Proton exchange membrane fuel cell

From Wikipedia, the free encyclopedia
Jump to: navigation, search
Diagram of a PEM fuel cell

Proton exchange membrane fuel cells, also known as polymer electrolyte membrane (PEM) fuel cells (PEMFC), are a type of fuel cell being developed for transport applications as well as for stationary fuel cell applications and portable fuel cell applications. Their distinguishing features include lower temperature/pressure ranges (50 to 100 °C[citation needed]) and a special polymer electrolyte membrane. PEMFCs operate on a similar principle to their younger sister technology PEM electrolysis. They are a leading candidate to replace the aging alkaline fuel cell technology, which was used in the Space Shuttle.[1]


PEMFCs are built out of membrane electrode assemblies (MEA) which include the electrodes, electrolyte, catalyst, and gas diffusion layers. An ink of catalyst, carbon, and electrode are sprayed or painted onto the solid electrolyte and carbon paper is hot pressed on either side to protect the inside of the cell and also act as electrodes. The pivotal part of the cell is the triple phase boundary (TPB) where the electrolyte, catalyst, and reactants mix and thus where the cell reactions actually occur.[2] Importantly, the membrane must not be electrically conductive so the half reactions do not mix. Operating temperatures above 100°C are desired so the water byproduct becomes steam and water management becomes less critical in cell design.


For more details on this topic, see Fuel cell.

A Proton exchange membrane fuel cell transforms the chemical energy liberated during the electrochemical reaction of hydrogen and oxygen to electrical energy, as opposed to the direct combustion of hydrogen and oxygen gases to produce thermal energy.

A stream of hydrogen is delivered to the anode side of the membrane electrode assembly (MEA). At the anode side it is catalytically split into protons and electrons. This oxidation half-cell reaction or Hydrogen Oxidation Reaction (HOR) is represented by:
At the Anode:

\mathrm{H}_2 \rightarrow \mathrm{2H}^+ + \mathrm{2e}^- E^o = 0\,VSHE \left ( 1 \right )

The newly formed protons permeate through the polymer electrolyte membrane to the cathode side. The electrons travel along an external load circuit to the cathode side of the MEA, thus creating the current output of the fuel cell. Meanwhile, a stream of oxygen is delivered to the cathode side of the MEA. At the cathode side oxygen molecules react with the protons permeating through the polymer electrolyte membrane and the electrons arriving through the external circuit to form water molecules. This reduction half-cell reaction or oxygen reduction reaction (ORR) is represented by:

At the cathode:

\frac{1}{2}\mathrm{O}_2 + {2H}^+ + {2e}^- \rightarrow \mathrm{H}_2\mathrm{O} E^o =1.229\,VSHE \left ( 2 \right )

Overall reaction:

\mathrm{H}_2 +  \frac{1}{2}\mathrm{O}_2 \rightarrow \mathrm{H}_2\mathrm{O} E^o = 1.229\,VSHE \left ( 3 \right )

The reversible reaction is expressed in the equation and shows the reincorporation of the hydrogen protons and electrons together with the oxygen molecule and the formation of one water molecule.

Polymer electrolyte membrane[edit]


To function, the membrane must conduct hydrogen ions (protons) but not electrons as this would in effect "short circuit" the fuel cell. The membrane must also not allow either gas to pass to the other side of the cell, a problem known as gas crossover. Finally, the membrane must be resistant to the reducing environment at the cathode as well as the harsh oxidative environment at the anode.

Splitting of the hydrogen molecule is relatively easy by using a platinum catalyst. Unfortunately however, splitting the oxygen molecule is more difficult, and this causes significant electric losses. An appropriate catalyst material for this process has not been discovered, and platinum is the best option.

