CO-selective catalysts for the CO2RR.
The CO2 that comes from the use of fossil fuels accounts for about 65% of the global greenhouse gas emission, and it plays a critical role in global climate changes. Among the different strategies that have been considered to address the storage and reutilization of CO2, the transformation of CO2 into chemicals and fuels with a high added-value has been considered a winning approach. This transformation is able to reduce the carbon emission and induce a “fuel switching” that exploits renewable energy sources. The aim of this chapter is to categorize different heterogeneous electrocatalysts which are being used for CO2 reduction, based on the desired products of the above mentioned reactions: from formic acid and carbon monoxide to methanol and ethanol and other possible by products. Moreover, a brief description of the kinetic and mechanism of the CO2 reduction reaction) and pathways toward different products have been discussed.
- CO2 electroreduction
- faradaic efficiency
Nowadays, global warming and CO2 emissions as well as atmospheric CO2 concentration are central topics in politics and scientific debate. The global energy supply based on fossil fuels has reached an unprecedented scale leading to excess anthropogenic CO2 emission. CO2 accumulates in the atmosphere and its concentration has surpassed 409 ppm in 2019 much higher than the 270 ppm during the pre-industrial era . As a well-known greenhouse gas, accumulated CO2 traps more infrared radiation, breaking the energy balance on the earth’s surface. Using CO2 as feedstock to produce valuable carbon-based chemicals is considered to be a feasible approach to close the carbon cycle and mitigate the climate change. Many strategies have been developed for CO2 valorisation, including thermochemical, photochemical, electrochemical and biological approaches [2, 3, 4, 5]. Among these methods, electrochemical conversion presents several advantages. Firstly, this method can use green chemicals as electrolytes and electricity from renewable energy sources, thus not contributing to new CO2 emissions while transforming it . Secondly, the products and conversion rates can be tuned by utilizing different catalysts and applying various potentials [7, 8]. Finally, the electrolyzer and electrolysis process for CO2 conversion can be developed based on the already existing technologies such as water electrolyzers, polymer electrolyte membrane fuel cells, solid oxide fuel cells and so on . However, the CO2 reduction reaction (CO2RR) involves several proton-assisted multiple-electron-transfer processes with similar standard potentials (V
From the kinetic point of view, it is even more challenging to form chemical bonds for the complex and energetic molecule products . Transferring one electron to the adsorbed CO2 molecule to activate it (generating the radical CO2*−) is believed to be the rate-determining step of the CO2RR on transition metal-based catalysts because of the high activation barrier needed for this step . Consequently, much more negative potentials than the standard ones are needed to drive the CO2RR. Therefore, an appropriately designed catalyst is essential in order to activate the CO2 molecules. Once CO2*− forms on the catalyst’s surface, its reactivity in this state controls the distribution of final products. Both early and later studies [13, 14, 15] of electrochemical CO2RR on various metal-based electrodes found that the radical CO2*− interacts with the surface of the catalyst in different ways, depending on the intrinsic electronic surface’s properties of the material. Hence, a suitable catalyst is necessary in order to selectively drive the CO2RR and to obtain a specific product. In the present chapter, numerous electrocatalysts are classified based on the CO2RR product, involving the reaction pathways and mechanism study.
2. CO-selective catalysts
CO is an important product from the reduction of CO2 since it has high relevance for the chemical industry . It is considered the most important C1-building block and is intensively used in large industrial processes such as Fischer-Tropsch synthesis of hydrocarbons and Monsanto/Cativa acetic acid synthesis. By a techno-economic analysis that takes into consideration the costs of CO2, electricity, separation, capital and maintenance, operation and the known product selectivity and outputs the levelized cost of the chemical produced, CO is one of the most economically viable and atom-economic targets .
In recent years, great efforts have been dedicated to the study of electrocatalysts for the electrochemical CO2RR to CO. Table 1 summarizes the most widely investigated types.
