NiFe Layered Double Hydroxide Electrocatalyst Prepared via an Electrochemical Deposition Method for the Oxygen Evolution Reaction

: Herein, we aimed to obtain NiFe layered double hydroxide (LDH) with a controlled phase and surface morphology as a highly active and stable oxygen evolution catalyst via the electrochemical deposition method, which was thermodynamically stable for the oxygen evolution reaction (OER) in an alkaline medium. The NiFe-LDH sample was analyzed by sophisticated instruments and tested as an electrocatalyst on Toray carbon (TC). The NiFe-LDH electrocatalyst showed an excellent performance with lower overpotential of 0.27 V at 35 mA cm − 2 and higher density of 125 mA cm − 2 for OER in the 1 M KOH electrolyte solution. Moreover, the prepared catalyst exhibited unpredictable long-time stability for 700 h. From our knowledge, NiFe-LDH is a robust highly stable electrocatalyst compared to the recent reports.


Introduction
Hydrogen energy is regarded as one of the major chemical forms of energy for various applications ranging from domestic to transportation sectors. [1,2]. A promising method of producing hydrogen is by electrochemical splitting of water into hydrogen and oxygen [3,4]. By electrochemical water splitting, high purity hydrogen can be produced. In addition, electrochemical water splitting is considered as an environmentally friendly technique with nearly no carbon emissions. Typically, the water splitting process combines the following two half-cell reactions happening on anodes and cathodes, respectively: (i) the oxygen evolution reaction (OER): 4OH − → O 2 + 2H 2 O + 4e − and (ii) the hydrogen evolution reaction (HER): 2H 2 O + 2e − → H 2 + 2OH [5][6][7]. The OER, also referred to as water oxidation, is a complex process from the kinetic perspective since it limits the overall efficiency of water splitting and is a multi-proton-coupled four-electron-transfer reaction [8][9][10][11]. Consequently, discovering an effective electrocatalyst is key for enhancing the sluggish OER kinetics [12]. Exploring new electrocatalytic materials with durable electrodes is crucial for the effective application of water splitting technology. In this regard, in recent years, the development of highly active and abundant earth-transition metals such as Co-, Ni-, Fe-, and Mn-based oxides, hydroxides, and phosphides has been explored [13]. In addition, bimetallic composite hydroxides outperform single-metal catalysts in electrocatalysis. It has been suggested that the presence of iron components can boost the OER activity of nickel-or cobalt-based oxide/hydroxide composites. Furthermore, iron is one of the most effective non-precious OER catalysts and exhibits very high activity [14]. However, relatively few studies have examined the impact of NiFe-based (oxy)hydroxides on the OER catalytic mechanism. Iron's effect on the catalytic activity of Ni catalysts remains largely undetermined. Recent studies have suggested that synergistic interactions between Fe and Ni (oxy)hydroxides and high oxidation states of the Fe and Ni centers are responsible for the good activity [15][16][17][18]. Additionally, it has been noted that there is a linear correlation between the iron surface coverage and the OER activity of Fe-based (oxy)hydroxide, highlighting the importance of surface Fe species in OER electrocatalysis [19]. Additionally, the iron impurities in the electrolytes, which take the form of free ions, may also influence the electrocatalytic activity during the water splitting reaction (within the concentration range of ppb to ppm). However, such Fe adsorption effect on OER activity is unknown. Notably, theoretical simulations have demonstrated that phosphate groups [20], N sites [21], and electronegative substrates [22] could increase the OER activity by promoting the partial electron removal from the active centers. Fe ions are expected to contribute a significant amount of electronegative surface at this situation and may tend to promote the electrocatalytic activity (NiFe-based catalysts) by a similar electron-transfer mechanism. Xiang et al. [23] explained that NiFe-LDH with a hydroxide interfacial layer displays enhanced activity for OER. The synergistic effect between NiFe-LDH and the hydroxide layer stimulates a sympathetic local chemical environment with the appropriate electronic structure, which directs optimal OH intermediates' adsorption, and that could enhance the OER activity. This is one of the primary motivations for this current work.
