Journal Archive

Johnson Matthey Technol. Rev., 2023, 67, (3), 249
doi: 10.1595/205651323X16648726195503

Advanced Supports for Noble Metal Catalysts in Proton Exchange Membrane Water Electrolysers: A Review

Improving the performance, stability, durability and cost of iridium- and platinum-based catalytic materials

  • Pere L. Cabot*
  • Laboratory of Electrochemistry of Materials and the Environment, Department of Materials Science and Physical Chemistry, Faculty of Chemistry, University of Barcelona, Martí and Franquès 1, 08028 Barcelona, Spain
  • María V. Martínez-Huerta
  • Institute of Catalysis and Petrochemistry, Spanish Council for Scientific Research (CSIC), C/ Marie Curie, 2. Cantoblanco, 28049 Madrid, Spain
  • Francisco Alcaide
  • Laboratory of Electrochemistry of Materials and the Environment, Department of Materials Science and Physical Chemistry, Faculty of Chemistry, University of Barcelona, Martí and Franquès 1, 08028 Barcelona, Spain; CIDETEC, Basque Research and Technology Alliance (BRTA), Paseo Miramón, 196, 20014 San Sebastián, Spain
  • *Email:
    Received 29th July 2020; Revised 21st September 2022; Accepted 3rd October 2022; Online 4th October 2022

Article Synopsis

Renewable and low-carbon hydrogen will contribute to a future climate-neutral economy as a fuel, clean energy carrier and feedstock. One of the main concerns when considering its production by the present proton exchange membrane water electrolysers (PEMWE) is the use of scarce and expensive noble metals as catalysts for the hydrogen evolution reaction (HER) and oxygen evolution reaction (OER), because they contribute to increase the cost of the technology. Several strategies have been developed to overcome this drawback, such as optimising the catalyst loading in the electrodes and alloying or using alternative catalyst supports, always with the aim to maintain or even increase electrolyser performance and durability. In this review, we examine the latest developments in HER and OER catalysts intended for practical PEMWE systems, which point in the short term to the use of platinum and iridium nanoparticles highly dispersed at low loadings on conductive non-carbon supports.

1. Introduction

Renewable energy sources have gained significant attention due to the limited amounts of fossil fuels and their environmental impact. The increasing release of carbon dioxide, nitrogen oxides, heavy metals, ashes, tars and organic compounds from the combustion of fossil fuels to meet global energy demand has led to a rapid increase in pollutants and greenhouse gases in the air (1, 2). Today, concerns about air pollution and climate change drive the search for environmentally friendly, accessible and economically attractive renewable energy sources as alternatives to fossil fuels.

Hydrogen is the ‘clean fuel of the future’ because water is the only product expected (although residual pollutants can appear depending on the purity of the fuel and the oxidiser). Pure hydrogen allows clean energy to be obtained (3). However, it is not directly available for use in nature and therefore, it has to be produced (4). The current annual production of hydrogen is about 0.1 billion tonnes, the most part being used for petroleum and metals refining (47%) and ammonia production (45%). A small fraction is applied for electronics fabrication, the food industry and as fuel for transportation (5).

Nikolaidis and Poullikkas (4) have summarised the main advantages and disadvantages of the different methods of hydrogen production. Steam reforming of hydrocarbons is the most developed method, with existing infrastructure and efficiencies in the range 74–85%. Partial oxidation and autothermal steam reforming of hydrocarbons are proven technologies with smaller efficiencies in the range 60–75%. All these methods produce CO2 as byproduct, depending on the fossil fuel. There are alternative methods using raw materials coming from renewable technologies, namely biomass and water. The pyrolysis of biomass presents efficiencies of 35–50% and is CO2-neutral, but its main disadvantages are tar formation and the variable hydrogen content depending on the seasonal availability and impurities of the feedstock. The dark fermentation of biomass also has good efficiencies in the range 60–80% and is CO2-neutral, but its major disadvantages are the formation of fatty acids, which are organic pollutants that should be removed, low hydrogen production rates, low yields and the need for large reactor volumes.

Production methods utilising water as the only raw material produce hydrogen through water splitting processes such as electrolysis, thermolysis and photoelectrolysis. Thermolysis of water, with efficiencies in the range 20–45%, is clean and sustainable with oxygen being the only byproduct, but its major disadvantages are the toxicity of the elements used, corrosion problems and the need for high capital investment. Photoelectrolysis of water is also interesting since it is free from emissions and oxygen is the only byproduct, but it requires sunlight, has efficiencies of about 0.06% and suitable photocatalytic materials are needed. Conversely, electrolysis is a proven technology, with existing infrastructures and good efficiencies in the range 40–60%, with only oxygen as byproduct. Although a high capital investment is required and hydrogen produced by this method is still more expensive than that obtained from hydrocarbon reforming, water electrolysis appears to be an environmentally friendly hydrogen generation process and will be a key technique in the hydrogen economy.

Electrolysis is already a basic technique to provide hydrogen in small quantities for applications such as the food and semiconductor industries (5). Despite this, water electrolysis only contributes about 4% of overall hydrogen production in the world today (5). This may significantly change in the next few decades since solar and wind renewable energy resources are expected to increase, replacing fossil fuels for environmental reasons. If energy production by these methods exceeds the electricity demand, energy storage as hydrogen fuel can be a potential solution (1). This is particularly interesting because renewable resources are intermittent and therefore excess energy in operation can be used in water electrolysis for hydrogen production.

Alkaline electrolysis is the oldest and most mature technique. It uses a thin ceramic porous diaphragm submerged in a liquid alkaline electrolyte (68). It is also possible to use anion exchange membrane technology in alkaline water electrolysis. However, this is a long way from commercialisation. In the meantime, water electrolysis using PEMWEs is a recent and very attractive technique from an industrial viewpoint because the PEMWE is a compact device of simple construction and flexible dynamic operation in which a proton exchange membrane (PEM) replaces the liquid electrolyte (9). Figure 1 shows a schematic of a single cell of a PEMWE (10). The PEM is an acidic solid polymer electrolyte with very good proton conductivity (solid polymer electrolyte in Figure 1). Perfluorinated sulfonic-acid (PFSA) PEM membranes such as Nafion® are commonly used (11). The anode and cathode reactions for water electrolysis in acidic media are given by Equations (i) and (ii) for the OER and HER, respectively (3):


The standard (reduction) electrode potentials are 1.23 V and 0.00 V vs. standard hydrogen electrode, respectively, therefore the standard Gibbs energy of the overall Equation (iii) (given by the summation of Equations (i) and (ii)):


is ΔGo = –2 × 96,486 C molH2O–1 × (–1.23 V) = 2.37 × 105 J molH2O–1 > 0, meaning that this process requires energy, which can be provided by a power source moving electrons from the anode to the cathode terminals. As shown in Figure 1, water is introduced in liquid or vapour form, depending on the temperature, in the anode compartment where Equation (i) takes place. The protons produced through Equation (i) are transported by the electric field through the PEM to the cathode, where they are reduced according to Equation (ii). The acidic solution is retained in the membrane, thus reducing corrosion problems. The PEM must be thin to reduce the ohmic drop, which reduces the voltage needed for water electrolysis. In addition, it is not an electron conductor and behaves as a separator between the anode and the cathode, thus avoiding internal short-circuits. Moreover, it presents good chemical, mechanical and dimensional stability, with low permeability to hydrogen and oxygen. The anode and the cathode catalyst layers or electrocatalyst layers (CLs in Figure 1) are placed on each side of the PEM. The gas diffusion layers allow diffusion of reactants through them. The set integrated by the PEM and CLs is known as the membrane electrode assembly (MEA). Note also that the reactants circulate through the gas channels of the bipolar plates (BPPs in Figure 1), which allow the complete stack to be built up by means of the electrical connection between the cathode and the anode of adjacent cells.

Fig. 1.

Scheme of a single cell of a PEMWE. Reproduced from (10) under a Creative Commons CC BY license

Although PFSAs suffer dehydration over 100°C (11) and there is a consequent thermal limit in its practical use, the PEM offers additional advantages to the liquid alkaline electrolyte: (a) there are no anionic concentration gradients (as the anionic charges are fixed, fewer species are transported and the complexity of the system is reduced); (b) the gases are evolved at the back of the electrodes and do not contribute to the internal cell resistance, which is mainly due to the PEM (5); and (c) they are free from carbonate formation problems, thus providing highly compressed and pure hydrogen with high efficiency (1).

However, unlike alkaline electrolytes, acidic electrolytes require corrosion-resistant noble metals as electrocatalysts (12). The main components affecting performance and durability of PEMWE stacks are MEAs, in which at present iridium is the electrocatalyst for the OER and platinum for the HER (1316). Current densities in the range 0.6–2.0 A cm–2 for applied single cell voltages between 1.8–2.2 V can now be obtained (17). PEMWEs are in the early market introduction phase in the energy sector and the focus is on their durability and reliability rather on their cost (13). A recent estimate is that MEAs represent about 19% of the overall stack cost (18). The PEM itself plays a role because it contributes a significant ohmic loss, increasing with thickness, and must ensure robustness and low hydrogen and oxygen crossover. Nafion® 115 and 117, 120–200 μm in thickness are currently used, typically contributing about 5% of the cost of the PEMWE stack, but there is the possibility of introducing nanoparticles (NPs) or nanofibres in thinner PEMs with lower ionic resistance resulting in good mechanical stability and low oxygen and hydrogen crossover (14, 15, 1922).

