Synthesis and Structural and Electrochemical Characterization of Carbon Fiber/MnO₂ Composites for Hydrogen Storage and Electrochemical Sensing

Highlights

What are the main findings?

• Electrochemically deposited MnO₂/CF composites exhibit a denser and more uniform MnO₂ coating, leading to superior hydrogen storage performance compared with chemically synthesized materials.
• Hydrogen exposure induces partial MnO₂ reduction (Mn⁴⁺ → Mn³⁺/Mn²⁺), confirming hydrogen uptake via MnOOH formation while preserving good electrochemical sensing behavior.

What is the implication of the main finding?

• The MnO₂/CF composites represent promising, low-cost hydrogen storage materials due to their high active MnO₂ content and reversible redox properties.
• Their combined hydrogen storage and electrochemical sensing capabilities broaden their potential use in sustainable energy devices and advanced composite systems.

Abstract

Hydrogen, as an alternative energy carrier, presents significant prospects for the transition to more environmentally friendly energy solutions. However, its efficient and safe storage remains a challenge, as materials with high adsorbent capacity and long-term storage capability are required. This study focuses on the synthesis and characterization of a composite material comprising carbon fiber and manganese dioxide (MnO₂/CFs), for the purpose of hydrogen storage. Carbon fiber was chosen as the basis for the composition of the composite material due to its large active surface area and its excellent mechanical, thermal, and electrochemical properties. The deposition of MnO₂ on the surface of carbon fibers took place through two different synthetic pathways: electrochemical deposition and chemical synthesis under different conditions. The electrochemical method enabled the production of a greater amount of oxide with optimized structural and chemical properties, whereas the chemical method was simpler but required more time to achieve comparable or lower-capacity performance. Elemental analysis of the electrochemically produced composites showcased an average of 40.5 ± 0.05 wt% Mn presence, which is an indicator of the quantity of MnO₂ on the surface responsible for hydrogen storage, while the chemically produced composites showcased an average of 7.6 ± 0.05 wt% Mn presence. Manganese oxide’s high specific capacity and reversible redox reaction participation make it suitable for hydrogen storage applications. The obtained results of the hydrogenated samples through physicochemical characterization indicated the formation of the MnOOH intermediate. Regarding these findings it may be remarked that carbon fiber/MnO₂ composites are promising candidates for hydrogen storage technologies. Finally, the fabricated carbon fiber/MnO₂ composites were applied successfully as working electrodes for analysis of the [Fe(CN)₆]^3−/4− redox system in aqueous KCl solutions.

1. Introduction

In recent years, concerns about the environmental impact of modern lifestyles have grown significantly, prompting a growing number of people to turn to renewable energy sources to meet their needs. A gradual shift away from fossil fuels is essential, with a focus on replacing them with renewable sources that have a lower environmental footprint. At the 2024 Climate Change Conference held in Azerbaijan, the establishment of the Climate Change Action Fund (CFAF) was announced. This fund, amounting to USD 1 billion annually, is supported by contributions from countries with heavy fossil fuel industries. The money is then redistributed to developing nations to invest in renewable energy systems. The primary aim of the conference was to promote progress toward the goals set in the Paris Agreement (2016) regarding the reduction of greenhouse gas emissions [1].

Hydrogen is emerging as a promising energy carrier, offering an alternative path toward decarbonization. It can be produced through various methods—conventional (using fossil fuels), renewable sources, or nuclear energy. While there is a clear trend toward renewable methods (such as wind, solar, hydroelectric, biomass, geothermal, and ocean thermal energy), the cost of hydrogen-related technologies remains a challenge for society [2]. Hydrogen has several advantages: it has a high energy content, is highly reactive, non-toxic, environmentally friendly, and can transport energy over long distances [3]. These properties are encouraging governments and industries to invest in hydrogen as a viable alternative energy solution. However, efficient and safe storage of hydrogen is crucial for its widespread use. Hydrogen can be stored in either liquid or gaseous form, either on the surface of solids (adsorption) or within them (absorption) [4]. The material-based hydrogen storage methods involve interactions between the hydrogen atom and the substrate. When adsorption is attributed to weak van der Waals forces, the process is referred to as physisorption. It typically occurs between hydrogen atoms and carbon-based structures, metal–organic frameworks, zeolites, or microporous polymers [5]. On the other hand, chemisorption involves the formation of ionic or covalent bonds with the surface atoms of solid materials such as metals, metal alloys, transition metal oxides, and sulfides [6,7].

The focus of this research is the use of carbon fibers as a hydrogen storage medium, specifically investigating how their storage capacity is affected by the deposition of manganese dioxide on their surface. It is reported that the manganese oxide decoration of carbon structures increases their hydrogen adsorption capabilities, acting as a catalyst due to its high surface area [8,9]. It has been reported that the presence of metal oxides in hydrogen storage materials, such as carbon nanostructures, enhances the adsorption capabilities via the hydrogen spillover phenomenon [8]. Hydrogen spillover is a surface phenomenon that refers to the migration of hydrogen atoms generated by H₂ splitting on a metal nanoparticle to another site of a catalyst with a hydrogen acceptor site. MnO₂ can act as a hydrogen spillover catalyst. The proposed oxide is a low-cost, highly abundant material with eco-friendly properties that can be deposited onto carbon fibers utilizing basic deposition methods [10,11].

The deposition of manganese dioxide onto carbon fibers can be achieved using various synthesis techniques, including electrodeposition, template-assisted methods, in situ redox deposition, precipitation, and hydrothermal synthesis [12,13,14,15]. In this study, two synthesis methods—in situ redox deposition and electrochemical synthesis—were employed and compared in terms of the concentration and morphology of the manganese dioxide deposited on the carbon fibers. Both methods require the activation of carbon fibers, which can be achieved by exposure to high-concentration acidic solutions such as HCl, HNO₃, or H₂SO₄. This treatment disrupts the graphene-like structure and introduces reactive functional groups (–COOH, –OH, and C=O) into the carbon lattice [16]. After activation, the in situ redox deposition method is based on the reaction between KMnO₄ and the CFs’ activated surface. More specifically, it involves the reduction of manganese from its +7-oxidation state in MnO₄⁻ to lower oxidation states, often forming MnO₂, which can be deposited onto the surface of the fiber. The following reaction takes place on the surface of CFs [14,17]:

4MnO⁴⁻ + 3C + 4H⁺ → 4MnO₂ + 3CO₂ + 2H₂O

(1)

