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Article

Bi/CeO2–Decorated CuS Electrocatalysts for CO2-to-Formate Conversion

by
Qi Wang
,
Tianshuang Bao
,
Xiangchuan Zhao
,
Yue Cao
,
Jun Cao
,
Qiaoling Li
* and
Weimeng Si
*
School of Materials Science and Engineering, Shandong University of Technology, Xincunxi Road 266th, Zibo 255000, China
*
Authors to whom correspondence should be addressed.
Molecules 2024, 29(13), 2948; https://doi.org/10.3390/molecules29132948
Submission received: 21 April 2024 / Revised: 14 May 2024 / Accepted: 13 June 2024 / Published: 21 June 2024
(This article belongs to the Special Issue Efficient Catalytic CO2 Chemical Fixation)
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Versions Notes

Abstract

:
The electrocatalytic carbon dioxide (CO2) reduction reaction (CO2RR) is extensively regarded as a promising strategy to reach carbon neutralization. Copper sulfide (CuS) has been widely studied for its ability to produce C1 products with high selectivity. However, challenges still remain owing to the poor selectivity of formate. Here, a Bi/CeO2/CuS composite was synthesized using a simple solvothermal method. Bi/CeO2–decorated CuS possessed high formate selectivity, with the Faraday efficiency and current density reaching 88% and 17 mA cm−2, respectively, in an H-cell. The Bi/CeO2/CuS structure significantly reduces the energy barrier formed by OCHO*, resulting in the high activity and selectivity of the CO2 conversion to formate. Ce4+ readily undergoes reduction to Ce3+, allowing the formation of a conductive network of Ce4+/Ce3+. This network facilitates electron transfer, stabilizes the Cu+ species, and enhances the adsorption and activation of CO2. Furthermore, sulfur catalyzes the OCHO* transformation to formate. This work describes a highly efficient catalyst for CO2 to formate, which will aid in catalyst design for CO2RR to target products.