|Electrocatalyst||Electrolyte||Potential (V vs. RHE)||Faradaic efficiency (%)||Current density (−mA cm−2)||Reference|
|Au Nanoparticles||0.5 M KHCO3||−0.67||90||5|||
|Au needles||0.5 M KHCO3||−0.35||95||15|||
|Ag nanowires||0.5 M KHCO3||−0.6||90||4.9|||
|Nanoporous Ag||0.5 M KHCO3||−0.6||92||18|||
|Ag-TiO2||0.1 M KHCO3||−1.3||35||30|||
|Zn nanoparticles||0.1 M KHCO3||−0.95||98.1||17.5|||
|ZnO particles||0.1 M KHCO3||−0.89||68||3.0|||
|Cu-Sn foam||0.1 M KHCO3||−0.8||93||6.7|||
|Cu-Sn||0.1 M KHCO3||−0.6||90||1.0|||
|Cu-SnO2||0.5 M KHCO3||−0.7||93||4.6|||
|Zn94Cu6 foam||0.5 M KHCO3||−0.95||90||8.0|||
|CuO-Sb2O3||0.1 M KHCO3||−0.8||90||5.0|||
|SnOx/Ag||0.5 M KHCO3||−0.6||85||0.7|||
|AuCu||0.1 M KHCO3||−0.8||50||—|||
|Mn-N-C||0.1 M KHCO3||−0.6||~80||< 5|||
|Ni-N-C||0.1 M KHCO3||−1.0||95||15|||
|Ni-N-C||0.1 M KHCO3||−0.81||80||13|||
|FeN4/C||0.1 M KHCO3||−0.6||93||1.5|||
|FeN5/Graphene||0.1 M KHCO3||−0.46||97||1.8|||
|Fe3+–N–C||0.5 M KHCO3||−0.47||95||21|||
|Zn-N-Graphene||0.5 M KHCO3||−0.5||91||10|||
|ZnN4/C||0.5 M KHCO3||−0.43||95||4.8|||
|Sb-NC||0.1 M KHCO3||−0.9||82||2.9|||
|Ni/Fe-N-C||0.5 M KHCO3||−0.7||98||7.4|||
|COF-366-Co||0.5 M KHCO3||−0.67||87||—|||
|COF-366-Co, COF-367-Co||0.5 M KHCO3||−0.66||91||3.3|||
|Fe porphyrin-graphene hydrogel||0.1 M KHCO3||−0.39||96||0.42|||
|Fe(III) porphyrin/graphene||0.1 M KHCO3||−0.54||98.7||1.68|||
2.1 Metals and bimetallic materials
From both experimental and theoretical studies, Au, Ag and Zn are the most selective metals for CO formation. The CO2RR on Au and Ag is characterized by low overpotentials, excellent selectivity and high activity [18, 19, 20, 30, 44]. On contrast, Zn shows relatively higher overpotentials, lower activity and moderate-to-high selectivity [8, 21].
Many bimetallic materials are demonstrated to selectively catalyze the CO2RR to CO, including Cu-Sn [22, 23, 24], Cu-Zn , Cu-Sb , Cu-Ag , Cu-Au  and so on. Among all these materials, Cu-Sn catalysts have attracted the most intensive attention due to the high selectivity, good activity and outstanding repeatability. In addition, compared with others, Cu and Sn are relatively more abundant and more cost-effective, making Cu-Sn catalysts more suitable for the large-scale implementation. Hence, further study on the Cu-Sn catalysts is expected to bring benefits to both the academic and industrial sectors related to the CO2 valorization.
2.2 Single metal atom supported on N-doped carbon
Single-metal-atom catalysts supported on porous N-doped carbon represent a class of catalysts with high atom efficiency. After introduced in 2015 by Varela et al. , it has gained much attention for CO2 reduction. Ni supported on N-C, in contrast to Ni nanoparticles that are known to be effective in the HER, is reported to be an efficient electrocatalyst for the CO2RR to CO [29, 31, 32]. Various types of Fe-N active sites have been identified and demonstrated to selectively promote the CO formation at very low overpotentials [29, 33, 34, 35]. Compared to the metallic Zn and ZnO, single atom Zn sites show much lower overpotentials where excellent CO selectivity has obtained [36, 37]. Sb atomic sites, compared to bulk Sb, Sb2O3, and Sb nanoparticles that exhibit poor activity and selectivity for the CO2RR, enable the CO formation with good selectivity at relatively high overpotentials . Isolated diatomic Ni-Fe sites anchored on nitrogenated carbon are also studied as an electrocatalyst for CO2 reduction . The catalyst exhibits high selectivity with CO Faradaic efficiency above 90% over a wide potential range from −0.5 to −0.9 V (98% at −0.7 V, vs. RHE), and robust durability.
