Morphological Engineering of Battery-Type Cobalt Oxide Electrodes for High-Performance Supercapacitors

1. Introduction

Nanomaterials have been used in various applications in recent decades, including microelectronic circuits, sensors, energy storage devices, piezoelectric devices, and fuel cells. In particular, have sparked widespread interest in supercapacitor applications owing to their large surface area, unique electrical characteristics, and tuneable morphology. Material characteristics at the nanoscale are intimately related to supercapacitor performance, notably energy storage capacity, power density, and cycle life. Nanomaterials have a high surface-to-volume ratio, which implies they can store more electroactive sites for ion adsorption and allow for faster charge/discharge rates. This makes them ideal for use as electrodes in sophisticated supercapacitors [1,2,3,4,5,6,7,8]. Carbon nanotubes, graphene, and activated carbon are prevalent carbon nanomaterials. EDLCs often use these materials, storing energy by physical ion adsorption on their high-surface area architectures [9,10]. Transition metal oxides, including Co₃O₄, MnO₂, and NiO, demonstrate pseudocapacitance by storing energy via reversible faradaic processes[11]. Nanostructuring of these oxides optimizes surface area and reduces diffusion distances, enhancing capacitance and cycle stability [12,13]. A multitude of individuals use conducting polymers such as polyaniline (PANI), polypyrrole (PPy), and polythiophene, which exhibit elevated capacitance via redox mechanisms. Wearable supercapacitors may include polymer nanostructures owing to their flexibility [14,15,16].

Cobalt oxide (Co₃O₄) has emerged as one of the most promising nanomaterials for supercapacitor applications due to its high theoretical specific capacitance (3560 F g^-1), excellent electrochemical stability, and advantageous redox characteristics [17,18]. The Co₃O₄ adopts a typical spinel crystal structure in which Co²⁺ ions occupy the tetrahedral interstitial sites, while Co³⁺ ions are located at the octahedral interstitial sites within the cubic close-packed arrangement of oxygen anions [19]. This unique structural configuration imparts Co₃O₄ with advantageous electronic and ionic transport properties, making it an attractive material for energy storage applications. Considerable research efforts are currently directed toward developing efficient synthesis methodologies for fabricating Co₃O₄ nanostructures with diverse morphologies, as these morphological variations can significantly influence their electrochemical characteristics, particularly in supercapacitor applications [20].

A wide range of morphologies, including nanorods [21,22] nanotubes [23,24], nanoflowers [25], and nanowires [26,27], has been reported in the literature, showcasing the adaptability of Co₃O₄ in various structural forms. To achieve these morphologies, multiple synthesis techniques have been employed, such as co-precipitation, sol-gel, hydrothermal, solution combustion methods, and colloidal approaches [28,29]. Each of these techniques offers distinct advantages in terms of controlling particle size, surface area, and porosity, which are critical parameters affecting the electrochemical performance of Co₃O₄.

