 2p), (b) iron (Fe 2p) and (c) sulphur (S 2p) of the fresh NiFeS-1/NF electrode.

Electrochemical activity

To examine the OER behavior of NiFeS-1/NF, NiFe-1/NF, Ni3S2/NF, and RuO2, LSV was performed between 1.0 and 1.9 V vs. RHE in 1 M KOH. To achieve a current density of 100 mA cm−2, the NiFeS-1/NF, NiFe-1/NF, and Ni3S2/NF catalysts required overpotentials of approximately 231, 371, and 491 mV, respectively (Fig. 5a). Similarly, we recorded OER linear sweep voltammograms for NiFeS-2/NF and NiFe-2/NF, our examined catalysts; the activity of NiFeS-1/NF was greater than that of NiFeS-2/NF because it required the lowest overpotential (ca. 231 mV) to achieve a current density of 100 mA cm−2 (Fig. S9a). When comparing the Ni3S2/NF, NiFe-1, and NiFe-2 alloys, NiFeS-1/NF displayed the greatest OER performance. Notably, RuO2, one of the best precious metal bi-functional water oxidation catalysts, requires a large overpotential of 461 mV to afford a current density of 100 mA cm−2 (Fig. 5a). The OER Tafel slopes for NiFeS-1/NF, NiFe-1/NF, and Ni3S2/NF were 55, 74, and 97 mV dec−1, respectively (Fig. 5b); the Tafel slope for RuO2 was 103 mV dec−1 (Fig. 5b). Thus, the lowest Tafel slope was that for NiFeS-1/NF, indicative of facile electrode kinetics, possibly due to the formation of an active phase during the reversible oxidation of nickel iron sulphide to nickel iron oxy-sulphide.38 In general, the metal chalcogenides follow the reaction steps based on their corresponding metal oxide analogues.39
McatOH → McatOH + e(3)
McatOH + OH → McatO˙ + H2O(4)
McatO˙ → SO + e(5)
2SO → 2S + O2(6)

image file: c6ta04499a-f5.tif
Fig. 5 (a) The OER polarisation curves and (b) the corresponding Tafel slopes of NiFeS-1/NF, NiFe-1/NF, Ni3S2/NF and RuO2. (c) OER mass activity of NiFeS-1/NF, NiFe-1/NF and Ni3S2/NF.

The adsorption of hydroxide on the catalyst surface plays an important role in the increased OER rate. The role of larger sulphur atoms in the NiFeS-1/NF facilitates more and easy adsorption of the OH ions, which increases the rate of the reaction kinetics and favours a low Tafel slope value.

These results suggest that the combination of nickel, iron, and sulfur atoms in NiFeS-1/NF and NiFeS-2/NF provides higher current densities and lower overpotentials when compared with those of NiFe-1/NF, NiFe-2/NF, Ni3S2/NF, and NF electrodes. Further, the mass activities of the OER for NiFeS-1/NF, NiFe-1/NF, Ni3S2/NF and RuO2 catalysts (Table 1) at 1.6 V are 276, 178, 149 and 100 mA mg−1, respectively (Fig. 5c). The mass activity of the NiFeS-1/NF catalyst was ∼1.5-fold higher than NiFe-1/NF, ∼1.9-fold higher than Ni3S2/NF catalysts and ∼2.8-fold higher than RuO2, indicating the outstanding activity of the NiFeS-1/NF catalyst. Also, the OER TOF of NiFeS-1/NF, NiFe-1/NF, Ni3S2/NF and RuO2 catalysts at 1.55 V is found to be 0.52, 0.38, 0.035 and 0.046 s−1, respectively (Table 1). The TOF of the NiFeS-1/NF catalyst was ∼15-fold higher than that of the Ni3S2/NF catalyst and ∼11-fold higher than that of a commercial noble metal OER catalyst, RuO2, indicating the incorporation of nickel, iron, and sulfur in the NiFeS-1/NF to improve the performance.