A cheaper alternative to platinum is Cerium(IV) oxide catalysator used by professor Vladimír Matolín in the development of PEMFC.[3][4][5]

The PEMFC is a prime candidate for vehicle and other mobile applications of all sizes down to mobile phones, because of its compactness. However, the water management is crucial to performance: too much water will flood the membrane, too little will dry it; in both cases, power output will drop. Water management is a very difficult subject in PEM systems, primarily because water in the membrane is attracted toward the cathode of the cell through polarization. A wide variety of solutions for managing the water exist including integration of electroosmotic pumps. Furthermore, the platinum catalyst on the membrane is easily poisoned by carbon monoxide (no more than one part per million is usually acceptable) and the membrane is sensitive to things like metal ions, which can be introduced by corrosion of metallic bipolar plates, metallic components in the fuel cell system or from contaminants in the fuel/oxidant.

PEM systems that use reformed methanol were proposed, as in Daimler Chrysler Necar 5; reforming methanol, i.e. making it react to obtain hydrogen, is however a very complicated process, that requires also purification from the carbon monoxide the reaction produces. A platinum-ruthenium catalyst is necessary as some carbon monoxide will unavoidably reach the membrane. The level should not exceed 10 parts per million. Furthermore, the start-up times of such a reformer reactor are of about half an hour. Alternatively, methanol, and some other biofuels can be fed to a PEM fuel cell directly without being reformed, thus making a direct methanol fuel cell (DMFC). These devices operate with limited success.

The most commonly used membrane is Nafion by DuPont, which relies on liquid water humidification of the membrane to transport protons. This implies that it is not feasible to use temperatures above 80 to 90 °C, since the membrane would dry. Other, more recent membrane types, based on polybenzimidazole (PBI) or phosphoric acid, can reach up to 220 °C without using any water management: higher temperature allow for better efficiencies, power densities, ease of cooling (because of larger allowable temperature differences), reduced sensitivity to carbon monoxide poisoning and better controllability (because of absence of water management issues in the membrane); however, these recent types are not as common.[6] PBI can be doped with phosphoric or sulfuric acid and the conductivity scales with amount of doping and temperature.[7] At high temperatures, it is difficult to keep Nafion hydrated, but this acid doped material does not use water as a medium for proton conduction. It also exhibits better mechanical properties, higher strength, than Nafion and is cheaper. However, acid leaching is a considerable issue and processing, mixing with catalyst to form ink, has proved tricky. Aromatic polymers, such as PEEK, are far cheaper than Teflon (PTFE and backbone of Nafion) and their polar character leads to hydration that is less temperature dependent than Nafion. However, PEEK is far less ionically conductive than Nafion and thus is a less favorable electrolyte choice. [8] Recently, protic ionic liquids and protic organic ionic plastic crystals have been shown as promising alternative electrolyte materials for high temperature (100–200 °C) PEMFCs.[9] [10] [11]

Gas Diffusion Layer[edit]

The GDL electrically connects the catalyst and current collector. It must be porous, electrically conductive, and thin. The reactants must be able to reach the catalyst, but conductivity and porosity can act as opposing forces. Optimally, the GDL should be composed of about one third Nafion or 15% PTFE. The carbon particles used in the GDL can be larger than those employed in the catalyst because surface area is not the most important variable in this layer. GDL should be around 15-35µm thick to balance needed porosity with mechanical strength.[12] Often, an intermediate porous layer is added between the GDL and catalyst layer to ease the transitions between the large pores in the GDL and small porosity in the catalyst layer. Since a primary function of the GDL is to help remove water, a product, flooding can occur when water effectively blocks the GDL. This limits the reactants ability to access the catalyst and significantly decreases performance. Teflon can be coated onto the GDL to limit the possibility of flooding.[8]


The maximal theoretical efficiency applying the Gibbs free energy equation ΔG=-237.13 kJ/mol and using the Lower Heating Value (LHV) of Hydrogen (ΔH=-285.84 kJ/mol) is 83% at 298 K. \eta=\frac{\Delta G}{ \Delta H}=1-\frac{T\Delta S}{\Delta H}

The practical efficiency of a PEM's is in the range of 40–60% using the Higher Heating Value of hydrogen (HHV). Main factors that create losses are:

  • Activation losses
  • Ohmic losses
  • Mass transport losses

Catalyst research[edit]

Much of the current research on catalysts for PEM fuel cells can be classified as having one of two main objectives:

  1. to obtain higher catalytic activity than the standard carbon-supported platinum particle catalysts used in current PEM fuel cells
  2. to reduce the poisoning of PEM fuel cell catalysts by impurity gases

Examples of these two approaches are given in the following sections.

