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Article

Ce–Metal–Organic Framework-Derived CeO2–GO: An Efficient Electrocatalyst for Oxygen Evolution Reaction

by
Patnamsetty Chidanandha Nagajyothi
1,
Krishnapuram Pavani
2,
Rajavaram Ramaraghavulu
3 and
Jaesool Shim
1,*
1
School of Mechanical Engineering, Yeungnam University, Gyeongsan 38541, Republic of Korea
2
I3N—Department of Physics, University of Aveiro, 3810-193 Aveiro, Portugal
3
Department of Physics, School of Applied Science, REVA University, Bangalore 560064, India
*
Author to whom correspondence should be addressed.
Inorganics 2023, 11(4), 161; https://doi.org/10.3390/inorganics11040161
Submission received: 15 December 2022 / Revised: 24 March 2023 / Accepted: 4 April 2023 / Published: 11 April 2023
(This article belongs to the Special Issue Electrochemical Study of Nanocarbon Based Materials)
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Abstract

:
The oxygen evolution reaction (OER) is a crucial half-reaction in water splitting. However, this reaction is kinetically sluggish owing to the four-electron (4 e−) transfer process. Therefore, the development of low-cost, stable, highly efficient, and earth-abundant electrocatalysts for the OER is highly desirable. Metal oxides derived from metal–organic frameworks (MOFs) are among the most efficient electrocatalysts for the OER. Herein, Ce–MOF-derived CeO2/graphene oxide (GO) composites were successfully prepared using a facile method. The composites with 0, 25, 50, and 100 mg GO were named CeO2, CeO2–GO-1, CeO2–GO-2, and CeO2–GO-3, respectively. The physicochemical characteristics of the electrocatalysts were assessed using several analytical techniques, including X-ray diffraction (XRD), scanning electron microscopy (SEM), high-resolution transmission electron microscopy (HR-TEM), X-ray photoelectron spectroscopy (XPS), and Brunauer–Emmett–Teller (BET) analysis. The TEM results revealed that the CeO2 had a sheet-like morphology and that a GO layer was noticeable in the synthesized CeO2–GO-3 composite. The characterization results confirmed the formation of impurity-free CeO2–GO composites. The OER activity and stability were measured using cyclic voltammetry (CV), linear sweep voltammetry (LSV), chronoamperometry (CA), and electrochemical impedance spectroscopy (EIS). The CeO2–GO-3 electrocatalyst has a smaller Tafel slope (176 mV·dec−1) and lower overpotential (240 mV) than the other electrocatalysts. In addition, it exhibited high cyclic stability for up to 10 h. Therefore, the inexpensive CeO2–GO-3 electrocatalyst is a promising OER candidate.