1. Introduction

In recent decades, the utilization of fossil fuels as energy sources has resulted in a notable rise in the concentration of carbon dioxide (CO2) in the atmosphere. This increase poses a threat to the sustainable development of societies [1]. The electrocatalytic CO2 reduction reaction (CO2RR) has emerged as a promising approach for transforming CO2 into valuable products using electricity derived from renewable energy sources [2,3,4]. This electrochemical process involves multielectron/proton transfer mechanisms to convert CO2 into various chemicals, such as CO, HCOOH, CH4, CH3OH, C2H4, CH3COOH, and CH3CH2OH [5,6,7,8]. In these processes, the reduction to formic acid, which is usually considered an economically viable and atom-economic target, only requires two proton-coupled electron transfers [9]. Metals, like Zn, Sn, Bi, Pb, Au, and Ag, that have weaker binding capacities for CO intermediates may produce CO or HCOOH [10,11]. In general, the formation of the product involves three steps: (1) the adsorption of reactants on the surface of the electrocatalyst; (2) the proton-coupled electron transfer to the reactants; and (3) the desorption of electrocatalyst surface products [12,13,14]. At present, there are three pathways for CO2 to generate HCOOH that proceed via *OCHO, *COOH, and *H intermediates, where * represents the holes on the catalyst surface or adsorption intermediates [15]. Koh et al. showed using theoretical calculations that the *OCHO pathway is more energetically favorable on a bismuth (Bi) surface [16]. First, the CO2− radical anion is formed by single-electron transfer to CO2 in which the oxygen in the CO2− radical anion binds to the electrode surface [17]. In this case, protonation occurs on the carbon atom and the HCOO* intermediate forms. Then, the *OCHO intermediate is formed by electron transfer. Finally, HCOOH is generated by the *OCHO protonation step [12,18]. Bi–based catalysts have attracted attention owing to their low toxicity and cost [19]. However, the high overpotential for CO2RR to HCOOH and poor electronic conductivity hinder the electrocatalytic performance for the selective generation of HCOOH. In addition, owing to the inevitable complex reaction pathways and inherent low efficiency, the activity and selectivity of Bi–based electrocatalysts need to be further improved [20]. The addition of Bi on other metal substrates improves the stability of the catalysts [21]. Additionally, the introduction of a second metal regulates the electronic structure of the catalyst, thereby enhancing its selectivity, stability, and activity towards CO2RR. As a CO2RR catalyst, copper (Cu) has high electronic conductivity and tunable selectivity. Thus, Cu has been introduced into Bi to form bimetallic Bi–Cu materials that can enhance the conversion of CO2 to HCOOH [22]. These Cu–Bi alloys can be prepared by co-deposition, which expands the interfacial active area for CO2RR. The CuBi3 catalyst has an exceptional electrochemical performance for CO2RR towards HCOOH, with a Faraday efficiency (FE) of ~98.4% and a HCOOH partial current density of 21.2 mA cm−2 in 0.1 M KHCO3. The CuBi3 catalyst has the ability to regulate electronic states and has outstanding adsorption of CO2, providing a lattice and spatially constrained environment for active sites [23]. Copper sulfide (CuS) produces C1 products with high selectivity [24], and sulfur (S) can change the electronic properties of Cu, thereby influencing its capacity to adsorb pertinent intermediates like HCOO* [25]. Chen et al. prepared CuS catalysts with different morphologies and compositions by adjusting the Cu/S raw material ratio and the reaction temperature. In the solvothermal synthesis, the higher Cu/S ratio and reaction temperature leads to a relatively high selectivity of CuS nanoflowers for the production of HCOOH, with an FE of ~52% [26]. A Cu electrode with different oxidation states (Cu+ and Cu0-dominated) is capable of directing specific CO2RR pathways to generate HCOOH [27]. However, the in situ formation of Cu+ is insufficient and easily reduces to Cu0. Therefore, precisely controlling the local structure of the catalysts to generate stable and abundant Cu+ active sites is required to improve the activity and selectivity of the catalysts. Chen et al. reported that Cu+ is stabilized by the strong interaction between CuO and CeO2 for the highly selective electrocatalytic reduction of CO2 to ethylene under mild conditions. Adjusting the CuO/CeO2 interface interaction significantly inhibits proton reduction and enhances CO2 reduction. In 0.1-M KHCO3, the ethylene FE is as high as 50.0% at −1.1 V vs. the reversible hydrogen electrode (RHE) [28]. Although previous studies on Cu–based catalysts have made great progress, it is still difficult to control the selectivity of CO2RR in Cu–based catalysts owing to the elusive influence of various entanglement factors on the complexity of the CO2RR pathway.
In this study, a simple strategy for the preparation of Bi– and CeO2–loaded CuS composites using the dissolution heat method is introduced. A synthesized Bi/CeO2/CuS catalyst was used to study the electrocatalytic performance of CO2RR to formate. Electrochemical tests demonstrated that Bi/CeO2/CuS effectively catalyzed the generation of formate from CO2, achieving a FEformate of 88% and current density of 17 mA cm−2. The incorporation of CeO2 enhanced conductivity and stabilized Cu+, which promoted CO2 adsorption and activation. The CuS structure of the Bi coating protected the stable existence of S and prevented the air-based oxidation of Cu. This study provides an effective catalyst for the production of HCOOH through CO2RR and helps to promote catalyst designs for CO2RR target products.

