# Carbon-Supported Fe Catalysts forCO2 Electroreduction to High-Added Value Products: A DEMS Study: Effect of the Functionalization of the Support

Authors: S. Pérez-Rodríguez; G. García; L. Calvillo; V. Celorrio; E. Pastor; M. J. Lázaro
Journal: International Journal of Electrochemistry
 (2011)

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## Abstract

Vulcan XC-72R-supported Fe catalysts have been synthesised for the electroreduction of CO2 to high-added value products. Catalysts were obtained by the polyol method, using ethylene glycol as solvent and reducing agent. Prior to the metal deposition, Vulcan was subjected to different oxidation treatments in order to modify its surface chemistry and study its influence on the physicochemical and electrochemical properties of the catalysts, as well as on the product distribution. The oxidation treatments of the supports modify their textural properties, but do not affect significantly the physicochemical properties of catalysts. However, DEMS studies showed that the carbon support degradation, the distribution of products, and the catalytic activity toward the CO2 electroreduction reaction depend significantly on the surface chemistry of the carbon support.


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## Body

## 1. Introduction

Carbon dioxide (CO2) emissions are the inevitable result from the burning of fossil fuels for electricity and energy (80% anthropogenic CO2) [1]. During the last years, CO2 concentration in the atmosphere has been increasing, being the major responsible of global warming. Therefore, reducing the CO2 concentration in the atmosphere has become a critical issue. Different methods have been developed to reduce its emissions, such as chemical, thermochemical, photochemical, electrochemical, and biochemical procedures [2–4]. Among them, the electrochemical reduction seems to be of particular interest since it could both mitigate the greenhouse gas emission and use CO2 as carbon source for producing a variety of useful products like (e.g., formic acid, methanol, etc.) for energy source [1, 4–8]. CO2 reduction would be carried out making use of renewable energy to result in a net decrease of CO2 emissions [9, 10].In recent years, different metallic electrodes have been studied for the electrochemical reduction of carbon dioxide, since the product distribution strongly depends on the used material, surface metallic arrangement, and surface energy [11–17]. Copper has been found to be one of the most effective electrode materials for the CO2 reduction process at atmospheric pressure and room temperature in aqueous solutions [11, 12, 16]. On the other hand, CO2 is hardly reduced on group VIII-X metal electrodes such as Fe, Co, and Ni, under similar conditions [15–17].One of the main problems of this process is the low solubility of CO2 in water at atmospheric pressure and room temperature. For this reason, in the last years, the electroreduction of CO2 has been studied at high pressure [18–21] or low temperatures [21–24] on different metal electrodes. It has been reported that, at low temperatures (ca. 2°C) or high pressures (ca. 30 atm), the catalytic activity of the electrodes toward the electrochemical CO2 reduction increases and the selectivity of the resultant products can change, even for metal catalysts of the group VIII-X [18–24]. In this context, Azuma et al. reported that the CO2 reduction efficiency increased dramatically on some metal electrodes, such as Ni, as the temperature decreased [24]. Conversely, at high pressure, formic acid and/or carbon monoxide are efficiently formed on metal electrodes of the group VIII-X. Moreover, the formation of short and long chain hydrocarbons such as methane, ethane, propane, and iso- and normal-butanes has also been observed on Fe, Co, and Ni electrodes [18–20].Since the solubility of CO2 in aprotic solvents is higher than in water, the electroreduction of CO2 has also been studied using organic molecules (methanol, acetonitrile, dimethyl formamide, propylene carbonate, etc.) as reaction medium [25–32]. Higher CO2 solubility increases the current density, however, the low electrolytic conductivity gives high ohmic losses. For this reason, methanol is often added into a supporting electrolyte in order to balance these two aspects. For example, Kaneco et al. reported that the faradic efficiencies for CO2 reduction products using Cu electrode in a methanol solution at low temperatures were better than those obtained without methanol at ambient temperature [29, 30]. In addition, Ohta et al. reported the formation mainly of methane, carbon monoxide and ethane, on different metal electrodes (among them Fe, Co, and Ni) using methanol into the supporting electrolyte [27].Therefore, the effective electrochemical reduction of CO2 on metal surfaces of the group VIII-X using high pressures, low temperatures, and/or nonaqueous solvents has been demonstrated. Among these metals, Fe is well known as catalyst for the hydrocarbon formation in the Fischer-Tropsch reaction. Therefore, its catalytic activity toward the electrochemical CO2 reduction is expected to be interesting [33].On the other hand, carbon materials have also been used as electrodes for the electrochemical CO2 reduction. However, until now, the electrocatalytic activity of these electrodes is not clear. Christensen et al. reported that CO2 is reduced to CO and carbonate on a glassy carbon electrode in acetonitrile solution [32]. Moreover, Hara et al. reported the formation of hydrocarbons such as methane, ethane, ethylene, propane, and n-butane during the electrochemical CO2 reduction on a glassy carbon electrode under 30 atm [34]. However, there are not many studies about the electroreduction of CO2 on metal catalysts supported on carbon materials in aqueous electrolytes. These electrodes could have different properties than those of the corresponding metal or carbon material. The support could improve the dispersion of the metal and, therefore, the activity and/or selectivity could be changed. Nowadays, among all kinds of carbon supports, carbon blacks are the most commonly used, especially for electrochemical applications (e.g., in the fuel cells field), due to their mesoporous distribution and their graphite characteristics. Vulcan XC-72 is the most frequently used because of its good compromise between electrical conductivity and high specific surface area [35, 36]. The surface chemistry of carbon materials can be modified by oxidation treatments in gas or liquid phase in order to create functional groups. These functional groups may significantly affect the dispersion and anchoring of the metal on the carbon materials and, therefore, may affect the performance of the electrocatalysts. In addition, it is well known that surface oxygen groups are the responsible for both the acid-base and the redox properties of the carbon materials. It has been reported that the acidic groups on the carbon surface decrease the hydrophobicity of the carbon, whereas the less acidic groups improve the interaction between metal particles and carbon materials [37]. However, the functionalization of Vulcan XC-72R has not been studied for the CO2 electroreduction reaction.In this work, different Fe catalysts supported on Vulcan XC-72R have been prepared for studying the electroreduction of CO2 in aqueous solution under 1 atm and room temperature. Prior to the metal deposition, Vulcan was subjected to different oxidation treatments, using HNO3 or HNO3-H2SO4 1 : 1 (v/v) mixture as oxidizing agents, in order to create functional groups. In this way, the influence of the surface chemistry of the carbon support on the physicochemical and electrochemical properties of the catalysts for the CO2 electroreduction process can be studied.In the present communication, the modified and unmodified carbon supports were characterized by X-ray diffraction (XRD), scanning electron microscopy (SEM), temperature programmed desorption (TPD), and N2-physisorption. On the other hand, carbon-supported catalysts (Fe/C) were characterized by energy dispersive X-ray analysis (EDX), XRD, SEM, and N2-physisorption. In addition, the electrochemical properties of the catalysts and the formation of gaseous and volatile products of the reduction of CO2 were followed by in-situ differential electrochemical mass spectrometry (DEMS).


## 2. Experimental

### 2.1. Functionalization of Vulcan XC-72R

In order to create functional groups, Vulcan XC-72R (Cabot) was modified with different oxidation treatments in liquid phase, using concentrated HNO3 (65% wt.) (Nc) and an HNO3-H2SO4 1 : 1 (v/v) mixture (NS) as oxidizing agents [38]. The oxidation treatments were carried out at room (Ta) and boiling temperature (Tb) for 0.5 or 2 h. The nomenclature used for the different materials and the oxidation conditions are summarized in Table 1.Table 1
Nomenclature of functionalizated Vulcan XC-72R.
SampleOxidizing agentTemperature (°C)Time (h)Vulcan———Vulcan NSTa0.5HNO3-H2SO4 1 : 1 (v/v)250.5Vulcan NcTb0.5Concentrated HNO3 (65%)1150.5Vulcan NcTb2Concentrated HNO3 (65%)1152


### 2.2. Synthesis of the Carbon-Supported Fe Electrocatalysts

Fe electrocatalysts were prepared by polyol method, using ethylene glycol (EG) as solvent and reducing agent. The synthesis involved the following steps: first, the metal precursor, Cl3Fe · 6H2O (Sigma-Aldrich), was dissolved in ethylene glycol under sonication and the pH was adjusted to 11 using a 1 M NaOH/EG solution. Then, a known amount of Vulcan was added to the metal solution and the resultant suspension was heated at 195°C for 2 h under mechanical stirring. Subsequently, the mixture was quickly cooled in a cold-water bath and the pH was adjusted to 1 using HCl (37%, Sigma-Aldrich). Finally, catalysts were filtered, washed with water, and dried at 70°C. Appropriate amounts of metal precursors were used to obtain a theoretical metal loading of 20 wt.%.