1. Introduction

Electrochemical water splitting is a promising method for producing pollution-free, clean hydrogen [1]. Water electrolysis consists of two half-reactions (OER and HER): the oxygen evolution reaction at the anode and the hydrogen (H2) evolution reaction at the cathode [2]. However, the OER is kinetically slow owing to its four-electron transfer process [3]. Therefore, highly effective and reliable OER electrocatalysts must be developed to address this limitation. Noble metal oxide catalysts, such as RuO2 and IrO2, are among the most efficient electrocatalysts for OER activity; however, their high prices and scarcity limit their large-scale application [4]. Therefore, the development of OER electrocatalysts with high activity, long-term stability, and low cost is essential.
Metal-organic frameworks (MOFs) are a new class of porous materials composed of metal ions or clusters connected to organic ligands via coordination bonds to form one-dimensional, two-dimensional, and three-dimensional (1D, 2D, and 3D) structures [5]. Recently, MOFs have emerged as promising candidates for energy- and environment-related applications [6,7] owing to their unique characteristics, such as high porosity, high specific surface areas, good thermal stability, and ease of modification [8,9]. However, the poor electrical conductivity of pure MOFs limits their use in electrochemistry applications [10]. To overcome these limitations, the conversion of MOFs (MOFs as precursors or templates) into metal oxides, porous carbon materials, metal hydroxides [11], metal phosphides [12], metal sulfides [13], selenides [14], or their composites [11,15] has been widely investigated for electrochemical applications.
MOF-derived materials exhibit unique properties, such as tailorable morphologies, hierarchical porous structures, chemical and structural stabilities, high electrical conductivity, and simple surface functionalization [16]. Moreover, they play significant roles in various energy-related applications, such as lithium-ion batteries [17], OER [18], methanol oxidation reactions [19], urea oxidation reactions [20], fuel cells [21], and HER [22]. Gao Han et al. [23] synthesized a bimetal oxide CuCoO2 using ZIF-67 and Cu-BTC (Co and Cu sources) through a single-step solvothermal procedure. The synthesized CuCoO2 was used as an electrocatalyst for the OER. With a low overpotential, a smaller Tafel slope, and good durability in a 1.0 M KOH solution, the synthesized CuCoO2 exhibited higher OER activity.
Cerium oxide, also known as ceria (CeO2), has drawn considerable attention owing to its low cost, non-toxicity, earth-abundance, and tunable oxygen vacancies via a reversible transition between the Ce3+ and Ce4+ oxidation states, and high oxygen (O2) storage capacity [24,25]. These properties make CeO2 a promising material for various applications, such as photocatalytic, forensic, electrochemical [26], and humidity sensors [27], as well as catalytic oxidation [28], supercapacitors [29], and biological [30] applications. However, pure CeO2 exhibits limited OER/ORR performance owing to its weak electronic conductivity [25,31]. The best method to improve the dispersibility and conductivity of CeO2 is through deposition on conducting carbon-based materials [31].
Graphene oxide (GO) is the oxidized form of graphene with a layered structure and shows good mechanical, electrical, and thermal properties due to its structural and morphological characteristics [32,33]. GO structures comprise oxygen-based functional groups, such as hydroxyl (–OH), carboxyl (–COOH), epoxide (C–O–C), and carbonyl (C=O), that enable the dispersibility of the material in water [33,34]. In addition, as these oxygenated functional groups are chemically active, GO can be decorated with a variety of materials [35], such as metals, metal oxides, ZIFs, MOFs, and MOF-derived metal oxides. GO-based composites have a high potential for various applications in energy- and environment-related fields, including dye removal (GO/SiO2NH2) [36], heavy metal removal (TiO2/GO) [32], photochemical degradation of toluene (GO-TiO2) [37], proton exchange membrane fuel cell (CeO2–GO) [38], supercapacitors (GO, GO–CuO, and GO–ZnO) [39], OER (CeO2/Cu–MOF/GO) [40], HER (Pd@GO/MOF) [41], OER, ORR, and Zn–air batteries (ZnCo–ZIF@GO) [42]. Malik et al. [43] synthesized CeO2 from a GO@Ce–MOF precursor and used it as an electrocatalyst for OER applications. According to Dongyang et al. [44], a simple chemical co-precipitation process was used to produce CeO2 nanoparticles decorated on GO. CeO2/GO is used as an electrode material in supercapacitor applications; the CeO2/GO electrode demonstrated exceptional supercapacitive behavior with high specific capacitance. Kasinath and Byrappa [45] synthesized hexagonal CeO2@nitrogen-doped GO composites for OER and ORR studies. The CeO2/NGO composites revealed a high anodic onset potential for ORR and OER activity (0.925 V vs. RHE for ORR and 1.2 V for OER) with a high current density in 0.5 M KOH.
In this study, we successfully synthesized Ce–MOF-derived CeO2–GO composites using a simple, room-temperature synthesis method followed by annealing at 400 °C in the air for 1 h. The as-synthesized composites were used as electrocatalysts for the OER. Compared with the CeO2–GO-1 and CeO2–GO-2 composites, the CeO2–GO-3 electrocatalyst exhibited higher OER activity and stability. The synthetic process is illustrated in Scheme 1.