As previously stated, the development of novel electrocatalytic materials and their preparation method, as well as the type of electrodes used, are crucial factors influencing the electrochemical reactions during the application of water splitting. Currently, sol-gel synthesis, colloidal synthesis, zeolitic imidazolate frameworks, and solvo-(or) hydrothermal procedures are among the solution-based techniques, which are the most frequently used method to synthesize the NiFe (oxy)hydroxides electrocatalyst [24][25][26][27][28][29][30][31][32][33]. However, there are some significant problems with the catalyst efficacy with solution-based techniques such as (i) limited control over nanomaterial size; (ii) uneven catalyst loading and distribution over conductive substrates (such as carbon cloth, nickel foam, or Toray carbon); and (iii) lack of methods to track crystal growth in real time during synthesis. In this context, the electrochemical deposition technique has emerged as a promising method for synthesizing electrocatalysts with precise control over the nanomaterials' size and with even catalyst distribution on the conductive surfaces. Moreover, electrochemical deposition does not require any complicated experimental requirements such as high pressure/temperature. In addition, electrochemical deposition makes it possible to control the growth process of nanomaterials while simultaneously increasing their degree of irreversibility by interatomic interactions. Additionally, electrochemical deposition is a simple process that has the potential for scale up into large-scale industrial production [34].
Herein, the electrochemical deposition of NiFe-LDH has been carried out over the Toray carbon (TC) (as cathode) and graphite sheet (as anode) in the electrochemical setup. The fabricated NiFe-LDH on Toray carbon has been used as an active electrocatalyst for the efficient splitting of water molecules (OER) in 1 M KOH. The electrochemically fabricated NiFe-LDH electrocatalyst showed an overpotential of 0.18 V for OER with excellent stability for over 700 h in the two-electrode system.

Results and Discussion
The XRD pattern of the Fe, Ni, and NiFe-LDH film deposited on the TC sheet is shown in Figure 1. The XRD peaks of Fe on the TC sample observed at 26.9, 44.8, 52.2, 54.9, and 76.8˚ corresponded to the (120), (400), (422), (221), and (533) planes, respectively. In addition, the XRD peaks represented the formation of Fe(OH)2 (JCPDS no. 29-0713) and γ-Fe2O3 (JCPDS no. 39-1346) with cubic structure (Figure 1a) [35,36]. Meanwhile, the diffraction peaks appeared for the Ni sample at 26.7° (101), 38.4° (102), 44.6° (111), and 52° (200), which revealed the presence of Ni in the form of Ni(OH)2 (JCPDS 14-0117) and the Ni matrix, as shown in Figure 1b [37]. Figure 1c shows the diffraction peaks corresponding to NiFe-LDH (JCPDS no 40-0215) at the two theta angles of 26.7°, 44.5°, and 54.5° corresponding to the (006), (018), and (110) planes for NiFe-LDH and 51.8° (200) and 76.2°(220) for Ni3Fe, respectively [38]. Further, it was observed that the diffraction peaks of NiFe-LDH are shifted towards lower angles when compared to Fe(OH)2 and Ni(OH)2. The obtained XRD result clearly confirmed the formation of NiFe-LDH.  FE-SEM images demonstrated the surface morphology of Ni, Fe, and NiFe-LDH on TC, as shown in Figure 3. Figure 3a illustrates that the TC sheet was fully covered with  Ni/Ni(OH)2 nanosheets, which is in the range of ~100-200 nm. The self-protected Ni/Ni(OH)2 nanosheets are uniformly formed during the electrochemical deposition process. Moreover, the FE-SEM image indicated that a nano-spike surface morphology for Fe was on the TC sheet, as shown in Figure 3b. Furthermore, Figure 3c shows TC has been uniformly covered with the Ni and Fe complex, which provided high surface area as well as active centers to support the water oxidation process. The formation of NiFe -LDH is shown clearly in Figure 3c.  