Single atoms of selected transition metals anchored in N-doped carbon have emerged as unique and promising electrocatalysts because of the maximal atom utilization and high efficiency. Most of them perform differently from their bulk metal or oxide species, due to the metal–matrix interfacial interaction that leads to the manipulation of the electronic structures of the materials and to the emergence of additional active sites. Despite the big progress made in the recent years, many challenges remain in the development of the single atom catalysts. For example, the loading of metals is usually low, leading to relatively low geometric current density and thus limitations for practical applications. In addition, big efforts have to focus on
2.3 Immobilized molecular catalysts
Homogeneous electrocatalysis constitutes an efficient way of converting CO2 to various products but some distinct challenges persist . For example, the catalyst stability and recyclability are usually poor; only a small portion of the catalyst molecules at the reaction interface is active, while most of them are passive; some catalysts have poor solubility; product separation could be difficult. To overcome these disadvantages, great efforts have been dedicated to the immobilization of molecular catalysts on electrode surfaces for the heterogeneous CO2RR. Being fixed on carbon supports, the porphyrin- and phthalocyanine-based catalysts with Fe and Co centers are very selective for CO formation at relatively low overpotentials [41, 42, 43, 45]. The catalytic performance can be affected by both the intrinsic properties of the catalysts such as the structure and the metal center, and the extrinsic factors such as the catalyst immobilization methods, the support material and the catalyst loading. A deeper understanding of those intrinsic and extrinsic factors can enable the optimization of supported molecular catalysts in order to achieve the CO2RR performance as high as that of the nanostructured metals, metal alloys and single atom catalysts supported on N-carbon materials .
The mechanism study of CO2RR on metal-based materials is widely studied, in combination of in-situ spectroscopic analyses and DFT calculations [45, 46]. As shown in Figure 1, it is suggested that the CO2RR to CO process on metallic Zn or Ag surface includes four elementary reaction steps: (1) one electron transfers to CO2 to form CO2*−; (2) one proton transfers to CO2*− to obtain COOH* intermediate; (3) an electron and a proton transfer to COOH* to form CO*; (4) CO* desorbs to produce CO. Another possible pathway is supposed to include three main steps: (1) an electron coupled with a proton transfers to CO2 to form COOH* intermediate; (2) another electron coupled with a proton transfers to COOH* to form CO*; (3) CO* desorbs to produce CO.
3. Formate-selective catalysts
Due to the large storage and safety requirements for CO during carbon sequestration and storage (CCS), the production of liquid formic acid is becoming a more attractive solution. Formic acid could be directly used as a feedstock for fuel cells and as a precursor for manufacturing value-added chemicals such as formate esters, methanol, and other carboxylic acids and derivatives . Some heavy metals, including Pb, Hg, In, Cd, and Tl, are efficient electrocatalysts for converting CO2 into formate/formic acid. However, the defects of the high toxicity and/or high cost are standing in the way for their large-scale applications . Other earth abundant metals like Sn, Cu and Bi gained a lot of attentions in recent years. Table 2 has summarized some of the important results for formic acid production through electrocatalysis of CO2.
|Electrocatalyst||Electrolyte||Potential (V vs. RHE)||Current Density (−mA cm−2)||FE (%)||Reference|
|B-doped Pd||0.1 M KHCO3||−0.5 V||10||70|||
|S-modified Cu||0.1 M KHCO3||−0.8||20||80|||
|Pd needles||0.5 M KHCO3||−0.2||10||91|||
|Sn(S)/Au||0.1 M KHCO3||−0.75||55||94|||
|nano-SnO2/C||0.1 M NaHCO3||−1.16||6.2||86.2|||
|BiOx/C||0.5 M NaCl||−1.13||12.5||96|||
|Cu–Au||0.5 M KHCO3||−0.6||10.2||81|||
|Bi nanotubes||0.5 M KHCO3||−1||39.4||97|||
|Sulfur-doped indium||0.5 M KHCO3||−0.98||58.9||95|||
|SnO2||0.1 M KHCO3||−1.06||11||82|||
3.1 Metal and metal oxides
From the pioneer work of
3.2 Metal sulfides
In very recent years, sulfur-modified metals have been explored as electrocatalysts, showing promising catalytic performance for the CO2RR. CuxS is one of the most intensively studied sulfides, which can selectively produce HCOOH . SnSx , PbSx , BiSx  and InSx  are also demonstrated to be effective catalysts for the CO2RR to HCOOH. Even though the promising performance, the role of S in the electrochemical performance is not clear until now. In order to design catalysts with higher activity, selectivity and stability, it is necessary to acquire a deeper understanding of how S functions during CO2RR by performing both in-situ/operando experiments and theoretical studies.