2. Results and Discussion

2.1. Characterization of the Electrocatalysts

Figure 1a displays the X-ray diffraction (XRD) patterns of the pristine CeO2 and CeO2–GO electrocatalysts. The XRD data of Ce–MOF, as shown in Figure S1, exhibit sharp and narrow peaks. All diffraction peaks matched the XRD patterns of previous reports [46,47]. After calcination, the Ce–MOF was fully converted into cubic-structured CeO2. The four characteristic peaks at 28.4°, 33.1°, 47.3°, and 56.3° can be attributed to the (111), (200), (220), and (311) planes (Figure 1a) [48], which are in good agreement with JCPDS 00-004-0593. The average crystallite size was found using the Debye–Scherrer equation [49],
D = k λ β   c o s θ
where D is the average crystallite size (nm), k is constant (0.9), λ is the wavelength of X-ray radiation (1.5416 Å), θ is diffraction angle, and β is the full-width half maxima of diffraction peaks. From XRD data, the average size was found to be in the range of 10 to 15 nm. The calculated lattice parameters and volume were found to be (for pure cubic structure a = b = c; α = β = γ = 90°) a = 1.5411 Å and V = 161.05 Å3. Malik et al. [43] reported similar results for CeO2 derived from the GO–Ce–MOF. A GO peak in the CeO2–GO electrocatalysts was noted at 10.8° (001), indicating the presence of GO in all synthesized samples [50]. Compared with CeO2–GO-1 and CeO2–GO-2, the CeO2–GO-3 electrocatalyst showed the peak (10.8°) intensity, increasing with an increase in graphene oxide.
The Fourier-transform infrared spectra (FTIR) of the pure CeO2 and CeO2–GO electrocatalysts are presented in Figure 1b. The FTIR spectrum of GO exhibits a prominent peak at 3409 cm−1, which is attributed to the O–H stretching; further absorption peaks at 1717, 1606, 1258, and 1051 cm−1 correspond to the C=O stretching vibrations, C=C, C–O–C bending, and C–O stretching groups [51,52,53], respectively. A Ce–O stretching vibration was observed in the CeO2–GO composites at 535 cm−1 [43,54]. The bands at 1621 and 1059 cm−1 are related to the bending vibration of the hydroxyl (–OH) groups of water molecules [55] and Ce–O–Ce stretching vibration [56], respectively. Most of the GO peaks were significantly reduced after the CeO2–GO composite formation.