2. Results and Discussion

Figure 1a,b present scanning electron microscope (SEM) images of CuS that display flower-like shapes. The nanosheets possessed smooth surfaces and had an interval range of 0.5–1 μm. A CuS catalyst loaded with Bi and CeO2, as shown in Figure 1c,d, revealed an uneven surface, and the nanosheets exhibited rough surfaces that are thicker at the edges. The uneven surface offered a high specific surface area. In addition, the nanoflower morphology provided more under-coordinated sites for CO2RR.
Figure 2a presents transmission electron microscope (TEM) images of a Bi/CeO2/CuS catalyst. There was material cover around the CuS. The lattice interplanar spacings of nanosheets measured 0.26 nm, 0.34 nm, and 0.31 nm, corresponding to the (200) plane of Bi2O3, the (111) plane of CuS, and the (111) plane of CeO2 [29,30], respectively (Figure 2b). CeO2 covered the surface of the CuS, providing oxygen to the neighboring Cu [31]. Figure 2c–g show the elemental distributions of Cu, S, and Ce. The distribution of CeO2 on the surface of the CuS nanosheets was uniform, and there was no observed particle agglomeration.
The crystal structure of the sample was analyzed using X-ray diffraction (XRD), and the diffraction spectra (Figure 3) displayed distinctive peaks at the 2θ positions of 29.2°, 31.7°, 32.8°, and 47.9°, which corresponded to the CuS crystals (PDF#06–0464) [32]. The peaks at the 2θ positions of 29.2°, 33.07°, 46.7°, and 56.34° corresponded to the CeO2 crystals (PDF#43–1002). The XRD pattern of the Bi/CeO2/CuS catalyst revealed clear diffraction peaks of Bi2O3 and CeO2 [33,34]. These results indicated the successful preparation of Bi/CeO2/CuS.
The valence and electronic structures of the elements Cu, S, and Ce in the Bi/CeO2/CuS catalyst were investigated using XPS. In the Cu 2p spectrum (Figure 4a), two main peaks appeared at 932.38 eV and 952.23 eV, corresponding to Cu 2p3/2 and Cu 2p1/2, respectively. These could be divided into Cu2+2p3/2 (932.13 eV), Cu2+2p3/2 (933.83 eV), Cu2+2p1/2 (952.13 eV), and Cu2+2p1/2 (954.13 eV) [35]. The two subpeaks with binding energies located at ~931.58 and 951.28 eV indicated the presence of Cu–S bonds. The characteristic peaks at ~933.3 and 954.13 eV, as well as two satellite peaks at 945.23 eV and 963.08 eV, were attributed to Cu–O for the surface oxidation of Cu in air [28,36]. For Bi/CeO2/CuS, a positive shift of Cu 2p was observed, indicating that electron transfer occurred on the surface of the Cu [22]. The two peaks in the S 2p XPS spectrum (Figure 4b) with binding energies at 164.43 eV and 165.13 eV were attributed to S 2p3/2 and S 2p1/2, corresponding to metal sulfide [24]. In the Ce 3d spectrum, as shown in Figure 4c, the peaks of CeO2 at 881.23, 887.18, 899, 903.53, 909.03, and 914.53 eV were attributed to the mixed configurations of the 3d94f1, 3d94f2, and 3d94f0 Ce4+ states. The peaks at 884.78 and 908.78 eV were attributed to the mixed configuration of the 3d94f1 and 3d94f2 Ce3+ states. Thus, CeO2 contained Ce3+ and Ce4+ [28]. In addition, the binding energies of the Ce elements in the Bi/CeO2/CuS composite were less than that of CeO2, indicating that CeO2 gained electrons, and the electron cloud density of CeO2 in the Bi/CeO2/CuS composite materials increased [37]. As shown in Figure 4c, the Bi 4f spectrum had four peaks at 157.88, 159.68, 163.28, and 165.03 eV. The first double peak at 157.88 and 163.28eV corresponded to the Bi 4f7/2 and 4f5/2 of Bi0 [38]. The second double peak at 159.68 and 165.03 eV was attributed to a layer of Bi2O3 [22].