The anodic electrochemical deposition utilizes Mn(CH₃COO)₂ as a precursor compound, which requires a lower potential for its decomposition and results in a higher deposition rate. A less acidic environment, achieved by using Na₂SO₄ as the medium, favors a hydrolysis pathway: initially, Mn²⁺ ions diffuse to the electrode surface. The following reaction involves the oxidation to Mn³⁺, which, in a less acidic environment, is unstable, and forms the intermediate MnOOH upon contact with water, which, under specific conditions, can be further converted to MnO₂. Under these conditions, the following sequence typically represents the electrochemical oxidation of Mn²⁺ ions:

Mn²⁺ → Mn³⁺ + e⁻

(2)

Hydrolysis pathway:

Mn³⁺ + 2H₂O → MnOOH + 3H⁺

(3)

MnOOH → MnO₂ + H⁺ + e⁻

(4)

This study employs both chemical and electrochemical synthesis methods for the fabrication of composite materials consisting of carbon fibers and manganese dioxide, with the aim of identifying the most effective deposition route and the optimal conditions for producing MnO₂-coated carbon fiber structures. Furthermore, the research assesses the hydrogen storage potential of the synthesized materials through comprehensive characterization of their morphology and composition using scanning electron microscopy (SEM), Energy-dispersive X-ray spectroscopy (EDS), X-ray photoelectron spectroscopy (XPS), Raman spectroscopy, and thermogravimetric analysis (TGA) [18].

2. Materials and Methods

2.1. Materials and Tools

Carbon fibers (CFs, diameter ≈ 7.25 μm, purchased by Chembiotin, Athens, Greece), Hydrogen Chloride (HCl, 37 wt%, Chem-lab, M_r = 36.46 g/mol), Potassium manganate (VII) (KMnO₄, 99 wt%, ChemSolute, Renningen, Germany), Nitric Acid (HNO₃, 65 wt%, Merck, Darmstadt, Germany), Manganese (II) Acetate (Mn(CH₃COO)₂, Purity: 99.3 wt%, M_r = 245.09, BLD Pharmatech, Shanghai, China), Sodium Sulfate Decahydrate (Na₂SO₄·10H₂O, M_r = 322.19 g/mol, Merck) and high-purity hydrogen (99.9%) gas was used without further purification.

Potassium hexacyanoferrate (III) (>99.0 wt%), potassium hexacyanoferrate (II) trihydrate (>98.5 wt%), and potassium chloride (>99.0 wt%) were purchased from Sigma-Aldrich(Darmstadt, Germany) and used without further purification. For the electrochemical measurements, a stock solution of the binary mixture K₃Fe(CN)₆/K₄Fe(CN)₆ with a concentration of 1.0 × 10⁻² mol∙L⁻¹ was prepared by dissolving the appropriate amounts of salts in KCl aqueous solution (1.0 mol∙L⁻¹). The stock solution of K₃Fe(CN)₆/K₄Fe(CN)₆ was prepared immediately prior to the electrochemical experiments by using doubly distilled water. The solutions of [Fe(CN)₆]^3−/4− in a concentration range of 7.0 × 10⁻⁵–1.0 × 10⁻³ mol∙L⁻¹ were prepared directly in the electrochemical cell by the progressive addition of the required volume of stock solution in KCl solution (1.0 mol∙L⁻¹).

All electrochemistry measurements were performed on an electrochemical working station Zahner (IM6/6EX, Kronach, Germany). The obtained results were analyzed by means of Thales software (version 4.15). A three-electrode system configuration consisting of a CF-based working electrode, a platinum auxiliary electrode, and a Ag/AgCl (saturated KCl) reference electrode was used for electrochemistry measurements. The electrochemical impedance spectra (EIS) were recorded in the frequency range from 0.1 Hz to 100 kHz at the half-wave potential of [Fe(CN)₆]^3−/4− (+0.275 V vs. Ag/AgCl). The recorded impedance spectra were analyzed by means of an equivalent electrical circuit (R_s + (C_dl/(R_ct + Z_w))). The elements of the circuit can be explained as follows: R_s is the solution resistance, C_dl is the modified layer/solution interface capacitance, R_ct is the electron-transfer resistance due to electron transfer at a modified layer/solution interface, and Z_w is the Warburg diffusion impedance due to the diffusion of the redox couple [Fe(CN)₆]^3−/4− in solution. All experiments were carried out at room temperature. Prior to all measurements, solutions were deoxygenated by purging with high-purity nitrogen.

Surface morphology and elemental analysis were carried out using a JEOL JSM6390LV scanning electron microscope (JEOL Ltd., Tokyo, Japan) at an accelerating voltage of 20 kV, equipped with an Oxford INCA PentaFETx3 EDS detector (Oxford Instruments, Oxfordshire, UK) and a field emission scanning electron microscope (FE-SEM, Jeol JSM-7000F, JEOL Ltd., Tokyo, Japan) operating at 15 keV. The XPS spectra were carried out on KRATOS AXIS Ultra DLD (Delay Line Detector, Kratos Analytical Ltd., Manchester, UK). The Raman spectra of samples were recorded using a confocal microscope Raman spectrometer system equipped with a 532 nm laser (inVia Reflex, Renishaw, UK), and the fitting of the peaks was performed with WireTM 3.4 software. Thermal analysis was performed with a Mettler Toledo e 851 TG instrument (Mettler Toledo, Columbus, OH, USA). The deposition of high-purity hydrogen was conducted using a gas chromatograph GC-14 A Shimadzu (ID: Shimadzu-G0-0235, Shimadzu Corporation, Kyoto, Japan). A galvanostat was employed to supply the desired current in the closed-circuit configuration of the electrochemical deposition system. The ultrasonic cleaning unit employed in the experimental setup was an Elma Transsonic T460/H (Elma D-78224/T 460 H, Elma Schmidbauer GmbH, Singen, Germany), a precision ultrasonic bath designed for laboratory applications. The magnetic stirrer with integrated heating functionality used was the ARGOlab M2-A (ARGOlab, Carpi, Italy), an analog-controlled magnetic hotplate stirrer.