The surface chemical states of the Ce–MOF-derived CeO2 and CeO2–GO-3 electrocatalysts were studied using X-ray photoelectron spectroscopy (XPS; Figure 2a). A survey scan revealed the presence of Ce 3d, O 1s, and C 1s in the electrocatalysts. The Ce 3d spectra of the CeO2 and CeO2–GO-3 electrocatalysts were fitted to eight peaks: the Ce 3d3/2 peaks at 900.1/900.3, 906.7/906.8, and 916.0/916.1 eV; Ce 3d5/2 peaks at 881.6/881.8, 887.9/888.0, and 897.5/897.6 eV, which are associated with Ce4+; and peaks at 884.6/884.8 eV (Ce 3d5/2) and 903.1/903.3 eV (Ce 3d3/2) associated with Ce3+ (Figure 2c). These values are consistent with those reported in the literature [57,58,59]. The deconvolution of the O 1s spectra displayed two peaks at 528.6/528.8 and 531.0/531.1 eV (Figure 2b), which are attributed to the lattice and adsorbed oxygen [60,61]. In the composite, the C 1s spectrum (Figure 2d) peaks at 284.5/284.4, 285.8/286.1, 288.4/288.1, and 289.5 eV are ascribed to the C=C, C-O bonds, carbonyl (C=O), and carboxyl (HO–C=O) bonds [62,63,64], respectively. The 289.5 eV small peak vanished in the CeO2 electrocatalyst but was clearly visible in the CeO2–GO-3 electrocatalyst.
The morphologies of the Ce–MOF-derived CeO2 and CeO2–GO electrocatalysts were characterized via scanning electron microscopy (SEM; Figure 3). The CeO2 sample had a rod-like morphology with the appearance of some merging rods having sheet-like structures (Figure 3a-1,a-2). Kohantorabi and Gholami [65] and Ye et al. [66] reported similar morphologies using benzene-1,3,5-tricarboxylic acid, and cerium nitrate hexahydrate, respectively. CeO2 rods were visible in CeO2–GO-1 and a few GO sheets were observed. The rods were uniformly spread on the GO sheets (Figure 3b-1,b-2). As the GO weight was increased, layered GO sheets with smooth surfaces were observed in the CeO2–GO-2 and CeO2–GO-3 samples (Figure 3c-1–d-2). These results confirmed the successful decoration of CeO2 on the GO sheets.
Energy-dispersive X-ray spectroscopy (EDS) was performed to identify the elements in the electrocatalyst, and the corresponding results are shown in Figure S2. The EDS spectrum validated the presence of O, Ce, and C in the electrocatalyst. Figure 4a,b shows the TEM images of the CeO2–GO-3 electrocatalyst. The synthesized CeO2 was confirmed to have a sheet-like morphology in the TEM images, and a GO layer was visible in the synthesized composites. The HR-TEM images (Figure 4c and Figures S3–S5) showed a fringe spacing of 0.311, 0.315, and 0.163 nm, which is consistent with the d-spacing of the (111), (111), and (311) planes of CeO2. The corresponding selected area electron diffraction (SAED) pattern displayed the polycrystalline nature of the synthesized catalyst (Figure 4d). The ring pattern of the SAED results suggests a similar plane ((111), (222), and (311)); therefore, the electrocatalyst matched well with the XRD results.