The catalytic performances of Bi/CeO2/CuS were investigated in a sealed H-type electrolytic cell with a three-electrode system. The experiment utilized a CO2–saturated 0.5 M KHCO3 electrolyte. Figure 5a shows the linear sweep voltammetry (LSV) curves of CuS, CeO2, and Bi/CeO2/CuS in N2–saturated and CO2–saturated electrolytes with a scan rate of 10 mV s−1. For the lack of active sites, CeO2 does not respond to CO2. The cathodic current densities in the CO2–saturated electrolytes were higher than those in the N2–saturated electrolytes within the potential range of −0.2 V to −1.1 V vs. RHE. Additionally, the Bi/CeO2/CuS catalysts had lower onset potentials than the CuS in the CO2–saturated electrolytes. Furthermore, the current density of the Bi/CeO2/CuS was significantly higher than that of the CuS, suggesting that Bi/CeO2/CuS has a comparatively superior activity of CO2RR [22]. At a potential of −1.1 V vs. RHE, the current density of CeO2/CuS reached 47.3 mA cm−2, which was 1.3 times higher than that of the CuS. This enhancement was attributed to the reduction of Ce4+ to Ce3+ in CeO2, which created a conductive network (Ce4+/Ce3+) and improved the conductivity of the catalyst, enhancing the electrocatalytic performance of the CuS.
To further demonstrate the superior electrocatalytic performance of Bi/CeO2/CuS over CuS, CV curves were obtained at different scanning speeds (20, 40, 60, 80, and 100 mV s−1) (Figure 5b), and the electrochemical active area of the sample was evaluated by calculating the double-layer capacitance (Cdl). As shown in Figure 5c, the Cdl (8.67 mF cm−2) of Bi/CeO2/CuS was greater than that of CuS (3.24 mF cm−2). The addition of CeO2 effectively increased the active area of the reaction, and the unique structure of Bi/CeO2/CuS resulted in good electrocatalytic activity. To reveal the mechanism behind the performance enhancement, the reaction kinetics of the catalyst in the electrocatalytic reduction of CO2 were studied. The Tafel slope was obtained by fitting the LSV curve to evaluate different catalysts’ CO2RR kinetic performances. As shown in Figure 5d, the Tafel slope of Bi/CeO2/CuS (399.4 mV dec−1) was much smaller than that of CuS (799.7 mV dec−1), indicating that Bi/CeO2/CuS is more prone to generate *CO2− intermediates compared with CuS [39,40]. In a further comparison of the conductivity of the CuS and Bi/CeO2/CuS catalysts, the electrochemical impedance spectra of CuS and Bi/CeO2/CuS were determined in 0.1-M CO2–saturated KHCO3 solution at −0.9 V vs. RHE. As shown in Figure 5e, the Bi/CeO2/CuS exhibited an obviously smaller equivalent series resistance than that of CuS, illustrating its faster catalytic kinetics [41]. In addition, chronocoulometry was used to evaluate the electrochemically effective area of the catalysts (Figure S5), which were 0.0132 cm2 and 0.032 cm2 for CuS and Bi/CeO2/CuS, respectively. This indicated that the Bi/CeO2/CuS catalyst possessed a high electroactive surface area, which enhanced the electrochemical response [42].
The electrocatalytic reduction of CO2 by Bi/CeO2/CuS was investigated at various constant potentials using the constant potential method. The liquid product obtained from electrocatalytic CO2 production was found to be pure formate (Figure 6a and Figure S3). Figure 6a shows the FEs for formate production from the catalysts at different potentials, with Bi/CeO2/CuS exhibiting the highest FE for formate at all potentials. The maximum FE of formate reached 88% at −0.9 V vs. RHE. Compared with the Bi/CeO2/CuS catalyst, the FEHCOOH of CuS was significantly lower. These results indicated that Bi/CeO2/CuS had the highest electrochemical reduction activity for CO2. Moreover, the FE of Bi/CeO2/CuS was higher than that of CuS, suggesting that Bi/CeO2/CuS is more suitable for the electrochemical reduction of CO2 and that it exhibits higher selectivity towards formate. This can be attributed to the S atom energy in the Cu lattice, which effectively reduces the Gibbs free energy for the conversion of CO2 into *OCHO intermediates. These intermediates play crucial roles in the formation of formate. Additionally, Bi doping is conducive to the adsorption and activation of CO2 and accelerated electron transfer processes [43]. Therefore, Bi/CeO2/CuS demonstrates the capability to generate formate with high selectivity [44,45]. Ce4+ in CeO2, which is easily reduced at a negative potential [46], stabilizes Cu+ species. This increases the adsorption and activation of CO2, as well as the conversion of HCOO* intermediates, which further improves the FE of formate. Figure 6b shows the FE of formate at different potentials, with a potential window of −0.4 V to −0.9 V vs. RHE for the generation of formate for Cu–based catalysts [47]. The FE of formate decreased