### 2.3. Physicochemical Characterization

Metal content of the electrocatalysts was obtained using a Hitachi S-3400 N microscope coupled to a Röntec XFlash analyzer.Temperature programmed desorption (TPD) experiments were carried out in a U-shaped quartz reactor using a Micromeritics Pulse Chemisorb 2700. The temperature was increased positively at a rate of 10°C min−1 up to 1050°C under Ar flow. The amounts of CO and CO2 desorbed from the carbon samples were analyzed online by mass spectroscopy using a Thermostar GSD 301 T (Balzers).Nitrogen adsorption and desorption isotherms were measured at −196°C using a Micromeritics ASAP 2020. The total surface area was determined using the (Brunauer, Emmett and Teller) BET equation and total pore volume was determined using the single point method atP/P0=0.99. The micropore volume was determined using the t-plot method. Pore size distribution (PSD) curves were obtained from the analysis of the adsorption branch of the nitrogen isotherm using the (Barrett, Joyner and Halenda) BJH method. The maximum of the PSD was used as the average pore diameter.X-Ray diffraction (XRD) patterns were recorded using a Bruker AXS B8 Advance diffractometer with aθ-θ configuration and using Cu Kα radiation.


### 2.4. Preparation of Working Electrodes

The working electrodes (7 mm of diameter, 0.25 mm of thickness) were prepared depositing a layer of the catalysts ink onto one side of a carbon cloth previously treated at 320°C for 1 h. Catalyst inks were prepared by mixing 0.5 mg of catalyst, 0.01 g of Nafion dispersion (5 wt.%, Sigma-Aldrich), and 10μL of ultrapure water. The final metal load of the working electrodes was 0.26 mg Fe/cm2.


### 2.5. DEMS Setup

A scheme of the DEMS setup used for the in situ spectrometric and electrochemical measurements is described in detail in [39]. Briefly, the working electrode (WE) is fixed between a PTFE membrane (Scimat) and a carbon glassy rod, which also keeps the electric contact. The cell was designed to follow “in-situ” the electrochemical properties of electrodes and, simultaneously, the gaseous species produced on the electroactive surface through mass spectrometry. Thus, the experimental setup allows the simultaneous acquisition of mass spectrometric cyclic voltammograms (MSCVs) for selected m/z (mass to charge) ratios and conventional voltammograms (CVs) or simultaneous mass spectrometric transients (MSTs) and conventional current transient curves.


### 2.6. Electrochemical Measurements

Electrochemical experiments were carried out in a three-electrode electrochemical cell at room temperature and atmospheric pressure. A large area carbon rod was used as a counter electrode, whereas an Ag/AgCl/Sat. KCl electrode placed inside a Luggin capillary was employed as reference. All potentials in the text are referred to this electrode. The potenciostat-galvanostat was an Autolab PGSTAT302 (Ecochemie). The electrochemical cell was directly attached to the vacuum chamber of a mass spectrometer (Balzers QMG112) with a Faraday cup detector.The working electrode was immersed into 0.5 M H2SO4 (Merck, p.a.) electrolyte solution, which was deaerated with argon (N50). In order to analyze the activity of catalysts towards the reduction of CO2, previously to each measure, CO2 (99,99%, Air Liquide) was bubbled during 30 min.


## 2.1. Functionalization of Vulcan XC-72R

In order to create functional groups, Vulcan XC-72R (Cabot) was modified with different oxidation treatments in liquid phase, using concentrated HNO3 (65% wt.) (Nc) and an HNO3-H2SO4 1 : 1 (v/v) mixture (NS) as oxidizing agents [38]. The oxidation treatments were carried out at room (Ta) and boiling temperature (Tb) for 0.5 or 2 h. The nomenclature used for the different materials and the oxidation conditions are summarized in Table 1.Table 1
Nomenclature of functionalizated Vulcan XC-72R.
SampleOxidizing agentTemperature (°C)Time (h)Vulcan———Vulcan NSTa0.5HNO3-H2SO4 1 : 1 (v/v)250.5Vulcan NcTb0.5Concentrated HNO3 (65%)1150.5Vulcan NcTb2Concentrated HNO3 (65%)1152


## 2.2. Synthesis of the Carbon-Supported Fe Electrocatalysts

Fe electrocatalysts were prepared by polyol method, using ethylene glycol (EG) as solvent and reducing agent. The synthesis involved the following steps: first, the metal precursor, Cl3Fe · 6H2O (Sigma-Aldrich), was dissolved in ethylene glycol under sonication and the pH was adjusted to 11 using a 1 M NaOH/EG solution. Then, a known amount of Vulcan was added to the metal solution and the resultant suspension was heated at 195°C for 2 h under mechanical stirring. Subsequently, the mixture was quickly cooled in a cold-water bath and the pH was adjusted to 1 using HCl (37%, Sigma-Aldrich). Finally, catalysts were filtered, washed with water, and dried at 70°C. Appropriate amounts of metal precursors were used to obtain a theoretical metal loading of 20 wt.%.


## 2.3. Physicochemical Characterization

Metal content of the electrocatalysts was obtained using a Hitachi S-3400 N microscope coupled to a Röntec XFlash analyzer.Temperature programmed desorption (TPD) experiments were carried out in a U-shaped quartz reactor using a Micromeritics Pulse Chemisorb 2700. The temperature was increased positively at a rate of 10°C min−1 up to 1050°C under Ar flow. The amounts of CO and CO2 desorbed from the carbon samples were analyzed online by mass spectroscopy using a Thermostar GSD 301 T (Balzers).Nitrogen adsorption and desorption isotherms were measured at −196°C using a Micromeritics ASAP 2020. The total surface area was determined using the (Brunauer, Emmett and Teller) BET equation and total pore volume was determined using the single point method atP/P0=0.99. The micropore volume was determined using the t-plot method. Pore size distribution (PSD) curves were obtained from the analysis of the adsorption branch of the nitrogen isotherm using the (Barrett, Joyner and Halenda) BJH method. The maximum of the PSD was used as the average pore diameter.X-Ray diffraction (XRD) patterns were recorded using a Bruker AXS B8 Advance diffractometer with aθ-θ configuration and using Cu Kα radiation.


## 2.4. Preparation of Working Electrodes

The working electrodes (7 mm of diameter, 0.25 mm of thickness) were prepared depositing a layer of the catalysts ink onto one side of a carbon cloth previously treated at 320°C for 1 h. Catalyst inks were prepared by mixing 0.5 mg of catalyst, 0.01 g of Nafion dispersion (5 wt.%, Sigma-Aldrich), and 10μL of ultrapure water. The final metal load of the working electrodes was 0.26 mg Fe/cm2.


## 2.5. DEMS Setup

A scheme of the DEMS setup used for the in situ spectrometric and electrochemical measurements is described in detail in [39]. Briefly, the working electrode (WE) is fixed between a PTFE membrane (Scimat) and a carbon glassy rod, which also keeps the electric contact. The cell was designed to follow “in-situ” the electrochemical properties of electrodes and, simultaneously, the gaseous species produced on the electroactive surface through mass spectrometry. Thus, the experimental setup allows the simultaneous acquisition of mass spectrometric cyclic voltammograms (MSCVs) for selected m/z (mass to charge) ratios and conventional voltammograms (CVs) or simultaneous mass spectrometric transients (MSTs) and conventional current transient curves.


## 2.6. Electrochemical Measurements

Electrochemical experiments were carried out in a three-electrode electrochemical cell at room temperature and atmospheric pressure. A large area carbon rod was used as a counter electrode, whereas an Ag/AgCl/Sat. KCl electrode placed inside a Luggin capillary was employed as reference. All potentials in the text are referred to this electrode. The potenciostat-galvanostat was an Autolab PGSTAT302 (Ecochemie). The electrochemical cell was directly attached to the vacuum chamber of a mass spectrometer (Balzers QMG112) with a Faraday cup detector.The working electrode was immersed into 0.5 M H2SO4 (Merck, p.a.) electrolyte solution, which was deaerated with argon (N50). In order to analyze the activity of catalysts towards the reduction of CO2, previously to each measure, CO2 (99,99%, Air Liquide) was bubbled during 30 min.