2.2. OER Activity

We further explored the OER activity of the synthesized electrocatalysts under alkaline conditions. Figure 5 shows the cyclic voltammetry (CV) curves of the CeO2, CeO2–GO-1, CeO2–GO-2, and CeO2–GO-3 electrocatalysts under the three-electrode setup at room temperature. The CV curves were measured at a constant potential between 0.1~0.6 V against Hg/HgO at various scan rates (5–100 mVs−1). These CV curves revealed that the current density increased with increasing GO content in the electrocatalyst owing to the increase in ion transport between the electrocatalyst (CeO2) and GO (CeO2–GO-3). Similarly, cerium oxide/reduced GO nanocomposites exhibited excellent photocatalytic and supercapacitor activities owing to the increased charge transport between the electrocatalysts [67,68]. Additionally, CeO2/multi-walled carbon nanotube nanocomposites have higher capacitive performance and long-term stability [69], and the electrocatalytic performance increased after the introduction of carbon-based materials. Comparative CV curves of the electrocatalysts at a standard scan rate (60 mV s−1) are shown in Figure S6. All electrocatalysts exhibited cathodic peaks at approximately 0.472, 0.502, 0.489, and 0.514 V and anodic peaks at approximately 0.304, 0.303, 0.301, and 0.296 V for CeO2, CeO2–GO-1, CeO2–GO-2, and CeO2–GO-3, respectively. These CV curves reveal that CeO2–GO-3 exhibits a larger integral area, suggesting its higher electrochemical performance. The CV curves retained faradaic peaks even at higher scan rates, indicating a fast charge transport in the electrode system.
The electrochemical OER activity was measured in the same electrolyte using linear sweep voltammetry (LSV), as revealed in Figure 6a. However, the GO content, which increased the OER performance, also increased, and the CeO2–GO-3 electrocatalyst showed a higher current density at higher potentials. The overpotential decreased with increasing GO content in the electrocatalysts. The overpotentials of the CeO2, CeO2–GO-1, CeO2–GO-2, CeO2–GO-3, and RuO2 electrocatalysts were 420, 360, 300, and 240, and 230 mV, respectively, at a fixed current density of 10 mA cm−2. Among the electrocatalysts, CeO2–GO-3 exhibited a lower overpotential; however, compared with standard RuO2, there was not much difference. The electrocatalytic activity trend during the OER process followed the order CeO2–GO-3 > CeO2–GO-2 > CeO2–GO-1 > CeO2.
The Tafel slope is a crucial parameter for identifying the relationship between the overpotential and steady-state current density of electrocatalysts [66]. Figure 6b shows Tafel slopes of 261, 293, 185, 176, and 101 mV dec−1 for CeO2, CeO2–GO-1, CeO2–GO-2, CeO2–GO-3, and RuO2 electrocatalysts, respectively. The CeO2–GO-3 electrocatalyst revealed a smaller Tafel slope than the other electrocatalysts, showing its higher OER activity owing to the higher percentage of GO. However, compared with RuO2, the CeO2–GO-3 Tafel slope value was higher. The electrochemical active surface area (ECSA) is directly related to the electrochemical performance of the electrocatalysts [69,70]. A higher ECSA indicates better electrochemical performance. In the present work, the ECSA was measured using the CV curves in the non-faradaic region; the corresponding CVs are shown in Figure S7. The CeO2–GO-3 electrocatalyst showed a higher ECSA (57.5 mF cm−2) than the other electrocatalysts (35.4, 39.4, and 40.5 mF cm−2 for CeO2, CeO2–GO-1, and CeO2–GO-2, respectively), as shown in Figure 6c.
Electrochemical impedance spectroscopy (EIS) was used to analyze the electrochemical dynamics of the electrocatalysts. Figure 6d and Table S1 show the EIS analysis of the electrocatalysts. The CeO2–GO-3 electrocatalyst exhibited a smaller Rct than the other electrocatalysts, revealing its lower charge transfer resistance owing to the increased electron transfer rate. The stability of electrocatalysts is a crucial parameter for OER activity. Therefore, chronoamperometry (CA) was used for the room-temperature analysis for approximately 10 h. Figure 6e depicts the CA curves of the electrocatalysts in a 1.0 M KOH solution, where the CeO2–GO-3 electrocatalysts show a higher current density than the other electrocatalysts. Additionally, we compared our as-prepared materials to previously published OER electrocatalysts, which are depicted in Table S2.
The surface area plays a key role in electrochemical studies. In the present work, the surface area was measured via two different methods: the Brunauer–Emmett–Teller (BET) method using nitrogen (N2) gas adsorption and desorption and ECSA using the CV curves in the non-faradaic region of the electrocatalysts. Figure S8 shows the adsorption and desorption curves of the electrocatalysts. According to the IUPAC classification, these curves exhibit Type IV isotherms; all electrocatalysts showed similar type IV isotherms, which can be observed in mesoporous materials with a pore size of 2–50 nm [71]. The CeO2–GO-3 electrocatalyst exhibited a higher BET surface area compared with the other electrocatalysts. In particular, the BET surface values for CeO2, CeO2–GO-1, CeO2–GO-2, and CeO2–GO-3 were 61.58, 80.77, 101.48, and 110.35 m2 g−1, respectively. The pore volume and size of the CeO2–GO-3 electrocatalyst were higher than those of the other electrocatalysts. These values are tabulated in the inset of Figure S8. Therefore, the electrocatalyst with a higher surface area exhibits higher electrocatalytic performance. In the present study, the CeO2–GO-3 electrocatalyst showed a higher surface area and better electrocatalytic performance compared with the other electrocatalysts.