The MEA is normally fabricated by directly depositing the electrocatalysts onto the PEM or by transferring them onto the PEM by a decal process (23). This latter procedure is known as the catalyst coating membrane approach (24, 25). The OER presents a more sluggish kinetics than the HER, therefore it significantly contributes to the overall polarisation. Iridium metal and IrO2 are the present state-of-the-art OER catalyst in PEMWEs (12, 14), providing a suitable balance between activity and stability and representing about 8% of the stack cost. With a typical loading of 2 mgIr cm–2 (23), an amount of about 500 kg of iridium is needed for a gigawatt-plant working at 4 W cm–2 (14). This is a large amount of iridium considering the annual worldwide production of about 9000 kg year–1 (2). Therefore, there is a need to reduce the iridium loading while improving the OER performance. The catalyst for the HER is platinum with a loading of about 0.3–0.5 mg cm–2 (12, 20, 26), contributing about 6% of the MEA cost, although it has been pointed out that this could be significantly reduced without performance loss (25). Other important components of PEMWEs are the bipolar plates and the porous transport layers, which contribute about 68–74% of the overall stack cost. The cell and stack balances account for the remaining percentage (14, 18).

PEMWEs use noble metals because of the advantages mentioned above. After intensive research, new components based on non-noble metals may be possible in the long-term, but in the short-term, there is still room to achieve better performance, durability and cost reduction with iridium and platinum (14). It is estimated that the overall cost could be reduced by about half by using advanced manufacturing techniques, especially for flow fields and separators (18). The catalytic material and catalyst loading are also crucial to obtain suitable performance, durability and cost (14). A good strategy to decrease catalyst cost may be to improve the stability of the support, enabling better dispersion to increase their utilisation.

Feng et al. (21) have summarised the degradation mechanisms of PEMWE components. The main problems with the electrocatalysts were dissolution, deactivation and agglomeration together with support passivation which would impede the current flow. This points to promising solutions such as addition of inert oxides, the use of binary or ternary solid-solution catalysts or tailoring the morphology of the catalyst. Recent PEMWE degradation studies suggested that the measured cell voltage increase was mainly due to reversible changes in the oxidation state of the iridium-based catalyst and that the real degradation took place in the ohmic and mass transport overpotential region at high current densities and long-time operation (13).

In this review, recent approaches to improve performance, stability, durability and cost of iridium- and platinum-based catalytic materials in current use are examined as specific objectives in the short-term development of PEMWEs. Attention is paid to catalyst loading and dispersion onto different supports, especially non-carbonaceous ones, which are particularly important in the anode of the PEMWEs due to the oxidative nature of this environment.

2. Supported Catalysts for the Hydrogen Evolution Reaction

As mentioned in the previous section, the most effective electrocatalysts for the HER in practical PEMWE are those based on platinum. However, the high cost and scarcity of platinum are a drawback in the development of PEMWE for large-scale applications. Reducing the amount of platinum is the main strategy to decrease the cathode cost contribution to PEMWEs (25, 2730). Platinum black has been employed in the cathode of PEMWEs (30), but the platinum loading can be reduced by improving the catalyst dispersion on high specific surface area supports based on carbon or non-carbon materials. A further strategy involves the development of platinum-based alloys.

2.1 Platinum-Based Catalysts Supported on Carbon Materials

It is generally accepted that highly dispersed platinum-on-carbon is the benchmark HER catalyst for PEMWEs, the carbon black Vulcan® XC-72 being the most common (15, 19, 22, 23, 25, 26, 29, 31, 32). Carbon-based materials are widely used as electrocatalyst supports because of their large surface area, high electron conductivity and stability. A PEMWE single cell based on Nafion® NR117 containing 0.4 mgPt cm–2 (40 wt% platinum supported on Vulcan® XC-72) and 2.5 mg cm–2 of IrO2 was reported (32) and it showed 1.7 V at 1 A cm–2 and 90°C. The average voltage degradation rate was ca. 35.5 μV h–1 after 4000 h at these experimental conditions.

Other materials like graphitic nanofibers (GNF) have been proposed as catalyst supports because their textural properties can favour the transport of gases. In particular, the performance of GNF-supported catalysts was found to be better than that of catalysts supported on Vulcan® XC-72 (33). A reduced electrolysis cell voltage (1.67 V vs. 1.72 V at 1 A cm–2 and 90°C) was obtained using Pt/GNF cathodes instead of Pt/XC-72 with the same platinum content (40 wt%).

However, the use of carbon supports for stabilising atomic-scale platinum is challenging because the interaction of the support with platinum atoms must be controlled. Recently, an ultra-low loading of platinum dispersed on single walled carbon nanotubes (SWNTs) (0.19−0.75 at% platinum and a platinum loading of ~114−570 ngPt cm–2, respectively) was reported in a three-electrode cell with promising properties in terms of electrocatalytic activity and durability for HER in acidic liquid electrolyte (34). More recently, an electrocatalyst comprising platinum nanowires on SWNTs with ultralow platinum content (340 ngPt cm–2) has been used for HER (35). A comparable activity (10 mA cm–2 at –18 mV vs. reversible hydrogen electrode (RHE)) to that of state-of-the-art Pt/C (10 mA cm–2 at –16 mV vs. RHE) was reached in acidic aqueous electrolyte. However, it is worth mentioning that HER kinetics cannot be measured accurately in acidic media, because it is limited entirely by hydrogen diffusion (36) which requires suitable gas transport techniques (37). In fact, PEMWE single cell tests recorded at 55°C using Nafion® 115 membrane and 0.02 mg cm–2 of Pt/C or Pt/SWNT at the cathode, while having 3 mg cm–2 of IrRuOx at the anode, revealed similar activity. However, the stability of the electrolyser setup operating the cell at the constant current density of 1 A cm–2 was better for the MEA containing the Pt/SWNT catalyst.

The hydrogen and oxygen permeation between cathode and anode through the membranes of the PEMWEs has been investigated (3840) and although oxygen permeation is lower than that of hydrogen, it increased with current density and temperature, as did hydrogen permeation. The oxygen content in the hydrogen product was found to be three to four times greater when using platinum-free instead of platinum cathode catalysts (39). This was explained by the lower activity for the oxygen reduction using the platinum-free catalyst, so that less permeated oxygen was reduced at the cathode of the PEMWE and consequently, the oxygen flow within hydrogen was higher. It has also been reported that permeated oxygen can be reduced to hydrogen peroxide at the cathode (two-electron reaction), which can be further transformed into hydroxyl radicals, OH, through Fenton’s reaction with active metal ion impurities (such as Fe2+ and Cu2+) (40). These radicals produce membrane degradation.

2.2 Platinum-Based Catalysts Supported on Non-Carbon Materials

Carbon oxidation of oxygen cathodes has been reported in polymer electrolyte fuel cells (40, 41) and could also be expected in PEMWEs under certain conditions. It is therefore interesting to explore non-carbonaceous supports with high specific surface area. Titania has demonstrated very good chemical resistance and thermal stability (42). Shi et al. (43) found that when using a carbon-free Pt/TiO2 cathode in a PEMWE, the membrane degradation rate was lower compared to a Pt/C cathode. This was explained by the higher rate of hydrogen peroxide generation on the carbon surface of the latter, which led to the formation of OH and OOH radicals responsible for membrane degradation by reaction with residual active ions such as Fe2+.

Platinum NPs supported on nitrogen-doped black titania (Pt/Nx:TiO2–x) have been reported to show robust durability and onset potentials for the HER which were somewhat smaller than those of commercial Pt/C catalyst (44). Different platinum catalysts supported on niobium-doped titania nanotubes (TNTs) have been synthesised and tested for the HER in acidic media (45). They showed better electrochemical performance for HER in acidic aqueous solution than those reported in recent literature for synthesised and commercial platinum supported catalysts. These results make Pt/Nb-TNT catalysts, in particular those containing 3 at% niobium, very promising for the HER in PEMWEs.

2.3 Platinum-Based Alloy Catalysts

A further way to reduce the platinum loading in the cathode is by developing active platinum-based alloys. An example is a recently developed platinum-iron alloy stabilised with platinum-skin layers supported on carbon black for HER in acidic media (46). The performance and durability of this catalyst were examined in a PEMWE single cell, which incorporated a MEA consisting of PtxAL–PtFe/C (0.20 mgPt cm–2) and a conventional anode IrO2 + platinum black (0.92 mgPt+Ir cm–2). The electrolyte membrane was commercial Nafion® NRE212 (50 μm thick). The initial cell voltage was 1.57 V at 1.0 A cm–2 and 80°C and presented an average degradation rate of ~70 μV h–1 after 1000 h of continuous operation. This relatively high degradation rate at rather moderate operating conditions was mainly due to the anode, since the cathode operated stably with low H2O2 production (the cathode potential varied only ~10 mV during this operating time). The challenge in the case of noble metal-based bimetallic structures is that they may change during the reaction (47).