2.2. Synthesis of MnO₂/Carbon Fiber Composites

Two distinct synthetic pathways were used in this study to produce the MnO₂/CFs composites: an in situ redox deposition and an electrochemical deposition. In the in situ redox deposition method, 50 mL of 37 wt% HCl were transferred into a 100 mL glass beaker. Pre-fabricated carbon fibers were then immersed in the acid solution and stirred using a mechanical stirrer at 200 rpm for 1 h at a temperature of approximately 28 °C. Following acid treatment, the surface-oxidized carbon fibers were thoroughly rinsed with deionized water to remove residual acid. Subsequently, the acid-treated carbon fibers were transferred to another 100 mL beaker containing 50 mL of an aqueous 0.1 M KMnO₄ solution. To prepare the KMnO₄ solution, 1.5804 g of KMnO₄ (measured using a four-decimal precision balance) were dissolved in deionized water and diluted to 100 mL in a volumetric flask, followed by stirring to ensure complete dissolution. The carbon fibers were then immersed in the KMnO₄ solution and subjected to sonication for 30 min. After sonication, the samples were rinsed with deionized water (Figure 1). This deposition process was repeated for varying contact durations between the carbon fibers and the KMnO₄ solution: 2, 6, and 24 h, respectively (

Table 1. Tabulated conditions applied during in situ redox deposition synthesis.

Repetition	Reaction Time
a	30 min
b	2 h
c	6 h
d	24 h

). Finally, all samples were dried in a convection oven at 90 °C for 8 h. The growth of MnO₂ is based on the redox reaction between MnO₄ and carbon:

4MnO₄ + 3C + 4H⁺ ⟶ 4MnO₂ + 3CO₂ + 2H₂O

(5)

In addition to the in situ redox deposition method described earlier, an electrochemical route was also developed for the synthesis of the compound. The basic principle of the electrodeposition process involves the use of an electric current of 20.0 mA∙cm⁻² to transfer metal ions from an electrolyte bath containing 0.1 M Mn(CH₃COO)₂ and 0.1 M Na₂SO₄ onto the carbon fibers. The average area of one carbon fiber is approximately 0.0182 cm², and the sample bundle, on average, consists of 50 CFs, which calculates the overall area to 0.91 cm². The carbon fibers act as the working electrode, while a pure platinum sheet was used as a counter electrode [19].

For the preparation of the electrolyte bath solution, 6.1273 g of Mn(CH₃COO)₂ and 8.0547 g of Na₂SO₄·10H₂O were precisely weighed using an analytical balance with four-decimal precision. Each salt was dissolved separately in a small volume of deionized water in two separate 50 mL beakers. The resulting solutions were transferred into a 250 mL volumetric flask, including the rinse water from each beaker to ensure complete transfer. The flask was filled with deionized water up to the calibration mark (250 mL total volume). The solution was then thoroughly stirred to ensure homogeneity.

Approximately 100 mL of the prepared electrolyte was transferred to a 200 mL beaker, which was placed on a heating plate. One end of the carbon fiber electrode was immersed in the electrolyte solution, and the other end was connected to the anode terminal of a galvanostat via a conductive wire. Similarly, the platinum electrode was immersed in the solution and connected to the cathode terminal (Figure 2). A constant current density of 20.0 mA∙cm⁻² was applied to the closed circuit for a regulated time and temperature. Then, the fibers were rinsed thoroughly 5 times with deionized water. The manganese dioxide-coated carbon fibers (MnO₂/CFs) were subsequently transferred to a crucible and dried in an oven at 80 °C for 24 h [12].

This procedure was repeated while applying different heat temperatures and reaction durations to test which conditions provide CFs with maximum MnO₂ concentration (

Table 2. Tabulated conditions applied during electrochemical deposition synthesis.

Repetition	Time (min)	Temperature (°C)	Applied Current (mA∙cm−2)
a	10	52	20
b	20	28	20
c	20	32	20

).

2.3. Adsorption of Hydrogen Gas into the Constructed MnO₂/CFs

The exposure of the synthesized carbon fiber–manganese dioxide (CFs-MnO₂) composites to hydrogen gas was conducted utilizing a gas chromatograph, Shimadzu GC-14A. For the purpose of this experiment, the chromatographic column was replaced with an empty stainless-steel column (length 5 cm × internal diameter ¼″), in order to accommodate the sample fibers. High-purity hydrogen (99.999%, Aerialco, Thessaloniki, Greece), supplied via a dedicated gas cylinder, was the carrier gas utilized for the samples’ hydrogenation. A measured quantity of CFs, consisting of approximately 50 CFs per bundle with a length of 8 cm each, was tightly packed within the metallic tube to ensure controlled exposure to the hydrogen environment. The tube was then securely integrated into the chromatographic oven, ensuring a hermetically sealed connection to prevent any gas leakage. Operational parameters, including the exposure temperature and duration, were manually programmed on the device. Following parameter input, the system was activated to initiate the exposure process. The hydrogen gas flow was 30 mL/min at a set temperature of 240 °C for a duration of 6 h. Upon completion of the defined exposure period and subsequent cooling of the system to ambient temperature, the treated samples were collected for further analysis. The characterization process aimed to quantify the extent of hydrogen adsorption by the samples.

This procedure was applied to the following samples:

Sample #1: MnO₂-CFs synthesized via the in situ redox deposition method for 30 min.

Sample #2: MnO₂-CFs synthesized via the electrochemical method for 20 min at 28 °C.

Table 3. Tabulated synthetic conditions of the produced samples.

Repetition	Synthetic Conditions	Exposure to H2	Sample Acronym
Carbon fibers	acidic pretreatment at 28 °C	NO	CF
Carbon fibers	acidic pretreatment at 28 °C	YES	CF/H2
Sample #1	in situ redox deposition method for 30 min at 28 °C	NO	MnO2/CF #1
Sample #1′	in situ redox deposition method for 30 min at 28 °C	YES	MnO2/CF/H2 #1
Sample #2	electrochemical deposition method for 20 min at 28 °C	NO	MnO2/CF #2
Sample #2′	electrochemical deposition method for 20 min at 28 °C	YES	MnO2/CF/H2 #2

tabulates the synthetic conditions of the samples as well as their acronyms.

