Effect of PEG on Performance of NiMnO Catalyst for Hydrogen Evolution Reaction

Introduction

The world's energy consumption of fossil energy such as coal, oil, and natural gas brings many questions, such as energy shortage and serious environmental pollution (Zou and Zhang, 2015; Ojha et al., 2018). H₂ is a promising clean and renewable source of energy with extremely high calorific value (285.8 kJ mol⁻¹). Electrocatalytic cracking water to H₂ becomes feasible for the impetus of electrochemical HER is derived from electricity from tidal energy, wind energy, geothermal energy, etc. Researchers have found that platinum-based catalysts are the most efficient catalysts for HER (Chen et al., 2013; Zhou W. et al., 2016; Wu et al., 2019; Eiler et al., 2020; Li and Baek, 2020). However, platinum is very rare in the earth's crust, making it extremely expensive. Therefore, it is necessary to develop a metal catalyst with abundant resources as an alternative. After the efforts of scientists, they found that transition metal oxide is an efficient catalyst for the HER of H₂O decomposition (Wang et al., 2017; Han et al., 2019; Liang et al., 2020).

The atomic number of nickel is 28. The abundance of nickel in Earth's crust is > 50 ppm. And nickel is an earth-abundant first row transitional metal (Jamesh et al., 2015). Ni possesses very strong ductility and corrosion-resistance. The addition of nickel could significantly improve the stability and activity of catalyst for HER (Chu et al., 2018; Zhang et al., 2019). Another rich transition metal element manganese on the earth is also an important catalyst raw material. There are many defects, which created in MnO₂, can strengthen the stability and activity for HER. δ-MnO₂ Nanosheet demonstrates favorable stability and activity for HER (Leonard and Bard, 2013; Liu et al., 2017; Zhao et al., 2017). The δ-MnO₂ phase includes trivalent and tetravalent manganese. It will create defects in the catalyst structure. Therefore, the defects and oxygen vacancies can generate the Mn³⁺ active sites, which can afford half-metalicity. This can significantly increase the electronic conductivity of the catalyst, and thus the reaction efficiency is significantly improved (Mohammed-Ibrahim and Sun, 2019).

The performance of HER catalysts is highly correlated to the synthetic methods. On account of the inherent pitfalls, i.e., unable to control the concentration gradient and dispersibility of metal particles (Arevalo and Chirik, 2019), the traditional synthetic methods, such as precipitation and wet impregnation, have been gradually phased out. For the past few years, by combining surfactant with traditional co-precipitation method was raised and widespread used for catalyst preparation (Das et al., 2015; Chong et al., 2018; Xu et al., 2018; Toloman et al., 2019).

Due to the hydroxyl protons exchange between cetyltrimethyl ammonium bromide (CTAB) and hydrous metal hydroxide gels would lower surface tension and interfacial energy of H₂O exist in the pores (Sohn and Ozkan, 2016). Therefore, CTAB can assist-synthesized a high specific surface area oxide catalyst. Moreover, the pore structure did not collapse during the calcination process. Likewise, polyvinyl pyrrolidone (PVP), a non-ionic polymer surfactant could play a similar role (Tan et al., 2014; Wang et al., 2019). In addition, some surfactants possess amphiphilic property, This series of molecules can generate thermodynamically stable gathers of intrinsically nano-scale both in solution and at the solid liquid interphases (Lee et al., 2019; Liu et al., 2019). Surfactants have a unique ability to self-organize at interface or in solution, modify interfacial properties and enhance the compatibility between materials of very different characteristics (Carswell et al., 2003; Hosseini et al., 2016).

In this article, NiMnO catalysts were synthesized by polyethylene glycol surfactant assist- solvent-thermal method, and then the electrochemical catalytic properties for HER were estimated. The as-prepared catalysts were explored by N₂ adsorption-desorption, X-ray diffraction (XRD), and scanning electron microscopy (SEM). Besides, we have performed a series of electrochemical tests (cyclic voltammetry, linear sweep voltammetry, electrochemical impedance spectroscopy, and chronopotentiometry), and derived some electrochemical parameters (Tafel slopes, electrochemical double-layer capacitance, and Turnover frequency).

Experimental

Sample Synthesis

Materials: Polyethylene glycol (PEG, M_w = 20,000) and ethanol were supplied by Guangzhou Chemical Reagent Factory. Ni(CH₃COO)₂•4H₂O, Mn(CH₃COO)₂•4H₂O and urea were supplied by Shanghai Macklin Biochemical Co., Ltd. The water (18.25 mΩ cm⁻¹) used in the experiments was purified by Millipore system (Milli-Q Academic). All reagents used throughout this manuscript were analytical reagent grade.