## 3. Results

### 3.1. Characterization of the Supports

SEM and XRD techniques were used to study the morphology of carbon support, before and after the oxidation treatments. SEM images (not shown) prove that Vulcan XC-72R is formed by an aggregation of spherical carbon nanoparticles (primary particles) with range sizes of 30–60 nm. After the oxidation treatments, the structure of Vulcan was not altered significantly. However, the most severe oxidation treatment (NcTb2) resulted in a partial destruction of its morphology, since primary particles did not show a spherical shape.Figure1 shows the XRD patterns of all the carbon supports. In all the samples, a peak around 2θ = 25° was observed, which is associated to the graphite (002) diffraction line. Also, (100) and (101) reflections of the graphite, at 2θ = 24.8° and 2θ = 43.5°, can be observed. These peaks confirm that Vulcan has an intermediate structure between amorphous and graphitic. After the oxidation treatments, the same peaks were observed, indicating that the original structure of Vulcan was maintained. However, the intensity of the peaks increased with the severity of the oxidation treatment, except for the sample Vulcan NcTb2. This increase is attributed to the removal of the more amorphous carbon. In other words, the structure ratio crystalline/amorphous increases. On the other hand, the sample Vulcan NcTb2 did not follow the same tendency, which is attributed to the partial destruction of the original structure of Vulcan (i.e., both amorphous and crystalline structures are damaged), as observed by SEM.Figure 1
XRD patterns of carbon supports.The surface chemistry of the supports was studied by TPD experiments. These measurements give information about the surface oxygen groups created during the oxidation treatments. Acidic groups (carboxylic groups, lactones, and anhydrides) are decomposed into CO2 at lower temperatures and basic and neutral groups (anhydrides, phenols, quinones and carbonyls) are decomposed into CO at higher temperatures during the TPD experiments [40]. In order to estimate the type and the amount of oxygen groups created during the oxidation treatments, CO2 and CO profiles can be deconvoluted. Thus, the decomposition temperature can be related to the type of the functional groups created [40]. Deconvolution profiles were carried out with Excel software, using a Gaussian function to fit each functional group contribution and the corresponding addition of Gaussian curves was fitted minimizing the square of the deviations by a numerical routine (conjugate gradient method). Other authors have used this method [41].As can be seen in Table2, the original material had a negligible amount of surface oxygen groups. After the oxidation treatments, the number of surface oxygen groups increased, being the treatment with HNO3 at boiling temperature during 2 h (NcTb2) the most effective at creating functional groups. In addition, it is observed that the ratio CO/CO2, which can be taken as a measure of the surface acidity [42], decreased as the severity of the treatment increased.Table 2
Quantification of surface oxygen groups as CO and CO2 amounts desorbed during the TPD experiments.
SampleCO2 and CO peak area (μmolg−1)CO + CO2 (μmolg−1)CO/CO2CarboxylicLactoneAnhydridePhenolQuinone + carbonylVulcan———————Vulcan NSTa0.55452566541288121601.54Vulcan NcTb0.55562435848069920371.42Vulcan NcTb27993626363296328191.34Deconvolution of CO2 profiles showed that carboxylic groups were mainly created. It is expected that these groups decrease the hydrophobic character of the carbon materials, improving their interaction with the metal. On the other hand, deconvolution of CO profiles showed that phenols, quinones, and carbonyls were mainly created. It is expected that these groups, which are stable at higher temperatures, act as metal anchoring sites, hindering the agglomeration of metal particles [42].In order to further investigate how the pore structure and textural properties of the Vulcan XC-72R were changed during the oxidation treatments (see Section2.1 for oxidation treatments details), supports were characterized by means of N2-physisorption. Table 3 contains the textural properties of the carbon materials obtained by N2-physisorption. Vulcan XC-72R has a high specific surface area (210 m2 g −1) and a large total pore volume (0.38 cm3 g−1). Nevertheless, after the oxidation treatments, the specific surface area of all the samples decreased indicating a partial destruction of the original morphology, being this effect more significant at the carbon material oxidized with the most severe treatment (Vulcan NcTb2). However, no significant change was observed in the pore volume. In fact, carbon supports are mainly mesoporous materials but also contain an appreciable amount of micropores, which is maintained after the surface oxidation. Results suggest that all carbon materials present a broad pore size distribution (PSD) in the range of mesoporosity.Table 3
Textural properties of the supports and Fe electrocatalysts.
SampleSBET (m2/g)SMICRO (m2/g)SMESO (m2/g)VTOTAL (cm3/g)VMICRO (cm3/g)VMESO (cm3/g)Vulcan2101021080.380.060.32Vulcan NSTa0.5200104960.400.060.34Vulcan NcTb0.518191900.380.050.33Vulcan NcTb215977820.380.040.33Fe/Vulcan17576990.410.040.36Fe/Vulcan NSTa0.5166551110.490.030.46Fe/Vulcan NcTb0.514858900.410.030.37Fe/Vulcan NcTb213954850.420.030.38


### 3.2. Physicochemical Characterization of the Electrocatalysts

The catalysts metal loading was determined by SEM-EDX. All catalysts present similar iron content to the nominal value of 20% (Table4). However, a clear correlation between oxygen groups present in the surface and metal loading can be discerned. As the number of oxygenated groups increased, the amount of deposited Fe increased, since these oxygenated groups acted as anchoring sites. Additionally, homogeneous metal dispersion and deposition on all the carbon materials was observed by SEM images.Table 4
Metal load of the carbon-supported Fe electrocatalysts.
Electrocatalysts% metal (wt.)Fe/Vulcan16.7Fe/Vulcan NSTa0.518.4Fe/Vulcan NcTb0.518.9Fe/Vulcan NcTb221.8Fe/C catalysts were analyzed by XRD technique and their patterns are given in Figure2. In all the electrocatalysts, except in the sample Fe/Vulcan NSTa0.5, six characteristic peaks appeared at 2θ = 30.1, 35.5, 43.1, 57.0, 62.6, which can be assigned to (2 2 0), (3 1 1), (4 0 0), (5 1 1), and (4 4 0) planes of Fe3O4 (magnetite) (JCPDS 88-0866), respectively. No diffraction peaks corresponding to iron metal or iron oxides species (FeO or Fe2O3) were observed. However, the intensity of the Fe3O4 diffraction peaks was not so relevant than that expected for 20 wt.% of iron load. This result suggests that another crystal phase with particle size inferior to 2 nm coexisted with Fe3O4 crystals and/or part of the metal was deposited on carbon materials forming a stable but not crystalline structure. In this context, it is important to mention that particle size smaller than 2 nm cannot be achieved by XRD analysis. Other authors have obtained similar results depositing Fe on carbon supports [43]. Additionally, it is noticeable that the diffraction peak at ca. 2θ = 25°, which is associated to the graphite (002) diffraction line of the support, is still observed after the iron deposition.Figure 2
XRD patterns of 20% Fe/C catalysts.Textural properties of catalysts obtained by N2-physisorption are summarized in Table 3. Catalysts showed a lower surface area than the corresponding carbon supports, which is attributed to the metal particles loading on the pore surface. In particular, a reduction of the microporosity was observed after the catalysts loading, indicating that the metal was mainly distributed in the micropore structure of the support. PSD continued being broad in the mesoporosity range. However, the pore volume in the 20–50 nm pore diameter range is reduced, whereas in the 50–100 nm pore diameter range is increased. These results indicate that iron was deposited on the micropores or mesopores with average pore diameter lower than 50 nm, in agreement with the N2-physisorption results.


### 3.3. Electrochemical Performances of the Fe Electrocatalysts

The electrochemical properties of the Fe catalysts were studied in 0.5 M H2SO4, at room temperature and atmospheric pressure by DEMS. In this sense, DEMS studies provide more information than a simple electrochemical technique (i.e., cyclic voltammetry or chronoamperometry) such as the detection of volatile and gaseous products and intermediates generated in the electrochemical reactions with excellent sensibility. In this context, to the best of our knowledge, this is the first time that CO2 reduction on carbon-supported Fe catalysts is analyzed by DEMS technique.First, several potential cycles (not shown) between −0.2 and −1.8 V in 0.5 M H2SO4, previously deaerated with Ar, were recorded to clean and activate the catalyst surface. In this context, the voltammetric profile remains similar during the activation step for all catalysts, indicating a minimal (or inexistent) alteration of the electroactive surface. After that, in situ spectroelectrochemical experiments were carried out in acid solution with and without dissolved CO2.