2.4. Characterization of MnO₂/CFs Composites

A range of analytical techniques was employed to characterize the synthesized fibers, with the aim of determining the final product’s composition, evaluating the physicochemical properties of the fibers, and assessing their effectiveness in hydrogen storage applications. Techniques such as X-ray photoelectron spectroscopy (XPS, Kratos Analytical, Shimadzu, Japan)), scanning electron microscopy (SEM, Zeiss SUPRA 35VP, Jena, Germany), energy-dispersive X-ray spectroscopy (EDS, Zeiss, Jena, Germany), Fourier-transform infrared spectroscopy (FTIR, Darmstadt, Germany), and Raman spectroscopy Renishaw inVia spectrometer, New Mills, United Kingdom) were utilized. The spectra of the dry powders were taken by a Perkin Elmer FT-IR spectrometer (Spectrum One, Waltham, MA, USA). The spectra were recorded using the Spectrum v.5.3.1 (2004) software, in the wave number range of 4000–500 cm⁻¹ with the scan number of 32 and at the resolution of 4 cm⁻¹. The background spectrum was measured from the KBr disk (Lot. EA12323DA Sigma Aldrich, for spectroscopy, Darmstadt, Germany) formed using a Specac manual hydraulic press at 15 tons for 10 min. Additionally, hydrogen adsorption capacity was assessed through gravimetric methods such as thermogravimetric analysis (TGA) to quantify the performance of the composites in hydrogen uptake under controlled conditions. Supplemental information about hydrogen adsorption of the composites can also be obtained through XPS and Raman spectroscopy. This comprehensive approach enabled a detailed understanding of the material properties that influence storage efficiency.

3. Results and Discussion

3.1. Morphological, Elemental, and Structural Characterization

The final MnO₂–CFs composite materials, synthesized via in situ redox deposition and electrochemical deposition methods prior to hydrogen exposure, were analyzed using EDS quantification to determine the manganese concentration, thereby evaluating the relative efficiency of each synthesis environment.

Theoretically, considering the redox deposition, a progressively increasing concentration of MnO₂ on the sample surface is expected as the contact time between the fibers and the reagent increases [17]. This does not apply to the samples with reaction times of 2 h and 6 h, respectively (

Table 4. Tabulated parameters of EDS quantification of the samples prepared via redox deposition.

Repetition	Time	Mn wt%
a	30 min	-
b	2 h	6.83
c	6 h	2.52
d	24 h	10.06

), which, due to inadvertent handling errors or uncontrolled variables during the setup, may have influenced the reproducibility. The pronounced decrease in Mn% observed between the repetitions b and c during electrochemical depletion could be the result of procedural inconsistencies during sample preparation or measurement.

Further characterization was conducted on the samples with the highest manganese content from each synthesis method—specifically, the in situ redox deposition sample with a reaction duration of 24 h (MnO₂/CF #1) and the electrochemical deposition sample with a reaction time of 20 min at 28 °C (MnO₂/CF #2) (

Table 5. Tabulated parameters of EDS quantification of the samples prepared via electrodeposition.

Repetition	Time (min)	Temperature (°C)	Mn wt%
a	10	52	50.74
b	20	28	52.31
c	20	32	9.92

).

Based on the comparison of SEM/EDS results, conclusions can be drawn regarding the effectiveness of the in situ redox deposition method and electrodeposition synthesis for producing the desired material.

The SEM images of sample MnO₂/CF #1 reveal dispersed bright and speckled features across the carbon fiber surface (Figure 3), corresponding to MnO₂ deposits. The distribution appears non-uniform, with areas of higher local concentration, while untreated CFs exhibit a relatively smooth and featureless surface (Figure 4). It may be remarked that the particulate structures observed on the surface of the carbon fibers are likely by-products from the activation process. During activation, the carbon fibers are treated with acidic solutions (such as HCl), which may cause oxidation of the fiber surface. This oxidation process can lead to the formation of small particles, which are likely residues from the oxidation treatment. These particles are not related to the final MnO₂ deposition process. The EDS results of sample MnO₂/CF #1 (Figure 5 and

Table 6. Tabulated values of the EDS analysis of samples MnO₂/CF #1 and MnO₂/CF #2.

Element	C (wt%)	O (wt%)	Mn (wt%)
MnO2/CF #1	76.61	15.73	7.65
MnO2/CF #2	35.68	23.75	40.58

) confirm the presence of Mn on the fiber surface, along with oxygen originating from surface oxidation of the carbon fibers and Mn–O bonding of the deposited manganese oxides.

The electrochemically deposited MnO₂ layer is relatively dense and uniform, with a coating thickness in the micrometer range, approximately 8.10 μm (Figure 6). However, certain regions show thinner coverage or partial exposure of the underlying carbon fibers, indicating some degree of non-uniformity. The corresponding EDS analysis (Figure 5 and Table 6) confirms the successful deposition, showing strong Mn peaks together with oxygen contributions consistent with MnO₂ formation and minimal impurities.

Raman spectroscopy reveals the characteristic D and G bands of carbon fibers at approximately 1350 cm⁻¹ and 1580 cm⁻¹, respectively, in a plain activated carbon fiber sample (CF/H₂) (Figure 7,

Table 7. Quantitative analysis of Raman spectra for CFs after activation and H₂ treatment (CF/H₂).

Curve Name	Center	Width	Height	% Gaussian	Type	Area
Curve 1	311.87	259.42	102.0	8.08	Mixed	40,476
Curve 2	1004.12	0.41	114.8	98.50	Mixed	51
Curve 3	1376.74	254.11	925.8	35.40	Mixed	327,352
Curve 4	1592.52	108.66	925.1	54.05	Mixed	130,393
Curve 5	2824.33	687.65	224.0	0	Mixed	241,986

) and the sample MnO₂/CF #2, composed electrochemically (Figure 7,

Table 8. Quantitative analysis of Raman spectra for sample MnO₂/CF/H₂ #2 (after H₂ treatment).

Curve Name	Center	Width	Height	% Gaussian	Type	Area
Curve 1	292.40	171.25	47.8	83.89	Mixed	9373
Curve 2	653.93	805.04	133.6	0	Mixed	16,892
Curve 3	1379.26	248.72	630.8	56.08	Mixed	201,916
Curve 4	1592.34	106.58	662.1	72.80	Mixed	84,840
Curve 5	2797.97	681.39	184.5	0.47	Mixed	1972

). A comparative analysis between a MnO₂-free sample and a MnO₂-containing sample demonstrates the presence of a prominent phonon band at 650 cm⁻¹, attributed to Mn–O A₁g symmetric stretching vibrations, as well as a weaker band within the 200–500 cm⁻¹ range, corresponding to Mn–O bending vibrations. In general, the MnO₂-containing sample exhibits distinct peaks within the 200–800 cm⁻¹ region—characteristic of manganese dioxide—which are absent in the MnO₂-free sample. Taking into account the sample MnO₂/CF #2, it is estimated using the peak areas that the ratio ${\displaystyle \frac{I_d}{I_g}}$ = 2.51, while the sample CF/H₂ exhibits ${\displaystyle \frac{I_d}{I_g}}$ = 2.38, both showcasing structural defects in the carbon structure. The structural defects were induced by acid treatment, conducted prior to deposition, which led to the formation of functional groups within the graphite matrix of the carbon fibers (CFs) [11,20,21].