The HR-TEM images revealed the size and morphology of Ni, Fe, and NiFe-LDH on TC, as shown in Figure 4. In Figure 4a, Ni forms a nanosheet-like morphology with a size of 200 nm, which confirmed the sheet was protected on TC in the controllable size. Hence, the Fe nano-spikes were vertically grown onto the TC surface ( Figure 4b). Furthermore, Figure 4b shows nano-spikes with sizes in the range of ~50-100 nm. The nano-spike can provide support to enlarge the surface area of Ni. Figure 4c shows theHR-TEM image of NiFe-LDH on the TC surface, and the nano-spike of 100 nm in size with well-defined surface morphology is observed in Figure 4c. The SAED patterns of Ni, Fe, and NiFe-LDH are shown in Figure 4d-f, which confirm the materials have goodcrystallinity. FE-SEM images demonstrated the surface morphology of Ni, Fe, and NiFe-LDH on TC, as shown in Figure 3. Figure 3a illustrates that the TC sheet was fully covered with Ni/Ni(OH) 2 nanosheets, which is in the range of~100-200 nm. The self-protected Ni/Ni(OH) 2 nanosheets are uniformly formed during the electrochemical deposition process. Moreover, the FE-SEM image indicated that a nano-spike surface morphology for Fe was on the TC sheet, as shown in Figure 3b. Furthermore, Figure 3c shows TC has been uniformly covered with the Ni and Fe complex, which provided high surface area as well as active centers to support the water oxidation process. The formation of NiFe -LDH is shown clearly in Figure 3c. Ni/Ni(OH)2 nanosheets, which is in the range of ~100-200 nm. The self-protected Ni/Ni(OH)2 nanosheets are uniformly formed during the electrochemical deposition process. Moreover, the FE-SEM image indicated that a nano-spike surface morphology for Fe was on the TC sheet, as shown in Figure 3b. Furthermore, Figure 3c shows TC has been uniformly covered with the Ni and Fe complex, which provided high surface area as well as active centers to support the water oxidation process. The formation of NiFe -LDH is shown clearly in Figure 3c.  The HR-TEM images revealed the size and morphology of Ni, Fe, and NiFe-LDH on TC, as shown in Figure 4. In Figure 4a, Ni forms a nanosheet-like morphology with a size of 200 nm, which confirmed the sheet was protected on TC in the controllable size. Hence, the Fe nano-spikes were vertically grown onto the TC surface ( Figure 4b). Furthermore, Figure 4b shows nano-spikes with sizes in the range of ~50-100 nm. The nano-spike can provide support to enlarge the surface area of Ni. Figure 4c shows theHR-TEM image of NiFe-LDH on the TC surface, and the nano-spike of 100 nm in size with well-defined surface morphology is observed in Figure 4c. The SAED patterns of Ni, Fe, and NiFe-LDH are shown in Figure 4d-f, which confirm the materials have goodcrystallinity. The HR-TEM images revealed the size and morphology of Ni, Fe, and NiFe-LDH on TC, as shown in Figure 4. In Figure 4a, Ni forms a nanosheet-like morphology with a size of 200 nm, which confirmed the sheet was protected on TC in the controllable size. Hence, the Fe nano-spikes were vertically grown onto the TC surface (Figure 4b). Furthermore, Figure 4b shows nano-spikes with sizes in the range of~50-100 nm. The nano-spike can provide support to enlarge the surface area of Ni. Figure 4c shows theHR-TEM image  The XPS study was examined to prove the presence of elements and the oxidation state of as-prepared Fe on TC, Ni on TC, and NiFe-LDH on TC, as shown in Figure 6. The high-resolution XPS spectrum of Ni on TC revealed that Ni's main peaks occurred at the binding energies of 859.8 and877.3 eV for 2p3/2 and for 2p1/2, respectively, as shown in Figure 6a. In addition, the satellite peaks were presented at about the binding energies of 865 and 883 eV for 2p3/2 and 2p1/2, respectively (Figure 6a). From the result, we clearly observed the presence of NiO on the TC sheet (Figure 6a). Figure 6b shows the highresolution spectrum of Fe on TC; the peaks of Fe 2p3/2 and Fe 2p1/2 appeared at the binding energies of 711 and 723 eV, respectively, which confirmed that the iron exists in +3 oxidation states in the substrate of TC [39]. Furthermore, Figure 6c shows the survey spectrum of NiFe-LDH. The major peaks appeared at 859.1, 713.4, and 531.3 eV corresponding to Ni, Fe, and O elements, respectively. The survey spectrum confirmed the presence of constituted elements in NiFe-LDH. Additionally, the high-resolution spectra of the Ni 2p and Fe 2p main peaks are displayed at the binding energies of 860 The XPS study was examined to prove the presence of elements and the oxidation state of as-prepared Fe on TC, Ni on TC, and NiFe-LDH on TC, as shown in Figure 6. The highresolution XPS spectrum of Ni on TC revealed that Ni's main peaks occurred at the binding energies of 859.8 and877.3 eV for 2p 3/2 and for 2p 1/2 , respectively, as shown in Figure 6a. In addition, the satellite peaks were presented at about the binding energies of 865 and 883 eV for 2p 3/2 and 2p 1/2 , respectively (Figure 6a). From the result, we clearly observed the presence of NiO on the TC sheet (Figure 6a). Figure 6b shows the high-resolution spectrum of Fe on TC; the peaks of Fe 2p 3/2 and Fe 2p 1/2 appeared at the binding energies of 711 and 723 eV, respectively, which