#### 3.3.1. Cyclic Voltammetry (CV) and Mass Spectrometric Cyclic Voltammetry (MSCV)

Figure3 shows the CVs and the corresponding MSCVs for all the carbon-supported Fe catalysts in free CO2 sulphuric acid solution. The CVs for all the catalysts (Figure 3(a)) present a similar feature, that is, a very high cathodic current at potentials lower than −0.5 V, which may be related to the hydrogen evolution reaction. However, a close inspection of the same figure shows up that the onset potential for the cathodic current starts at different potentials for the different electrodes. The latter becomes clear from the MSCVs for m/z = 2 (Figure 3(c)), which is related to the molecular hydrogen formation. Therefore, it is possible to state that the previous carbon treatment influences the water electro-reduction, and that the catalytic activity towards this reaction on the present Fe/C electrodes in a CO2 free acid solution increases in the following way: Fe/Vulcan NcTb2 ≈ Fe/Vulcan NcTb0.5 < Fe/Vulcan NSTa0.5 ≪ Fe/Vulcan. Also, it is important to mention that the electrochemical behavior of all the electrodes remains similar after the electrochemical study without CO2. The latter indicates that the electroactive surface is not damaged (or it is minimum) by these experiments.CVs and MSCVs for Fe/C catalysts in 0.5 M H2SO4 (sweep rate 10 mV s−1, Ei=-0.2 V versus Ag/AgCl/Sat.). Inset shows a zoom of the onset potential region during the cathodic scan.
(a)(b)(c)(d)Additionally to the H2 formation, the mass signals m/z = 16 (CH4+: methane), 30 (CH3CH3+ or H2CO+: ethane or formaldehyde), 29 (CH3CH2+ or CHO+: ethane/ethanol or an aldehyde), and 45 (HCOO+ or CH3CHOH+: formic acid or ethanol) were monitored during the cathodic scan. Figures 3(b) and 3(d) show the only two signals (m/z = 29 and 45) that increase during the excursion toward negative potentials. In this condition (no presence of dissolved CO2), the species associated to the mass signals 29 and 45 must be formed from the carbon support degradation. Interestingly, the mass signal 45 depends strongly on the carbon support treatment and its intensity rises in the order: Fe/Vulcan < Fe/Vulcan NcTb0.5 < Fe/Vulcan NcTb2 < Fe/Vulcan NSTa0.5. It is noticeable that the onset potential for the mass signal 45 formation at the catalyst previously treated with a mix of nitric and sulphuric acid is much lower than at the other catalysts (around 0.2 V), while the nontreated catalyst (Fe/Vulcan) presents a very small m/z = 45 signal at potentials more negative than −1.3 V. In the same way, both catalysts treated only with nitric acid develop the same onset potential for this m/z ratio, but its production on the Fe/Vulcan NcTb2 is somehow higher.On the other hand, the ion current intensity and onset potential for the mass signal 29 are quite similar for all Fe/C catalysts. However, a close inspection of this figure shows a small but visible trend in its production, which diminishes in the subsequent way: Fe/Vulcan > Fe/Vulcan NSTa0.5 > Fe/Vulcan NcTb2. Fe/Vulcan NcTb0.5 catalyst presents a different behavior toward the mass signal 29 production, in which the onset potential is equal to Fe/Vulcan NcTb2 electrode and the ion current intensity increases linearly as the applied potential becomes more negative.Summarizing, at the present conditions (CO2-free solution), nontreated catalyst (Fe/Vulcan) presents the highest and lowest catalytic activity towards hydrogen and mass signal 45 production, respectively. Treated catalysts develop similar behavior toward hydrogen evolution and the ionic current for the m/z = 45 depends strongly on the catalyst surface (see Table 2), that is, the mass signal 45 is enhanced on the catalysts that present oxygen groups on the surface. Additionally, mass signal 29 intensity modestly depends on the previous history of the carbon support.Figure4 displays the CVs and MSCVs (m/z = 2, 29, and 45) for all the Fe/C catalysts studied in the present work in acidic solution in the presence of dissolved carbon dioxide. Also, the m/z = 16, 30, and 32 were studied, but do not present an ionic current change during the cathodic scan. It is important to note that the intensity as well as the behavior of the mass signals 2, 29 and 45 are totally different to those observed in Figure 3 (in absence of dissolved CO2). Interestingly, in presence of dissolved CO2, the hydrogen evolution (Figure 3(c)) decreases on Fe/Vulcan, Fe/Vulcan NcTb0.5 and Fe/Vulcan NcTb2, while it increases on Fe/Vulcan NSTa0.5. Moreover, the latter catalyst presents an onset potential shift to more positive potentials for hydrogen formation reaction, that is, water reduction is favored on Fe/Vulcan NSTa0.5 in CO2 containing solution. Also, the the ratio m/z = 29 Figure 3(b) changes abruptly when CO2 is present in the working solution. The ion current intensity for this mass signal in a CO2-containing solution is higher than in a CO2-free one, and it drops off in the sequence: Fe/Vulcan NSTa0.5 > Fe/Vulcan > Fe/Vulcan NcTb2 ≈ Fe/Vulcan NcTa0.5, whereas the onset potential is quite similar for all the electrodes.CVs and MSCVs for CO2-saturated solution in 0.5 M H2SO4 on Fe/C catalysts (sweep rate 10 mV s−1, Ei=-0.2 V versus Ag/AgCl/Sat.).
(a)(b)(c)(d)On the other hand, Figure4(d) shows an important enhancement of the mass signal 45 at all the catalysts when CO2 is present in the solution. These experimental facts unequivocally indicate that carbon dioxide is reduced to form hydrocarbonated compounds such as formic acid. The formation of acids, alcohols, or other molecules, which contain longer hydrocarbon chains, is not discarded but this characterization is not the principal purpose of the present work: the main reasons of the present study are to know if it is possible to electrochemically reduce CO2 on iron catalysts and to establish if the carbon support influences on this particular reaction. Therefore, only the mass signals 2 and 45 are going to be followed along the present manuscript.


#### 3.3.2. Current Transient (CT) and Mass Spectrometric Transient (MST)

Potentiostatic pulse experiments were performed from a potential where nonfaradaic reactions occur (Ei=-0.2 V) to a final potential (Ef=-1.8 V) where the CO2 reduction reaction is controlled by mass diffusion. Current transients for all the Fe/C catalysts used in the present work in absence (a) and presence (b) of dissolved CO2 in sulphuric acid solution can be seen in Figure 5. It is observed similar faradaic current intensities than those obtained during the potentiodymanic experiments (Figures 3(a) and 4(a)), that is, Fe/Vulcan NcTb2 presents at both mediums (in presence and absence of dissolved CO2) the lowest faradaic current, while the other catalysts develop similar faradaic currents. Consistent with the results presented above, molecular hydrogen production is significantly influenced by the presence of CO2 (Figure 6). Fe/Vulcan and Fe/Vulcan NSTa0.5 electrodes present the highest catalytic activity toward H2 formation in absence and presence of CO2, respectively. Also, it is noticeable that the signal for m/z = 2 decreases abruptly on Fe/Vulcan, Fe/Vulcan NcTb0.5, and Fe/Vulcan NcTb2 catalysts, while the same reaction is enhanced on the Fe/Vulcan NSTa0.5 when CO2 is present in solution.CTs for CO2-free (a) and CO2-saturated (b) solution in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).
(a)(b)MSTs for CO2-free (a) and CO2-saturated (b) solution in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).
(a)(b)Figure7(a) shows the MSTs for the mass signal 45. Currents obtained are of the same order of magnitude than in the voltammetric experiments. However, a close inspection of the curves reveals that the m/z = 45 signal continuously increases on Fe/Vulcan catalyst along the time, while the other catalysts present a constant ionic current. The latter suggests that the support time degradation is more important at this material. In this sense, it is important to remind that Fe/Vulcan electrode presents small quantity of oxygenated species on the surface (see Table 2), that is, this catalyst suffers a dreadful condition at this potential. On the other hand, when CO2 is present in solution (Figure 7(b)) the intensity of the mass signal 45 changes dramatically (about five fold times), as it was observed before the MSCV experiments (Section 3.3.1). In fact, the ionic current intensities for the mass signal 45 grow up on the studied catalysts in the following way: Fe/Vulcan NcTb2 < Fe/Vulcan < Fe/Vulcan NcTb0.5 < Fe/Vulcan NSTa0.5.MSTs for CO2-free (a) and CO2 saturated (b) solution in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).
(a)(b)In order to acquire a realistic result of hydrocarbon production from carbon dioxide reduction, the mass signal 45 was subtracted from the ionic current signals obtained with dissolved CO2 in solution (Figure 7(b)) and those acquired in a CO2-free solution (Figure 7(a)) and represented in Figure 8. In this context, it is really important to know that this subtraction can be only done if all the parameters concerning to the mass spectrometer are constant [44], and because of this, our mass spectrometer setup was build up to make all this parameters accurate [39]. Therefore, Figure 8 shows a realistic catalytic activity toward carbon dioxide reduction. In fact, it can be observed that the typical features of a reaction controlled by mass diffusion, and even more important that the carbon dioxide reduction, or what is the same in this event, the hydrocarbon production depends strongly on the catalyst support and it increases as follows: Fe/Vulcan NcTb2 < Fe/Vulcan < Fe/Vulcan NSTa0.5 ≈ Fe/Vulcan NcTb0.5.Figure 8
Corrected MSTs for CO2 electroreduction in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).