There is, of course, an alternative way to decrease the cathode platinum loading. Optimising the MEA manufacture would lead to optimal use of the catalyst and, by extension, the cell performance (25). The PEMWE durability at low catalyst loadings is then the issue. Highly active sites may result from synergistic effects between the supporting materials and the electronic properties of the metal when downsizing to single-atom catalysts, as shown in three-electrode cells (47, 48). However, the undesirable tendency to aggregation remains to be solved.

3. Catalysts for the Oxygen Evolution Reaction

Even though the electrochemical splitting of water has been known since the 19th century, more knowledge is needed to understand the OER mechanism and to find the ideal catalyst in terms of activity and stability (49). For large-scale production of water electrolysers, the development of highly active, stable and inexpensive OER catalysts is critical (50).

Due to the sluggish kinetics and the highly oxidative and acidic conditions of the OER, the electrocatalysts used on the anode side must be noble metal-based, mainly iridium and ruthenium, because they show the best performance in terms of activity and stability in the operation conditions (5153). Considering the industrial importance of PEMWEs, several studies on electrocatalytic properties of iridium- and ruthenium-based catalysts on OER performance in acidic media are discussed in a large body of literature (31, 49, 5254).

Metallic ruthenium and RuO2 are known to be the most active catalysts for the OER in acidic media (51, 55, 56). However, several studies have determined that ruthenium has low stability compared to iridium and other metals, even under mild operation conditions (53, 57, 58). Danilovic et al. (58) used X-ray absorption spectroscopy together with potentiodynamic OER measurements to establish a functional link between activity and stability of monometallic oxides during the OER in acidic media. They found that the most active oxides (gold ≫ platinum < iridium < ruthenium ≫ osmium) were, in fact, the least stable (gold ≫ platinum > iridium > ruthenium ≫ osmium) materials. Discarding osmium because of its very low stability, RuO2 also degrades during OER in acidic media. At potentials higher than 1.4 V, the oxidation of RuO2 to non-conductive RuO4 is favoured and tends to dissolve rapidly (53, 59). Therefore, this reaction greatly modifies RuO2 properties, significantly losing its electrocatalytic activity and stability during extended PEMWE operation (52).

A comparative study carried out during OER using an electrochemical scanning flow cell connected to an inductively coupled plasma mass spectrometer, revealed that IrO2 was more stable than RuO2, with a difference in dissolution of ca. 30 times under similar conditions (53). IrO2 still has outstanding activity and stability and, for this reason, is used as the state-of-the-art catalyst in PEMWE systems (14, 54).

Unfortunately, the loading of iridium in the anode is significantly higher than the noble metal in the cathode due to the sluggish OER kinetics and stability issue. Moreover, iridium is extremely rare and expensive. For relatively small systems (kilowatt range), the iridium and platinum catalysts comprise about 5–10% of the stack cost (60). The catalyst cost is expected to increase for larger systems (megawatt range), whereas the cost of the other stack components will be lower (61). Therefore, reducing the loading of precious metals, while maintaining higher activity and optimal stability, is critical to enable large-scale implementation of PEMWEs. For the anode, several strategies are currently pursued, such as reducing the particle size and assuring uniform distribution over a conductive support to make all nanoparticles electrochemically accessible. When the particle size is reduced (for a given catalyst loading), the effective surface area is increased and thus, more active sites for the OER are formed (62, 63).

3.1 Iridium-Based Core-Shell Catalysts

In a similar way to platinum, the combination of IrO2 with other metals in core-shell structures allows less iridium to be used and, in addition, can display a superior OER activity. Tackett et al. (64) described FeN3 core-IrO2 shell structures with superior OER activity in which the nitride was protected from the acidic media by the shell. The activity increase was related to electronic effects of the substrate-surface interaction. Nong et al. (65) prepared an electrochemically dealloyed IrNi core-IrOx shell combined with a mesoporous corrosion-resistant antimony-doped tin oxide support (antimony-tin oxide (ATO)), which behaved as highly efficient and stable OER catalysts in acidic medium. The higher OER activity on both geometric surface and iridium-mass basis compared to the IrOx /C and IrOx /ATO benchmarks was explained by electronic and strain effects, which could modify the chemisorption and reactivity of intermediates at the surface. More recently, Jiang et al. (66) electrodeposited thin iridium films (~68 nm thick) on WOx nanorods, thus allowing a uniform iridium dispersion on the poorly conducting WOx and the use of a low loading of the precious metal. Current densities of 2.2 A cm–2 were obtained at 2.0 V in a laboratory PEMWE with improved stability over 1000 h at 0.5 A cm–2 for a reduced loading of 0.14 mgIr cm–2, which was assigned to the stability of WOx and the fixed iridium coating.

3.2 Iridium-Based Catalysts with Metal Oxides

IrO2 can also be mixed with different metal oxides to create electrocatalysts with improved activity and stability for the OER such as RuxIr1–xO2 (59), Ru60Pt30Ir10 (67), Ir0.7Ru0.3Ox (6870) and Ir0.40Sn0.30Nb0.30O2 (71). Computational studies have revealed that the superiority of these mixed metal oxides is due to the stable formation of the intermediates involved in the OER mechanism (7275). Tang et al. (76) found that by switching the host structure of the Ir4+ oxygen-coordination octahedra from corner- and edge-sharing rutile (IrO2) to purely corner-sharing perovskite (SrIrO3), the OER activity increased by more than one order of magnitude. Density functional theory calculations revealed that the adsorption energetics on SrIrO3 depended sensitively on the electron-electron interaction, whereas for IrO2, it depended rather weakly. Yang et al. (77) reported high-activity face-sharing perovskite structures. Despite that the 6H-SrIrO3 perovskite contained 27.1 wt% less iridium than IrO2, its iridium mass activity was seven times greater than the latter due to the existence of face-sharing IrO6 octahedral dimers, which facilitated the OER rate determining step by weakening the iridium-oxygen binding.

Another promising solution to decrease the iridium amount is the use of one-dimensional nanoarray electrodes, which shows promise in high catalyst utilisation and enhanced electron and mass transfer (7880). Zhao et al. (80) prepared IrOx nanotube arrays by electrodepositing IrO2 NPs onto ZnO nanorod surfaces to produce IrO2-coated core–shell nanorod arrays, followed by wet chemical etching the ZnO nanorods away. The IrOx nanotube arrays showed 2.7 times higher turnover frequency (TOF) than that of commercial IrO2 NPs in the OER. Lu et al. (78) prepared vertically aligned IrOx nanoarrays by electrodeposition using titania nanotube arrays as templates. IrOx open-end nanotube arrays with tunable length range were obtained by modulating the scan rate in the electrodeposition process. IrOx nanoarrays performed almost the same OER current density with one twentieth iridium loading amount compared with commercial IrO2 NPs.

3.3 Iridium-Based Nanostructured Thin Film Catalysts

Another strategy to improve the electrochemically active surface area was the preparation of iridium-based nanostructured thin film (NSTF) electrodes, developed by 3M, USA, which are less sensitive to agglomeration and corrosion due to the special catalyst morphology (21, 8183). The NSTF catalysts were obtained by physical vapour deposition (PVD) of catalysts onto a supported monolayer of oriented crystalline organic-pigment whiskers. Whiskers are corrosion resistant, therefore eliminating the high voltage corrosion affecting most carbon supports (31). Lewinski et al. (81) prepared an ultra-thin continuous film of iridium deposited on arrays of organic nanowhiskers (PR149). NSTF was shown to be able to operate at 0.25 mgIr cm–2 and attain high current densities of 10 A cm–2 at ~2 V at 80°C.

More recently, Jensen et al. (83) reported the use of a modified PVD technique to prepare interconnected nanoporous thin films by selective leaching of heterogeneous Ir–Co templates formed by an alternating magnetron sputtering process. This approach allowed the preparation of extended surface area catalysts with higher porosity and iridium dispersion, while maintaining high intrinsic activities. Mirshekari et al. (84) used reactive spray deposition technology, a flame-based process in which catalyst nanoparticles are synthesised by combusting solutions of metal-organic precursors in combustible solvents, to fabricate MEAs with very small amounts of catalyst. Anode and cathode contained only 0.3 mgIr cm–2 (in the form of Ir/IrOxNPs) and 0.2 mgPt cm–2 (platinum NPs on Vulcan XC-72R), respectively. With the purpose of reducing the hydrogen crossover, the MEA contained a thin platinum recombination layer (RL) 100–200 nm in thickness (0.025 mgPt cm–2) between the Nafion® 211 and the Nafion® 117 membranes of the anode and cathode, respectively. The cell operated for 3000 h at 50°C with 1.8 A cm–2 with no significant losses in performance.