confirmed that the iron exists in +3 oxidation states in the substrate of TC [39]. Furthermore, Figure 6c shows the survey spectrum of NiFe-LDH. The major peaks appeared at 859.1, 713.4, and 531.3 eV corresponding to Ni, Fe, and O elements, respectively. The survey spectrum confirmed the presence of constituted elements in NiFe-LDH. Additionally, the high-resolution spectra of the Ni 2p and Fe 2p main peaks are displayed at the binding energies of 860 and 877.6 eV and 713.4 and 725.5 eV, respectively, which represent the presence of Ni and Fe in NiFe-LDH (Figure 6d,e). From the spectra, we identified that the peaks are slightly shifted towards higher binding energies compared to bare Ni and Fe, due to the formation of NiFe-LDH. Furthermore, Figure 6f shows the O1s high-resolution spectra, which shows that two major peaks appearing at 530.3 and 532.2 eV are attributed tometal hydroxides (M-OH) and intercalated water molecules into NiFe-LDH (H 2 O), respectively [40].  (Figure 6d,e). From the spectra, we identified that the peaks are slightly shifted towards higher binding energies compared to bare Ni and Fe, due to the formation of NiFe-LDH. Furthermore, Figure 6f shows the O1s high-resolution spectra, which shows that two major peaks appearing at 530.3 and 532.2 eV are attributed tometal hydroxides (M-OH) and intercalated water molecules into NiFe-LDH (H2O), respectively [40].  The electrochemical studies were carried out by a conventional three-electrode system (NiFe-LDH as a working electrode, Pt wire as a counter electrode, and Hg/HgSO 4 as a reference electrode) in 1 M KOH electrolyte with a scan rate of 10 mV s −1 for the OER. For all the electrochemical measurements, the potential of Hg/HgO was changed into reversible hydrogen electrode (RHE) via the basic formula of [41], We have quantified the catalysts' deposition on Toray carbon. The amount of the coating is 1 mg for all the three types of samples. Figure 7 shows the LSV curve of TC, Fe, Ni, and NiFe-LDH on TC. The NiFe-LDH exhibited the lowest onset potential of 1.41 V, which is lower than that of the bare TC (1.57 V), Fe on TC (1.53 V), and Ni on TC (1.52 V). The shifting of the redox peak at 1.45 V is due to change of electronic structure configuration, conductivity, and active sites in NiFe-LDH. Moreover, Gao et al. [42] observed that the Fe 2+ -NiFe-LDH exhibits enhanced activity for the OER. Their theoretical survey proposed that the Fe-O-Fe oxygen-bridged metal motifs have a beneficial effect on the catalysis for OER (where the Fe atom is judged as the active site), while the Fe-O-Fe couples can be built by the introduction of Ni-sited Fe atoms into NiFe-LDH, which could be active as stable high-valent motifs and that can enhance the OER intrinsic activity. At the onset potential of 1.5 V, NiFe-LDH displays a current density up to 35 mA cm −2 , which is one-fold higher in value than Fe on TC and Ni on TC. This result demonstrated the excellent improvement of the electrocatalytic activity toward OER. The combination of NiFe-LDH represented much lower onset potential than the Ni and Fe deposited on TC. This significant improvement of OER activity is due to the formation of (oxy)hydroxide phases in the NiFe-LDH electrocatalyst. Furthermore, Table S1 shows the comparison of the obtained result with reported results. In addition, we observed the Tafel values for all the as-prepared electrocatalysts as shown in Figure 7b. The Tafel slope value of NiFe-LDH is 0.095 V dec −1 in low overpotential ranges, which ismuch lower than that of Ni (0.237 V dec −1 ) and Fe on TC (0.248 V dec −1 ), demonstrating a faster kinetics reaction during the OER. Moreover, we have plotted the comparison of the onset potential, in which the onset potential at 35 mA cm −2 and overpotential for all electrocatalysts is shown in Figure 7c. From the comparison plot, the NiFe-LDH showed the lowest potential values compared to the others. We confirmed that the (oxy)hydroxide phases are very suitable for OER in an alkaline medium. The stability testing is another important key factor for estimating the electrocatalytic performance in an alkaline solution. Hence, the various chronopotentiometry measurements of 60, 50, 40, and 30 mA cm −2 were worked out to estimate the durability of NiFe-LDH. It showed no evident change in the onset potential for each 100 h test (Figure 7d) and validated the outstanding durability of the NiFe-LDH electrocatalyst for the OER in an alkaline electrolyte. It is important to note that after 700 h of chronopotentiometry measurement testing during OER