## 3.1. Characterization of the Supports

SEM and XRD techniques were used to study the morphology of carbon support, before and after the oxidation treatments. SEM images (not shown) prove that Vulcan XC-72R is formed by an aggregation of spherical carbon nanoparticles (primary particles) with range sizes of 30–60 nm. After the oxidation treatments, the structure of Vulcan was not altered significantly. However, the most severe oxidation treatment (NcTb2) resulted in a partial destruction of its morphology, since primary particles did not show a spherical shape.Figure1 shows the XRD patterns of all the carbon supports. In all the samples, a peak around 2θ = 25° was observed, which is associated to the graphite (002) diffraction line. Also, (100) and (101) reflections of the graphite, at 2θ = 24.8° and 2θ = 43.5°, can be observed. These peaks confirm that Vulcan has an intermediate structure between amorphous and graphitic. After the oxidation treatments, the same peaks were observed, indicating that the original structure of Vulcan was maintained. However, the intensity of the peaks increased with the severity of the oxidation treatment, except for the sample Vulcan NcTb2. This increase is attributed to the removal of the more amorphous carbon. In other words, the structure ratio crystalline/amorphous increases. On the other hand, the sample Vulcan NcTb2 did not follow the same tendency, which is attributed to the partial destruction of the original structure of Vulcan (i.e., both amorphous and crystalline structures are damaged), as observed by SEM.Figure 1
XRD patterns of carbon supports.The surface chemistry of the supports was studied by TPD experiments. These measurements give information about the surface oxygen groups created during the oxidation treatments. Acidic groups (carboxylic groups, lactones, and anhydrides) are decomposed into CO2 at lower temperatures and basic and neutral groups (anhydrides, phenols, quinones and carbonyls) are decomposed into CO at higher temperatures during the TPD experiments [40]. In order to estimate the type and the amount of oxygen groups created during the oxidation treatments, CO2 and CO profiles can be deconvoluted. Thus, the decomposition temperature can be related to the type of the functional groups created [40]. Deconvolution profiles were carried out with Excel software, using a Gaussian function to fit each functional group contribution and the corresponding addition of Gaussian curves was fitted minimizing the square of the deviations by a numerical routine (conjugate gradient method). Other authors have used this method [41].As can be seen in Table2, the original material had a negligible amount of surface oxygen groups. After the oxidation treatments, the number of surface oxygen groups increased, being the treatment with HNO3 at boiling temperature during 2 h (NcTb2) the most effective at creating functional groups. In addition, it is observed that the ratio CO/CO2, which can be taken as a measure of the surface acidity [42], decreased as the severity of the treatment increased.Table 2
Quantification of surface oxygen groups as CO and CO2 amounts desorbed during the TPD experiments.
SampleCO2 and CO peak area (μmolg−1)CO + CO2 (μmolg−1)CO/CO2CarboxylicLactoneAnhydridePhenolQuinone + carbonylVulcan———————Vulcan NSTa0.55452566541288121601.54Vulcan NcTb0.55562435848069920371.42Vulcan NcTb27993626363296328191.34Deconvolution of CO2 profiles showed that carboxylic groups were mainly created. It is expected that these groups decrease the hydrophobic character of the carbon materials, improving their interaction with the metal. On the other hand, deconvolution of CO profiles showed that phenols, quinones, and carbonyls were mainly created. It is expected that these groups, which are stable at higher temperatures, act as metal anchoring sites, hindering the agglomeration of metal particles [42].In order to further investigate how the pore structure and textural properties of the Vulcan XC-72R were changed during the oxidation treatments (see Section2.1 for oxidation treatments details), supports were characterized by means of N2-physisorption. Table 3 contains the textural properties of the carbon materials obtained by N2-physisorption. Vulcan XC-72R has a high specific surface area (210 m2 g −1) and a large total pore volume (0.38 cm3 g−1). Nevertheless, after the oxidation treatments, the specific surface area of all the samples decreased indicating a partial destruction of the original morphology, being this effect more significant at the carbon material oxidized with the most severe treatment (Vulcan NcTb2). However, no significant change was observed in the pore volume. In fact, carbon supports are mainly mesoporous materials but also contain an appreciable amount of micropores, which is maintained after the surface oxidation. Results suggest that all carbon materials present a broad pore size distribution (PSD) in the range of mesoporosity.Table 3
Textural properties of the supports and Fe electrocatalysts.
SampleSBET (m2/g)SMICRO (m2/g)SMESO (m2/g)VTOTAL (cm3/g)VMICRO (cm3/g)VMESO (cm3/g)Vulcan2101021080.380.060.32Vulcan NSTa0.5200104960.400.060.34Vulcan NcTb0.518191900.380.050.33Vulcan NcTb215977820.380.040.33Fe/Vulcan17576990.410.040.36Fe/Vulcan NSTa0.5166551110.490.030.46Fe/Vulcan NcTb0.514858900.410.030.37Fe/Vulcan NcTb213954850.420.030.38


## 3.2. Physicochemical Characterization of the Electrocatalysts

The catalysts metal loading was determined by SEM-EDX. All catalysts present similar iron content to the nominal value of 20% (Table4). However, a clear correlation between oxygen groups present in the surface and metal loading can be discerned. As the number of oxygenated groups increased, the amount of deposited Fe increased, since these oxygenated groups acted as anchoring sites. Additionally, homogeneous metal dispersion and deposition on all the carbon materials was observed by SEM images.Table 4
Metal load of the carbon-supported Fe electrocatalysts.
Electrocatalysts% metal (wt.)Fe/Vulcan16.7Fe/Vulcan NSTa0.518.4Fe/Vulcan NcTb0.518.9Fe/Vulcan NcTb221.8Fe/C catalysts were analyzed by XRD technique and their patterns are given in Figure2. In all the electrocatalysts, except in the sample Fe/Vulcan NSTa0.5, six characteristic peaks appeared at 2θ = 30.1, 35.5, 43.1, 57.0, 62.6, which can be assigned to (2 2 0), (3 1 1), (4 0 0), (5 1 1), and (4 4 0) planes of Fe3O4 (magnetite) (JCPDS 88-0866), respectively. No diffraction peaks corresponding to iron metal or iron oxides species (FeO or Fe2O3) were observed. However, the intensity of the Fe3O4 diffraction peaks was not so relevant than that expected for 20 wt.% of iron load. This result suggests that another crystal phase with particle size inferior to 2 nm coexisted with Fe3O4 crystals and/or part of the metal was deposited on carbon materials forming a stable but not crystalline structure. In this context, it is important to mention that particle size smaller than 2 nm cannot be achieved by XRD analysis. Other authors have obtained similar results depositing Fe on carbon supports [43]. Additionally, it is noticeable that the diffraction peak at ca. 2θ = 25°, which is associated to the graphite (002) diffraction line of the support, is still observed after the iron deposition.Figure 2
XRD patterns of 20% Fe/C catalysts.Textural properties of catalysts obtained by N2-physisorption are summarized in Table 3. Catalysts showed a lower surface area than the corresponding carbon supports, which is attributed to the metal particles loading on the pore surface. In particular, a reduction of the microporosity was observed after the catalysts loading, indicating that the metal was mainly distributed in the micropore structure of the support. PSD continued being broad in the mesoporosity range. However, the pore volume in the 20–50 nm pore diameter range is reduced, whereas in the 50–100 nm pore diameter range is increased. These results indicate that iron was deposited on the micropores or mesopores with average pore diameter lower than 50 nm, in agreement with the N2-physisorption results.


## 3.3. Electrochemical Performances of the Fe Electrocatalysts

The electrochemical properties of the Fe catalysts were studied in 0.5 M H2SO4, at room temperature and atmospheric pressure by DEMS. In this sense, DEMS studies provide more information than a simple electrochemical technique (i.e., cyclic voltammetry or chronoamperometry) such as the detection of volatile and gaseous products and intermediates generated in the electrochemical reactions with excellent sensibility. In this context, to the best of our knowledge, this is the first time that CO2 reduction on carbon-supported Fe catalysts is analyzed by DEMS technique.First, several potential cycles (not shown) between −0.2 and −1.8 V in 0.5 M H2SO4, previously deaerated with Ar, were recorded to clean and activate the catalyst surface. In this context, the voltammetric profile remains similar during the activation step for all catalysts, indicating a minimal (or inexistent) alteration of the electroactive surface. After that, in situ spectroelectrochemical experiments were carried out in acid solution with and without dissolved CO2.