The G band appears near ~1580 cm⁻¹ in the Raman spectra of sp² carbon materials and originates from the in-plane stretching of C–C bonds, specifically the E2g vibrational mode of sp2 carbon atoms within the hexagonal lattice [22]. The D band appears around ~1350 cm⁻¹ and is activated by structural disorder in sp² carbon systems. The D band originates from a double-resonance scattering process with A₁g symmetry, in which phonons near the K point of the Brillouin zone are involved. Unlike the G band, it is forbidden in perfect crystalline graphite and only becomes Raman-active in the presence of defects, edges/curvature, finite crystallite size, or heteroatomic substitutions. Its intensity increases with the density of defects or disruption of the sp² network [23]. For carbon-based materials like graphene, carbon nanotubes, or amorphous carbon, the intensity ratio of the D band to the G band is used as a quantitative metric that reflects the degree of structural order/disorder, defect density, and crystallite size in sp² carbon systems. Amorphous carbon phases, vacancies, and dopants cause significant increases in D-band, indicating structural disorder in carbon materials.

Raman spectroscopy was used to investigate the sample with a 24 h chemical synthesis, both prior to (MnO₂/CF #1) (Figure 7,

Table 9. Quantitative analysis of Raman spectra for sample MnO₂/CF #1 (prior H₂ treatment).

Curve Name	Center	Width	Height	% Gaussian	Type	Area
Curve 1	353.03	0.58	1016.4	67.35	Mixed	724
Curve 2	562.88	28.96	454.1	0.05	Mixed	20,650
Curve 3	626.48	121.26	461.7	0	Mixed	87,984
Curve 4	971.85	69.17	65.5	100	Mixed	4823
Curve 5	1385.85	240.69	550.4	67.36	Mixed	162,914
Curve 6	1588.74	100.06	578.5	76.52	Mixed	68,498
Curve 7	2706.68	3367.90	77.7	0	Mixed	409,360
Curve 8	2795.67	698.06	187.4	20.94	Mixed	191,797

) and after exposure (MnO₂/CF/H₂ #1) (Figure 7,

Table 10. Quantitative analysis of Raman spectra for sample MnO₂/CF/H₂ #1 (after H₂ treatment).

Curve Name	Center	Width	Height	% Gaussian	Type	Area
Curve 1	496.11	56.26	265.4	14.34	Mixed	22,366
Curve 2	566.26	31.00	463.8	65.34	Mixed	17,824
Curve 3	628.83	143.59	713.3	43.27	Mixed	138,445
Curve 4	1370.96	283.65	731.0	56.85	Mixed	266,025
Curve 5	1395.16	105.33	736.1	68.88	Mixed	94,747
Curve 6	2853.22	560.41	142.1	36.19	Mixed	110,512
Curve 7	3283.12	220.93	25.9	100	Mixed	6080

) to hydrogen gas. The intensity ratio I_D/I_G for MnO₂/CF #1 is 2.37, calculated using the integrated areas of the respective peaks, while sample MnO₂/CF/H₂ #1 exhibits an I_D/I_G ratio of 2.81, indicating the presence of structural defects in the carbon framework in both cases.

The peaks observed in the range 200–800 cm⁻¹ in both spectra can be attributed to the presence of MnO₂. More specifically, for the sample prior to hydrogen exposure (Figure 7, Table 9), peaks 1 (~353 cm⁻¹), 2 (~562 cm⁻¹), 3 (~626 cm⁻¹), and 4 (~971 cm⁻¹) correspond to bending and twisting modes of Mn–O bonds (arising from Mn in different polymorphic forms). The highest of these four peaks (peak 4), which is absent in the spectrum of the hydrogen-exposed sample, may be associated with more stable or rigid MnO₂ structures, such as β-MnO₂. In the spectrum of the same material after hydrogen treatment (Figure 7, Table 10), the number of peaks within the 200–800 cm⁻¹ range is reduced, their intensity increases, and a shift toward higher wavenumbers is observed. This behavior may be attributed to a phase transformation of manganese and/or its partial reduction to lower oxidation states, such as the formation of MnO [24,25].

The structure of the synthesized fibers was further examined using FTIR spectroscopy. Specifically, Figure 8 presents the FTIR spectra of the following: (a) acid-treated carbon fibers; and (b) MnO₂/CF/H₂ #2, which was synthesized via electrochemical deposition for 20 min at 28 °C and subsequently exposed to H₂ treatment.

Considering the spectrum of sample #2′, the broad band at 3500–3700 cm⁻¹, corresponding to O–H bending vibrations, indicates the presence of hydroxyl groups, which may be attributed to either adsorbed water or the partial reduction in MnO₂. The broad band at 2220–2260 cm⁻¹ is assigned to C≡N stretching vibration; CFs made from polyacrylonitrile often retain small amounts of nitrile (–C≡N) groups. The band observed at 1054 cm⁻¹ is likely associated with C–OH bending vibrations, suggesting surface oxidation of the carbon fibers. The peak at 1525 cm⁻¹ corresponds to C=C bending vibrations, characteristic of the carbon fiber backbone. Alternatively, it may arise from O–H bending involving oxygen atoms coordinated to manganese [26,27]. Expected Mn–O bending absorptions typically occur in the region of 400–700 cm⁻¹. In the recorded FTIR spectrum, several low-intensity peaks are indeed observed within this range, notably at 671 cm⁻¹, which supports the presence of manganese oxides. Additionally, the peak at 773 cm⁻¹ may be attributed to a characteristic adsorption of manganese oxides with a tunnel-type structure [28]. Regarding the spectrum of the acid-treated carbon fibers, it is evident that the peaks due to manganese vibrations are absent (671 cm⁻¹, 773 cm⁻¹).

X-ray photoelectron spectroscopy (XPS) spectra of the MnO₂/CFs produced electrochemically for 20 min at 28 °C (sample #2) were used to determine the surface composition of the material prior to and after hydrogen exposure and to examine the oxidation state of Mn.