Extensive research has demonstrated the effectiveness of various methodologies in synthesizing Co₃O₄ nanostructures with enhanced functional properties. For example, Kalpana et al. conducted a comparative analysis of the supercapacitive performance of Co₃O₄ nanocrystals fabricated using co-precipitation (Co₃O₄-C) and hydrothermal (Co₃O₄-H) techniques. Both samples exhibited a spinel-type cubic crystal structure and pseudocapacitive behavior. Notably, the hydrothermally synthesized Co₃O₄-H, characterized by a distinctive flower-like morphology, achieved a significantly higher specific capacitance of 366 F/g at a current density of 0.5 A/g, compared to the spherical Co₃O₄-C particles, which exhibited a specific capacitance of 233 F/g at 0.5 A/g [25]. Kalyanjyoti et al. synthesized highly stable Co₃O₄ nanocrystals, including 0D nanospheres and 2D hexagonal platelets, through a solvothermal method. The morphology transition from nanospheres to platelets was found to be reaction time-dependent. Electrochemical analysis revealed that the hexagonal platelets exhibit exceptional capacitive performance, achieving a specific capacitance of 476 F/g at a current density of 0.5 A/g. This superior performance is attributed to their morphology, which enhances ion accessibility. Further improvements in capacitance could be achieved by incorporating large surface area supports or conductive fillers [30]. Co₃O₄ nanoparticles were synthesized by Shwetha et al. using the solution combustion method, with variations in the fuel-to-oxidizer ratio. The electrode produced with a F/O ratio of 1 demonstrated exceptional performance, achieving a specific capacitance of 205 F/g at a scan rate of 2 mV/s, 166 F/g at a current density of 0.5 A/g, and retaining 90% of its capacitance after 5,000 cycles. Its uniform particle distribution and high surface area make it a highly promising material for supercapacitor applications [31]. Rose Babu et al. synthesized cobalt oxide nanoparticles hydrothermally at various temperatures and analyzed their structural, optical and electrochemical properties. The material showed a specific capacitance of 450 F/g at 1 A/g and retained over 88% capacitance over 10,000 cycles at 20 A/g, indicating excellent stability and low charge transfer resistance [32]. The Co₃O₄@N-MWCNT composite was synthesized by Rajendra Kumar et al. through a sonication-assisted thermal reduction process, specifically tailored for enhanced supercapacitor performance. This method facilitated the integration of Co₃O₄ nanoparticles onto nitrogen-doped multi-walled carbon nanotubes, improving both the electrical conductivity and electrochemical stability of the composite. The electrode exhibited an impressive electrochemical capacitance of 225 F/g at a current density of 0.5 A/g [33]. Tao et al. developed a novel flexible Co₃O₄ electrode with an amorphous, hydroxyl-rich structure created through the electrochemical oxidation of a cobalt-based metal-organic framework. The electrode features large micro rods, small nanoparticles, and abundant mesopores, which enhance electron transfer, active interface exposure, and electrolyte ion penetration. The Co₃O₄ electrode demonstrates a high specific capacitance of 226.1 C/g and excellent rate performance, outperforming crystalline, hydroxyl-deficient Co₃O₄ electrodes [34].

Building on these advancements, the present study focuses on synthesizing Co₃O₄ nanocubes using a facile hydrothermal technique. Potassium hydroxide solution was employed as a reducing agent at varying molar ratios to explore its influence on microstructural and electrochemical properties of materials. The synthesized Co₃O₄ nanocube with a 1:1 molar ratio exhibited remarkable battery-type behavior, delivering a specific capacitance of 412 C/g at 1 A/g. Furthermore, they demonstrated excellent cyclic stability, retaining 88% of their capacitance at 3 A/g even after 10,000 cycles. These results underscore the potential of this approach for producing high-performance electrode materials tailored for advanced supercapacitor applications.

2. Materials and Methods

2.1. Raw Materials

Sigma-Aldrich provided cobalt(II) nitrate hexahydrate (Co(NO₃)₂.6H₂O) and polyvinylidene fluoride (PVDF), while spectrochem chemicals and Thames-Baker provided potassium hydroxide (KOH)(99%) and N-methyl pyrrolidone (NMP). We utilized all of the compounds directly, without any additional purification. All synthesis methods were carried out using deionized water and ethanol.

2.2. Synthesis Procedure

In a typical synthesis (Scheme 1), cobalt nitrate hexahydrate and KOH were used as precursors in a stoichiometric ratio. Initially, a 1 M cobalt nitrate solution was prepared in 20 mL of deionized water and stirred for 1 h to ensure homogeneity. Then, 20 mL of 1 M KOH was added drop wise while continuously stirring with a magnetic stirrer for an additional hour. The resulting mixture was transferred to a 100 mL Teflon-lined autoclave, where the reaction was conducted at 200 °C for 24 h. After cooling the autoclave to room temperature, the resulting material was washed and rinsed four times with ethanol and distilled water to remove any impurities. The precipitate was then dried at 80 °C for 5 h and subsequently calcinated at 400 °C for 4 h with a heating rate of 3 °C/min. The sample synthesized with a 1:1 precursor ratio of cobalt nitrate and KOH is designated as COK 11. For comparison, samples prepared with different ratios of Co(NO₃)₂.6H₂O and KOH, specifically 1:3 and 1:5 are labeled COK 13, and COK 15, respectively.

2.3. Microstructural and Electrochemical Measurements

The microstructural properties of the Co₃O₄ nanocubes were analyzed using X-ray diffraction (XRD) using a Rigaku miniflex600 apparatus with the CuKα radiation (0.15406 nm). The morphology of the produced cobalt oxide was evaluated using a field emission scanning electron microscope (FE-SEM) equipped with energy dispersive X-ray analysis (EDAX), and a high-resolution transmission electron microscope (HR-TEM). The structural changes of porous Co₃O₄ nanocubes were explored using X-ray photoelectron spectroscopy (XPS, Thermo scientific) with Al Kα radiation under the pressure of 5×10^-9 Torr and Fourier transform infrared (FTIR, Nicolet, IR300).