### 3.3.1. Cyclic Voltammetry (CV) and Mass Spectrometric Cyclic Voltammetry (MSCV)

Figure3 shows the CVs and the corresponding MSCVs for all the carbon-supported Fe catalysts in free CO2 sulphuric acid solution. The CVs for all the catalysts (Figure 3(a)) present a similar feature, that is, a very high cathodic current at potentials lower than −0.5 V, which may be related to the hydrogen evolution reaction. However, a close inspection of the same figure shows up that the onset potential for the cathodic current starts at different potentials for the different electrodes. The latter becomes clear from the MSCVs for m/z = 2 (Figure 3(c)), which is related to the molecular hydrogen formation. Therefore, it is possible to state that the previous carbon treatment influences the water electro-reduction, and that the catalytic activity towards this reaction on the present Fe/C electrodes in a CO2 free acid solution increases in the following way: Fe/Vulcan NcTb2 ≈ Fe/Vulcan NcTb0.5 < Fe/Vulcan NSTa0.5 ≪ Fe/Vulcan. Also, it is important to mention that the electrochemical behavior of all the electrodes remains similar after the electrochemical study without CO2. The latter indicates that the electroactive surface is not damaged (or it is minimum) by these experiments.CVs and MSCVs for Fe/C catalysts in 0.5 M H2SO4 (sweep rate 10 mV s−1, Ei=-0.2 V versus Ag/AgCl/Sat.). Inset shows a zoom of the onset potential region during the cathodic scan.
(a)(b)(c)(d)Additionally to the H2 formation, the mass signals m/z = 16 (CH4+: methane), 30 (CH3CH3+ or H2CO+: ethane or formaldehyde), 29 (CH3CH2+ or CHO+: ethane/ethanol or an aldehyde), and 45 (HCOO+ or CH3CHOH+: formic acid or ethanol) were monitored during the cathodic scan. Figures 3(b) and 3(d) show the only two signals (m/z = 29 and 45) that increase during the excursion toward negative potentials. In this condition (no presence of dissolved CO2), the species associated to the mass signals 29 and 45 must be formed from the carbon support degradation. Interestingly, the mass signal 45 depends strongly on the carbon support treatment and its intensity rises in the order: Fe/Vulcan < Fe/Vulcan NcTb0.5 < Fe/Vulcan NcTb2 < Fe/Vulcan NSTa0.5. It is noticeable that the onset potential for the mass signal 45 formation at the catalyst previously treated with a mix of nitric and sulphuric acid is much lower than at the other catalysts (around 0.2 V), while the nontreated catalyst (Fe/Vulcan) presents a very small m/z = 45 signal at potentials more negative than −1.3 V. In the same way, both catalysts treated only with nitric acid develop the same onset potential for this m/z ratio, but its production on the Fe/Vulcan NcTb2 is somehow higher.On the other hand, the ion current intensity and onset potential for the mass signal 29 are quite similar for all Fe/C catalysts. However, a close inspection of this figure shows a small but visible trend in its production, which diminishes in the subsequent way: Fe/Vulcan > Fe/Vulcan NSTa0.5 > Fe/Vulcan NcTb2. Fe/Vulcan NcTb0.5 catalyst presents a different behavior toward the mass signal 29 production, in which the onset potential is equal to Fe/Vulcan NcTb2 electrode and the ion current intensity increases linearly as the applied potential becomes more negative.Summarizing, at the present conditions (CO2-free solution), nontreated catalyst (Fe/Vulcan) presents the highest and lowest catalytic activity towards hydrogen and mass signal 45 production, respectively. Treated catalysts develop similar behavior toward hydrogen evolution and the ionic current for the m/z = 45 depends strongly on the catalyst surface (see Table 2), that is, the mass signal 45 is enhanced on the catalysts that present oxygen groups on the surface. Additionally, mass signal 29 intensity modestly depends on the previous history of the carbon support.Figure4 displays the CVs and MSCVs (m/z = 2, 29, and 45) for all the Fe/C catalysts studied in the present work in acidic solution in the presence of dissolved carbon dioxide. Also, the m/z = 16, 30, and 32 were studied, but do not present an ionic current change during the cathodic scan. It is important to note that the intensity as well as the behavior of the mass signals 2, 29 and 45 are totally different to those observed in Figure 3 (in absence of dissolved CO2). Interestingly, in presence of dissolved CO2, the hydrogen evolution (Figure 3(c)) decreases on Fe/Vulcan, Fe/Vulcan NcTb0.5 and Fe/Vulcan NcTb2, while it increases on Fe/Vulcan NSTa0.5. Moreover, the latter catalyst presents an onset potential shift to more positive potentials for hydrogen formation reaction, that is, water reduction is favored on Fe/Vulcan NSTa0.5 in CO2 containing solution. Also, the the ratio m/z = 29 Figure 3(b) changes abruptly when CO2 is present in the working solution. The ion current intensity for this mass signal in a CO2-containing solution is higher than in a CO2-free one, and it drops off in the sequence: Fe/Vulcan NSTa0.5 > Fe/Vulcan > Fe/Vulcan NcTb2 ≈ Fe/Vulcan NcTa0.5, whereas the onset potential is quite similar for all the electrodes.CVs and MSCVs for CO2-saturated solution in 0.5 M H2SO4 on Fe/C catalysts (sweep rate 10 mV s−1, Ei=-0.2 V versus Ag/AgCl/Sat.).
(a)(b)(c)(d)On the other hand, Figure4(d) shows an important enhancement of the mass signal 45 at all the catalysts when CO2 is present in the solution. These experimental facts unequivocally indicate that carbon dioxide is reduced to form hydrocarbonated compounds such as formic acid. The formation of acids, alcohols, or other molecules, which contain longer hydrocarbon chains, is not discarded but this characterization is not the principal purpose of the present work: the main reasons of the present study are to know if it is possible to electrochemically reduce CO2 on iron catalysts and to establish if the carbon support influences on this particular reaction. Therefore, only the mass signals 2 and 45 are going to be followed along the present manuscript.


### 3.3.2. Current Transient (CT) and Mass Spectrometric Transient (MST)

Potentiostatic pulse experiments were performed from a potential where nonfaradaic reactions occur (Ei=-0.2 V) to a final potential (Ef=-1.8 V) where the CO2 reduction reaction is controlled by mass diffusion. Current transients for all the Fe/C catalysts used in the present work in absence (a) and presence (b) of dissolved CO2 in sulphuric acid solution can be seen in Figure 5. It is observed similar faradaic current intensities than those obtained during the potentiodymanic experiments (Figures 3(a) and 4(a)), that is, Fe/Vulcan NcTb2 presents at both mediums (in presence and absence of dissolved CO2) the lowest faradaic current, while the other catalysts develop similar faradaic currents. Consistent with the results presented above, molecular hydrogen production is significantly influenced by the presence of CO2 (Figure 6). Fe/Vulcan and Fe/Vulcan NSTa0.5 electrodes present the highest catalytic activity toward H2 formation in absence and presence of CO2, respectively. Also, it is noticeable that the signal for m/z = 2 decreases abruptly on Fe/Vulcan, Fe/Vulcan NcTb0.5, and Fe/Vulcan NcTb2 catalysts, while the same reaction is enhanced on the Fe/Vulcan NSTa0.5 when CO2 is present in solution.CTs for CO2-free (a) and CO2-saturated (b) solution in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).
(a)(b)MSTs for CO2-free (a) and CO2-saturated (b) solution in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).
(a)(b)Figure7(a) shows the MSTs for the mass signal 45. Currents obtained are of the same order of magnitude than in the voltammetric experiments. However, a close inspection of the curves reveals that the m/z = 45 signal continuously increases on Fe/Vulcan catalyst along the time, while the other catalysts present a constant ionic current. The latter suggests that the support time degradation is more important at this material. In this sense, it is important to remind that Fe/Vulcan electrode presents small quantity of oxygenated species on the surface (see Table 2), that is, this catalyst suffers a dreadful condition at this potential. On the other hand, when CO2 is present in solution (Figure 7(b)) the intensity of the mass signal 45 changes dramatically (about five fold times), as it was observed before the MSCV experiments (Section 3.3.1). In fact, the ionic current intensities for the mass signal 45 grow up on the studied catalysts in the following way: Fe/Vulcan NcTb2 < Fe/Vulcan < Fe/Vulcan NcTb0.5 < Fe/Vulcan NSTa0.5.MSTs for CO2-free (a) and CO2 saturated (b) solution in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).
(a)(b)In order to acquire a realistic result of hydrocarbon production from carbon dioxide reduction, the mass signal 45 was subtracted from the ionic current signals obtained with dissolved CO2 in solution (Figure 7(b)) and those acquired in a CO2-free solution (Figure 7(a)) and represented in Figure 8. In this context, it is really important to know that this subtraction can be only done if all the parameters concerning to the mass spectrometer are constant [44], and because of this, our mass spectrometer setup was build up to make all this parameters accurate [39]. Therefore, Figure 8 shows a realistic catalytic activity toward carbon dioxide reduction. In fact, it can be observed that the typical features of a reaction controlled by mass diffusion, and even more important that the carbon dioxide reduction, or what is the same in this event, the hydrocarbon production depends strongly on the catalyst support and it increases as follows: Fe/Vulcan NcTb2 < Fe/Vulcan < Fe/Vulcan NSTa0.5 ≈ Fe/Vulcan NcTb0.5.Figure 8
Corrected MSTs for CO2 electroreduction in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).