3.4 Iridium-Based Catalysts Supported on Conductive Materials

One of the most remarkable ways to achieve highly active electrode with low loading amount of iridium content is the use of conductive supports (67, 8588). It has been shown that supports are important not only to increase the active surface area of the catalysts, but also to integrate the catalyst-support feature or to improve the charge transfer efficiency between them (89). Stability under the harsh conditions of the cell is one of the main requirements that catalyst supports should meet.

Conductive supports based on carbon materials are routinely used in fuel cell technology. However, under the high potential of the OER, most carbons are easily corroded. Better results were obtained using advanced carbon supports such as carbon nanobowls (90) and nanotubes (91). The stability and activity of iridium nanocrystals supported on carbon nanobowls during the OER at 10 mA cm–2 in 0.1 M HClO4 significantly outperformed that of commercial Ir/C (80). IrO2 supported on carbon nanotubes also exhibited similar stability during the OER at the same current density in 0.1 M H2SO4 (88).

3.5 Iridium-Based Catalysts Supported on Metal Oxides

Alternatively, oxide-based supports such as titania (89, 9294), Ti4O7 Magneli phases (70, 9598) and doped tin oxide (60, 85, 87, 99101) have been proposed.

3.5.1 Titania-Based Supports

Titania supports offer low cost, very high thermal and chemical stability under anode conditions and commercial availability. However, titania suffers low electric conductivity (about 10–6 S cm–1 at T < 200°C) and low adsorption/desorption capability toward the species and charge in the OER (31, 102104). Fuentes et al. (92) developed IrRu(1:1) electrocatalysts supported on anatase titania with high activity towards the OER, which showed a 53% higher current per gram of metal than that of unsupported electrocatalyst of the same composition. The higher catalyst utilisation of supported electrocatalysts for the OER was consistent with small, well-dispersed nanoparticles. Mazúr et al. (102) prepared IrO2 NPs (60 wt%) supported on commercial titania powders, with specific surface areas from 10 m2 g–1 to 90 m2 g–1. They found that the lower the specific surface area of the support the higher was the electrochemical activity of the catalyst. This was explained by the formation of a thin layer of more conductive IrO2 on the surface of the non-conductive titania, which was able to cover the support with low specific surface area, thus providing the entire material with enough electron conductivity. Rozain et al. (105) synthesised IrO2 catalysts on micro-sized titanium particles (50 wt% titanium), showing that for IrO2 loadings less than 0.5 mgIrO2 cm–2, the performance of the PEMWE was better than that prepared with unsupported IrO2.

Assuming that titanium was oxidised to TiO2 during the OER, Bernt et al. studied the influence of the ionomer content (24) and of the iridium loading (25) on the performance of a PEMWE using IrO2/TiO2 (75 wt% iridium) as the anode electrocatalyst. The best performance was found for 11.6 wt% of the ionomer (24). The performance losses below and over this value were ascribed to a higher proton conduction resistance and to an oxygen higher mass transport resistance, respectively. The iridium loading was varied between 0.20–5.41 mgIr cm–2. The optimal performance at operational current densities (≥1 A cm–2) was for 1–2 mgIr cm–2. The CL became very thin and inhomogeneous when its loading was reduced to <0.5 mgIr cm–2, resulting in a much higher performance loss than expected based simply on the OER kinetics losses (54). This is illustrated in Figure 2(a), where a scanning electron microscopy (SEM) image of the MEA section is shown. On the anode side, there is a porous transport layer (PTL) made of sintered titanium, which facilitates water transport to the CL, composed of IrO2/TiO2 and ionomer. Separated by the Nafion® 212 membrane is the cathode, made of 4.8 wt% Pt/C and ionomer, covered by a carbon paper PTL. The thickness of the iridium-based CL depends on the iridium load, as shown in Figure 2(b), which shows a couple of examples in the insets. Figures 3(a) and 3(b) depict the cross-sectional and top views in the case of a low iridium loading. Figures 3(c) and 3(d) show schemes of the electrical connections in the case of thick and thin anode CLs, whereas in Figure 3(e), the titanium PTLs have been replaced by a carbon PTL with a microporous layer.

Fig. 2.

(a) SEM image of the cross-section of a MEA showing an IrO2/TiO2 + ionomer anode CL and a Pt/C + ionomer cathode CL, separated by a Nafion® 212 membrane. The anode and the cathode PTLs were made of titanium and carbon paper, respectively; (b) anode thickness as a function of the iridium loading, with two SEM cross-sectional pictures for different thicknesses as insets. Reproduced from (25) under Creative Commons Attribution 4.0 License (CC BY)

Fig. 3.

(a) Cross section; and (b) top-view SEM images of thin iridium-based CLs. The schemes illustrating the electronic transport between the titanium PTLs and the CLs are shown in: (c) for thick; and (d) thin CLs. In (e), the titanium-based PTLs have been replaced by a carbon PTL with a MPL. Reproduced from (25) under Creative Commons Attribution 4.0 License (CC BY)

Cheng et al. (106) synthesised a composite IrOx-TiO2-Ti catalyst with mixed valence iridium species. It was shown that titania was beneficial for the formation of Ir(III) and mixed Ir(III/IV) oxyhydroxides, resulting in a high surface concentration of adsorbed hydroxyl and controllable iridium valence, thus explaining its high OER activity.

Additional durability studies were performed with titania-supported IrO2 (Elyst Ir75 0480 from Umicore, Belgium) with an iridium loading of 2mgIr cm–2 (107). It was observed that the performance of the MEA electrolyser decreased after cycling the anode potential between ~0 VRHE in the open circuit voltage-periods and high potentials when current was applied to the electrolyser. This degradation was due to the formation of the less conductive hydrous Ir(OH)x phase and the gradual passivation of the titanium porous transport layer (titanium-PTL), which increased the internal ohmic resistance.

The conductivity of titania could be significantly improved by doping with donor species such as metal ions. The group of Hong and Lv extensively studied the effect of doping the titania support for IrO2 with vanadium (108), niobium (109, 110), tantalum (111) and tungsten (112) on the physical properties and OER activity of the catalysts. They obtained highly active IrO2 supported on mesoporous niobium (20 at%)-doped titania with specific surface area of 132 m2 g–1 by means of the modified evaporation-induced self-assembly method (109). The authors found that the majority of the OER activity increase was due to the niobium-doping, which enhanced the specific surface area and surface activity of charge and species transfer. Subsequent treatment of niobium-doped titania with hydrogen resulted in higher electrical conductivity, increased surface active sites and enhanced OER performance (110). Single cell tests showed that the catalyst treated in hydrogen at 750°C led to the optimum OER activity (1.832 V at 1 A cm–2), which was superior to that of unsupported IrO2 (1.858 V at 1 A cm–2) and remained stable for 100 h operating at a current density of 1 A cm–2.

They also studied the effect of vanadium doping of the titania support, synthesised by a modified evaporation-induced self-assembly technique (108). IrO2 supported on titania samples doped with different amounts of vanadium (0 at%, 10 at%, 20 at% and 30 at%) were evaluated. In a single cell, the OER performance gradually increased with vanadium dopant from 0 at% to 20 at%, followed by a performance deterioration with vanadium amount reaching 30 at% due to the corrodible V2O5 precipitate. Recently, the incorporation of tungsten to obtain IrO2/Ti1–xWxO2 (x = 0.05, 0.1 and 0.2), resulted in an active electrocatalyst for the OER. Of all the Ti1–xWxO2 supports, the highest electrocatalytic activity was obtained with Ti0.9W0.1O2. With optimised IrO2 loading, the applied potential in a single water electrolysis cell was 1.79 V to obtain 1 A cm–2 at 80°C. Durability tests for 40IrO2/Ti0.9W0.1O2 at 0.5 A cm–2 and 1 A cm–2 indicated that the cell voltages were stable over 100 h.

Hu et al. (113) synthetised IrO2 dispersed on a corrosion-resistant Nb0.05Ti0.95O2 support (83 m2 g−1) by the sol-gel method. The IrO2 loading of 26 wt% exhibited the best mass normalised OER activity, which was explained by uniform support of the IrO2 NPs on the surface, thus providing conductive channels to reduce the grain boundary resistance. Recently, Alcaide et al. (89) prepared IrO2 and IrRuOx (50 wt%) supported on titania nanotubes and niobium-doped titania nanotubes (3 at% niobium). They observed that niobium doping of titania significantly increased the surface area of the support from 145 m2 g–1 to 260 m2 g–1. The highest OER performance of IrO2/Nb-TiO2 nanotubes was assigned to the good dispersion and accessibility of the IrO2 NPs, the high specific surface area of the support and the electron donor properties of the Nb4+ species to the conduction band of titania. The stability with the Nb-TiO2 nanotubes was also better than that of unsupported IrO2.