Based on the Mn 2p XPS spectra of sample MnO₂/CF #2 prior to hydrogen exposure (Figure 9i), the surface composition is predominantly manganese in the +4 oxidation state (Mn⁴⁺), corresponding to MnO₂. This is evidenced by the characteristic Mn 2p_3/2 and Mn 2p_1/2 peaks observed at 641.985 eV and 653.480 eV, respectively (spin-energy difference of 11,495 eV), along with the presence of shake-up satellite features typically associated with Mn⁴⁺ [29]. Quantitative analysis indicates that Mn⁴⁺ accounts for approximately 96% of the total manganese signal. A minor contribution from Mn²⁺ (MnO) is also detected, represented by weaker peaks at 640.303 eV (2p_3/2) and 650.476 eV (2p_1/2), comprising about 4% of the surface Mn species.

Following hydrogen exposure (MnO₂/CF/H₂ #2), the Mn 2p spectrum reveals significant changes in the oxidation state distribution (Figure 9ii). New peaks appear at 639.869 eV (2p_3/2) and 651.064 eV (2p_1/2), corresponding to Mn²⁺ species, now constituting approximately 7.9% of the manganese signal. Additionally, peaks at 641.400 eV (2p_3/2) and 652.824 eV (2p_1/2) are attributed to Mn³⁺ species, which account for 36.1%. The proportion of Mn⁴⁺ consequently decreases to 56%, indicating a partial surface reduction in MnO₂ upon hydrogen treatment. This suggests that not all Mn⁴⁺ species participated in the hydrogen storage process [10,11,12].

The comparison of Mn 3s XPS spectra between the two samples also confirms the partial reduction in MnO₂ to lower oxidation states (Figure 10).

The O 1s XPS spectra of MnO₂/CFs provide information about the environment of O on the surface of the material before and after hydrogen exposure (Figure 11). In Figure 11, the band at 529.56 eV (33.8%) is attributed to the lattice oxygen in metal oxides, meaning Mn–O bonds within the MnO₂ structure. The band at 531.222 eV (25.2%) corresponds to carbonyl oxygen (C=O) groups, which may appear due to the previous oxidation of the carbon surface, while the band at 533.162 eV reveals the presence of C–O bonds (41%), which may occur due to air exposure. The XPS spectrum of O 1s after H conditioning showcases the same bands increased in concentration (69.4%) for the Mn–O bond at 529.784 eV, while the peaks for C=O at 531.136 eV and C–O at 533.372 eV decrease at 12.6% and 6.0%. This phenomenon suggests that the hydrogen treatment might have reacted with or removed some of these oxidized carbon species, possibly through hydrogenation reactions, forming volatile products like water or hydrocarbons. The band at 531.926 eV corresponds to –OH, meaning the formation of a hydrolyzed manganese oxide and proving the reduction in Mn [10,11,12].

By integrating the data obtained from both the O 1s and Mn 2p XPS spectra, it is possible to quantify the percentage of MnO₂ present on the surface of the material before and after hydrogen conditioning, although the quantitative comparison of the two samples is not comparable due to uneven deposition of the material. Further information will be shown in Appendix A.

3.2. Thermal Behavior Characterization

The study of TGA diagrams of the synthesized MnO₂/CFs materials under inert and oxidative atmospheres provides insight into the fiber composition and their hydrogen adsorption capacity. The thermogravimetric curve reflects various mass changes occurring during the decomposition process. The inclusion of the first derivative (DTG) in the diagram aids in detecting subtle mass changes that may not be clearly visible in the standard mass loss curve as a function of temperature [30].

TGA studies of carbon fibers in an oxidative environment (presence of O₂) show a gradual mass loss of 1.6% up to 450 °C, followed by a sharp mass reduction between 500 and 820 °C, attributed to oxidative activity on the fiber surface. In contrast, carbon fibers in an inert atmosphere (N₂), under the same heating rate (20 °C/min), exhibit minor mass changes, with a mass loss of approximately 1.2% between 200 and 450 °C [31]. Manganese dioxide (MnO₂) in the presence of air (O₂) exhibits a mass change at T ≈ 250–400 °C due to the following reaction:

6MnO₂ → 3Mn₂O₃ + 3O₂

(6)

and another mass change at 400–600 °C attributed to the following transformation [32]:

3Mn₂O₃ → 2Mn₃O₄ + 0.5O₂

(7)

Under inert conditions (N₂), the same transformations occur but at higher temperatures, with a mass loss of approximately 9% at T ≈ 500–600 °C, and an additional ~3% mass loss at 700–800 °C, corresponding to the same respective conversions [33].

Both sample MnO₂/CF #1 before and sample MnO₂/CF/H₂ #1 after hydrogen exposure were studied under inert conditions (N₂ atmosphere). In the case of sample #1, a mass increase from 100% to 105% is observed up to 500 °C, followed by a 1% mass loss (Figure 12). In contrast, the hydrogen-exposed sample (MnO₂/CF #1) shows a continuous mass decrease from 400 °C to 800 °C. In DTG curve, a negative peak appears around 500 °C, corresponding to a mass loss of approximately 7%. A contradiction seems to exist because, according to the literature, MnO and Mn₂O₃, which are manganese oxide phases, are known to gain mass under inert conditions, and these forms should be present after hydrogen exposure (i.e., in sample MnO₂/CF/H₂ #1). However, the TGA results suggest its presence in the pre-exposure sample (MnO₂/CF #1), while the post-exposure sample (MnO₂/CF/H₂ #1) exhibits mass loss, indicative of MnO₂ decomposition. This inconsistency may stem from an experimental error during sample handling, sampling procedures, or during the hydrogen exposure process.

Samples MnO₂/CF #2 and MnO₂/CF/H₂ #2, before and after hydrogen exposure, respectively, were analyzed under both inert (N₂) and oxidizing (O₂) atmospheres. In the TGA spectrum of sample MnO₂/CF #2, initial thermal stability is observed up to 500 °C, followed by a sharp mass loss of approximately 87%, reaching a plateau at 700 °C (Figure 13). Beyond this temperature, the residual mass stabilizes at 13%. Comparing these results with known TGA profiles of pure carbon fibers suggests that the remaining mass likely corresponds to the presence of MnO₂ or other impurities. Weight loss in an oxidizing environment may be attributed to the total decomposition of carbon fibers to gas CO₂, which takes place at 400–600 °C. Similarly, in the hydrogen-treated sample (MnO₂/CF/H₂ #2), thermal stability is also maintained up to 500 °C, followed by a sharp mass loss of around 75%, resulting in a final residual mass of approximately 25% (Figure 13). The hydrogen-treated sample consists of a higher percentage of MnO and MnOOH, which are the reduction products of MnO₂. Thus, in the hydrogen-treated sample, an increase of about 12% in residual mass is observed. This increase may be attributed to MnO₂ transformations upon reduction, leading to the formation of manganese oxides with higher thermal stability and greater residual mass.