when the applied constant potential was more negative than −0.9 V vs. RHE, which was caused by transport limitations [48]. The formate partial current densities of the catalysts at different point positions were calculated and compared. As shown in Figure 6c, the formate partial current density of Bi/CeO2/CuS was higher than that of CuS, showing an increasing trend from −0.8 V to −1.05 V vs. RHE. To further verify the stability of Bi/CeO2/CuS in the electrocatalytic reduction of CO2, a constant potential test was carried out at a potential of −0.9 V vs. RHE (Figure 6d). The Bi/CeO2/CuS catalyst exhibited an apparently stabilized FEHCOOH and current density at −0.9 V vs. RHE in CO2–saturated 0.5-M KHCO3 for over 6 h. Meanwhile, the FEHCOOH remained above 85%.
The structural stability of Bi/CeO2/CuS after CO2RR at −0.9 V vs. RHE was characterized by XRD and SEM. As shown in Figure 7a, the obvious diffraction peak belonged to carbon paper. Other peaks correspond to the main peak position of Bi/CeO2/CuS (29.2–32.8°, 46.7–48.2°, 55.2°, 58.6–59.5°). Affected by the C peak, the peak resolution of Bi/CeO2/CuS is reduced, merging into a typical broad peak. Figure 7b show the SEM images after the reaction. The morphology remains uniform particles, similar to the morphology before the reaction. Based on the XRD and SEM results, we believe that the catalysts are relatively stable. Comparing with the previous results in Table 1, it can be seen the Bi/CeO2/CuS fabricated in this research has good performance as a CO2 electrochemical catalysts.
The possible reaction pathway of CO2RR to HCOOH over the Bi/CeO2/CuS catalyst is shown in Figure 8. The CO2 was adsorbed by the catalyst, and it captured an electron and proton to form the *COOH intermediate, which was further converted into HCOOH with the help of electrons. In addition, the HCOO* intermediate produced HCOOH [25]. Specifically, the adsorbed CO2 was activated to form *CO2, the *CO2 was protonated to form the HCOO* intermediate, and proton–electron transfer formed HCOOH [49]. The mechanism is as follows [24,25]:
CO2 + e− → *CO2−
*CO2− + H+ → *OCHO
*OCHO + e− + H+ → HCOOH.
The HCOO* intermediate generated HCOOH on Cu (111) through proton–electron pair transfer (formate binds to the surface through its O atom) [14]. The doping of S into Cu (111) affects the formation of HCOOH. The presence of S weakens the adsorption and desorption of HCOO* and *COOH, and inhibits the formation of CO [24]. Additionally, the presence of S species facilitates the formation of the key *OCHO intermediates toward HCOOH production [50]. Furthermore, the incorporation of S into the Cu surface lowers the performance of the Cu catalyst for H2 evolution [51]. However, the addition of CeO2 forms a Ce3+/Ce4+ conductive network, which improves the catalyst’s conductivity [46], reduces the electron density of the Cu2+ site, and changes the valence state of Cu at the Bi/CeO2/CuS interface [28]. The Bi nanoparticles provide active sites and facilitate electron transfer.
Table 1. Comparison of FEHCOOH for Bi/CeO2/CuS electrode with reported Cu–based electrocatalysts.
Table 1. Comparison of FEHCOOH for Bi/CeO2/CuS electrode with reported Cu–based electrocatalysts.
CatalystsCell TypeElectrolyteFE(%)Current Density
(mA cm−2)		Ref.
Cu-xSH-cell0.1 M KHCO37413.9[52]
CuSxH-cell0.1 M KHCO37512[24]
Cu7S4 NSsFlow cell1 M KOH82.7456[53]
GDY/CuSxH-cell0.1 M KHCO37065.6[54]
CuS/N,S-rGOH-cell0.5 M KHCO38224.2[36]
Sn–Cu@SnGDE1 M KHCO384.230[55]
CuBi3H-cell0.1 M KHCO398.421.2[23]
Bi@NCAH-cell0.5 M KHCO395–[43]
Bi-PVP/CC-600H-cell0.5 M KHCO38154[56]
Bi-NFsH-cell0.1 M KHCO392.328.5[41]
Bi/CeO2/CuSH-cell0.5 M KHCO38817This work
Cu-xS: Sulfur-doped Cu2O–derived Cu catalyst; CuSx: Sulfur-doped Cu catalyst; Cu7S4 NSs: Cu7S4 nanosheets; GDY/CuSx: Graphdiyne/copper sulfide heterostructure; CuS/N,S-rGO: CuS anchored on nitrogen and sulfur Co-doped graphene; Sn–Cu@Sn: Sn–Cu@Sn dendrites that have a core@shell architecture. CuBi3: Co-deposition to prepare Cu–Bi alloy. Bi@NCA: Bi nanoparticles were anchored on N–doped carbon aerogel. Bi-PVP/CC-600: Ultrasmall Bi nanoparticles confined in carbon nanosheets. Bi-NFs: Bi nanoflowers.