## 3.3.1. Cyclic Voltammetry (CV) and Mass Spectrometric Cyclic Voltammetry (MSCV)

Figure3 shows the CVs and the corresponding MSCVs for all the carbon-supported Fe catalysts in free CO2 sulphuric acid solution. The CVs for all the catalysts (Figure 3(a)) present a similar feature, that is, a very high cathodic current at potentials lower than −0.5 V, which may be related to the hydrogen evolution reaction. However, a close inspection of the same figure shows up that the onset potential for the cathodic current starts at different potentials for the different electrodes. The latter becomes clear from the MSCVs for m/z = 2 (Figure 3(c)), which is related to the molecular hydrogen formation. Therefore, it is possible to state that the previous carbon treatment influences the water electro-reduction, and that the catalytic activity towards this reaction on the present Fe/C electrodes in a CO2 free acid solution increases in the following way: Fe/Vulcan NcTb2 ≈ Fe/Vulcan NcTb0.5 < Fe/Vulcan NSTa0.5 ≪ Fe/Vulcan. Also, it is important to mention that the electrochemical behavior of all the electrodes remains similar after the electrochemical study without CO2. The latter indicates that the electroactive surface is not damaged (or it is minimum) by these experiments.CVs and MSCVs for Fe/C catalysts in 0.5 M H2SO4 (sweep rate 10 mV s−1, Ei=-0.2 V versus Ag/AgCl/Sat.). Inset shows a zoom of the onset potential region during the cathodic scan.
(a)(b)(c)(d)Additionally to the H2 formation, the mass signals m/z = 16 (CH4+: methane), 30 (CH3CH3+ or H2CO+: ethane or formaldehyde), 29 (CH3CH2+ or CHO+: ethane/ethanol or an aldehyde), and 45 (HCOO+ or CH3CHOH+: formic acid or ethanol) were monitored during the cathodic scan. Figures 3(b) and 3(d) show the only two signals (m/z = 29 and 45) that increase during the excursion toward negative potentials. In this condition (no presence of dissolved CO2), the species associated to the mass signals 29 and 45 must be formed from the carbon support degradation. Interestingly, the mass signal 45 depends strongly on the carbon support treatment and its intensity rises in the order: Fe/Vulcan < Fe/Vulcan NcTb0.5 < Fe/Vulcan NcTb2 < Fe/Vulcan NSTa0.5. It is noticeable that the onset potential for the mass signal 45 formation at the catalyst previously treated with a mix of nitric and sulphuric acid is much lower than at the other catalysts (around 0.2 V), while the nontreated catalyst (Fe/Vulcan) presents a very small m/z = 45 signal at potentials more negative than −1.3 V. In the same way, both catalysts treated only with nitric acid develop the same onset potential for this m/z ratio, but its production on the Fe/Vulcan NcTb2 is somehow higher.On the other hand, the ion current intensity and onset potential for the mass signal 29 are quite similar for all Fe/C catalysts. However, a close inspection of this figure shows a small but visible trend in its production, which diminishes in the subsequent way: Fe/Vulcan > Fe/Vulcan NSTa0.5 > Fe/Vulcan NcTb2. Fe/Vulcan NcTb0.5 catalyst presents a different behavior toward the mass signal 29 production, in which the onset potential is equal to Fe/Vulcan NcTb2 electrode and the ion current intensity increases linearly as the applied potential becomes more negative.Summarizing, at the present conditions (CO2-free solution), nontreated catalyst (Fe/Vulcan) presents the highest and lowest catalytic activity towards hydrogen and mass signal 45 production, respectively. Treated catalysts develop similar behavior toward hydrogen evolution and the ionic current for the m/z = 45 depends strongly on the catalyst surface (see Table 2), that is, the mass signal 45 is enhanced on the catalysts that present oxygen groups on the surface. Additionally, mass signal 29 intensity modestly depends on the previous history of the carbon support.Figure4 displays the CVs and MSCVs (m/z = 2, 29, and 45) for all the Fe/C catalysts studied in the present work in acidic solution in the presence of dissolved carbon dioxide. Also, the m/z = 16, 30, and 32 were studied, but do not present an ionic current change during the cathodic scan. It is important to note that the intensity as well as the behavior of the mass signals 2, 29 and 45 are totally different to those observed in Figure 3 (in absence of dissolved CO2). Interestingly, in presence of dissolved CO2, the hydrogen evolution (Figure 3(c)) decreases on Fe/Vulcan, Fe/Vulcan NcTb0.5 and Fe/Vulcan NcTb2, while it increases on Fe/Vulcan NSTa0.5. Moreover, the latter catalyst presents an onset potential shift to more positive potentials for hydrogen formation reaction, that is, water reduction is favored on Fe/Vulcan NSTa0.5 in CO2 containing solution. Also, the the ratio m/z = 29 Figure 3(b) changes abruptly when CO2 is present in the working solution. The ion current intensity for this mass signal in a CO2-containing solution is higher than in a CO2-free one, and it drops off in the sequence: Fe/Vulcan NSTa0.5 > Fe/Vulcan > Fe/Vulcan NcTb2 ≈ Fe/Vulcan NcTa0.5, whereas the onset potential is quite similar for all the electrodes.CVs and MSCVs for CO2-saturated solution in 0.5 M H2SO4 on Fe/C catalysts (sweep rate 10 mV s−1, Ei=-0.2 V versus Ag/AgCl/Sat.).
(a)(b)(c)(d)On the other hand, Figure4(d) shows an important enhancement of the mass signal 45 at all the catalysts when CO2 is present in the solution. These experimental facts unequivocally indicate that carbon dioxide is reduced to form hydrocarbonated compounds such as formic acid. The formation of acids, alcohols, or other molecules, which contain longer hydrocarbon chains, is not discarded but this characterization is not the principal purpose of the present work: the main reasons of the present study are to know if it is possible to electrochemically reduce CO2 on iron catalysts and to establish if the carbon support influences on this particular reaction. Therefore, only the mass signals 2 and 45 are going to be followed along the present manuscript.


## 3.3.2. Current Transient (CT) and Mass Spectrometric Transient (MST)

Potentiostatic pulse experiments were performed from a potential where nonfaradaic reactions occur (Ei=-0.2 V) to a final potential (Ef=-1.8 V) where the CO2 reduction reaction is controlled by mass diffusion. Current transients for all the Fe/C catalysts used in the present work in absence (a) and presence (b) of dissolved CO2 in sulphuric acid solution can be seen in Figure 5. It is observed similar faradaic current intensities than those obtained during the potentiodymanic experiments (Figures 3(a) and 4(a)), that is, Fe/Vulcan NcTb2 presents at both mediums (in presence and absence of dissolved CO2) the lowest faradaic current, while the other catalysts develop similar faradaic currents. Consistent with the results presented above, molecular hydrogen production is significantly influenced by the presence of CO2 (Figure 6). Fe/Vulcan and Fe/Vulcan NSTa0.5 electrodes present the highest catalytic activity toward H2 formation in absence and presence of CO2, respectively. Also, it is noticeable that the signal for m/z = 2 decreases abruptly on Fe/Vulcan, Fe/Vulcan NcTb0.5, and Fe/Vulcan NcTb2 catalysts, while the same reaction is enhanced on the Fe/Vulcan NSTa0.5 when CO2 is present in solution.CTs for CO2-free (a) and CO2-saturated (b) solution in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).
(a)(b)MSTs for CO2-free (a) and CO2-saturated (b) solution in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).
(a)(b)Figure7(a) shows the MSTs for the mass signal 45. Currents obtained are of the same order of magnitude than in the voltammetric experiments. However, a close inspection of the curves reveals that the m/z = 45 signal continuously increases on Fe/Vulcan catalyst along the time, while the other catalysts present a constant ionic current. The latter suggests that the support time degradation is more important at this material. In this sense, it is important to remind that Fe/Vulcan electrode presents small quantity of oxygenated species on the surface (see Table 2), that is, this catalyst suffers a dreadful condition at this potential. On the other hand, when CO2 is present in solution (Figure 7(b)) the intensity of the mass signal 45 changes dramatically (about five fold times), as it was observed before the MSCV experiments (Section 3.3.1). In fact, the ionic current intensities for the mass signal 45 grow up on the studied catalysts in the following way: Fe/Vulcan NcTb2 < Fe/Vulcan < Fe/Vulcan NcTb0.5 < Fe/Vulcan NSTa0.5.MSTs for CO2-free (a) and CO2 saturated (b) solution in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).
(a)(b)In order to acquire a realistic result of hydrocarbon production from carbon dioxide reduction, the mass signal 45 was subtracted from the ionic current signals obtained with dissolved CO2 in solution (Figure 7(b)) and those acquired in a CO2-free solution (Figure 7(a)) and represented in Figure 8. In this context, it is really important to know that this subtraction can be only done if all the parameters concerning to the mass spectrometer are constant [44], and because of this, our mass spectrometer setup was build up to make all this parameters accurate [39]. Therefore, Figure 8 shows a realistic catalytic activity toward carbon dioxide reduction. In fact, it can be observed that the typical features of a reaction controlled by mass diffusion, and even more important that the carbon dioxide reduction, or what is the same in this event, the hydrocarbon production depends strongly on the catalyst support and it increases as follows: Fe/Vulcan NcTb2 < Fe/Vulcan < Fe/Vulcan NSTa0.5 ≈ Fe/Vulcan NcTb0.5.Figure 8
Corrected MSTs for CO2 electroreduction in 0.5 M H2SO4 on Fe/C catalysts (Ei=-0.2 V, Ef=-1.8 versus Ag/AgCl/Sat.).