Table 1 OER and HER mass activities (MA) and turn over frequency (TOF) of various catalysts
Catalysts OER HER
TOF (s−1) @1.55 V MA (mA mg−1) @1.6 V TOF (s−1) @−0.18 V MA (mA mg−1) @−0.18 V
NiFeS-1/NF 0.520 276 0.0520 23
NiFe-1/NF 0.380 178 0.0210 6
Ni3S2/NF 0.035 149 0.0067 3
RuO2 0.046 100
Pt/C 0.0049 31

Based on the excellent OER activity of the NiFeS-1/NF catalyst, we also studied the HER activity in 1 M KOH electrolyte and compared it with several control catalysts. To achieve a current density of −10 mA cm−2, the NiFeS-1/NF, NiFe-1/NF, and Ni3S2/NF catalysts required overpotentials of 180, 269, and 318 mV, respectively (Fig. 6a). We observed a similar trend among NiFeS-2/NF, NiFe-2, and Ni3S2/NF (Fig. S9b). The HER Tafel slopes of NiFeS-1/NF, NiFe-1/NF, and Ni3S2/NF were 53, 69, and 74 mV dec−1, respectively. Generally, transition metal chalcogenides follow the Tafel–Volmer–Heyrovsky mechanism (eqn (7)–(9)) in the alkaline medium. The rate determining step in the hydrogen evolution reaction for the low overpotential is Tafel and Volmer steps. Hence, compared to the control samples, the NiFeS-1/NF exhibits a low Tafel slope around 53 mV dec−1 due to the favourable Tafel and Volmer steps.40,41

Mcat + H2O + e ⇌ McatHad + OH (Volmer reaction)(7)
McatHad + H2O + e ⇌ H2 + Mcat + OH (Heyrovsky)(8)
2McatHad ⇌ H2 + Mcat (Tafel)(9)

image file: c6ta04499a-f6.tif
Fig. 6 (a) The HER polarisation curves and (b) the corresponding Tafel slopes of NiFeS-1/NF, NiFe-1/NF, Ni3S2/NF and RuO2. (c) HER mass activity of NiFeS-1/NF, NiFe-1/NF and Ni3S2/NF.

In addition, compared with the HER activity of NiFeS-1/NF, the state-of-the-art Pt/C (40%) catalyst exhibited an overpotential of 69 mV at −10 mA cm−2 with a Tafel slope of 39 mV dec−1 (Fig. 6b). This low HER performance of the NiFeS-1/NF relative to Pt/C (40%) may have been due to the decreased hydrogen adsorption and desorption of hydroxide species. Nevertheless, considering its low cost and facile coating, NiFeS-1/NF displayed excellent HER activity. In addition, the HER mass activities of NiFeS-1/NF, NiFe-1/NF, Ni3S2/NF and Pt/C (40%) catalysts at −0.180 V are 23, 6, 3 and 31 mA mg−1, respectively (Fig. 6c). The mass activity of the NiFeS-1/NF catalyst was ∼3.8-fold higher than that of NiFe-1/NF and ∼7.5-fold higher than that of the Ni3S2/NF catalyst, but, slightly lower than Pt/C (40%), indicating the outstanding HER activity of NiFeS-1/NF (Table 1). Moreover, the NiFeS-1/NF exhibits ~8 fold higher than Ni3S2/NF catalyst (Table 1). The OER performance of NiFeS-1/NF (231 mV@100 mA cm−2) is much better. The TOF of NiFeS-1/NF, NiFe-1/NF, Ni3S2/NF and Pt/C (40%) catalysts at −0.180 V is 0.052, 0.021, 0.0067 and 0.0049 s−1, respectively. The TOF of the NiFeS-1/NF catalyst was ∼1 order magnitude higher than that of a commercial HER Pt/C (40%) catalyst and ∼8-fold higher than that of Ni3S2/NF catalysts (Table 1).