3. Experimental Section

3.1. Materials

Copper chloride dihydrate (CuCl2·2H2O, AR, 99%), thiourea (CH4N2S, AR, 99%), ethylene glycol (C2H6O2, AR, 98%), cerium (III) nitrate hexahydrate (Ce(NO3)3·6H2O, 99.9%), bismuth (III) nitrate hexahydrate (Bi(NO3)3·5H2O, AR.), nafion (5 wt.%), potassium bicarbonate (KHCO3), dimethyl sulfoxide (C2H6OS), deuterium oxide (D2O), and absolute ethanol were purchased from Macklin, Shanghai, China. CO2 (99.999%) was purchased from Shandong Baiyan Chemical Co., Ltd., Zibo, China. Carbonized paper (hydrophobic) was purchased from Shanghai Hesen Electric Co., Ltd., Shanghai, China.

3.2. Catalyst Preparation

3.2.1. Synthesis of CuS Nanosheets

The CuS nanosheets were prepared in accordance with the solvothermal method [50]. Briefly, 0.85 g CuCl2·2H2O was dissolved in 30 mL ethylene glycol and stirred for 30 min in water bath at 90 °C. The mixture was stirred to obtain a uniform solution. Then, 1.52 g thiourea dissolved in 25 mL ethylene glycol was added slowly into the CuCl2·2H2O solution, and stirring continued for 30 min. The mixture was transferred to 100 mL polytetrafluoroethylene-lined stainless steel high-pressure reactor at 170 °C for 5 h. Finally, the obtained black product was centrifuged and washed several times with absolute ethanol and deionized water. It was then dried in a vacuum oven at 60 °C for 6 h to obtain CuS nanosheets.

3.2.2. Synthesis of Bi/CeO2/CuS Nanosheets

Briefly, 100 mg of CuS nanosheets was dispersed into 40 mL of deionized water and stirred for 1 h. Subsequently, 20 mL 0.023 mol L−1 Ce(NO3)3 of ethanol solution was dropped into the CuS dispersion with continuous stirring. Then, 200 mg of Bi(NO3)3·5H2O was added to the solution. The mixture then underwent hydrothermal synthesis at 170 °C for 5 h. Finally, the obtained black product was centrifuged and washed several times with absolute ethanol and deionized water. Then, the obtained powder was dried at 60 °C for 6 h in vacuum oven to obtain Bi/CeO2/CuS nanosheets.

3.2.3. Preparation of Working Electrodes

To construct the cathode electrode, 10 mg of powder prepared above was suspended in 1 mL acetone supplemented with 20 μL Nafion (5 wt%) via ultrasound. Then, the catalyst slurry (0.1 mL) was slowly drop cast onto a PTFE–hydrophobized carbon fiber paper (1 cm × 1 cm) to achieve a catalyst loading of ~1.0 mg cm−2.

3.3. Catalyst Characterization

The crystal structure of the catalyst was analyzed using an X-ray diffractometer from Bruker AXS (Billerica, MA, USA), using Cu Kα radiation in the wide 2θ range of 10–90°. The morphology and elemental mapping images of the catalysts were characterized using an FEI Sirion 200 field emission SEM (Portland, OR, USA). TEM images were recorded on an FEI Tecnai F20 TEM (Portland, OR, USA) at an operating voltage of 200 KV. XPS spectra were recorded on a K-Alpha (Thermo Fisher Scientific Co., Ltd., Waltham, MA, USA) instrument. The liquid product was quantitatively analyzed using a Bruker AVANCE 400 MHz (Billerica, MA, USA) nuclear magnetic resonance spectrometer. A gas chromatograph (Shandong Lunan Ruihong Chemical Instrument Co., Ltd.; SP-7890 Plus, Tengzhou, China) was used for the quantitative analysis of gas products.

3.4. CO2RR Performance

The CO2RR performance of the catalyst was tested using the three-electrode system of CS-350 electrochemical workstation (Wuhan Correst Instrument Co., Ltd., Wuhan, China). The experiment was performed using a sealed H-type electrolytic cell, and an air tightness test was conducted prior to the experiment. The working electrode consisted of catalyst-loaded carbon paper, an Ag/AgCl reference electrode, and a carbon rod counter electrode. A proton exchange membrane was utilized to separate the cathode chamber and the anode chamber, and a 0.5-M KHCO3 solution was employed as the electrolyte. Before each test, continuously bubbling high-purity CO2 (at a rate of 20 mL min−1) into the electrolyte for 30 min is recommended. Cyclic voltammetry scans at a scanning rate of 100 mV s−1 to activate and stabilize the electrode material were performed. LSV was conducted at a scanning rate of 10 mV s−1 in N2–saturated and CO2–saturated 0.5-M KHCO3 solution with a voltage range from 0 to −1.1 V (vs. RHE). The potentiostatic method was used to test the Faraday efficiency of catalysts, with a potential range of −0.7 V~−1.1V (vs. RHE). The Tafel slope (b) was obtained by fitting the linear portion of the Tafel plot to the Tafel equation (η = b lgJ + a) [57]. The test voltage for electrochemical impedance test was −0.1 V, test frequency 105–0.01 Hz, and amplitude 5 mV. Double-layer capacitance was determined by CV with different scan rates from 20 to 100 mV s−1 [58]. All of the electrochemical tests were performed without iR compensation.