The electrochemical performance of the prepared cobalt oxide electrodes was evaluated in a 3 M KOH aqueous electrolyte within a voltage range of 0.0 to 0.5 V at room temperature, using a CHI 608C electrochemical workstation (Instrument Inc., USA) in a three-electrode glass cell. The working electrode was prepared by combining 80 wt.% active material, 10 wt.% PVDF, and 10 wt.% carbon black. After grinding these components for 3 h, a small amount of NMP solution was added to form a smooth slurry. Cleaned nickel foam pieces (1.5 cm²) were coated with the slurry through a drop-casting technique and dried overnight at 100 °C.

For electrode preparation, commercial nickel foam sheets were cut into 1.5 cm × 1 cm pieces. Some foam pieces were immersed in 3 M hydrochloric acid and then sonicated for 15 min to remove the NiO layer and any residual hydrocarbons on the surface. The cleaned foams were then rinsed with deionized water and ethanol in an ultrasonic bath and dried in a vacuum oven for later use. The electrode's mass loading was 2.02 mg/cm². The Ag/AgCl and a platinum strip were used as reference and counter electrodes, respectively.

3. Results and Discussion

The SEM micrographs shown in Figure 1(a)-Figure 1(c) illustrate the hydrothermal synthesis of COK-11 to COK-15 samples, using cobalt nitrate as the precursor and potassium hydroxide (KOH) as both a reducing agent and a morphological control agent. At an equimolar ratio of cobalt nitrate to KOH (COK-11), the resulting particles exhibit a well-defined cubic morphology (Figure 1a). Each cubic particle (Figure 1a-i) consists of smaller, approximately spherical grains that assemble to form mesoporous networks at the inter-grain junctions [35,36]. The morphology of the particles undergoes a substantial transformation with variations in KOH concentration. When the precursor-to-reducing agent ratio increases to 1:3 or 1:5, the morphology shifts predominantly to spherical particles (Figure 1b) or agglomerated particle clusters (Figure 1c), respectively. The measured particle size range of the prepared COK 11, COK 13, and COK 15 samples was found to be 200-250, 60-100, and 100-400 nm, respectively.

Energy dispersive X-ray spectroscopy (EDS) analysis (Figure S1) confirms the elemental composition of the synthesized COK-11 powder, with cobalt (41.20 at.%) and oxygen (58.80 at.%) present in a stoichiometric ratio consistent with the spinel cobalt oxide (Co₃O₄) phase. The elemental mapping of COK-11 also confirms the uniform distribution of cobalt and oxygen throughout the scanning area of the nanocubes, shown in Figure S2. Conversely, a lower ratio of 1:0.5 yields a heterogeneous mixture of irregularly shaped cubic particles interspersed with scattered grains, as shown in Figure S3.

Transmission electron microscopy analysis (Figure 2) provides additional insights into the morphology and crystallinity of the synthesized COK 11 nanomaterials. Figure 2(a) and Figure 2(b) reveal cubic nanoparticles, corroborating the SEM findings, with an average side length of approximately 250 nm and a calculated volume of 10⁶ nm³. High-resolution TEM (HR-TEM) imaging shows distinct lattice fringes, with Figure 2c and the top and down insets in Figure 2c displaying a measured d-spacing of 0.245 nm, corresponding to the (311) crystallographic plane of the spinel Co₃O₄ structure. Furthermore, the uniform spatial distribution of cobalt (Co) signals from the L and K shells and oxygen (O) signals from the K shell in line scan (Figure 1d) further validate the successful formation of Co₃O₄ nanocube, with cobalt atoms in +2 and +3 oxidation states balanced by oxygen in a -2 oxidation state. Also, the size of the nanocube was found to be 250 nm.