Increasing catalytic activity[edit]

As mentioned above, platinum is by far the most effective element used for PEM fuel cell catalysts, and nearly all current PEM fuel cells use platinum particles on porous carbon supports to catalyze both hydrogen oxidation and oxygen reduction. However, due to their high cost, current Pt/C catalysts are not feasible for commercialization. The U.S. Department of Energy estimates that platinum-based catalysts will need to use roughly four times less platinum than is used in current PEM fuel cell designs in order to represent a realistic alternative to internal combustion engines.[13] Consequently, one main goal of catalyst design for PEM fuel cells is to increase the catalytic activity of platinum by a factor of four so that only one-fourth as much of the precious metal is necessary to achieve similar performance.

One method of increasing the performance of platinum catalysts is to optimize the size and shape of the platinum particles. Decreasing the particles’ size alone increases the total surface area of catalyst available to participate in reactions per volume of platinum used, but recent studies have demonstrated additional ways to make further improvements to catalytic performance. For example, one study reports that high-index facets of platinum nanoparticles (that is Miller indexes with large integers, such as Pt (730)) provide a greater density of reactive sites for oxygen reduction than typical platinum nanoparticles.[14]

Since the most common and effective catalyst, platinum, is extremely expensive, alternative processing is necessary to maximize surface area and minimize loading. Deposition of nanosized Pt particles onto carbon powder (Pt/C) provides a large Pt surface area while the carbon allows for electrical connection between the catalyst and the rest of the cell. Platinum is so effective because it has high activity and bonds to the hydrogen just strongly enough to facilitate electron transfer but not inhibit the hydrogen from continuing to move around the cell. However, platinum is less active in the cathode oxygen reduction reaction. This necessitates the use of more platinum, increasing the cell’s expense and thus feasibility. Many potential catalyst choices are ruled out because of the extreme acidity of the cell.[8]

The most effective ways of achieving the nanoscale Pt on carbon powder, which is currently the best option, are through vacuum deposition, sputtering, and electrodeposition. The platinum particles are deposited onto carbon paper that is permeated with PTFE. However, there is an optimal thinness to this catalyst layer, which limits the lower cost limit. Below 4 nm, Pt will form islands on the paper, limiting its activity. Above this thickness, the Pt will coat the carbon and be an effective catalyst. To further complicate things, Nafion cannot be infiltrated beyond 10 um, so using more Pt than this is an unnecessary expense. Thus the amount and shape of the catalyst is limited by the constraints of other materials.[12]

A second method of increasing the catalytic activity of platinum is to alloy it with other metals. For example, it was recently shown that the Pt3Ni(111) surface has a higher oxygen reduction activity than pure Pt(111) by a factor of ten.[15] The authors attribute this dramatic performance increase to modifications to the electronic structure of the surface, reducing its tendency to bond to oxygen-containing ionic species present in PEM fuel cells and hence increasing the number of available sites for oxygen adsorption and reduction.

Further efficiencies can be realized using an Ultrasonic nozzle to apply the platinum catalyst to the electrolyte layer or to carbon paper under atmospheric conditions resulting in high efficiency spray.[16] Studies have shown that due to the uniform size of the droplets created by this type of spray, due to the high transfer efficiency of the technology, due to the non-clogging nature of the nozzle and finally due to the fact that the ultrasonic energy de-agglomerates the suspension just before atomization, fuel cells MEA's manufactured this way have a greater homogeneity in the final MEA, and the gas flow through the cell is more uniform, maximizing the efficiency of the platinum in the MEA.[17]

Very recently, a new class of ORR electrocatalysts have been introduced in the case of Pt-M (M-Fe[18] and Co) systems with an ordered intermetallic core encapsulated within a Pt-rich shell.[19] These intermetallic core-shell (IMCS) nanocatalysts were found to exhibit an enhanced activity and most importantly, an extended durability compared to many previous designs. While the observed enhancement in the activities is ascribed to a strained lattice, the authors report that their findings on the degradation kinetics establish that the extended catalytic durability is attributable to a sustained atomic order.