## 4. Discussion

Although the electrochemical reduction of carbon dioxide has been hugely studied, the reaction mechanism is not exactly known. Most of the reactions on different metal catalysts at diverse conditions, involving homogeneous and heterogeneous catalysis, were proposed by Sullivan [8] and assume a high availability of protons. In general, four principal pathways can be considered during the carbon dioxide reduction in acidic media [44]: (i) CO(g) formation via disproportionation; (ii) CO2•- radical formation; (iii) •COOH(ad) formation; (iv) the formation of adsorbed reduced-CO2 species giving a range of reduced-CO2 and products (CO, hydrocarbons and alcohols). The main proposed reactions in the CO2 reduction mechanism are given as follows:(1)CO2+e-⟶CO2(ad)•-,(2)CO2(ad)•-+H+⟶•COOH(ad),(3)CO2(ad)•-+e-+2H+⟶CO(ad)+H2O.
From CO(ad) species, a series of products CH2CO, CH3CHO, C2H5OH, C2H4, C2H6, C3H7OH, and CH3OH can be formed [44]. On the other hand, •COOH(ad) species can suffer a nucleophilic attack to form CO(ad) or alternatively may be released as formic acid:
(4)•COOH(ad)+e-⟶COOH(ad)-⟶COOH-,
or via hydrated form:
(5)•COOH(ad)+e-+H2O⟶HCOOH.
Considering the same equations, a mechanism that represents our present study can be proposed. The following mechanism is quite similar to that described by Dubé and Brisard [45] for CO2 electroreduction on polycrystalline Cu electrodes in acidic media. First, adsorbed hydrogen is formed during the cathodic sweep by the reaction
(6)H++e-⟶H(ad),
or by water dissociation:
(7)H2O+e-⟶H(ad)+OH-,
followed by hydrogen evolution:
(8)2H(ad)⟶H2.
Then, carbon dioxide bubbled trough the solution may adsorb and react on the iron-based catalysts in acidic solution in the subsequent way:
(9)CO2⟷CO2(ad),(10)CO2(ad)+2H(ad)⟶CO(ad)+H2O,(11)CO2(ad)+H(ad)⟶COOH(ad),(12)COOH(ad)+H(ad)⟶HCOOH,(13)COOH(ad)+H(ad)⟶CO(ad)+H2O.The present mechanism is limited by the hydrogen (6) and carbon dioxide (9) adsorption reactions, which are necessary steps to form hydrogenated molecules. In fact, the availability of protons and the adsorbed hydrogen coverage on the surface have a strong influence on these reactions. Moreover, the metal surface must interact preferentially with a CO2 species than with adsorbed hydrogen, otherwise, hydrogen evolution reaction will be predominant at the electrode and carbon dioxide reduction reaction will be hindered.Accordingly, two main pathways are possible.(i)
CO(ad) formation (reaction (10)): the production of this species is favored when the metal surface is highly covered by adsorbed hydrogen and prefer to react with adsorbed carbon dioxide instead of reacting with each other. Therefore, the hydrogen evolution reaction will be apparently inhibited in this event. It seems that this path is governing on Fe/Vulcan NcTb2, Fe/Vulcan, Fe/Vulcan NcTb0.5 catalysts. In fact, it is clearly observed in the MSCVs and MSTs for m/z = 2 of all catalysts (with the exception of Fe/Vulcan NSTa0.5) in absence and presence of dissolved CO2 (Figures 3, 4, and 6), in which the mass current signal associated to H2 production decreases in presence of dissolved carbon dioxide. So, these iron catalysts have a preference to adsorb CO2 instead of producing molecular hydrogen, and consequently, adsorbed hydrogen reacts with adsorbed carbon dioxide to produce hydrogenated species mainly through reaction (10). As it was described before, from adsorbed carbon monoxide it is possible to form products such as HCOH, CH2CO, CH3CHO, C2H5OH, C2H4, C2H6, C3H7OH and CH3OH [45, 46].(ii)
COOH(ad) production (reaction (11)): this pathway gives mainly formic acid as a final product (reaction (12)). Reaction (11) is favoured on surfaces with preference to produce molecular hydrogen, and therefore, with a low H2 coverage. In other words, adsorbed hydrogen species prefer to react with each other to form molecular hydrogen instead to react with adsorbed carbon dioxide. Therefore, hydrogen evolution reaction is usually favoured in parallel to this reaction. Nevertheless, adsorbed carbon monoxide formation (reaction (13)) cannot be discarded. Thus, if CO(ad) is produced, the operative mechanism will be the same than that described above (reaction path i). In this context, Fe/Vulcan NSTa0.5 catalyst is the only one that does not follow the behavior observed for the other catalysts. In fact, this catalyst enhances the hydrogen evolution (m/z = 2) and mass signal 45 in presence of CO2. The latter suggests that Fe/Vulcan NSTa0.5 catalyst follows principally the reaction path (ii).Furthermore, the native oxygenated species on the carbon support may follow the same reactions during the cathodic scan (at least in absence of dissolved CO2, see Figures 3 and 7(a)).In this context, the mass signal 29 can be attributed to the first reaction path (i), whilem/z = 45 can be associated with formic acid production (ii). Nevertheless, the last mass signal also could be linked to the reaction path (i), that is, it could be related to a fragmentation of a long hydrogenated species such as ethanol, which presents 27, 29, 31, and 45 ion current signals. In this sense, in a forthcoming work, will be discussed in detail the species produced during the carbon dioxide reduction on iron catalysts.Additionally, it is observed that all the present surface reactions are strongly affected by the carbon support. This statement is observed in the MSCVs form/z = 2, 29, and 45 in Figures 3 and 4, and strongly confirmed by the MSTs for molecular hydrogen and formic acid production depicted in Figures 6 and 7, respectively. It seems that surface oxygen groups enhance the catalytic activity toward CO2 reduction. However, Fe/Vulcan NcTb2 presents the lowest ion current intensities, suggesting that longer treatment times of carbon support in nitric acid destroy (at least partially) the support structure, and consequently, the catalytic activity towards CO2 diminishes.On the other hand, the surface chemistry of the carbon support could explain the different catalytic activity toward CO2 reduction recorded on Fe/Vulcan NSTa0.5. Vulcan NSTa0.5 is the only support that suffered the oxidation treatment at ambient temperature in the presence of nitric and sulphuric acid. A temperature effect must be discarded since the material catalyst supported on untreated Vulcan follows the same behavior than the other catalysts. Therefore, the presence of sulphuric acid in the treatment that provides high quantity of oxygenated species on the surface seems to be the main responsible for the different behavior observed during the carbon dioxide reduction on Fe/Vulcan NSTa0.5 electrode.


## 5. Conclusions

Fe catalysts supported on Vulcan XC-72R were synthesized by the polyol method, using ethylenglycol as solvent and reducing agent. Before the metal deposition, surface chemistry of the Vulcan was modified by different oxidation treatments in order to study the influence of the surface chemistry of the support on the catalytic properties of the materials. During these treatments surface oxygen groups were created, being HNO3 treatment at boiling temperature for 2 h the most effective in creating functional groups, while HNO3-H2SO4 treatment at room temperature produces the highest CO/CO2 ratio of functional groups in the surface. These treatments strongly affect the behavior of the iron-based catalysts toward the carbon dioxide reduction. In fact, two main reaction paths were identified during the carbon dioxide reduction, both influenced by the surface properties of the carbon support. Additionally, these treatments also modified the textural and morphological properties of Vulcan. A decrease of the surface area, as well as a partial destruction of its structure, was observed as the severity of oxidation treatments increased. Finally, Fe/Vulcan NSTa0.5 and Fe/Vulcan NcTb0.5 present the highest and lowest catalytic activity toward the hydrogen evolution reaction, though both catalysts develop the highest production of the mass signal 45 (formic acid and/or higher carbon-chain products) in presence of dissolved CO2.



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*Source: 249804-2011-12-08.xml*