Synthesis of NiMnO catalyst: Typically, 2.043 g of Ni(CH₃COO)₂•4H₂O and 3.036 g of Mn(CH₃COO)₂•4H₂O were placed in 40 mL anhydrous ethanol to form a homogeneous solution under magnetic stirring for 2 h at room temperature, 7 g of Urea was dissolved in 10 mL deionized water, different weight of PEG (0, 2, and 3 g) were dispersed in 10 mL anhydrous ethanol under magnetic stirring for 1 h at room temperature, which resulting in three samples, marked as NMO, NMO-PEG-2g, and NMO-PEG-3g. Then, The PEG suspension and the Urea solution were dripped into the Ni(CH₃COO)₂•4H₂O-Mn(CH₃COO)₂•4H₂O solution in sequence under stirring. Kept stirring for 2 h at room temperature, the mixture was transferred into the Teflon-lined stainless-steel autoclave and heat at 180°C for 10 h for the solvent-thermal reaction. After the reaction was completed and being cooled to room temperature, the precipitates were collected by centrifugation and washed with deionized water and ethanol for three times, then dried in an oven at 80°C for 6 h to get catalyst. After dried, the catalyst was subjected to bake in a muffle furnace at 750°C for 120 min.

Microstructural Characterizations

X-ray diffraction (XRD) data was obtained by a PANalytical PW3040/60 X-ray diffractometer with Cu Kα radiation (40 kV, 30 mA). Scanning electron microscope (SEM) measurements were observed by a ZEISS-Merlin microscope at 10 kV. Brunauer-Emmett-Teller (BET) surface area analysis (N₂ adsorption) of the catalysts was obtained using an ASAP2020M system (Micromeritics). Inductively coupled plasma-atomic emission spectrometry (ICP-AES) was conducted on a PerkinElmer NexION 300X.

Electrochemical Measurements

Five milligram NiMnO catalyst was dispersed in 10 mL isopropanol (Sigma-Aldrich) aqueous solution containing Nafion (15 wt.%, Sigma-Aldrich) (isopropanol: Nafion solution: water = 1:4:10 volume ratio). And then, sonicated for 30 min to formulate a homogeneous suspension (catalyst contain 0.5 mg mL⁻¹). 10 μL of the above-mentioned suspension was coated on the glassy carbon electrode (CHI) with a diameter of 4 mm used as working electrode after infrared drying. Saturated calomel electrode (SCE) was used as reference electrode. Graphite flake was used as counter electrode. The electrolyte was 1.0 M KOH which was bubbled by high-purity argon 5 min before the measurement and continue until the measurement was completed. Cyclic voltammetry was conducted at 10 mV s⁻¹. Linear sweep voltammetry (LSV) was collected by the glassy carbon electrode at a scan rate of 5mV s⁻¹. Tafel slopes were calculated based on the corresponding LSV curves. Electrochemical impedance spectroscopy (EIS) was measured in the frequency scope from 105 to 0.01 Hz. The stability measurements were detected by chronopotentiometry at a constant current density of 10 mA mg⁻². All voltages involved in the article vs. SCE were adjust to the reversible hydrogen electrode (RHE). Calibration using the following formula: E(RHE) = E(SCE) + 0.0591pH + 0.2415 – 0.000761 (T – 298.15). T represents the room temperature.

Results and Discussion

The NiMnO catalyst was synthesized by a solvent-thermal route using urea as a precipitant. The chemical reactions involve the thermal decomposition of urea, following by the generation of ${\text{CO}}_3^{2-}$ ions and the subsequent precipitation of the NiMnO catalyst under solvothermal conditions.

$\begin{array}{l}\text{N}{\text{H}}_2\text{CON}{\text{H}}_2+{\text{H}}_2\text{O}\to 2\text{N}{\text{H}}_3+\text{C}{\text{O}}_2\end{array}$

$\begin{array}{l}{\text{NH}}_3+{\text{H}}_2\text{O}\to {\text{NH}}_4^{+}+{\text{HO}}^{-}\end{array}$

$\begin{array}{l}{\text{CO}}_2+2{\text{OH}}^{-}\to {\text{CO}}_3^{2-}+{\text{H}}_2\text{O}\end{array}$

$\begin{array}{l}{\text{Ni}}^{2+}+{\text{Mn}}^{2+}+{\text{CO}}_3^{2-}\to {\text{NiMnCO}}_3\end{array}$

SEM images (Figure 1) show that the NiMnO can be successfully synthesized through solvent-thermal reaction. Different amounts of PEG resulted in different morphologies of the catalysts, among which the surface area of NMO-PEG-3g appeared to be largest. PEG can prevent NiMnCO₃ from aggregation and compression. Meanwhile, the PEG with more mass represents more molecular chains, making it easier for PEG molecules to be entangled or spiraled with other PEG molecules through hydrogen bonds. This distortion will greatly increase the specific surface area of NMO due to the volatilization of PEG and CO₂ after roasting with NMCO₃ at 750°C. Larger specific surface area can increase the reaction active sites, which is beneficial to the catalytic activity. The N₂ adsorption–desorption isotherms and pore-size distribution indicate that the NiMnO catalysts added PEG form a macropore structure. There are only a few micropores in the structure of the NiMnO catalyst without adding PEG (Figure 2 and Figure S2). The NiMnO produced when no PEG was added exhibited a 4–7 μm spherical structure. With the addition of PEG, scales appeared on the surface of the prepared catalyst. A well petal-like sheet has been formed in NMO-PEG-3g. And there are rich fluffy structures on the sheet. These structures are conducive to the electrochemical catalytic HER.