Reducing poisoning[edit]

The other popular approach to improving catalyst performance is to reduce its sensitivity to impurities in the fuel source, especially carbon monoxide (CO). Presently, pure hydrogen gas is not economical to mass-produce by electrolysis or any other means. Instead, hydrogen gas is produced by steam reforming light hydrocarbons, a process which produces a mixture of gases that also contains CO (1–3%), CO2 (19–25%), and N2 (25%).[20] Even tens of parts per million of CO can poison a pure platinum catalyst, so increasing platinum’s resistance to CO is an active area of research.

For example, one study reported that cube-shaped platinum nanoparticles with (100) faces displayed a fourfold increase in oxygen reduction activity compared to randomly faceted platinum nanoparticles of similar size.[21] The authors concluded that the (111) facets of the randomly shaped nanoparticles bonded more strongly to sulfate ions than the (100) facets, reducing the number of catalytic sites open to oxygen molecules. The nanocubes they synthesized, in contrast, had almost exclusively (100) facets, which are known to interact with sulfate more weakly. As a result, a greater fraction of the surface area of those particles was available for the reduction of oxygen, boosting the catalyst’s oxygen reduction activity.

In addition, researchers have been investigating ways of reducing the CO content of hydrogen fuel before it enters a fuel cell as a possible way to avoid poisoning the catalysts. One recent study revealed that ruthenium-platinum core–shell nanoparticles are particularly effective at oxidizing CO to form CO2, a much less harmful fuel contaminant.[22] The mechanism that produces this effect is conceptually similar to that described for Pt3Ni above: the ruthenium core of the particle alters the electronic structure of the platinum surface, rendering it better able to catalyze the oxidation of CO.

Lowering cost[edit]

One promising catalyst that uses far less expensive materials—iron, nitrogen, and carbon—has long been known to promote the necessary reactions, but at rates that are far too slow to be practical.[23] Recently, a Canadian research institute has dramatically increased the performance of this type of iron-based catalyst. Their material produces 99 A/cm3 at 0.8 volts, a key measurement of catalytic activity[citation needed]. That is 35 times better than the best nonprecious metal catalyst so far, and close to the Department of Energy's goal for fuel-cell catalysts: 130 A/cm3.[24] It also matches the performance of typical platinum catalysts. The only problem at the moment is its durability because after only 100 hours of testing the reaction rate dropped to half. Another significant source of losses is the resistance of the membrane to proton flow, which is minimized by making it as thin as possible, on the order of 50 µm.


Due to their lightweight, PEMFCs are most suited for transportation applications. PEMFCs for busses, which use compressed hydrogen for fuel, can operate at up to 40% efficiency. Generally PEMFCs are implemented on busses over smaller cars because of the available volume to house the system and store the fuel. Technical issues for transportation involve incorporation of PEMs into current vehicle technology and updating energy systems. Full fuel cell vehicles are not advantageous if hydrogen is sourced from fossil fuels; however, they become beneficial when implemented as hybrids. There is potential for PEMFCs to be used for stationary power generation, where they provide 5kW at 30% efficiency; however, they run into competition with other types of fuel cells, mainly SOFCs and MCFCs. Whereas PEMFCs generally require high purity hydrogen for operation, other fuel cell types can run on methane and are thus more flexible systems. Therefore, PEMFCs are best for small scale systems until economically scalable pure hydrogen is available. Furthermore, PEMFCs have the possibility of replacing batteries for portable electronics, though integration of the hydrogen supply is a technical challenge particularly without a convenient location to store it within the device. [25]


Before the invention of PEM fuel cells, existing fuel cell types such as solid-oxide fuel cells were only applied in extreme conditions. Such fuel cells also required very expensive materials and could only be used for stationary applications due to their size. These issues were addressed by the PEM fuel cell. The PEM fuel cell was invented in the early 1960s by Willard Thomas Grubb and Leonard Niedrach of General Electric.[26] Initially, sulfonated polystyrene membranes were used for electrolytes, but they were replaced in 1966 by Nafion ionomer, which proved to be superior in performance and durability to sulfonated polystyrene.