3.5.2 TinO2n–1-Based Supports

Non-stoichiometric titanium sub-oxides, TiO2–x, have drawn considerable attention due to their high electronic conductivity. In particular, the titanium sub-oxides Magneli phases, TinO2n–1, such as Ti5O9 and Ti4O7 or a mixture, which are known by the commercial name Ebonex®, are highly conductive and corrosion resistant in acidic media during the OER (95, 96). Metallic iridium NPs supported on Ti4O7 were synthetised by Wang et al. (86) via a conventional sodium borohydride reduction method in anhydrous ethanol at room temperature. The catalyst exhibited improved OER kinetics in acidic media and higher TOF compared to iridium-black. A study comparing IrO2 electrocatalysts supported on commercial Ebonex® and titanium-suboxides (TinO2n –1) prepared in-house was carried out by Siracusano et al. (114). The results showed expected electronic conductivity for both electrocatalysts and superior OER activity of the catalyst based on titanium-suboxides prepared in-house compared to the commercial support. These results were attributed to better dispersion and larger occurrence of active catalytic sites on the surface of the suboxide prepared in-house.

3.5.3 Antimony-Tin Oxide-Based Supports

ATO has been considered as an alternative support material for OER catalysts because it exhibits relatively high electrical conductivity and corrosion resistance. Some dissolution of the dopant has been reported during the OER at high anodic potentials in sulfuric acid. However, it withstands anodic conditions better than indium-doped tin oxide, known as indium-tin oxide (ITO) (101). Liu et al. (115) synthetised antimony-tin oxide nanowires (nw) as supporting materials for IrO2 NPs which exhibited significant improvement in mass activity when compared to the same catalyst supported on antimony-tin oxide NPs and pure IrO2. The OER performance was further confirmed by PEMWE tests at 80°C; the IrO2/ATO-nw catalyst reached 2 A cm–2 at 1.62 V vs. RHE (80°C) with an activity loss of 0.76 mV h–1 after 646 h at 0.45 A cm–2.

Wang et al. (116) found that IrO2 supported on ATO aerogels allowed the use of noble metal to be reduced while keeping the same OER current per unit geometric surface area. Furthermore, the highly porous structure of SnO2:Sb aerogel was successfully retained by using vanadium additives under atmospheric drying. However, vanadium did not play an active role in OER catalysis. Similarly, iridium NPs supported on SnO2:Sb aerogel allowed the use of precious metal to be decreased by more than 70% while enhancing the electrocatalytic activity and stability (60). Operando near-ambient pressure X-ray photoelectron spectroscopy on MEAs revealed a low degree of iridium oxidation, attributed to the oxygen spill-over from iridium to SnO2:Sb where the formation of highly unstable Ir3+ species was mitigated.

A comprehensive overview of the stability and degradation of catalysts during the OER in acidic media was given by Spöri et al. (117). They established that the degree of metal immobilisation on the support depends on the interface between the support surface (groups) and the metal oxide and influences the extent of particle detachment or dissolution during the OER process. These interactions can range from weak electrostatic attraction to stronger connections through surface chemical bonds or formation of an overlayer on the support, which can also affect the activity by decreasing or increasing electron density to the catalyst surface. More recently, several reviews address electrocatalyst performance in terms of activity, stability and efficiency (17, 118, 119). Kim et al. (17) have reviewed the latest advances in iridium-based, ruthenium-based and even non-noble metal-based multimetallic electrocatalysts for the OER in acidic media, with emphasis on their stability and reference to machine learning models. Wang et al. (118) have summarised the OER performance of selected catalysts in acidic and alkaline media. Also related to this point, an in-depth literature review of the OER mechanism, with special emphasis on the adsorption and lattice oxygen evolution mechanisms to elucidate the catalyst degradation, has recently been published by Chen et al. (119).

4. Performance of Selected Proton Exchange Membrane Water Electrolysers

Table I shows the performance of selected PEMWE single cells in recent years, generally at 80°C, including catalyst loading, operating conditions, type of membrane and degradation rate, which have been discussed in this paper. In this review, we have seen many different anodic and cathodic catalysts which have been studied in three-electrode cells and in laboratory PEMWEs. Note that the latter have been generally tested using platinum supported on carbon cathodes and different PEMs, also applying different voltages, resulting in different current densities. It is therefore not easy to extract the best PEMWEs, since changing the anode, the cathode, the membrane, the temperature, the cell voltage or catalyst loadings can lead to significant changes in the cell performance. Optimisation of all these parameters should be performed. However, promising results can be ascertained.

Table I

Performance Data of Selected PEMWE Single Cells Made with Different Components Under the Indicated Conditions from 2009 to 2021

Operating conditions
Catalyst Loading, mg cm–2 Catalyst Loading, mg cm–2 Voltage, V Current density, A cm–2 Temperature, °C Membrane Degradation rate Ref.
Ir/IrOx 0.3 Pt/C 0.2 2.09 1.8 50 Nafion® 211/Pt RL/Nafion® 117 24 μV h–1, 1.8 A cm–2, 3000 h (84)
Ir@WOx 0.14 70 wt% Pt/C 0.4 2.0 2.2 80 Nafion® 115 49.7 μV h–1, 0.5 A cm–2, 1030 h (66)
IrO2 1.40 60 wt% Pt/C 0.50 1.80 2.0 80 Nafion® D520 N/A (15)
IrO2 0.90 55.5–58.5 wt% Pt/C 0.25 1.80 3.6 80 Nafion® 212 N/A (26)
RuO2 3.0 30 wt% Pd/B3-CNPs 0.70 1.86 0.50 80 Nafion® 115 2.04 V, 500 h, 1 A cm–2 (29)
Ir0.7Ru0.3Ox 0.40 40 wt% Pt/C 0.10 1.82 3.0 80 Aquivion® membrane (E98-09S) 90 μV h–1, 800 h (69)
Ir/SnO2:Sb 0.50 (Ir) 40 wt% Pt/C 1.0 N/A N/A N/A Aquivion® membrane (E87-05S) N/A (60)
IrO2 1.40 60 wt% Pt/C 0.50 1.80 1.1 80 Nafion® 117 200 h, 2 A cm–2 (22)
IrO2/Sb-SnO2 (7/3) 0.50 40 wt% Pt/C 5.00 1.70 ~1.3 80 Nafion® 211 N/A (100)
IrO2 + Pt black (1:1) 0.92 Ptx AL–PtFe/C 0.20 1.57 1.0 80 Nafion® 212 ~70 μV h–1, 1 A cm–2, 1000 h (46)
IrO2 2.10 55.5–58.5 wt% Pt/C 0.40 1.80 6.0 80 N/A N/A (23)
IrO2 (75%) /TiO2 1.50–2.0 (Ir) 4.8 wt% Pt/C 0.025 (Pt) 1.79 3.6 80 Nafion® 212 N/A (25)
IrO2 (20%) /gCNH N/A Pt/C 4.0 (Pt) 1.80 ~0.7 80 Nafion® 115 N/A (88)
IrRuOx 3.0 Pt black 0.086 1.80 ~1.8 80 Nafion® 115 N/A (30)
Ir black 2.0 Pt/C 1.0 1.80 ~1.3 80 Nafion® N115/Pt (0.02 mg cm–2)/Nafion® NR212 190 μV h–1, 1 A cm–2 (19)
IrO2 2.50 40 wt% Pt/C 0.40 1.70 1.0 90 Nafion® 117 35.5 μV h–1 (32)
40 wt% IrO2/V-TiO2 (20 at% V) 2.50 40 wt% Pt/C 0.50 1.80 0.6 80 Nafion® 117 N/A (108)
Ir0.7Ru0.3Ox 1.0 40 wt% Pt/C 0.40 1.70 1.0 80 Nafion® NR212 81 μV h–1 (70)
IrO2/Ti (50 wt% Ti) 0.1 46 wt% Pt/C 0.25 1.73 1.0 80 Nafion® NRE 115CS 1000 h, 20 μV h–1 (105)
Ru@Pt (core-shell) 0.10 Pt@WO3 (core-shell) 0.10 1.80 1.0 80 Nafion® 117 N/A (61)
IrO2/Sb-SnO2 nanowire 0.75 40 wt% Pt/C 0.20 1.62 2.0 80 Nafion® NR212 0.76 mV h–1, 0.45 A cm–2 at 35°C (115)
67 wt% IrO2/Tin O2n –1 1.0 30 wt% Pt/Vulcan XC-72 1.0 1.80 0.700 80 Nafion® 115 N/A (114)

General trends can be observed: (a) current densities and cell voltages are similar, but the most recent papers use less iridium at the anode due to better dispersion of the precious metal, either on a supporting material or unsupported, although obtained using a different synthesis procedure; (b) a gain in the PEMWE stability is also seen, with several factors affecting PEMWE stability including anode structure and membrane degradation; and (c) limiting the permeation of gases through the membrane leads to better PEMWE stability since radicals formed at the cathode produce membrane degradation.