The structural properties and phase composition of the synthesized powders were analyzed using X-ray diffraction (XRD), shown in Figure 3a. Distinct diffraction peaks were observed at angles of 18.8°, 31.1°, 36.6°, 38.4°, 44.6°, 55.5°, 59.2°, 65.1°, and 77.1°, corresponding to the crystallographic planes (111), (220), (331), (222), (400), (422), (333), (440), and (533), respectively. These peaks confirm the formation of Co₃O₄, consistent with previous reports [10,37]. Also, the XRD examination revealed a cubic structure with a space group of Fd-3m, which corresponds to the data reported on JCPDS card no. 42-1467. The synthesized material displayed moderate crystallinity, as evidenced by the intensity of the diffraction peaks. The calculated lattice parameters a = b = c = 8.0925 Å slightly exceed the theoretical value of 8.084 Å. This may be due to nanoscale effects, defect-induced strain, and synthesis conditions. These factors collectively modify the atomic arrangement, leading to a measurable expansion of the unit cell [38]. The average crystallite size (D) of the synthesized samples was estimated using Scherrer's equation [39,40]:

$$D = {\displaystyle \frac{k\lambda }{\beta \cos \theta }},$$

(1)

where k is a shape factor with a value of 0.9, λ represents the Cu K_α radiation wavelength, β is the full width at half-maximum (FWHM), and θ represents the Bragg angle. According to this computation, the average crystal sizes of COK 11, COK 13, and COK 15 were 30.6, 24.3, and 21.3 nm, respectively. Additionally, the micro-strain (ε) and dislocation density (δ) values of the obvious peaks were 0.00332 and 1.11×10¹⁵ for COK 11, 0.00435 and 2.39×10¹⁵ for COK 13 and 0.00472 and 2.70×10¹⁵ for COK 15. These values indicate that crystal size decreases as the ratio increases, and the micro-strain and dislocation density increase. This trend is typical in materials science whereas smaller crystal sizes often lead to higher strain and dislocation densities due to the increased surface area and defects.

Microstructural results concluded that under supercritical water conditions, the OH⁻ ions from KOH serve a dual role as both reducing agent and saturation-inducing agents, facilitating the dissolution and recrystallization processes necessary for nucleation. The rapid precipitation of cobalt oxide nanoparticles occurs due to chemical interactions in the homogeneously hydrolyzed metal solutions. The nucleation and growth dynamics are primarily governed by the molar concentration of KOH relative to the cobalt precursor under hydrothermal reaction conditions. At 0.5 M KOH, a mixed morphology of scattered and cubic particles is observed (Figure S1). A uniform cubic morphology develops at 1.0 M KOH (Figure 1a and Figure 2a), whereas aggregated spherical particles dominate at concentrations of ≥3M KOH (Figure 1c and Figure 1d). These findings highlight the critical role of KOH concentration in determining particle morphology. The hydrothermal reaction leading to Co₃O₄ formation can be described by the following chemical equations (1) and (2), which outline the transformation from dissolved precursors to the crystalline spinel phase.

$${Co\left({NO}_3\right)}_2+2 KOH⟺ {Co\left(OH\right)}_2+{2K(NO}_3),$$

(2)

$$3{Co\left(OH\right)}_2\stackrel{Hy. 210 °c}{\Rightarrow } {\mathrm{C}\mathrm{o}}_3{\mathrm{O}}_4+2H_2\mathrm{O}.$$

(3)

Figure 3 (b and c) shows Co 2p and O 1s XPS spectra. These depict the chemical and valence states at the surface of the COK 11 sample. The peaks at 780.81 and 796.63 eV correspond to Co 2p_3/2 and Co 2p_1/2, respectively, with a spin-orbit splitting of 15.82 eV [41,42]. This demonstrates the Co₃O₄ phase, a common cobalt oxide with mixed Co²⁺ and Co³⁺ oxidation states. The Co 2p_3/2 spectrum is deconvoluted into two peaks at 780.55 and 781.98 eV, attributable to Co³⁺ and Co²⁺ on the surface, and two satellite peaks at 786.0 and 790.83 eV, revealing the distinctive electronic transitions inside cobalt oxides [43]. However, the Co 2p_1/2 spectrum is deconvoluted into peaks at 796.2 and 797.47 eV, corresponding to Co³⁺ and Co²⁺ contributions, followed by satellite peaks at 802.50 and 806.29 eV, verifying the mixed oxidation states [44]. Figure 3c also shows a two-peak O 1s spectrum at 529.67 and 530.72 eV. The peak at 529.67 eV is attributed to lattice oxygen (O_latt., O²⁻), which is inherent in the crystalline structure of Co₃O₄. The signal at 530.72 eV indicates oxygen species adsorbed on surface vacancies (O_surf, O⁻, O₂²⁻, and OH⁻) [45,46]. These surface-adsorbed oxygen species are often the result of crystal lattice defects or vacancies, which play an important role in improving the electrochemical characteristics of the materials.