The OER performance of NiFeS-1/NF (231 mV@100 mA cm−2) is much better than those of the recently reported non-noble catalysts such as Fe11.8%Ni3S2/NF (253 mV@100 mA cm−2),15 NiFe LDH/NF (269 mV@10 mA cm−2),42 NiFe foam (320 mV@10 mA cm−2),10 Ni3Se2–Ni foam (0.270 mV@10 mA cm−2),43 oxidized carbon cloth (431 mV@10 mA cm−2),44 CoMnO@CN (334 mV@100 mA cm−2),45 Co(OH)2 (561 mV@100 mA cm−2),46 FeNi@NC (411 mV@100 mA cm−2)47 and DeLNiFeP/rGO (271 mV@100 mA cm−2).23 Meanwhile, NiFeS-1/NF also outperforms the recently reported non-noble HER catalysts such as Mo2C (190@−10 mA cm−2)48 and NiS2/GS (190 mV@10 mA cm−2)21 (Table 2).

Table 2 Comparison of bi-functional OER and HER activities with recent non-precious catalysts in 1 M KOHa
Catalysts OER HER References
Overpotential η (mV) Durability test (h) Overpotential η (mV) Durability test (h)
a NA – not available.
NiFeS-1/NF 231@100 mA cm −2 200 180@−10 mA cm −2 200 This work
NiFe-1/NF 371@100 mA cm−2 NA 318@−10 mA cm−2 NA This work
Fe11.8%Ni3S2/NF 253@100 mA cm−2 14 NA NA 15
NiFe LDH/NF 269@10 mA cm−2 0.5 NA NA 38
NiFe foam 320@10 mA cm−2 10 NA NA 10
Ni3Se2–Ni foam 0.270@10 mA cm−2 42 NA NA 39
Oxidised carbon cloth (ONPPGC/OCC) 431@10 mA cm−2 10 NA NA 40
CoMnO@CN 334@100 mA cm−2 32 NA NA 41
Co(OH)2 561@100 mA cm−2 2.9 NA NA 42
FeNi@NC 411@100 mA cm−2 2.5 NA NA 43
DeLNiFeP/rGO 271@100 mA cm−2 24 NA NA 23
Mo2C NA NA 190@−10 mA cm−2 NA 44
NiS2/GS NA NA 190@−10 mA cm−2 24 20

The superior activity of NiFeS-1/NF is also attributed to the fast electronic movement which can be understood from the Nyquist plot of NiFeS-1/NF and NiFe-1/NF as shown in Fig. 7a. The EIS data reveal a much smaller charge transfer resistance (Rct) of about 20 Ω for NiFeS-1/NF than that of NiFe-1/NF with (43 Ω). Moreover, the double layer capacitance (Cdl) extracted from the fitted Randles circuit as shown in Fig. 7a for NiFeS-1/NF is 10 mF cm−2 (ref. 3 and 4) and for NiFe-1/NF is 3 mF cm−2. The higher capacitance of NiFeS-1/NF reflected its higher electrochemical active surface area (ECSA), presumably the main reason for its outstanding water splitting catalytic OER and HER performance (Table 1).19,45

image file: c6ta04499a-f7.tif
Fig. 7 (a) Electrochemical Z-fitted impedance spectra of NiFe-1/NF and NiFeS-1/NF (b) OER chronopotentiometric durability of NiFeS-1/NF and (c) HER chronopotentiometric durability of NiFeS-1/NF.