3.3 Bimetallic catalysts
Compared with the pure metals, bimetallic catalysts with tuned electronic and structural properties are of particular interest. Early studies by
In recent years, many works have been dedicated to understand the mechanism of the CO2RR to HCOOH, including computational, electrokinetic and in situ analysis) [60, 61, 62]. As depicted in Figure 2, the formation of formate generally goes through the following pathway: 1) CO2·− radical anion is firstly formed via a one-electron transfer and bonded to the electrode surface through O atom, 2) protonation of CO2·− on the carbon atom leads to the formation of a HCOO· intermediate and 3) a second electron transfer and protonation step results in the HCOOH product .
4. C1+ hydrocarbon selective electrocatalyst
The production of hydrocarbons through electrochemical reduction of CO2 (a carbon-neutral fuel alternative to fossil fuels) is of interest because the infrastructure to store, transport and use methane and other hydrocarbons as fuel is already well established . The major challenge for these products is to find the selective electrocatalysts to manage to reduce the CO2 molecule with 8 and 12 electrons (methane and ethane). Considering the stability of the CO2 molecule and the multi-electron-coupled-proton pathways, high energy barriers are needed to overcome for the formation of the intermediates and final product .
According to major reports, Cu-based materials are the main type of electrocatalysts that can produce hydrocarbon compounds including CH4 and thus become the object under the most intensive study .
4.1 Cu alloys
Hirunsit et al. examined Cu3X alloys by using computational methods to examine the electrochemical reduction to CH4. In an important report, Kenis and co-workers recently reported the differences between ordered, disordered, and phase-separated Cu@Pd nanoparticles with respect to product selectivity . Gewirth and co-workers showed that Cu-Ag alloys from additive-controlled electrodeposition exhibited ~60% FE for C2H4 in an alkaline flow electrolyzer. In this case, by tuning the Ag-loading an optimized C2H4 selectivity can be achieved. The Ag sites were believed to play the role of a promoter for CO formation during electrochemical CO2 reduction .
4.2 Other metallic alloys
Although copper gained a lot of attention for hydrocarbon production through electrochemical reduction of CO2, some other metallic alloys have also shown to be quite noteworthy for this application. For example, Lewis and co-workers reported nickel–gallium alloys of different compositions prepared by drop-casting and a subsequent temperature-programmed reduction method . The alloy foil was slightly enriched in zinc both at the surface and in the bulk, with a surface alloy composition of 61.3 at% zinc and a predominantly Ag5Zn8 bulk phase. The FECH4 values at 1.43 V vs. RHE were five times and three times higher with the alloys than those produced at pure Ag and Zn electrodes, respectively.
The summary of some recent reports for C1+ hydrocarbons are being reported in Table 3.
|Electrocatalyst||Electrolyte||Main Product||Potential (V vs. RHE)||Current Density (−mA cm−2)||FE (%)||Reference|
|Cu nanowires/rGO||0.5 M KHCO3||Methane||−1.25||12||55|||
|Cu-Porphyrin||0.5 M KHCO3||Methane||−0.98||15||47|||
|Pd decorated Cu||0.5 M KHCO3||Methane||−0.96||57||46|||
|CuS@Ni Foam||0.1 M KHCO3||Methane||−1.1||7.3||73|||
|Complex-derived Cu nanocluster||0.5 M KHCO3||Methane||−1.06||19.7||66|||
|n-Cu/C||0.1 M NaHCO3||Methane||−1.35||10||76|||
|Mesoporous Cu||0.1 M KHCO3||Ethylene||−1.3||11.8||46|||
|O2-plasma-treated Cu||0.1 M KHCO3||Ethylene||−0.9||12||60|||
|Anodized-Cu||0.1 M KHCO3||Ethylene||−1.08||19||38|||
As for the possible pathways for electrochemical reduction of CO2 to hydrocarbons, In an attempt to elucidate the mechanism of CO2 reduction, it was found that CO is a key intermediate in the formation of CH4 and C2H4  and that the products of CO2 reduction reaction depend on the metal’s binding energy to CO . Based on these findings, one strategy for efficient electrochemical CO2 conversion is to separate the process into two steps: CO2 reduction to CO, followed by CO reduction to oxygenates and hydrocarbons . The schematic of the possible pathways toward methane production has been illustrated in Figure 3.