FTIR spectroscopy was employed to analyze the structure of the synthesized Co₃O₄ nanoparticles. Figure 3d shows their FTIR spectrum recorded at room temperature in the 500-4000 cm⁻¹ range. Metal oxides generally exhibit characteristic FTIR peaks below 1000 cm⁻¹, attributed to the intra-atomic vibrations. The FTIR spectrum of COK 11 nanoparticles reveals two prominent bands, corresponding to metal-oxygen bonds in its spinel structure. The band at ~660 cm^-1 is linked to Co³⁺− O stretching vibrations in octahedral sites, while the band around 560 cm^-1 is due to Co²⁺− O stretching in tetrahedral sites. These bands are crucial for identifying the Co₃O₄ phase and align well with the reported data in the literature [47,48].

The electrochemical performance of the synthesized cobalt oxide (Co₃O₄) electrodes was systematically evaluated using CV, GCD, and EIS analysis in a 3M aqueous potassium hydroxide (KOH) electrolyte at ambient temperature. Figure 4a illustrates the current response of the prepared electrode samples, along with a comparison to bare nickel foam, at a scan rate of 60 mV/s within a potential window of 0 to 0.5 V. All tested electrodes exhibited a distinct pair of redox peaks, an oxidative peak around 0.4 V and reduction peak near 0.3 V. These peaks correspond to the reversible redox transition between Co²⁺ and Co³⁺ oxidation states during the electrochemical reactions. The following equations can represent these redox processes [31]:

$${Co}_3{O}_4+{OH}^{-}+H_{2}O\leftrightarrow 3CoOOH+e^{-},$$

(4)

$$CoOOH+{OH}^{-}\leftrightarrow {CoO}_2+H_{2}O+e^{-}.$$

(5)

Notably, the COK 11 electrode demonstrated a significantly larger integral area in the CV curve than other samples, suggesting enhanced electrochemical activity. This improvement can be attributed to its unique surface morphology, characterized by nanocubic structures offering abundant electroactive sites and interconnected pores, facilitating efficient ion transport within the electrolyte. Figure 4(b-d) further confirms that, across all cobalt oxide electrodes, the current response and integral area of the CV curves increased proportionally with the applied scan rate. This behavior highlights the involvement of both surface-controlled and diffusion-controlled redox mechanisms in the charge storage process [49,50]. The relative contribution of these mechanisms was assessed using the power-law relationship (I = av^b), where b serves as an indicator of the reaction kinetics [51,52]. For the COK 11-15 electrodes, the calculated b-values ranged from 0.41 to 0.52 (Figure 4e), indicating a predominant diffusion-controlled mechanism occurred during the charge storage process. The specific capacity (Q_sp) of the electrode was derived from the CV data using the following equation [51,53]:

$$Q_{sp}\left(C{g}^{-1}\right)= {\displaystyle \frac{1}{m}}{\int }_{V_i}^{V_f}I\left(V\right)dV,$$

(6)

• where ${\int }_{V_i}^{V_f}I\left(V\right)dV$ represents the integral area of the CV curve, ‘m’ is the mass of the active electrode material (in mg), and ‘ν’ is the scan rate (in mV/s). The calculated specific capacities of the COK 11 electrode were 440, 306, 210, 136, 104, 85, and 71.5 C/g at a scan rate of 5, 10, 20, 40, 60, 80, and 100 mV/s, respectively, as shown in Figure 4f. In comparison, the COK 13 and COK 15 electrodes exhibited lower specific capacities of 270, 230, 145, 105, 85, 72, and 64 C/g, and 250, 175, 132, 91, 74, 63, and 54 C/g, respectively, under the same scan rates.

Among all the electrodes studied, the COK 11 electrode displayed superior specific capacities, corroborating the results of CV measurements and the observed microstructural characteristics. Figure 4f also reveals a general decline in specific capacity with increasing scan rates. This decrease can be attributed to the limited interaction time available between the electrolyte ions and the electrode surface during rapid faradaic reactions, which constrains charge storage efficiency under high scan rates [54,55].