Under inert conditions (N₂), we observe the weight change attributed mainly to the behavior of the deposited Mn oxides on the surface of CFs, as the carbon fibers do not decompose under an inert atmosphere. More specifically, MnO₂/CF #2 exhibits a slight mass loss of approximately 0.5% up to 130 °C, with a DTG minimum peak at 70 °C (Figure 14). Between 150 and 300 °C, a gradual 0.5% mass decrease is observed, with a DTG peak at 250 °C, which is consistent with the typical TGA behavior of carbon fibers. In the range of 350–500 °C, a minor additional mass loss may be attributed to the conversion of MnO₂ to Mn₂O₃, which occurs due to high temperature exposure and releases gas O₂.

In contrast, MnO₂/CF/H₂ #2, after exposure to hydrogen, shows a gradual mass increase from 100% to 108% with rising temperature, a behavior that aligns with TGA data for MnO and Mn₂O₃ phases, which are known to undergo mass gain in inert environments due to their thermal oxidation characteristics (Figure 14) [31].

3.3. Electrochemical Response of CF-Electrodes Towards [Fe(CN)₆]^3−/4−

The electrochemical responses of bare CF and MnO₂-modified CF electrodes towards ferrocyanide/ferricyanide [Fe(CN)₆]^3−/4− standard redox system were studied by means of the cyclic voltammetry method in aqueous KCl solution (1.0 mol∙L⁻¹). The results obtained for all studied electrodes are presented in

Table 11. Anodic peak potential (E_p^ox), cathodic peak potential (E_p^red), half-wave potential (E_1/2), anodic and cathodic peak potential separation (ΔE_p), anodic and cathodic peak current ratios (i_p^ox/i_p^red), anodic peak current density (i_p^ox), active surface area (A), heterogeneous electron transfer rate constant (k_s), charge-transfer resistance (R_ct), and lower limit of detection (LOD) determined for standard redox system [Fe(CN)₆]^3−/4− (1.0 mol∙L⁻¹ KCl) on bare CF, MnO₂/CF #1, MnO₂/CF/H₂ #1, MnO₂/CF #2, and MnO₂/CF/H₂ #2 electrodes at the scan rate of 0.02 V∙s⁻¹.

Parameters	MnO2-Modified CF Electrodes
	CF	MnO2/CF #1	MnO2/CF/H2 #1	MnO2/CF #2	MnO2/CF/H2 #2
Epox/V	0.314	0.307	0.315	0.320	0.393
Epred/V	0.244	0.239	0.234	0.234	0.157
E1/2/V (a)	0.279	0.273	0.274	0.277	0.275
ΔEp/V (b) (c)	0.070	0.068	0.081	0.086	0.236
ipox/ipred	0.90	0.90	0.93	0.93	0.94
A/cm2	0.55	0.81	1.74	1.56	4.64
ipox/μA·cm−2 (c)	105	107	105	105	105
ks/10−3 cm·s−1 (d)	16.9	19.5	8.1	5.9	0.34
Rct/Ω (e)	28.4	23.2	42.4	63.4	78.5
LOD/μM (f)	3.0	1.0	5.0	3.0	8.0

^(a) The E_1/2 values were determined as the average values of E_p^ox and E_p^red; ^(b) the ΔE_p values were estimated as ΔE_p = E_p^ox − E_p^red; ^(c) the values were determined at the concentration of 1.0 × 10⁻³ mol∙L⁻¹ and the scan rate of 0.02 V∙s⁻¹; ^(d) the k_s values were determined from electrochemical absolute rate relation ψ = (D_o/D_R)a/2k_s(nπFvD_o/RT)^−1/2, where ψ is kinetic parameter, a the charge-transfer coefficient (a ≈ 0.5), D_o, D_R are the diffusion coefficients of oxidized and reduced species, respectively (D_o ≈ D_R), and n is the number of electrons involved in the redox reaction (n = 1); ^(e) the EIS were analyzed by means of equivalent electrical circuit (R_s + (C_dl/(R_ct + Z_w))) (software Thales, version 4.15); ^(f) the LOD values were estimated by means of the linear regression model.