Durability tests

To examine the stability of the electrodes, we used the best NiFeS-1/NF catalyst to perform chronopotentiometry of the OER and HER for approximately 200 h each. Fig. 7b presents the OER chronopotentiometry response of NiFeS-1/NF in 1 M KOH at a current density of 80 mA cm−2 for 200 h of continuous operation. The NiFeS-1/NF electrode displayed an initial voltage of 1.6 V; after 200 h of operation, it reached a voltage of 1.72 V, corresponding to 7.5% decay. Moreover, the NiFeS-1/NF catalyst exhibited a HER performance loss of only 1.8% at the end of the 200 h HER stability test with a current density of −10 mA cm−2 (Fig. 7c). These OER and HER chronopotentiometry stability results suggest that the NiFeS-1/NF catalyst exhibits excellent long-term stability in alkaline electrolytes. This outstanding stability of the NiFeS-1/NF electrode may be due to (i) the improved stability of nickel-incorporated iron in alkaline media,8,10,49 (ii) the prevention of nickel corrosion by iron during prolonged operation in alkaline media,10,16 and (iii) the formation of an active phase during the electrochemical tuning of nickel iron sulphide to nickel iron oxy-sulphide,38 resulting in a highly durable HER and OER electrode for water splitting. Hence, alloying of iron with nickel and the incorporation of sulfur may have been responsible for the sustainable high current over the long period (200 h) of operation.

Post analysis

We examined the SEM morphology of the NiFeS-1/NF electrode after the 200 h OER and HER durability studies. Unlike the structure observed after the HER durability test, the SEM morphology observed for the electrode after the OER durability study featured wrecks at low magnification that is visible in Fig. S10a, but its honeycomb structure remained undisturbed (Fig. S10c). We suspect that the wrecks found at low magnification were due to the prolonged bubble evolution during OER operation; these bubbles did not disturb the nanostructured honeycomb structure. After the HER durability test, no wrecks appeared in the low-magnification image (Fig. S10b), and the honeycomb morphology was undisturbed at high magnification (Fig. S10d). Thus, the HER durability test did not disturb the morphology, in contrast to the electrode after the OER durability test.

We performed the post-XPS analysis of the NiFeS-1/NF electrode after the OER and HER tests to examine its surface properties. Compared with a fresh electrode, after the OER durability test the electrode had formed metal oxides that were responsible for its corrosion, whereas the HER durability test led to the formation of only a few metal sulfate impurities (Fig. S11 & S12). In addition, the OER electrode stability was tested using cyclic stability by CV measurements to understand the stability of NiFeS-1/NF. The cyclic stability measurement was examined by performing repeated potentiodynamic cycling for 5000 cycles in the potential range of 1.0 to 1.7 vs. RHE at a scan rate of 50 mV s−1 (Fig. S13a). After 2500 and 5000 cycles, LSV for the NiFeS-1/NF catalyst was carried out which shows a loss of about 70 and 110 mV at 100 mA cm−2, respectively (Fig. S13b). The gradual decrement in performance after 2500 and 5000 potentio-dynamic cycles was due to the oxidation of nickel and iron in the potential range of 1.3 to 1.45 V. And after 5000 CV cycles of cyclic measurements, the XRD pattern of the NiFeS-1/NF was analysed which exhibits the Fe11Ni8S16 (PDF no. 00-022-067), Fe2O3 (PDF no. 00-039-0239) and NiO2 (PDF no. 01-089-8397) phases (Fig. S13c). Hence, the XPS, and XRD studies reveal that the NiFeS-1/NF surface is partially oxidized to nickel oxide and iron oxide.

MEA performance

We examined the NiFeS-1/NF//AEM//NiFeS-1/NF and NF//AEM//NF electrodes individually as both anodes and cathodes for forming MEAs. Fig. 8a displays the water electrolyzer during electrochemical water splitting using NiFeS-1/NF as both the anode and cathode. Fig. 8b presents the full water splitting properties in plots of the voltage versus current density operation of the electrolyzers constructed using NiFeS-1/NF (both anode and cathode) for NiFeS-1/NF, and NF devices. The MEA constructed with NiFeS-1/NF exhibited 274 mA cm−2 at 2.0 V. This performance is comparable with that of the recently reported channeled bipolar electrodes coated with Pt/C as the catalyst.14 We calculated the amount of hydrogen produced from the displacement of water using these catalysts (Fig. 8c).
image file: c6ta04499a-f8.tif
Fig. 8 (a) Alkaline electrolyte membrane (AEM) water electrolyzer set up during full water splitting. (b) Current density versus applied voltage plot of the PEM water electrolyzer using NiFeS-1/NF and NF as both the anode and cathode and (c) hydrogen generation rate in mmol h−1 cm−2 for the PEM water electrolyzer using NiFeS-1/NF and NF alone as both the anode and cathode (solid line for H2 generation rate from displacement and dotted line for the H2 generation rate calculated from the coulombic charge).