FIGURE 1

Figure 1. SEM images of (a) NMO, (b) NMO-PEG-2g, (c) NMO-PEG-3g.

FIGURE 2

Figure 2. XRD patterns of NiMnO catalysts.

The composition and morphology of the electroactive catalysts were further investigated using XRD (Figure 2). The XRD peaks were indexed to crystal facets of MnO₂ (JCPDS Card No. 86-0172) and NiO (JCPDS Card No. 78-0210). MnO₂ has a smaller K_sp value than NiO, and [Mn(NH³)_n]²⁺ has a smaller K_f value than [Ni(NH³)_n]²⁺, which indicates that MnO₂ is more easily precipitated than NiO (van Bommel and Dahn, 2009). Both MnO₂ and NiO can be indexed to a typical hexagonal carbonate structure with a space group of RC. The accurate content of each element in NiMnO is further corroborated by SEM coupled energy-dispersive X-ray spectroscopy (EDS) (Figure S1) and ICP-AES (Table S1). The Ni and Mn contents in the product are calculated to be 8:92 (atomic ratio) from the EDS, which are in good agreement with the ICP-AES results.

The electrocatalytic properties of NiMnO catalyst for HER in alkaline solution was evaluated using a standard three-electrode system. Comparing the three catalysts of NMO, NMO-PEG-2g, and NMO-PEG-3g, LSV results show that NMO-PEG-3g possesses excellent activities that are much better than the activity of NMO and NMO-PEG-2g (Figure 3A). The infrared- calibration polarization curve of NMO-PEG-3g exhibits favorable catalytic activity for HER with an onset potential of 36.3 mV. Under the same over-potential 0.1 V, NMO-PEG-3g exhibits better catalytic activity than that of NMO and NMO-PEG-2g. At 10 and 100 mA cm⁻², the NMO-PEG-3g catalyst obtains 140 and 256 mV over-potential, respectively.

FIGURE 3

Figure 3. (A) LSV curves of NMO, NMO-PEG-2g, and NMO-PEG-3g detected in 1 M KOH at a sweep rate of 5 mV s⁻¹; (B) Tafel plots for LSV curves of NMO, NMO-PEG-2g, and NMO-PEG-3g; (C) 1st, 1,000th, and 2,000th LSV curves at sweep rate of 50 mV s⁻¹; (D) Stability test of NMO-PEG-3g catalyst at an over-potential of 112 mV for 25 h.

Tafel slope is an important property inherent of the HER catalyst. Figure 3B exhibits the Tafel plots of these catalysts' series. Accordingly, NMO-PEG-3g exhibits a small Tafel slope of 94 mV dec⁻¹ (Figure 3B), which is much lower compared with NMO-PEG-2g (157 mV dec⁻¹) and NMO (189 mV dec⁻¹), demonstrating a faster HER kinetics of NMO-PEG-3g. These values mean the HER that occurred on NMO-PEG-3g catalyst follows the Volmer-Heyrovsky mechanism. The electrochemical desorption is the rate determining step. Stability is a fatal parameter that estimates the property of HER catalyst. At the LSV of 2,000th cycles, the performance of the NMO-PEG-3g improves than that at 1,000th cycles (Figure 3C). The cause of this phenomenon may be that the catalyst surface is activated in the process of electrochemical reaction, which fortifies reaction active sites. Figure 3D displays that NMO-PEG-3g endures the stability measurement of 112 mV for 25 h. As shown in Figure 3D, NMO-PEG-3g could keep a favorable HER current density at 14 mA cm⁻².

The principal parameters of catalytic activities could be the amount of reactive sites, electrochemically active surface area (ECSA) and charge transfer rate (Qu et al., 2016; Du et al., 2017). The ECSA is crucial to the HER catalytic reaction procedure. The electrochemical double-layer capacitance (C_dl) can be conducted to calculate the ECSA.