3. Materials and Methods

Ce–MOFs were synthesized using a previously reported method with slight modifications [46]. The required quantity of cerium nitrate hexahydrate (50.0 mM) was dissolved in a mixture of deionized water (DI) and ethanol (v/v of 1:1). Subsequently, trimesic acid (50.0 mM) was added to the milk-white suspension, which was stirred for 1 h at room temperature (RT). Thereafter, the temperature was increased until the solution evaporated. After cooling, the residue was collected and annealed at 400 °C in the air for 1 h to obtain the CeO2 pure phase. The CeO2–GO composites were prepared in the same manner with different GO contents (0, 25, 50, and 100 mg GO, denoted as CeO2, CeO2–GO-1, CeO2–GO-2, and CeO2–GO-3, respectively), as shown in Scheme 1. The chemicals, characterization, electrode preparation, and electrocatalytic performance followed are provided in the Supplementary Information (SI).

4. Conclusions

In this study, we successfully synthesized Ce–MOF-derived CeO2 and CeO2–GO electrocatalysts for the OER. The morphological and structural properties of the electrocatalysts were characterized. The TEM results indicated that the CeO2–GO-3 electrocatalyst had a sheet-like morphology with an effective attachment to the GO sheets. The electrocatalysts produced using a low-cost, stable, and simple synthesis method demonstrated good OER activity in the 1.0 M KOH electrolyte. The CeO2–GO-3 electrocatalyst had a low overpotential of 240 mV at 10 mA·cm−2 and a smaller Tafel slope (176 mV·dec−1) than the CeO2–GO-1 and CeO2–GO-2 electrocatalysts. Moreover, the CeO2–GO-3 electrocatalyst exhibited considerable electrochemical stability over 10 h under alkaline conditions. Thus, this study provides a new method for developing non-noble-metal-based electrocatalysts for clean energy production.

Supplementary Materials

The following supporting information can be downloaded at https://www.mdpi.com/article/10.3390/inorganics11040161/s1: Figure S1: XRD pattern of the pristine Ce–MOF; Figure S2: EDS analysis of CeO2–GO-3 electrocatalyst; Figure S3: d-spacing line profiles corresponding to the 0.311 (111) plane; Figure S4: d-spacing line profiles corresponding to the 0.315 (111) plane; Figure S5: d-spacing line profiles corresponding to the 0.163 (311) plane; Figure S6: Comparative CV curves at standard scan rate in aqueous 1.0 M KOH electrolyte; Figure S7: CV curves of the electrocatalysts in (a) 1.0 M KOH; CeO2, (b) CeO2–GO-1, (c) CeO2–GO-2, and d) CeO2–GO-3; Figure S8: N2adsorption–desorption profiles of CeO2, CeO2–GO-1, CeO2–GO-2, and CeO2–GO-3; Table S1: EIS fitted values and the equivalent circuit; Table S2: Comparison of OER performance of different electrocatalysts [43,72,73,74,75,76,77,78,79,80,81].

Author Contributions

P.C.N.: synthesis, characterization, and application study, K.P.: investigation and conceptualization, R.R.: investigation and writing—original draft, J.S.: resources and funding acquisition. All authors have read and agreed to the published version of the manuscript.

Funding

This research was funded by the National Research Foundation of Korea (NRF) grants funded by the Korean government, grant numbers 2020R1A4A1019227 and 2020R1A2C1012439; and the National Funds (OE) through FCT, Portugal, I.P., in the scope of the framework contract foreseen in numbers 4, 5, and 6 of Article 23 of the Decree-Law 57/2016, of 29 August, changed by Law 57/2017, of 19 July and also within the scope of the project i3N, UIDB/50025/2020 and UIDP/50025/2020, financed by national funds through the FCT/MEC.

Data Availability Statement

Data are available upon reasonable, by the Corresponding Authors.

Conflicts of Interest

The authors declare no conflict of interest.