PEM fuel cells were used in the NASA Gemini series of spacecraft, but they were replaced by Alkaline fuel cells in the Apollo program and in the Space shuttle.

Parallel with Pratt and Whitney Aircraft, General Electric developed the first proton exchange membrane fuel cells (PEMFCs) for the Gemini space missions in the early 1960s. The first mission to use PEMFCs was Gemini V. However, the Apollo space missions and subsequent Apollo-Soyuz, Skylab and Space Shuttle missions used fuel cells based on Bacon's design, developed by Pratt and Whitney Aircraft.

Extremely expensive materials were used and the fuel cells required very pure hydrogen and oxygen. Early fuel cells tended to require inconveniently high operating temperatures that were a problem in many applications. However, fuel cells were seen to be desirable due to the large amounts of fuel available (hydrogen and oxygen).[citation needed]

Despite their success in space programs, fuel cell systems were limited to space missions and other special applications, where high cost could be tolerated. It was not until the late 1980s and early 1990s that fuel cells became a real option for wider application base. Several pivotal innovations, such as low platinum catalyst loading and thin film electrodes, drove the cost of fuel cells down, making development of PEMFC systems more realistic.[27] However, there is significant debate as to whether hydrogen fuel cells will be a realistic technology for use in automobiles or other vehicles. (See hydrogen economy.)

See also[edit]