5. Concluding Remarks

In this review, an overview of the most recent advances in electrocatalysis for PEM water electrolysis has been provided, both for the HER at the cathode and the OER at the anode, paying special attention to the development of noble metal supported catalysts and their implementation into practical systems. For the former reaction, Pt/C is the most common catalyst, while for the latter the most used catalysts are iridium black and IrO2. Both noble metals are scarce and expensive. Several approaches to develop highly structured catalysts leading to high metal dispersion and, ultimately, lower loadings at the electrodes have been thoroughly reviewed. Regarding the HER, platinum supported on advanced carbon materials achieves the expected targets in terms of performance, but in the authors’ opinion, durability is an issue that requires the use of alternative titanium-based non-carbon supports. Regarding the OER, among the reviewed approaches and also in the authors’ opinion, the development of iridium-based catalysts supported on conductive metal oxides such as those based on niobium-doped titania and antimony-doped tin oxide could lead to the expected performance and durability required by industry players.

Overall, in the short term, the development of advanced supports for metal dispersion will allow the use of these noble metals to be optimised, reducing the cost and increasing the performance and durability of the electrolysers. In the long term, the development of non-noble catalysts and their implementation in real cells is mandatory to ensure the viability of the technology. In this sense, preliminary studies carried out with non-noble catalysts in half-cell configuration are promising, but further work is necessary to improve their stability and durability in practical cells. Thus, there is still a long way to go before their implementation in commercial PEMWEs.