3.5. Product Analysis

After electrolysis at a constant potential for 60 min, the gas products were collected using a gas collection bag and analyzed using a gas chromatograph equipped with a hydrogen flame ionization detector for CO and CH4 or a thermal conductivity detector for H2. The concentrations of the gas products were calculated from the ratio of the peak areas of the gas products and the standard gas. The FEs of the gas products were reported as the averages of three measurements.
Liquid products were analyzed by nuclear magnetic resonance spectrometry [59]. To quantify the concentration of formate, the concentration of 0.47-M dimethyl sulfoxide solution was used as the internal standard. A calibration curve was prepared using the NMR peak area of a standard concentration of HCOONa solution relative to the internal standard. Subsequently, the concentration of formate was determined by measuring the NMR peak area of formate relative to the internal standard, using the calibration curve as a reference. This approach enabled the accurate quantification of the formate concentration.
The FE was calculated as follows [60]:
FE (%) = (x × n × F/Q) × 100%,
where x represents the molar amount of the product produced (mol) and n represents the number of electrons transferred to form different products. For example, in the case of formate, n is 2. F represents the Faraday constant (96,485 C mol−1), and Q represents the total amount of electricity consumed throughout the reaction (C).
The FE of gas products was calculated as follows:
FE (%) = (N × Vp × Cst × P × F)/(Vst × R × T× j× t),
where N represents the number of electrons transferred to form gas molecules, Vp represents the peak area of gas products in GC spectrum, Cst represents the volume concentration of standard gas, P represents the standard atmospheric pressure (101.3 kpa), F represents the Faraday constant (96,485 C mol−1), Vst represents the peak area of standard gas in GC spectrum, T represents the room temperature (298 K), j represents the recorded current, and t represents the reaction time.

4. Conclusions

In this work, we demonstrated that Bi/CeO2/CuS can be used as a highly active and selective catalyst for the electrochemical reduction of CO2 to generate formate in a wide potential range. At −0.9 V vs. RHE, the FE of formate reached 88% and the current density was −17 mA cm−2. Bi/CeO2/CuS also showed excellent stability. After a 1 h reaction, FE of formate remained stable at −0.9 V vs. RHE, as did the structure. The S inhibited hydrogen evolution reactions, CeO2 improved the catalyst conductivity, and Bi provided active sites and facilitated electron transfer. This work provides an easily synthesizable catalyst for the generation of formate by electrocatalytic CO2 reduction, and these findings will aid in the rational design of Cu–based catalysts for the electroreduction of CO2.

Supplementary Materials

The following supporting information can be downloaded at: https://www.mdpi.com/article/10.3390/molecules29132948/s1, Reference [41] are cited in the supplementary materials. Figure S1. Survey of Bi/CeO2/CuS. Figure S2. CV curve of CuS. Figure S3. The FE for all products of CuS catalyst. Figure S4. The current density of Bi/CeO2/CuS at different potential. Figure S5. The effective surface area curves of different simples. Figure S6. Standard curve of formate. Figure S7. Formate yield of Bi/CeO2/CuS. Figure S8. (a–c) The NMR of different concentration standard, (d) The NMR of Bi/CeO2/CuS at −0.9 V vs. RHE. Figure S9. (a) The GC of standard, (b) The GC FID 1 image of simple, (c) The GC FID 2 image of simple, (d) The GC TCD image of simple.

Author Contributions

Data curation, formal analysis, and writing—original draft, Q.W.; investigation, methodology, and validation, T.B.; investigation and validation, X.Z.; supervision and validation, Y.C.; investigation and methodology, J.C.; conceptualization, resources, and writing—review and editing, Q.L.; conceptualization, funding acquisition, project administration, supervision, and writing—review and editing, W.S. All authors have read and agreed to the published version of the manuscript.

Funding

This work was supported by the National Natural Science Foundation of China (51502161 and 21706148), the Natural Science Foundation of Shandong Province (ZR2020ME041, ZR2022QB173, ZR2023MB054), the Joint Zibo-SDUT Fund (2019ZBXC358), and the Foundation of State Key Laboratory of Biobased Material and Green Papermaking, Qilu University of Technology (Shandong Academy of Sciences) (KF2019-06).