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Scheme 1. Schematic of the synthesis of the CeO2–GO-3 electrocatalyst.
Scheme 1. Schematic of the synthesis of the CeO2–GO-3 electrocatalyst.
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Figure 1. (a) XRD pattern and (b) FT−IR spectra of the electrocatalysts.
Figure 1. (a) XRD pattern and (b) FT−IR spectra of the electrocatalysts.
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Figure 2. XPS analysis of the CeO2 (top view) and CeO2–GO-3 (bottom view) electrocatalysts: (a) survey scans, (b) O 1s, (c) Ce 3d, and (d) C 1s.
Figure 2. XPS analysis of the CeO2 (top view) and CeO2–GO-3 (bottom view) electrocatalysts: (a) survey scans, (b) O 1s, (c) Ce 3d, and (d) C 1s.
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Figure 3. SEM analysis of the electrocatalysts; low and higher magnification of: (a-1,a-2) CeO2, (b-1,b-2) CeO2–GO-1, (c-1,c-2) CeO2–GO-2, and (d-1,d-2) CeO2–GO-3.
Figure 3. SEM analysis of the electrocatalysts; low and higher magnification of: (a-1,a-2) CeO2, (b-1,b-2) CeO2–GO-1, (c-1,c-2) CeO2–GO-2, and (d-1,d-2) CeO2–GO-3.
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Figure 4. TEM images of the CeO2–GO-3 electrocatalyst at (a) low and (b) high resolutions; (c) HR-TEM; and (d) SAED pattern.
Figure 4. TEM images of the CeO2–GO-3 electrocatalyst at (a) low and (b) high resolutions; (c) HR-TEM; and (d) SAED pattern.
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Figure 5. CV curves of the electrocatalysts in 1.0 M KOH at various scan rates for (a) CeO2, (b) CeO2–GO-1, (c) CeO2–GO-2, and (d) CeO2–GO-3.
Figure 5. CV curves of the electrocatalysts in 1.0 M KOH at various scan rates for (a) CeO2, (b) CeO2–GO-1, (c) CeO2–GO-2, and (d) CeO2–GO-3.
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Figure 6. Electrochemical investigation of the electrocatalysts: (a) LSV curves, (b) Tafel slope, (c) bar diagram of the ECSA values, (d) Nyquist plots, and (e) chronoamperometry curves.
Figure 6. Electrochemical investigation of the electrocatalysts: (a) LSV curves, (b) Tafel slope, (c) bar diagram of the ECSA values, (d) Nyquist plots, and (e) chronoamperometry curves.
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Nagajyothi, P.C.; Pavani, K.; Ramaraghavulu, R.; Shim, J. Ce–Metal–Organic Framework-Derived CeO2–GO: An Efficient Electrocatalyst for Oxygen Evolution Reaction. Inorganics 2023, 11, 161. https://doi.org/10.3390/inorganics11040161

AMA Style

Nagajyothi PC, Pavani K, Ramaraghavulu R, Shim J. Ce–Metal–Organic Framework-Derived CeO2–GO: An Efficient Electrocatalyst for Oxygen Evolution Reaction. Inorganics. 2023; 11(4):161. https://doi.org/10.3390/inorganics11040161

Chicago/Turabian Style

Nagajyothi, Patnamsetty Chidanandha, Krishnapuram Pavani, Rajavaram Ramaraghavulu, and Jaesool Shim. 2023. "Ce–Metal–Organic Framework-Derived CeO2–GO: An Efficient Electrocatalyst for Oxygen Evolution Reaction" Inorganics 11, no. 4: 161. https://doi.org/10.3390/inorganics11040161

APA Style

Nagajyothi, P. C., Pavani, K., Ramaraghavulu, R., & Shim, J. (2023). Ce–Metal–Organic Framework-Derived CeO2–GO: An Efficient Electrocatalyst for Oxygen Evolution Reaction. Inorganics, 11(4), 161. https://doi.org/10.3390/inorganics11040161

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