in alkaline medium, only a 3% reduction from the starting potential was observed. This indicates that (oxy)hydroxide phases of the NiFe-LDH electrocatalyst are very suitable for water electrolysis technology, which will support the replacement of noble metals and reduce the cost of the water electrolyzer. The electrochemical studies were carried out by a conventional three-electrode system (NiFe-LDH as a working electrode, Pt wire as a counter electrode, and Hg/HgSO4 as a reference electrode) in 1 M KOH electrolyte with a scan rate of 10 mV s −1 for the OER. For all the electrochemical measurements, the potential of Hg/HgO was changed into re- h test (Figure 7d) and validated the outstanding durability of the NiFe-LDH electrocatalyst for the OER in an alkaline electrolyte. It is important to note that after 700 h of chronopotentiometry measurement testing during OER in alkaline medium, only a 3% reduction from the starting potential was observed. This indicates that (oxy)hydroxide phases of the NiFe-LDH electrocatalyst are very suitable for water electrolysis technology, which will support the replacement of noble metals and reduce the cost of the water electrolyzer.  Figure 8 represents the electrochemical stability test and OER activity of Ni, Fe, and NiFe-LDH on TC at various temperatures (25, 55, and 85°C). As-prepared NiFe-LDH on the TC electrocatalyst exhibited high stability for 700 h with the onset potential of 1.56 V at room temperature (25°C). The onset potential suddenly dropped to 1.38 V at 85°C and then is was maintain more stable. The reason for the dropped potential is that, if we consider the stability under high-temperature conditions, the temperature rise induces the molecular collision, thereby enhancing the kinetic energy to accelerate the activity, especially at higher overpotentials. However, this might not be the case in the lower overpotentials where the activation energy of the OER should be overcome even if it has more  Figure 8 represents the electrochemical stability test and OER activity of Ni, Fe, and NiFe-LDH on TC at various temperatures (25,55, and 85 • C). As-prepared NiFe-LDH on the TC electrocatalyst exhibited high stability for 700 h with the onset potential of 1.56 V at room temperature (25 • C). The onset potential suddenly dropped to 1.38 V at 85 • C and then is was maintain more stable. The reason for the dropped potential is that, if we consider the stability under high-temperature conditions, the temperature rise induces the molecular collision, thereby enhancing the kinetic energy to accelerate the activity, especially at higher overpotentials. However, this might not be the case in the lower overpotentials where the activation energy of the OER should be overcome even if it has more kinetic energy with high temperature. That is why more deviation was encountered at low overpotential regions. Additionally, with the temperature increment, it is common to have an increase in the kinetic energy that influences the activity when the potential is applied to the electrode/electrolyte interface. From this result, we observed that temperature is also one of the key factors to enhance the electrocatalytic activity of NiFe-LDH on TC for OER in an alkaline medium. Moreover, NiFe-LDH on TC nanomaterials becomes very stable and exhibited excellent OER performance at higher temperatures. This is the first time that the NiFe-LDH electrocatalyst showed high stability over 700 h at a higher temperature.
have an increase in the kinetic energy that influences the activity when the potential is applied to the electrode/electrolyte interface. From this result, we observed that temperature is also one of the key factors to enhance the electrocatalytic activity of NiFe-LDH on TC for OER in an alkaline medium. Moreover, NiFe-LDH on TC nanomaterials becomes very stable and exhibited excellent OER performance at higher temperatures. This is the first time that the NiFe-LDH electrocatalyst showed high stability over 700 h at a higher temperature.

Preparation of Fe Electrode
The electro deposition of iron (Fe) on TC was undertaken in a sulphate iron bath (350 g L −1 FeSO4.7H2O, 10g L −1 glycine, 2 g L −1 citric acid, and 0.05 g L −1 of sodium lauryl sulphate). The electrochemical deposition was carried out using Toray carbon as the cathode and an electrolytic-grade Fe sheet as the anode. The electrolyte bath was maintained at pH 2-2.5 (at room temperature) at a current density of 4 A dm −2 and 2 A dm −2 for 30min. The electrochemical deposition process leads to a thin brown film deposited on the TC.