Institutional Review Board Statement

Not applicable.

Informed Consent Statement

Not applicable.

Data Availability Statement

Data are contained within the article or Supplementary Materials. The data sets generated during and/or analyzed during the current study are available from the corresponding author upon reasonable request.

Conflicts of Interest

The authors declare no conflicts of interest.

References

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Molecules 29 02948 g001
Figure 1. SEM images of (a,b) CuS and (c,d) Bi/CeO2/CuS.
Figure 1. SEM images of (a,b) CuS and (c,d) Bi/CeO2/CuS.
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Figure 2. (a) TEM images of Bi/CeO2/CuS; (b) high-resolution TEM images of Bi/CeO2/CuS; and (c–g) EDS mapping of Bi/CeO2/CuS.
Figure 2. (a) TEM images of Bi/CeO2/CuS; (b) high-resolution TEM images of Bi/CeO2/CuS; and (c–g) EDS mapping of Bi/CeO2/CuS.
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Figure 3. XRD patterns of Bi/CeO2/CuS, CuS, and CeO2.
Figure 3. XRD patterns of Bi/CeO2/CuS, CuS, and CeO2.
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Figure 4. XPS patterns of Bi/CeO2/CuS (a) Cu 2p, (b) S 2p, (c) Ce 3d, and (d) Bi 4f.
Figure 4. XPS patterns of Bi/CeO2/CuS (a) Cu 2p, (b) S 2p, (c) Ce 3d, and (d) Bi 4f.
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Figure 5. (a) LSV curves, (b) CV curves, (c) electrochemical active areas, (d) Tafel plots, and (e) electrochemical impedance spectra of Bi/CeO2/CuS and CuS.
Figure 5. (a) LSV curves, (b) CV curves, (c) electrochemical active areas, (d) Tafel plots, and (e) electrochemical impedance spectra of Bi/CeO2/CuS and CuS.
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Figure 6. (a) FEs of each product of Bi/CeO2/CuS, (b) FEs of formate for Bi/CeO2/CuS and CuS, (c) HCOOH partial current densities of Bi/CeO2/CuS and CuS, and (d) durability test of Bi/CeO2/CuS.
Figure 6. (a) FEs of each product of Bi/CeO2/CuS, (b) FEs of formate for Bi/CeO2/CuS and CuS, (c) HCOOH partial current densities of Bi/CeO2/CuS and CuS, and (d) durability test of Bi/CeO2/CuS.
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Figure 7. (a) XRD pattern and (b) SEM image of Bi/CeO2/CuS after CO2RR.
Figure 7. (a) XRD pattern and (b) SEM image of Bi/CeO2/CuS after CO2RR.
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Figure 8. Schematic diagram of the possible reaction pathways of the CO2RR to HCOOH.
Figure 8. Schematic diagram of the possible reaction pathways of the CO2RR to HCOOH.
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MDPI and ACS Style

Wang, Q.; Bao, T.; Zhao, X.; Cao, Y.; Cao, J.; Li, Q.; Si, W. Bi/CeO2–Decorated CuS Electrocatalysts for CO2-to-Formate Conversion. Molecules 2024, 29, 2948. https://doi.org/10.3390/molecules29132948

AMA Style

Wang Q, Bao T, Zhao X, Cao Y, Cao J, Li Q, Si W. Bi/CeO2–Decorated CuS Electrocatalysts for CO2-to-Formate Conversion. Molecules. 2024; 29(13):2948. https://doi.org/10.3390/molecules29132948

Chicago/Turabian Style

Wang, Qi, Tianshuang Bao, Xiangchuan Zhao, Yue Cao, Jun Cao, Qiaoling Li, and Weimeng Si. 2024. "Bi/CeO2–Decorated CuS Electrocatalysts for CO2-to-Formate Conversion" Molecules 29, no. 13: 2948. https://doi.org/10.3390/molecules29132948

APA Style

Wang, Q., Bao, T., Zhao, X., Cao, Y., Cao, J., Li, Q., & Si, W. (2024). Bi/CeO2–Decorated CuS Electrocatalysts for CO2-to-Formate Conversion. Molecules, 29(13), 2948. https://doi.org/10.3390/molecules29132948

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