5. Oxygenated alcohol selective electrocatalysts
The wide range of theoretically possible products from CO to C2+ alcohols and hydrocarbons and fuels makes the recent research to put a lot of efforts on production of more valuable products like oxygenated alcohols. The major problem as discussed before is due to a very stable structure of CO2 molecule, very high activation energy needed to transform it to more attractive molecules. This high activation barrier would cause high over potentials and in case of oxygenated alcohols like methanol or ethanol high numbers of electrons (6 and 12 respectively) needed to reduce CO2 molecule to desired products. So far many different metallic and alloys have been used as electrocatalysts for this application . Although the performance of other product formations such as CH3OH and C2H5OH were well below the target values, the market size of these chemicals was estimated to be much larger than those of HCOOH and CO . Thus, the co-production of economically viable HCOOH and CO with other products such as CH4,C2H4,CH3OH, and C2H5OH was suggested to cancel out the maximum voltage requirement .
5.1 Metal alloys
Of all metals, Cu has been identified as unique in that it is able to produce a number of “beyond CO” products such as hydrocarbons and organic oxygenates such as aldehydes and alcohols . Moreover, metal alloys can adjust the binding ability of active intermediates and thus are promising to enhance the reaction selectivity and kinetics. Lu et al.  have synthesized an aerogel with high porosity when [BMIM][BF4] and H2O with a molar ratio of 1:3 were selected as electrolytes, the faradaic efficiency (FE) and current density of CH3OH can be up to 80% and 31.8 mA/cm2, respectively, over the Pd83Cu17 aerogel which attributed to the valence states, ratios, and strong interaction of Pd and Cu . Also, a Zn/Ag foam electrocatalyst was prepared by Low et al. The active sites in this electrocatalyst are the strained submicron Zn dendrites, resulting in a FE of 10.5% for producing CH3OH .
5.2 Metal oxides
Metal oxide electrocatalysts have the merits of high selectivity and high energy efficiency . Cuprous oxide/polypyrrole particles with octahedral and icosahedra structure (Cu2O(OL-MH)/Ppy) can achieve a ultrahigh CH3OH activity and selectivity with FE of 93 ± 1.2% and 1.61 ± 0.02 μmol/(cm2·s) formation rate at −0.85 V . Albo and Irabien  used gas diffusion electrode loaded with Cu2O and achieved a FE of 42.3% for CH3OH formation, founding that Cu + can significantly affect the selectivity and activity toward CH3OH. Moreover, nano Cu2O has a higher stability and selectivity compared with Cu for CH3OH production. The result of more metallic alloys and metal oxide electrocatalysts for this application have been illustrated in Table 4.
|Electrocatalyst||Electrolyte||Main Product||Potential (V vs. RHE)||Current Density (−mA cm−2)||FE (%)||Reference|
|Cu2O/ZnO||0.5 M KHCO3||Methanol||−0.7||6.8||17.7|||
|Cu modified Pd||0.5 M KHCO3||Methanol||−0.46||0.5||19.5|||
|Cu nanoparticle/N-doped graphene||0.1 M KHCO3||Ethanol||−1.2||0.7||63|||
|B-and-N-co-doped Nanodiamond||0.1 M KHCO3||Ethanol||−1||1||93|||
|Cu2O films||0.1 M KHCO3||Ethylene and Ethanol||−0.99||35||34.3 and 16.4|||
It is noteworthy to mention that there are different pathways suggested for methanol and ethanol production via electrochemical reduction of CO2. One possible pathway for methanol production is believed to be produced through hydrogenation of methoxy intermediate (*OCH3) . In detail, the *CO species is formed first. Then, the *OCH3 intermediate is made from the competition between desorption of formaldehyde and the proton electron coupled transfer to formaldehyde bonded on local surface. At least, another proton electron coupled transfer occurring on *OCH3 species results in methanol . This possible pathway has been illustrated in Figure 4. In addition, the plausible pathway for ethanol production should be discussed alongside ethylene. Ethylene is generally believed to form through either dimerization of *CH2 species or proton electron coupled transfer to the carbon site of the ethylene oxide intermediate (*OCHCH2) that is derived from dimerization of *CO . Both routes might be the halfway leading to formation of ethanol by insertion of *CO species into *CH2 species or proton electron coupled transfer to the oxygen site of the *OCHCH2 species, correspondingly , as illustrated in Figure 5.
In this chapter different electrocatalysts for electrochemical reduction of CO2 to value added products have been discussed. A wide range of molecules from CO and HCOOH to hydrocarbons and oxygenated alcohols are possible products of this electrochemical reaction. Up to this date the main challenge of these electrocatalytic reactions remains on scaling up and eventually industrializing the production of these value added products. The main drawback of these electrocatalytic reactions are their relatively high overpotentials and low production rate for scaling up. Although the prospective of this technology are bright, the main effort still is to find the stable, abundant electrocatalyst to be used for efficient electrocatalytic reduction of CO2 at industrial scale.