The galvanostatic charge-discharge (GCD) profiles of the cobalt oxide electrodes were recorded at varying current densities within the same potential window used for CV measurements. These GCD curves exhibited voltage plateaus at ~0.4 and ~0.3 V versus Ag/AgCl, consistent with the redox peaks observed in the CV curves. The non-linear shape of the GCD profiles confirmed the battery-type electrochemical behaviour of the electrodes. The specific capacity (Cs) of the electrode was calculated using the formula [56,57]:

$${\mathrm{C}}_{\mathrm{s}} (\mathrm{C}/\mathrm{g}) = {\displaystyle \frac{I ∆t}{m }}.$$

(7)

Figure 5a illustrates the comparative GCD curves of COK 11, COK 13, and COK 15 samples at a current density of 1 A/g. Among these, the COK 11 electrode exhibited longer charge-discharge duration than COK 13, and COK 15, indicating superior charge storage capability. The specific capacities measured at 1 A/g were 412.8, 299.73, and 201.78 C/g for COK 11, COK 13, and COK 15, respectively. GCD profiles for these electrodes at current densities ranging from 1 to 4 A/g are presented in Figure 5 (b-d). The COK 11 electrode delivered specific capacities of 412.8, 350.22, 288, and 234.36 C/g at current densities of 1, 2, 3, and 4 A/g, respectively. Similarly, the COK 13 electrode achieved capacities of 299.73, 263.32, 212.58, and 169 C/g, while the COK 15 electrode yielded 201.78, 122.2, 71.82, and 52 C/g under the same current densities. These results demonstrate that the COK 11 electrode exhibited the highest rate capability (56.88%), outperforming COK 13 (54.71%) and COK 15 (25.77%).

To elucidate the electrochemical reaction kinetics, electrochemical impedance spectroscopy (EIS) was performed (Figure 5e). The Nyquist plots revealed two distinct regions: a high-frequency semicircle and a low-frequency linear tail. The semicircle corresponds to the charge-transfer resistance (R_ct) associated with redox reactions between the electrode material and the electrolyte, while the intercept on the real axis represents the equivalent series resistance (R_s). The linear portion at low frequencies indicates the ion diffusion impedance (Warburg impedance, W) [58,59,60]. All Nyquist plots were well-fitted to an equivalent circuit model R(CR)(QR)(CR) (inset in Figure 5e) with χ² values of 2.38×10^-3 (COK 11), 1.57×10^-3 (COK 13), and 1.74×10^-2 (COK 15). The R_s values for COK 11, COK 13, and COK 15 were 0.38, 0.53, and 0.94 Ω, respectively. Similarly, the charge transfer resistance (R_ct) values for COK 11 and COK 13 were both 0.37 Ω, indicating the superior electrochemical conductivity of COK 11. Furthermore, the steep linear segment in the Nyquist plot of COK 11 confirmed its excellent ion-diffusion properties. Figure 5f displays the cycling stability of the COK 11 electrode at a current density of 3 A g^-1. After 5000 cycles, the specific capacity retention is 93.67%, and after 10000 cycles, it retains 88% of its initial value, demonstrating exceptional long-term stability and durability. Furthermore, the specific capacity and cycling stability of the COK 11 electrode were compared with those of previously reported cobalt oxide electrodes, as presented in Table 1. The results demonstrate its superior electrochemical performance in a three-electrode system compared to the earlier cobalt oxide electrodes.

4. Conclusions

In summary, the hydrothermal synthesis of Co₃O₄ nanomaterials demonstrated that the morphology, crystal structure, and electrochemical properties of the particles are significantly influenced by the concentration of potassium hydroxide. The optimized 1:1 molar ratio of cobalt nitrate to KOH (COK 11) produced well-defined cubic nanostructures with uniform elemental distribution, as confirmed by SEM, TEM, and EDS analyses. The structural characterization through XRD, XPS, and FTIR further validated the formation of the Co₃O₄ spinel phase with characteristic lattice and surface oxygen features. Electrochemical evaluations revealed that the COK 11 electrode outperformed its counterparts in terms of specific capacity and electrochemical activity, attributable to its nano cubic morphology and interconnected porosity, which facilitated efficient ion transport and increased active surface area. The gradual decline in specific capacity with increased scan rates across all samples underscores the diffusion-controlled nature of the charge storage mechanism. The COK 11 electrode demonstrates a high specific capacity of 412.8 C/g (@ 1 A/g), remarkable rate capability (56.88%), and excellent cycle stability (88%) after 10000 cycles. It concludes that the critical role of synthesis parameters in tailoring the structural and electrochemical properties of cobalt oxide nanomaterials makes COK-11 a promising candidate for energy storage applications.