The amount of hydrogen generated during water electrolysis was 3.72 mmol h−1 cm−2 (Fig. 8c) which is close to the calculated coulombic efficiency from Fig. 8b at 1.8 V. Further, we analysed the morphology of the anode and cathode after the performance of the PEM assembly. The cathode exhibits the same honeycomb structure which shows that it was not severely affected (Fig. S14a and b). But, in the case of the anode, the morphology was disturbed slightly (Fig. S14c and d) due to the high anodic voltage operation. Also, the constructed alkaline water electrolyzer with NiFeS-1/NF exhibited performance similar to that of precious metal-based catalysts, suggesting the possibility of replacing them in alkaline electrolyte membrane water electrolyzers.


In summary, we have used a two-step, low-energy-consumption electrodeposition process for cost-effective deposition of nickel iron sulphide on NFs. From measurements of electrochemical activity, the NiFeS-1/NF catalyst exhibited a low OER overpotential of 231 mV, with this electrode generating a high current density of approximately 400 mA cm−2 at 1.47 V; it also displayed an overpotential of 180 mV for the HER, due to the composite effect of nickel, iron, and sulphide. This catalyst also displayed excellent durability, with continuous operation possible for approximately 200 h for the OER at 80 mA cm−2 and for the HER at −10 mA cm−2. Furthermore, a PEM water electrolyzer constructed with NiFeS-1/NF electrodes displayed behaviour competitive with that of established systems.


The authors acknowledge the DGIST R&D Program of the Ministry of Education, Science and Technology of Korea (16-RS-04) for financial support.