$\begin{array}{ll}\text{ECSA}=\frac{C_{\text{dl}}}{C_{\text{s}}}& (1)\end{array}$

C_s is the specific capacitance of the catalyst (mF cm⁻²). The Cs is generally valued as 0.040 mF cm⁻² in 1 M KOH. Cyclic voltammetry test is proceeded to verify the C_dl at different scan rates in the non-faradaic potential region. As the chart shows, these test outcomes show that the as prepared NMO-PEG-3g possesses the biger C_dl than NMO and NMO-PEG-2g (Figures 4A–D). The C_dl of NMO-PEG-3g is derived to be 78.93 mF cm⁻². The big numerical value of C_dl guarantees a competitive ECSA and efficient HER (shown in Table 1). BET specific surface area is identified to be immediate real surface area of catalyst (Sun et al., 2018). The S_BET of NMO-PEG-3g is 29.27 m² g⁻¹, which is bigger than those of NMO and NMO-PEG-2g.

FIGURE 4

Figure 4. (A) CV curves of NMO; (B) CV curves of NMO-PEG-2g; (C) CV curves of NMO-PEG-3g (at different scan rates of 20, 40, 60, 80, 100, 120, and 140 mV s⁻¹ in the non-faradaic potential region in 1 M KOH); (D) current density variation plotted against scan rate fitted to a linear regression enables the estimation of C_dl; (E) Nyquist plots of as-prepared catalysts; (F) quantitative H₂ measurement via water displacement.

TABLE 1

Table 1. Electrochemical parameters of the NiMnO as the HER catalyst in alkaline medium.

Turnover frequency (TOF) is a pivotal parameter to assess the HER activity of catalysts. TOF denotes the number of H₂ molecules generated per second per active site. TOF was inspected according to a method reported by scientists (Popczun et al., 2013, 2014; Zhou H. et al., 2016). Thus, the number of electrochemically effective surface sites on the catalyst was calculated as the following Equations (2) and (3):

$\begin{array}{l}\frac{\#Surfacesites(catalyst)}{c{m}^{2}geometricarea}=\frac{\#Surfacesites(flatstandard)}{c{m}^{2}geometricarea}\\ \times Roughnessfactor& (2)\end{array}$

$\begin{array}{ll}TOFpersite=\frac{\frac{\#TotalHydrogenTurnOvers}{c{m}^{2}geometricarea}}{\frac{\#Surfaceactivesites}{c{m}^{2}geometricarea}}& (3)\end{array}$

Then, deductions reveal that NMO-PEG-3g catalyst has a faster TOF value compared to that of NMO and NMO-PEG-2g. This also proves why the catalyst possesses the favorable activity for electro-catalytic HER. The electrode kinetics for HER was further measured by EIS. EIS measurements and corresponding equivalent circuit in Figure 4E are collected to verify the catalytic reaction mechanism of as prepared catalysts for HER in alkaline media. NMO-PEG-3g exhibits a nice semicircle in the low frequency region. This proves a lower interfacial charge-transfer resistance (R_ct = 10.6 Ω) of NMO-PEG-3g than that of NMO and NMO-PEG-2g. This would be related to the increase in the number of surface-active sites and the reduced ΔG_M−H during the H⁺ discharge reaction step, resulting in superior HER kinetics. The petal-like scales in NMO-PEG-3g catalyst could provide a large reaction area, resulting in faster electron transfer rates and favorable kinetics for HER. As shown in Figure 4F, the quantitative H₂ measurement demonstrates that the Faradic efficiency is close to 100%, which testifies that all charge generated in HER reaction procedures (Popczun et al., 2013) would be devoted to produce H₂.

Conclusions

In conclusion, the addition of PEG surfactant can directly affect the morphology of the prepared NiMnO catalyst by the solvothermal method. As prepared catalysts possess catalytic activities for the HER in alkaline media. Because the NiMnO catalyst prepared by adding 3 g of PEG possesses abundant petal-like scales, it brings a large specific surface area, high reaction efficiency, and has the best electrocatalytic activity. This experiment investigates that the morphology of the catalyst was controlled by changing the amount of surfactant to improve the catalytic activity of catalyst. Moreover, we will investigate the effect of PEG molecular weight on the structure of the prepared catalyst in subsequent experiments.

Data Availability Statement

All datasets generated for this study are included in the article/Supplementary Material.

Author Contributions

JZ, LC, and LL contributed conception and design of the study. JZ organized the database. LC performed the statistical analysis. LL wrote the first draft of the manuscript. WY, HZ, and SC wrote sections of the manuscript. All authors contributed to manuscript revision, read, and approved the submitted version.

Funding

This work was supported by the National Natural Science Foundation of China (No. 21776051) and Natural Science Foundations of Guangdong (No. 2018A030313423).

Conflict of Interest

The authors declare that the research was conducted in the absence of any commercial or financial relationships that could be construed as a potential conflict of interest.

Supplementary Material

The Supplementary Material for this article can be found online at: https://www.frontiersin.org/articles/10.3389/fchem.2020.00281/full#supplementary-material

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