. Representative CVs are illustrated in Figure 15a. In CV-curves depicted in Figure 15a, the redox system [Fe(CN)₆]^3−/4− exhibits a pair of reversible redox peaks on CF-based electrodes. The oxidation-reduction peak current ratio is equal to unity and independent of applied scan rate, indicating that there are no parallel chemical reactions coupled to the electrochemical process. Similarly, the oxidative and reductive peak currents are constant for numerous cycles, indicating that there are no chemical reactions coupled to the electron-transfer process and confirming that the redox system is stable in the time frame of the experiment and that the charge-transfer process occurring on MnO₂-modified CF electrodes is quite reversible. The half-wave potential estimated for [Fe(CN)₆]^3−/4− redox system on MnO₂-modified CF electrodes appears to be similar within experimental error (E_1/2 ≈ 0.275 V vs. Ag/AgCl), something that is quite expectable for reversible redox systems. Furthermore, the anodic and cathodic peak currents were found to vary linearly with the square root of scan rate in the investigated range of 0.02–0.10 V·s⁻¹, demonstrating that the studied redox system [Fe(CN)₆]^3−/4− is diffusion-controlled on CF-based electrodes. From the extracted electrochemical parameters presented in Table 11, it can be clearly seen that the anodic and cathodic peak potential separation (ΔE_p) estimated for [Fe(CN)₆]^3−/4− on bare CF and MnO₂-modified CF electrodes lies in the range from 0.068 to 0.236 V (at the scan rate of 0.02 V·s⁻¹), demonstrating differences between charge-transfer kinetics of [Fe(CN)₆]^3−/4− on the various MnO₂-modified CF composite films studied. Namely, the large peak separation of the MnO₂/CF #2 electrode (ΔE_p = 0.086 V) indicates poorer electron-transfer kinetics of [Fe(CN)₆]^3−/4− on this particular electrode compared to the other electrodes studied. The electron-transfer kinetics of MnO₂/CF #2 become even worse after the H₂-treatment. Thus, on the MnO₂/CF/H₂ #2 electrode, a fairly great value of peak potential separation has been estimated (ΔE_p = 0.236 V). The smallest peak potential separation has been obtained for MnO₂/CF #1 electrode (ΔE_p = 0.068 V), which is slightly smaller compared to that of the bare CF electrode (ΔE_p = 0.070 V), and it tends to increase after H₂-treatment. Consequently, on MnO₂/CF/H₂ #1, a slightly greater peak potential separation value has been obtained (ΔE_p = 0.081 V) compared to the untreated MnO₂/CF #1 electrode. Consequently, the heterogeneous electron transfer rate constants (k_s) determined for [Fe(CN)₆]^3−/4− on bare CF and MnO₂-modified CF electrodes by means of electrochemical absolute rate relation tend to increase in the following order: MnO₂/CF/H₂ #2 < MnO₂/CF #2 < MnO₂/CF/H₂ #1 < CF < MnO₂/CF #1 (Figure 15b). The EIS measurements were carried out on MnO₂-modified CF electrodes in the presence of [Fe(CN)₆]^3−/4− redox system for the estimation of charge-transfer resistance (R_ct) (Figure 15c). This parameter provides an estimation of the barrier to overall heterogeneous electron transfer occurring at the electrode–electrolyte interface. The estimated R_ct values are included in Table 11 along with the other electrochemical parameters of [Fe(CN)₆]^3−/4− on various MnO₂-modified CF electrodes. The R_ct values obtained on various MnO₂-modified CF electrodes are presented graphically in Figure 15d. It is quite interesting that the charge-transfer resistance estimated by means of EIS tends to decrease in the order: MnO₂/CF/H₂ #2 < MnO₂/CF #2 < MnO₂/CF/H₂ #1 < CF < MnO₂/CF #1 (similarly to k_s parameter), indicating that a diminishing of barrier of redox process with the simultaneous enhancement of electron-transfer kinetics takes place. For the estimation of the lower limit of detection and sensitivity of CF and MnO₂-modified CF electrodes towards [Fe(CN)₆]^3−/4−, the variation in oxidation peak current with the concentration of redox system in the concentration range of 7.0 × 10⁻⁵–1.0 × 10⁻³ mol∙L⁻¹ was examined. The electrochemical response of CF and MnO₂-modified CF electrodes towards [Fe(CN)₆]^3−/4−, plotted as oxidation peak current density versus concentration of electroactive compound, appears to be linear in the investigated concentration range. From the standard deviation of the electrochemical response and the slope of linear oxidation current-concentration plots, the lower limit of detections of bare CF and MnO₂-modified CF electrodes towards [Fe(CN)₆]^3−/4− were estimated and are included in Table 11. The results exhibit that the electrochemical quality of MnO₂-modified CF electrodes can be considered quite good.

Overall, the characterization techniques employed in this study offer a thorough understanding of the composition of the functionalized materials. In particular, Raman spectroscopy validated the surface modification of pure carbon fibers by the comparison of Id/Ig ratios, which showcases the structural defects in the carbon framework. X-ray photoelectron spectroscopy (XPS) results prove that the product obtained electrochemically showcases a partial reduction in Mn on the surface of the CFs when exposed to hydrogen gas and proves the formation of an MnOOH intermediate. The presence of the MnOOH intermediate can be validated by FTIR spectroscopy, which showcases the presence of -OH groups in the prepared sample in addition to the Mn-O bonds. The possible application of fabricated carbon fiber/MnO₂ composites as materials in electrochemical sensors has been studied in the presence of [Fe(CN)₆]^3−/4− in aqueous KCl solutions. The obtained results are rather promising and demonstrate the future potential application of carbon fiber/MnO₂ composites as working electrodes in electroanalysis.

The investigation into the hydrogen storage capabilities of these materials requires further investigation regarding the release mechanism of the bonded hydrogen, but suggests that the CFs/MnO₂ composite represents a promising avenue for enhancing energy storage technologies. This approach aligns with the growing demand for sustainable energy solutions. Such composite materials hold potential for a variety of industrial applications. One proposed application involves incorporating the modified fibers into textile structures capable of surface hydrogen storage, suitable for use in portable electronic devices, hybrid storage systems, and fuel cells. Additionally, these materials could function as hydrogen sensors or serve as catalysts in hydrogen production and processing reactions. Another prospective application of MnO₂/CFs lies in hydrogen storage tanks for fuel-cell electric vehicles (FCEVs), either as a primary storage material or as a reinforcing component in advanced polymer composites.

4. Conclusions

The synthesis and characterization of carbon fiber/manganese dioxide (MnO₂/CF) composites were successfully conducted using two distinct routes: in situ redox (chemical) deposition and electrochemical deposition. Based on the experimental analyses and results, the following conclusions were drawn:

• Both synthesis methods yielded MnO₂/CF composites with the desired structural and chemical features; however, the electrochemical deposition method produced a denser and more uniform MnO₂ layer, resulting in significantly higher manganese loading (up to ~52 wt%) compared to the chemical method (~10 wt%). SEM and EDS analyses confirmed the successful deposition of MnO₂ on the carbon fiber surface, which was further supported by the characteristic Mn–O vibrational bands observed in the Raman spectra.
• XPS analysis revealed that Mn existed predominantly in the +4 oxidation state prior to hydrogen exposure and partially reduced to Mn³⁺ and Mn²⁺ upon exposure. MnO₂ reduction was validated by the mass changes via TGA, in which the hydrogen-treated composites revealed different thermal behavior compared to untreated samples, which is consistent with oxide phase transitions.
• The formation of an MnOOH intermediate reduction phase following hydrogen exposure can be indicated by the evident peaks at 641.4 eV (2p_3/2) and 652.824 eV (2p_1/2) of the XPS results. Complementary FTIR spectra identified –OH functional groups, as shown by distinct O–H bending vibrations.
• The TGA results obtained under an O₂ atmosphere confirm the presence of manganese oxide products on the surface of the carbon fibers, as evidenced by the residual mass remaining after carbon fiber decomposition. Moreover, for the electrochemically produced material, the formation of oxide phases with enhanced thermal stability is evidenced by the higher residual mass of the hydrogen-treated sample (25% and 13% for samples MnO₂/CF/H₂ #2 and MnO₂/CF #2, respectively) under oxidizing conditions, as well as by the 7.5% greater mass gain observed for sample MnO₂/CF/H₂ #2 under inert conditions compared to the untreated sample.
• Electrochemical characterization indicated that MnO₂-modified CF electrodes exhibited good redox reversibility and enhanced charge-transfer kinetics. However, hydrogen exposure increased charge-transfer resistance slightly, likely due to surface modifications following hydrogen uptake.