Notes and references

  1. W. Zhu, X. Yue, W. Zhang, S. Yu, Y. Zhang, J. Wang and J. Wang, Chem. Commun., 2016, 52, 1486–1489 RSC.
  2. M. S. Burke, L. J. Enman, A. S. Batchellor, S. Zou and S. W. Boettcher, Chem. Mater., 2015, 27, 7549–7558 CrossRef CAS.
  3. B. A. Pinaud, J. D. Benck, L. C. Seitz, A. J. Forman, Z. Chen, T. G. Deutsch, B. D. James, K. N. Baum, G. N. Baum, S. Ardo, H. Wang, E. Miller and T. F. Jaramillo, Energy Environ. Sci., 2013, 6, 1983–2002 CAS.
  4. O. F. Selamet and M. S. Ergoktas, J. Power Sources, 2015, 281, 103–113 CrossRef CAS.
  5. C. D. Giovanni, A. Reyes-Carmona, A. Coursier, S. Nowak, J. M. Greneche, H. Lecoq, L. Mouton, J. Roziere, D. Jones, J. Peron, M. Giraud and C. Tard, ACS Catal., 2016, 6, 2626–2631 CrossRef CAS.
  6. D. Pletcher and X. Li, Int. J. Hydrogen Energy, 2011, 36, 15089–15104 CrossRef CAS.
  7. M. Carmo, D. L. Fritz, J. Mergel and D. Stolten, Int. J. Hydrogen Energy, 2013, 38, 4901–4934 CrossRef CAS.
  8. D. W. Kirk and S. J. Thorpe, ECS Trans., 2007, 14, 71–76 Search PubMed.
  9. W. Zhou, X. J. Wu, X. Cao, X. Huang, C. Tan, J. Tian, H. Liu, J. Wang and H. Zhang, Energy Environ. Sci., 2013, 6, 2921–2924 CAS.
  10. Y. Liang, Q. Liu, A. M. Asiri, X. Sun and Y. He, Int. J. Hydrogen Energy, 2015, 40, 13258–13263 CrossRef CAS.
  11. N. Guijarro, M. S. Prevot, X. Yu, X. A. Jeanbourquin, P. Bornoz, W. Bouree, M. Johnson, F. L. Formal and K. Sivula, Adv. Energy Mater., 2016, 6, 1–13 Search PubMed.
  12. B. C. M. Martindale and E. Reisner, Adv. Energy Mater., 2016, 6, 1–9 Search PubMed.
  13. W. G. Colella, B. D. James, J. M. Moton, G. Saur and T. Ramsden, Techno-economic Analysis of PEM Electrolysis for Hydrogen Production, Electrolytic Hydrog. Prod. Work,, 2014 Search PubMed.
  14. G. Aragon-Gonzalez, A. Leon-Galicia, R. Gonzalez-Huerta, J. M. R. Camacho and M. Uribe-Salazar, J. Phys.: Conf. Ser., 2015, 582, 012054 CrossRef.
  15. N. Cheng, Q. Liu, A. M. Asiri, W. Xing and X. Sun, J. Mater. Chem. A, 2015, 3, 23207–23212 CAS.
  16. A. E. Mauer, D. W. Kirk and S. J. Thorpe, Electrochim. Acta, 2007, 52, 3505–3509 CrossRef CAS.
  17. L. L. Feng, G. Yu, Y. Wu, G. D. Li, H. Li, Y. Sun, T. Asefa, W. Chen and X. Zou, J. Am. Chem. Soc., 2015, 137, 14023–14026 CrossRef CAS PubMed.
  18. R. Solmaz and G. Kardaş, Electrochim. Acta, 2009, 54, 3726–3734 CrossRef CAS.
  19. X. Long, G. Li, Z. Wang, H. Zhu, T. Zhang, S. Xiao, W. Guo and S. Yang, J. Am. Chem. Soc., 2015, 137, 11900–11903 CrossRef CAS PubMed.
  20. S. Klaus, M. W. Louie, L. Trotochaud and A. T. Bell, J. Phys. Chem. C, 2015, 119, 18303–18316 CAS.
  21. X. Wu, B. Yang, Z. Li, L. Lei and X. Zhang, RSC Adv., 2015, 5, 32976–32982 RSC.
  22. T. Liu, A. M. Asiri and X. Sun, Nanoscale, 2016, 8, 3911–3915 RSC.
  23. Y. Liu, H. Wang, D. Lin, C. Liu, P. C. Hsu, W. Liu, W. Chen and Y. Cui, Energy Environ. Sci., 2015, 8, 1719–1724 CAS.
  24. N. Jiang, L. Bogoev, M. Popova, S. Gul, J. Yano and Y. Sun, J. Mater. Chem. A, 2014, 2, 19407–19414 CAS.