Preparation of Ni Electrode
The electrochemical deposition of nickel (Ni) on Toray carbon was undertaken in a sulphate nickel bath (250 g L −1 NiSO4.7H2O, 45g L −1 NiCl2.6H2O, 30 g L −1 H3BO3, and 0.05g l −1 of sodium lauryl sulphate). The electrochemical deposition was carried out using TC as the cathode and an electrolytic-grade Ni sheet as the anode. The electrolyte bath was

Preparation of Fe Electrode
The electro deposition of iron (Fe) on TC was undertaken in a sulphate iron bath (350 g L −1 FeSO 4 ·7H 2 O, 10 g L −1 glycine, 2 g L −1 citric acid, and 0.05 g L −1 of sodium lauryl sulphate). The electrochemical deposition was carried out using Toray carbon as the cathode and an electrolytic-grade Fe sheet as the anode. The electrolyte bath was maintained at pH 2-2.5 (at room temperature) at a current density of 4 A dm −2 and 2 A dm −2 for 30min. The electrochemical deposition process leads to a thin brown film deposited on the TC.

Preparation of Ni Electrode
The electrochemical deposition of nickel (Ni) on Toray carbon was undertaken in a sulphate nickel bath (250 g L −1 NiSO 4 ·7H 2 O, 45 g L −1 NiCl 2 ·6H 2 O, 30 g L −1 H 3 BO 3 , and 0.05 g L −1 of sodium lauryl sulphate). The electrochemical deposition was carried out using TC as the cathode and an electrolytic-grade Ni sheet as the anode. The electrolyte bath was maintained at pH 4 (50 • C) at a current density of 6 A dm −2 and 8 A dm −2 for 30 min. The electrochemical deposition process leads to a thin silver film deposited on the TC.

Preparation of NiFe Electrode
The electrochemical deposition of NiFe on TC was undertaken in anickel iron sulphate bath (2-3 g L −1 NiCl 2 ·6H 2 O, 2.1 g L −1 FeCl 3 ·6H 2 O, and 25 g L −1 of H 3 BO 3 ). The electrochemical deposition was carried out using TC as the cathode and an electrolytic-grade graphite sheet as the anode. The electrolyte bath was maintained at pH 2.5 (55 • C) at a current density of 2 A dm −2 for 30 min.

Characterization
The crystal structure and plane of Ni, Fe, and NiFe-LDH were carried out using the (D8 ADVANCE, Bruker, Bengaluru, Karnataka, India) X-ray diffractometer with Cu-Ká (ë = 1.5405 Å) radiation in the range of 20-80 • . The Raman spectroscopy provided the information about the vibrational mode of molecules and the spectra were collected by Renishaw (Gloucestershire, UK) via Raman microscope with a 632.8 nm wavelength incident laser light. The structural morphology of as-prepared Ni, Fe, and NiFeLDH was investigated using FE-SEM (Carl Zeiss SUPRA 55V PFEI, Oberkochen, Germany) and HR-TEM (a FEI TECNAI G220 with an accelerating voltage of 200 kV, supplied from Sao Paulo, Brazil). The presence of elements was analyzed by the X-ray photoelectron spectroscopy (XPS) with a PHI 5000 Versa Probe ULVAC instrument (Chigasaki, Kanagawa, Japan).

Conclusions
In summary, we successfully used a facile route for the electrochemical deposition of the NiFe-LDH on TC as an electrocatalyst for the OER, which was an attractive method to control the morphology with (oxy)hydroxides phases. NiFe-LDH on the TC electrocatalyst showed the lowest onset potential (1.41 V) when compared to bare Ni (1.52 V) and Fe on TC (1.53 V) with the lowest Tafel value of 0.095 V dec −1 in the 1 M KOH electrolyte solution with ascan rate of 10 mV s −1 . Moreover, we tested the long-time stability of the NiFe-LDH on the TC electrocatalyst in the two-electrode system. The catalyst exhibited a high stability for 700 h with no change in the current density of 120 mA cm −2 . Hence, the NiFe-LDH on TC was demonstrated as a superior active and highly stable electrocatalyst in the OER from the water splitting at room temperature as well as high temperature. Therefore, it can be considered as a suitable electrocatalyst in the industrial-scale production of oxygen and hydrogen from water.