  1. 1.
    K. Bareiß, C. de la Rua, M. Möckl and T. Hamacher, Appl. Energy, 2019, 237, 862 LINK
  2. 2.
    P. C. K. Vesborg and T. F. Jaramillo, RSC Adv., 2012, 2, (21), 7933 LINK
  3. 3.
    M. Pudukudy, Z. Yaakob, M. Mohammad, B. Narayanan and K. Sopian, Renew. Sustain. Energy Rev., 2014, 30, 743 LINK
  4. 4.
    P. Nikolaidis and A. Poullikkas, Renew. Sustain. Energy Rev., 2017, 67, 597 LINK
  5. 5.
    Y. Naimi, and A. Antar, ‘Hydrogen Generation by Water Electrolysis’, in “Advances in Hydrogen Generation Technologies”, ed. M. Eyvaz, Ch. 1, InTechOpen, London, UK, 2018, 18 pp LINK
  6. 6.
    D. M. F. Santos, C. A. C. Sequeira and J. L. Figueiredo, Quim. Nova, 2013, 36, (8), 1176 LINK
  7. 7.
    D. Berndt and D. Spahrbier, ‘Batteries’, in “Ullmann’s Encyclopedia of Industrial Chemistry”, Wiley-VCH Verlag GmbH, Weinheim, Germany, 2005
  8. 8.
    J. Brauns and T. Turek, Processes, 2020, 8, (2), 248 LINK
  9. 9.
    A. S. Aricò, S. Siracusano, N. Briguglio, V. Baglio, A. Blasi Di and V. Antonucci, J. Appl. Electrochem., 2013, 43, (2), 107 LINK
  10. 10.
    X. Sun, K. Xu, C. Fleischer, X. Liu, M. Grandcolas, R. Strandbakke, T. S. Bjørheim, T. Norby and A. Chatzitakis, Catalysts, 2018, 8, (12), 657 LINK
  11. 11.
    A. Kusoglu and A. Z. Weber, Chem. Rev., 2017, 117, (3), 987 LINK
  12. 12.
    P. Millet, N. Mbemba, S. A. Grigoriev, V. N. Fateev, A. Aukauloo and C. Etiévant, Int. J. Hydrogen Energy, 2011, 36, (6), 4134 LINK
  13. 13.
    M. Suermann, B. Bensmann and R. Hanke-Rauschenbach, J. Electrochem. Soc., 2019, 166, (10), F645 LINK
  14. 14.
    P. Shirvanian and F. van Berkel, Electrochem. Commun., 2020, 114, 106704 LINK
  15. 15.
    P. Holzapfel, M. Bühler, C. Van Pham, F. Hegge, T. Böhm, D. McLaughlin, M. Breitwieser and S. Thiele, Electrochem. Commun., 2020, 110, 106640 LINK
  16. 16.
    T. Reier, M. Oezaslan and P. Strasser, ACS Catal., 2012, 2, (8), 1765 LINK
  17. 17.
    T. Kim, B. Kim, T. Kwon, H. Y. Kim, J. Y. Kim and K. Lee, Mater. Chem. Front., 2021, 5, (12), 4445 LINK
  18. 18.
    K. Ayers, N. Danilovic, R. Ouimet, M. Carmo, B. Pivovar and M. Bornstein, Annu. Rev. Chem. Biomol. Eng., 2019, 10, 219 LINK
  19. 19.
    C. Klose, P. Trinke, T. Böhm, B. Bensmann, S. Vierrath, R. Hanke-Rauschenbach and S. Thiele, J. Electrochem. Soc., 2018, 165, (16), F1271 LINK
  20. 20.
    J. Hu, J. Luo, P. Wagner, O. Conrad and C. Agert, Electrochem. Commun., 2009, 11, (12), 2324 LINK
  21. 21.
    Q. Feng, X.-Z. Yuan, G. Liu, B. Wei, Z. Zhang, H. Li and H. Wang, J. Power Sources, 2017, 366, 33 LINK
  22. 22.
    M. Bühler, F. Hegge, P. Holzapfel, M. Bierling, M. Suermann, S. Vierrath and S. Thiele, J. Mater. Chem. A, 2019, 7, (47), 26984 LINK
  23. 23.
    M. Stähler, A. Stähler, F. Scheepers, M. Carmo and D. Stolten, Int. J. Hydrogen Energy, 2019, 44, (14), 7053 LINK
  24. 24.
    M. Bernt and H. A. Gasteiger, J. Electrochem. Soc., 2016, 163, (11), F3179 LINK
  25. 25.
    M. Bernt, A. Siebel and H. A. Gasteiger, J. Electrochem. Soc., 2018, 165, (5), F305 LINK
  26. 26.
    M. Stähler, A. Stähler, F. Scheepers, M. Carmo, W. Lehnert and D. Stolten, Int. J. Hydrogen Energy, 2020, 45, (7), 4008 LINK
  27. 27.
    M. Bajdich, M. García-Mota, A. Vojvodic, J. K. Nørskov and A. T. Bell, J. Am. Chem. Soc., 2013, 135, (36), 13521 LINK
  28. 28.
    S. S. Kumar and V. Himabindu, Mater. Sci. Energy Technol., 2019, 2, (3), 442 LINK
  29. 29.
    S. S. Kumar and V. Himabindu, Renew. Energy, 2020, 146, 2281 LINK
  30. 30.
    Z. Kang, G. Yang, J. Mo, Y. Li, S. Yu, D. A. Cullen, S. T. Retterer, T. J. Toops, G. Bender, B. S. Pivovar, J. B. Green and F.-Y. Zhang, Nano Energy, 2018, 47, 434 LINK
  31. 31.
    M. Carmo, D. L. Fritz, J. Mergel and D. Stolten, Int. J. Hydrogen Energy, 2013, 38, (12), 4901 LINK
  32. 32.
    S. A. Grigoriev and A. A. Kalinnikov, Int. J. Hydrogen Energy, 2017, 42, (3), 1590 LINK
  33. 33.
    S. A. Grigoriev, M. S. Mamat, K. A. Dzhus, G. S. Walker and P. Millet, Int. J. Hydrogen Energy, 2011, 36, (6), 4143 LINK
  34. 34.
    M. Tavakkoli, N. Holmberg, R. Kronberg, H. Jiang, J. Sainio, E. I. Kauppinen, T. Kallio and K. Laasonen, ACS Catal., 2017, 7, (5), 3121 LINK
  35. 35.
    T. Rajala, R. Kronberg, R. Backhouse, M. E. M. Buan, M. Tripathi, A. Zitolo, H. Jiang, K. Laasonen, T. Susi, F. Jaouen and T. Kallio, Appl. Catal. B: Environ., 2020, 265, 118582 LINK
  36. 36.
    W. Sheng, H. A. Gasteiger and Y. Shao-Horn, J. Electrochem. Soc., 2010, 157, (11), B1529 LINK
  37. 37.
    C. M. Zalitis, D. Kramer and A. R. Kucernak, Phys. Chem. Chem. Phys., 2013, 15, (12), 4329 LINK
  38. 38.
    E. Price, Johnson Matthey Technol. Rev., 2017, 61, (1), 47 LINK
  39. 39.
    P. Trinke, B. Bensmann and R. Hanke-Rauschenbach, Electrochem. Commun., 2017, 82, 98 LINK
  40. 40.
    M. Chandesris, V. Médeau, N. Guillet, S. Chelghoum, D. Thoby and F. Fouda-Onana, Int. J. Hydrogen Energy, 2015, 40, (3), 1353 LINK
  41. 41.
    A. A. Franco and M. Gerard, J. Electrochem. Soc., 2008, 155, (4), B367 LINK
  42. 42.
    X. Chen and S. S. Mao, Chem. Rev., 2007, 107, (7), 2891 LINK
  43. 43.
    Y. Shi, L. Guo, Z. Lu, Z. Wang, Y. Gan, C. Guo, H. Tan and C. Yan, Energy Technol., 2019, 7, (5), 1800781 LINK
  44. 44.
    X. Wang, X. Yuan, X. Liu, W. Dong, C. Dong, M. Lou, J. Li, T. Lin and F. Huang, J. Alloys Compd., 2017, 701, 669 LINK
  45. 45.
    F. Alcaide, R. V. Genova, G. Álvarez, H.-J. Grande, Ó. Miguel and P. L. Cabot, Int. J. Hydrogen Energy, 2020, 45, (40), 20605 LINK
  46. 46.
    G. Shi, H. Yano, D. A. Tryk, S. Nohara and H. Uchida, Phys. Chem. Chem. Phys., 2019, 21, (6), 2861 LINK
  47. 47.
    C. Li and J.-B. Baek, ACS Omega, 2020, 5, (1), 31 LINK
  48. 48.
    N. Cheng, S. Stambula, D. Wang, M. N. Banis, J. Liu, A. Riese, B. Xiao, R. Li, T.-K. Sham, L.-M. Liu, G. A. Botton and X. Sun, Nat. Commun., 2016, 7, 13638 LINK
  49. 49.
    E. Fabbri and T. J. Schmidt, ACS Catal., 2018, 8, (10), 9765 LINK
  50. 50.
    N.-T. Suen, S.-F. Hung, Q. Quan, N. Zhang, Y.-J. Xu and H. M. Chen, Chem. Soc. Rev., 2017, 46, (2), 337 LINK
  51. 51.
    S. Trasatti, Electrochim. Acta, 1984, 29, (11), 1503 LINK
  52. 52.
    S. Park, Y. Shao, J. Liu and Y. Wang, Energy Environ. Sci., 2012, 5, (11), 9331 LINK
  53. 53.
    S. Cherevko, S. Geiger, O. Kasian, N. Kulyk, J.-P. Grote, A. Savan, B. R. Shrestha, S. Merzlikin, B. Breitbach, A. Ludwig and K. J. J. Mayrhofer, Catal. Today, 2016, 262, 170 LINK
  54. 54.
    M. Bernt, A. Hartig-Weiß, M. F. Tovini, H. A. El-Sayed, C. Schramm, J. Schröter, C. Gebauer and H. A. Gasteiger, Chem. Ing. Tech., 2020, 92, (1–2), 31 LINK
  55. 55.
    C. Iwakura, K. Hirao and H. Tamura, Electrochim. Acta, 1977, 22, (4), 329 LINK
  56. 56.
    E. A. Paoli, F. Masini, R. Frydendal, D. Deiana, C. Schlaup, M. Malizia, T. W. Hansen, S. Horch, I. E. L. Stephens and I. Chorkendorff, Chem. Sci., 2015, 6, (1), 190 LINK
  57. 57.
    M. Escudero-Escribano, A. F. Pedersen, E. A. Paoli, R. Frydendal, D. Friebel, P. Malacrida, J. Rossmeisl, I. E. L. Stephens and I. Chorkendorff, J. Phys. Chem. B, 2018, 122, (2), 947 LINK
  58. 58.
    N. Danilovic, R. Subbaraman, K.-C. Chang, S. H. Chang, Y. J. Kang, J. Snyder, A. P. Paulikas, D. Strmcnik, Y.-T. Kim, D. Myers, V. R. Stamenkovic and N. M. Markovic, J. Phys. Chem. Lett., 2014, 5, (14), 2427 LINK
  59. 59.
    R. Kötz and S. Stucki, Electrochim. Acta, 1986, 31, (10), 1311 LINK
  60. 60.
    V. A. Saveleva, L. Wang, O. Kasian, M. Batuk, J. Hadermann, J.-J. Gallet, F. Bournel, N. Alonso-Vante, G. Ozouf, C. Beauger, K. J. J. Mayrhofer, S. Cherevko, A. S. Gago, K. A. Friedrich, S. Zafeiratos and E. R. Savinova, ACS Catal., 2020, 10, (4), 2508 LINK
  61. 61.
    K. E. Ayers, J. N. Renner, N. Danilovic, J. X. Wang, Y. Zhang, R. Maric and H. Yu, Catal. Today, 2016, 262, 121 LINK
  62. 62.
    X. Xia, L. Figueroa-Cosme, J. Tao, H.-C. Peng, G. Niu, Y. Zhu and Y. Xia, J. Am. Chem. Soc., 2014, 136, (31), 10878 LINK
  63. 63.
    S. Siracusano, V. Baglio, S. A. Grigoriev, L. Merlo, V. N. Fateev and A. S. Aricò, J. Power Sources, 2017, 366, 105 LINK
  64. 64.
    B. M. Tackett, W. Sheng, S. Kattel, S. Yao, B. Yan, K. A. Kuttiyiel, Q. Wu and J. G. Chen, ACS Catal., 2018, 8, (3), 2615 LINK
  65. 65.
    H. N. Nong, H.-S. Oh, T. Reier, E. Willinger, M.-G. Willinger, V. Petkov, D. Teschner and P. Strasser, Angew. Chem. Int. Ed., 2015, 54, (10), 2975 LINK
  66. 66.
    G. Jiang, H. Yu, Y. Li, D. Yao, J. Chi, S. Sun and Z. Shao, ACS Appl. Mater. Interfaces, 2021, 13, (13), 15073 LINK
  67. 67.
    K. C. Neyerlin, G. Bugosh, R. Forgie, Z. Liu and P. Strasser, J. Electrochem. Soc., 2009, 156, (3), B363 LINK
  68. 68.
    S. Siracusano, N. Van Dijk, E. Payne-Johnson, V. Baglio and A. S. Aricò, Appl. Catal. B: Environ., 2015, 164, 488 LINK
  69. 69.
    S. Siracusano, S. Trocino, N. Briguglio, F. Pantò and A. S. Aricò, J. Power Sources, 2020, 468, 228390 LINK
  70. 70.
    L. Wang, V. A. Saveleva, S. Zafeiratos, E. R. Savinova, P. Lettenmeier, P. Gazdzicki, A. S. Gago and K. A. Friedrich, Nano Energy, 2017, 34, 385 LINK
  71. 71.
    K. Kadakia, M. K. Datta, O. I. Velikokhatnyi, P. Jampani, S. K. Park, P. Saha, J. A. Poston, A. Manivannan and P. N. Kumta, Int. J. Hydrogen Energy, 2012, 37, (4), 3001 LINK
  72. 72.
    I. C. Man, H.-Y. Su, F. Calle-Vallejo, H. A. Hansen, J. I. Martínez, N. G. Inoglu, J. Kitchin, T. F. Jaramillo, J. K. Nørskov and J. Rossmeisl, ChemCatChem, 2011, 3, (7), 1159 LINK
  73. 73.
    A. Eftekhari, Mater. Today Energy, 2017, 5, 37 LINK
  74. 74.
    J. Rossmeisl, Z.-W. Qu, H. Zhu, G.-J. Kroes and J. K. Nørskov, J. Electroanal. Chem., 2007, 607, (1–2), 83 LINK
  75. 75.
    M. T. M. Koper, J. Electroanal. Chem., 2011, 660, (2), 254 LINK
  76. 76.
    R. Tang, Y. Nie, J. K. Kawasaki, D.-Y. Kuo, G. Petretto, G. Hautier, G.-M. Rignanese, K. M. Shen, D. G. Schlom and J. Suntivich, J. Mater. Chem. A, 2016, 4, (18), 6831 LINK
  77. 77.
    L. Yang, G. Yu, X. Ai, W. Yan, H. Duan, W. Chen, X. Li, T. Wang, C. Zhang, X. Huang, J.-S. Chen and X. Zou, Nat. Commun., 2018, 9, 5236 LINK
  78. 78.
    Z.-X. Lu, Y. Shi, P. Gupta, X. Min, H. Tan, Z.-D. Wang, C. Guo, Z. Zou, H. Yang, S. Mukerjee and C.-F. Yan, Electrochim. Acta, 2020, 348, 136302 LINK
  79. 79.
    Q. Shi, C. Zhu, D. Du, J. Wang, H. Xia, M. H. Engelhard, S. Feng and Y. Lin, J. Mater. Chem. A, 2018, 6, (19), 8855 LINK
  80. 80.
    C. Zhao, H. Yu, Y. Li, X. Li, L. Ding and L. Fan, J. Electroanal. Chem., 2013, 688, 269 LINK
  81. 81.
    K. A. Lewinski, D. van der Vliet and S. M. Luopa, ECS Trans., 2015, 69, (17), 893 LINK
  82. 82.
    R. T. Atanasoski, L. L. Atanasoska, D. A. Cullen, G. M. Haugen, K. L. More and G. D. Vernstrom, Electrocatalysis, 2012, 3, (3–4), 284 LINK
  83. 83.
    A. W. Jensen, G. W. Sievers, K. D. Jensen, J. Quinson, J. A. Arminio-Ravelo, V. Brüser, M. Arenz and M. Escudero-Escribano, J. Mater. Chem. A, 2020, 8, (3), 1066 LINK
  84. 84.
    G. Mirshekari, R. Ouimet, Z. Zeng, H. Yu, S. Bliznakov, L. Bonville, A. Niedzwiecki, C. Capuano, K. Ayers and R. Maric, Int. J. Hydrogen Energy, 2021, 46, (2), 1526 LINK
  85. 85.
    H.-S. Oh, H. N. Nong, T. Reier, M. Gliech and P. Strasser, Chem. Sci., 2015, 6, (6), 3321 LINK
  86. 86.
    L. Wang, P. Lettenmeier, U. Golla-Schindler, P. Gazdzicki, N. A. Cañas, T. Morawietz, R. Hiesgen, S. S. Hosseiny, A. S. Gago and K. A. Friedrich, Phys. Chem. Chem. Phys., 2016, 18, (6), 4487 LINK
  87. 87.
    L. Solà-Hernández, F. Claudel, F. Maillard and C. Beauger, Int. J. Hydrogen Energy, 2019, 44, (45), 24331 LINK
  88. 88.
    A. B. Jorge, I. Dedigama, T. S. Miller, P. Shearing, D. J. L. Brett and P. F. McMillan, Nanomaterials, 2018, 8, (6), 432 LINK
  89. 89.
    R. V. Genova-Koleva, F. Alcaide, G. Álvarez, P. L. Cabot, H.-J. Grande, M. V. Martínez-Huerta and O. Miguel, J. Energy Chem., 2019, 34, 227 LINK
  90. 90.
    Q. Xue, W. Gao, J. Zhu, R. Peng, Q. Xu, P. Chen and Y. Chen, J. Colloid Interface Sci., 2018, 529, 325 LINK
  91. 91.
    R. Badam, M. Hara, H.-H. Huang and M. Yoshimura, Int. J. Hydrogen Energy, 2018, 43, (39), 18095 LINK
  92. 92.
    R. E. Fuentes, J. Farell and J. W. Weidner, Electrochem. Solid-State Lett., 2011, 14, (3), E5 LINK
  93. 93.
    M. García-Mota, A. Vojvodic, H. Metiu, I. C. Man, H.-Y. Su, J. Rossmeisl and J. K. Nørskov, ChemCatChem, 2011, 3, (10), 1607 LINK
  94. 94.
    M. Aizawa, S. Lee and S. L. Anderson, Surf. Sci., 2003, 542, (3), 253 LINK
  95. 95.
    F. C. Walsh and R. G. A. Wills, Electrochim. Acta, 2010, 55, (22), 6342 LINK
  96. 96.
    S.-S. Huang, Y.-H. Lin, W. Chuang, P.-S. Shao, C.-H. Chuang, J.-F. Lee, M.-L. Lu, Y.-T. Weng and N.-L. Wu, ACS Sustain. Chem. Eng., 2018, 6, (3), 3162 LINK
  97. 97.
    K. Huang, Y. Li and Y. Xing, J. Mater. Res., 2013, 28, (3), 454 LINK
  98. 98.
    A. Kitada, G. Hasegawa, Y. Kobayashi, K. Kanamori, K. Nakanishi and H. Kageyama, J. Am. Chem. Soc., 2012, 134, (26), 10894 LINK
  99. 99.
    M. P. Gurrola, J. Gutiérrez, S. Rivas, M. Guerra-Balcázar, J. Ledesma-García and L. G. Arriaga, Int. J. Hydrogen Energy, 2014, 39, (29), 16763 LINK
  100. 100.
    S.-B. Han, Y.-H. Mo, Y.-S. Lee, S.-G. Lee, D.-H. Park and K.-W. Park, Int. J. Hydrogen Energy, 2020, 45, (3), 1409 LINK
  101. 101.
    S. Geiger, O. Kasian, A. M. Mingers, K. J. J. Mayrhofer and S. Cherevko, Sci. Rep., 2017, 7, 4595 LINK
  102. 102.
    P. Mazúr, J. Polonský, M. Paidar and K. Bouzek, Int. J. Hydrogen Energy, 2012, 37, (17), 12081 LINK
  103. 103.
    Y.-C. Nah, I. Paramasivam and P. Schmuki, ChemPhysChem, 2010, 11, (13), 2698 LINK
  104. 104.
    G. Garcia-Belmonte, V. Kytin, T. Dittrlch and J. Bisquert, J. Appl. Phys., 2003, 94, (8), 5261 LINK
  105. 105.
    C. Rozain, E. Mayousse, N. Guillet and P. Millet, Appl. Catal. B: Environ., 2016, 182, 123 LINK
  106. 106.
    J. Cheng, J. Yang, S. Kitano, G. Juhasz, M. Higashi, M. Sadakiyo, K. Kato, S. Yoshioka, T. Sugiyama, M. Yamauchi and N. Nakashima, ACS Catal., 2019, 9, (8), 6974 LINK
  107. 107.
    A. Weiß, A. Siebel, M. Bernt, T.-H. Shen, V. Tileli and H. A. Gasteiger, J. Electrochem. Soc., 2019, 166, (8), F487 LINK
  108. 108.
    C. Hao, H. Lv, Q. Zhao, B. Li, C. Zhang, C. Mi, Y. Song and J. Ma, Int. J. Hydrogen Energy, 2017, 42, (15), 9384 LINK
  109. 109.
    C. Hao, H. Lv, C. Mi, Y. Song and J. Ma, ACS Sustain. Chem. Eng., 2016, 4, (3), 746 LINK
  110. 110.
    H. Lv, S. Wang, C. Hao, W. Zhou, J. Li, M. Xue and C. Zhang, ChemCatChem, 2019, 11, (10), 2511 LINK
  111. 111.
    H. Lv, G. Zhang, C. Hao, C. Mi, W. Zhou, D. Yang, B. Li and C. Zhang, RSC Adv., 2017, 7, (64), 40427 LINK
  112. 112.
    H. Lv, J. Zuo, W. Zhou, X. Shen, B. Li, D. Yang, Y. Liu, L. Jin and C. Zhang, J. Electroanal. Chem., 2019, 833, 471 LINK
  113. 113.
    W. Hu, S. Chen and Q. Xia, Int. J. Hydrogen Energy, 2014, 39, (13), 6967 LINK
  114. 114.
    S. Siracusano, V. Baglio, C. D’Urso, V. Antonucci and A. S. Aricò, Electrochim. Acta, 2009, 54, (26), 6292 LINK
  115. 115.
    G. Liu, J. Xu, Y. Wang and X. Wang, J. Mater. Chem. A, 2015, 3, (41), 20791 LINK
  116. 116.
    L. Wang, F. Song, G. Ozouf, D. Geiger, T. Morawietz, M. Handl, P. Gazdzicki, C. Beauger, U. Kaiser, R. Hiesgen, A. S. Gago and K. A. Friedrich, J. Mater. Chem. A, 2017, 5, (7), 3172 LINK
  117. 117.
    C. Spöri, J. T. H. Kwan, A. Bonakdarpour, D. P. Wilkinson and P. Strasser, Angew. Chem. Int. Ed., 2017, 56, (22), 5994 LINK
  118. 118.
    S. Wang, A. Lu and C.-J. Zhong, Nano Converg., 2021, 8, 4 LINK
  119. 119.
    Z. Chen, L. Guo, L. Pan, T. Yan, Z. He, Y. Li, C. Shi, Z.-F. Huang, X. Zhang and J.-J. Zou, Adv. Energy Mater., 2022, 12, (14), 2103670 LINK