  25. C. Tang, N. Cheng, Z. Pu, W. Xing and X. Sun, Angew. Chem., Int. Ed., 2015, 54, 9351–9355 CrossRef CAS PubMed.
  26. H. Zhu, J. Zhang, R. Yanzhang, M. Du, Q. Wang, G. Gao, J. Wu, G. Wu, M. Zhang, B. Liu, J. Yao and X. Zhang, Adv. Mater., 2015, 27, 4752–4759 CrossRef CAS PubMed.
  27. C. Xia, Q. Jiang, C. Zhao, M. N. Hedhili and H. N. Alshareef, Adv. Mater., 2016, 28, 77–85 CrossRef CAS PubMed.
  28. C. Tang, H. S. Wang, H. F. Wang, Q. Zhang, G. L. Tian, J. Q. Nie and F. Wei, Adv. Mater., 2015, 27, 4516–4522 CrossRef CAS PubMed.
  29. X. Lu and C. Zhao, Nat. Commun., 2015, 6, 6616 CrossRef CAS PubMed.
  30. S. W. Chou and J. Y. Lin, J. Electrochem. Soc., 2015, 162, A2762–A2769 CrossRef CAS.
  31. J. Y. Lin, J. H. Liao and S. W. Chou, Electrochim. Acta, 2011, 56, 8818–8826 CrossRef CAS.
  32. J. S. Kang, M. A. Park, J. Y. Kim, S. H. Park, D. Y. Chung, S. H. Yu, J. Kim, J. Park, J. W. Choi, K. J. Lee, J. Jeong, M. J. Ko, K. S. Ahn and Y. E. Sung, Sci. Rep., 2015, 5, 10450 CrossRef PubMed.
  33. X. Liu, X. Qi, Z. Zhang, L. Ren, Y. Liu, L. Meng, K. Huang and J. Zhong, Ceram. Int., 2014, 40, 8189–8193 CrossRef CAS.
  34. V. Biju and M. Abdul Khadar, J. Nanopart. Res., 2002, 4, 247–253 CrossRef CAS.
  35. A. R. Lennie and D. J. Vaughan, Mineral Spectroscopy, 1996, 5, 117–131 Search PubMed.
  36. M. Descostes, F. Mercier, N. Thromat, C. Beaucaire and M. Gautier-Soyer, Appl. Surf. Sci., 2000, 165, 288–302 CrossRef CAS.
  37. T. Yamashita and P. Hayes, Appl. Surf. Sci., 2008, 254, 2441–2449 CrossRef CAS.
  38. W. Chen, H. Wang, Y. Li, Y. Liu, J. Sun, S. Lee, J. S. Lee and Y. Cui, ACS Cent. Sci., 2015, 1, 244–251 CrossRef CAS PubMed.
  39. M. E. G. Lyons and M. P. Brandon, Int. J. Electrochem. Sci., 2008, 3, 1425–1462 CAS.
  40. I. Paseka, Electrochim. Acta, 1995, 40, 1633–1640 CrossRef CAS.
  41. A. Sivanantham, P. Ganesan and S. Shanmugam, Adv. Funct. Mater., 2016, 26, 4661–4672 CrossRef CAS.
  42. M. Gong, Y. Li, H. Wang, Y. Liang, J. Z. Wu, J. Zhou, J. Wang, T. Regier, F. Wei and H. Dai, J. Am. Chem. Soc., 2013, 135, 8452–8455 CrossRef CAS PubMed.
  43. A. T. Sedesi, J. Masud and M. Nath, Energy Environ. Sci., 2016, 9, 1771–1782 Search PubMed.
  44. J. Lai, S. Li, F. Wu, M. Saquib, R. Luque and G. Xu, Energy Environ. Sci., 2016, 9, 1210–1214 CAS.
  45. J. Li, Y. Wang, T. Zhou, H. Zhang, X. Sun, J. Tang, L. Zhang, A. M. Al-Enizi, Z. Yang and G. Zheng, J. Am. Chem. Soc., 2015, 137, 14305–14312 CrossRef CAS PubMed.
  46. X. Zhou, X. Shen, Z. Xia, Z. Zhang, J. Li, Y. Ma and Y. Qu, ACS Appl. Mater. Interfaces, 2015, 7, 20322–20331 CAS.
  47. X. Cui, P. Ren, D. Deng, J. Deng and X. Bao, Energy Environ. Sci., 2016, 9, 123–129 CAS.
  48. C. G. Morales-Guio, L. A. Stern and X. Hu, Chem. Soc. Rev., 2014, 43, 6555–6569 RSC.
  49. M. K. Bates, Q. Jia, H. Doan, W. Liang and S. Mukerjee, ACS Catal., 2016, 6, 155–161 CrossRef CAS.


Electronic supplementary information (ESI) available. See DOI: 10.1039/c6ta04499a

This journal is © The Royal Society of Chemistry 2016