  1. ^ Loyselle, Patricia; Prokopius, Kevin. "Teledyne Energy Systems, Inc., Proton Exchange Member (PEM) Fuel Cell Engineering Model Powerplant. Test Report: Initial Benchmark Tests in the Original Orientation". NASA. Glenn Research Center. Retrieved 15 September 2011. 
  2. ^ [Millington, Ben, Shangfeng Du, and Bruno G. Pollet. "The Effect of Materials on Proton Exchange Membrane Fuel Cell Electrode Performance." Journal of Power Sources 196.21 (2011): 9013-017. Web.].
  3. ^;jsessionid=CE66F4A7484F5D40CBD6FDEC51358F2C?rowId=GAP204%2F10%2F1169
  4. ^
  5. ^
  6. ^ Lee, J. S. et al. (2006). "Polymer electrolyte membranes for fuel cells". Journal of Industrial and Engineering Chemistry 12: 175–183. 
  7. ^ [Wainright, J. S. "Acid-Doped Polybenzimidazoles: A New Polymer Electrolyte." Journal of The Electrochemical Society 142.7 (1995): L121. Web.].
  8. ^ a b c [O'Hayre, Ryan P. Fuel Cell Fundamentals. Hoboken, NJ: John Wiley & Sons, 2006. Print.].
  9. ^ Jiangshui Luo, Jin Hu, Wolfgang Saak, Rüdiger Beckhaus, Gunther Wittstock, Ivo F. J. Vankelecom, Carsten Agert and Olaf Conrad (2011). "Protic ionic liquid and ionic melts prepared from methanesulfonic acid and 1H-1,2,4-triazole as high temperature PEMFC electrolytes". Journal of Materials Chemistry 21: 10426-10436. doi:10.1039/C0JM04306K. 
  10. ^ Jiangshui Luo, Annemette H. Jensen, Neil R. Brooks, Jeroen Sniekers, Martin Knipper, David Aili, Qingfeng Li, Bram Vanroy, Michael Wübbenhorst, Feng Yan, Luc Van Meervelt, Zhigang Shao, Jianhua Fang, Zheng-Hong Luo, Dirk E. De Vos, Koen Binnemans and Jan Fransaer (2015). "1,2,4-Triazolium perfluorobutanesulfonate as an archetypal pure protic organic ionic plastic crystal electrolyte for all-solid-state fuel cells". Energy & Environmental Science 8. doi:10.1039/C4EE02280G. 
  11. ^ Jiangshui Luo, Olaf Conrad and Ivo F. J. Vankelecom (2013). "Imidazolium methanesulfonate as a high temperature proton conductor". Journal of Materials Chemistry A 1. doi:10.1039/C2TA00713D. 
  12. ^ a b [Litster, S., and G. Mclean. "PEM Fuel Cell Electrodes." Journal of Power Sources 130.1-2 (2004): 61-76. Web.].
  13. ^ Hydrogen, Fuel Cells & Infrastructure Technologies Program Multi-Year Research, Development and Demonstration Plan, U.S. Department of Energy, October 2007.
  14. ^ N. Tian, Z.-Y. Zhou, S.-G. Sun, Y. Ding, Z. L. Wang (2007). "Synthesis of tetrahexahedral platinum nanocrystals with high-index facets and high electro-oxidation activity". Science 316 (5825): 732–735. doi:10.1126/science.1140484. PMID 17478717. 
  15. ^ V. R. Stamenkovic, B. Fowler, B. S. Mun, G. Wang, P. N. Ross, C. A. Lucas, N. M. Marković. Activity on Pt3Ni(111) via increased surface site availability (2007). "Improved Oxygen Reduction Activity on Pt3Ni(111) via Increased Surface Site Availability". Science 315 (5811): 493–497. doi:10.1126/science.1135941. PMID 17218494. 
  16. ^ Koraishy, Babar (2009). "Manufacturing of membrane electrode assemblies for fuel cells". 6.2.1: Singapore University of Technology and Design. p. 9. 
  18. ^ Sagar Prabhudev, Matthieu Bugnet, Christina Bock and Gianluigi Botton (2013). "Strained Lattice with Persistent Atomic Order in Pt3Fe2 Intermetallic Core–Shell Nanocatalysts". ACS Nano 7 (7): 6103–6110. doi:10.1021/nn4019009. PMID 23773037. 
  19. ^ Minna Cao, Dongshuang Wu and Rong Cao (2014). "Recent Advances in the Stabilization of Platinum Electrocatalysts for Fuel-Cell Reactions". ChemCatChem 1 (1): 26–45. doi:10.1002/cctc.201300647. 
  20. ^ G. Hoogers (2003). Fuel Cell Technology Handbook. Boca Raton, FL: CRC Press. pp. 6–3. ISBN 0-8493-0877-1. 
  21. ^ C. Wang, H. Daimon, T. Onodera, T. Koda, S. Sun. A general approach to the size- and shape-controlled synthesis of platinum nanoparticles and their catalytic reduction of oxygen (2008). "A General Approach to the Size- and Shape-Controlled Synthesis of Platinum Nanoparticles and Their Catalytic Reduction of Oxygen". Angewandte Chemie International Edition 47 (19): 3588–3591. doi:10.1002/anie.200800073. PMID 18399516. 
  22. ^ S. Alayoglu, A. U. Nilekar, M. Mavrikakis, B. Eichhorn. Ru–Pt core–shell nanoparticles for preferential oxidation of carbon monoxide in hydrogen (2008). "Ru–Pt core–shell nanoparticles for preferential oxidation of carbon monoxide in hydrogen". Nature Materials 7 (4): 333–338. doi:10.1038/nmat2156. PMID 18345004. 
  23. ^ Bullis, Kevin. (2009-04-02) A Catalyst for Cheaper Fuel Cells. Retrieved on 2013-04-19.
  24. ^ U.S. Department of Energy, Technical Plan: Fuel Cells, 2007.
  25. ^ [ Wee, Jung-Ho. "Applications of Proton Exchange Membrane Fuel Cell Systems." Renewable and Sustainable Energy Reviews 11.8 (2007): 1720-738. Web.]
  26. ^ PEM Fuel Cells. Retrieved on 2013-04-19.
  27. ^ Eberle, Ulrich; Mueller, Bernd; von Helmolt, Rittmar (2012-07-15). "Fuel cell electric vehicles and hydrogen infrastructure: status 2012". Royal Society of Chemistry. Retrieved 2013-01-08.