The Authors

Pere L. Cabot defended his PhD in 1984 at the University of Barcelona (UB), Spain, and is full Professor of the Department of Materials Science and Physical Chemistry (Section of Physical Chemistry) of the UB since 2003. His current research topic is electrocatalysis in fuel cell and electrolysers, with special interest in polymetallic nanostructures and catalysts supports. He has participated in 50 competitive research projects, 31 contracts with companies and published 170 research papers, three international patents, 23 books and book chapters and about 200 meeting presentations and invited lectures. He has also received three awards from private companies, related to research, development and innovation.

Maria Victoria Martínez Huerta has held a Tenured Scientist position at the Institute of Catalysis and Petrochemistry (ICP) of the Spanish Council for Scientific Research (CSIC) since 2010 and is the head of the Electrocatalysis for Energy and the Environment Group. Her research activity is dedicated to the development of electrocatalysts that improve the activity and stability of electrodes in electrochemical devices for storage and conversion of clean energy, mainly in those applications that use hydrogen as an energy carrier such as fuel cells and electrolysers. She has participated in 39 competitive research projects and published 89 research papers (indexed in Web of Science).

Francisco Alcaide holds a PhD in Chemistry (Physical Chemistry) from the University of Barcelona (2002). He has more than 25 years of experience in electrochemical technologies, especially in fuel cells and hydrogen. He has participated in or led about 50 national, European and international research, development and innovation projects and contracts with companies in technology transfer and innovation. He serves as independent expert and advisor for several national, international and European Commission public bodies. His research interests range from electrodics and electrocatalysis for clean energy and decarbonisation to batteries and water treatment. Alcaide currently works as Principal Investigator and Project manager at CIDETEC, Spain.

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