Metal–air electrochemical cell
A metal–air electrochemical cell is an electrochemical cell that uses an anode made from pure metal and an external cathode of ambient air, typically with an aqueous or aprotic electrolyte. During discharging of a metal–air electrochemical cell, a reduction reaction occurs in the ambient air cathode while the metal anode is oxidized. The specific capacity and energy density of metal–air electrochemical cells is higher than that of lithium-ion batteries, making them a prime candidate for use in electric vehicles. However, complications associated with the metal anodes, catalysts, and electrolytes have hindered development and implementation of metal–air batteries.
|Metal–air battery||Theoretical specific energy, Wh/kg
|Theoretical specific energy, Wh/kg
|Calculated open-circuit voltage, V|
|Tin–air at 1000 K||860||6250||0.95|
The remarkably high energy density of lithium metal (up to 3458 Wh/kg) inspired the design of lithium–air batteries. A lithium–air battery consists of a solid lithium electrode, an electrolyte surrounding this electrode, and an ambient air electrode containing oxygen. Current lithium–air batteries can be divided into four subcategories based on the electrolyte used and the subsequent electrochemical cell architecture. These electrolyte categories are aprotic, aqueous, mixed aqueous/aprotic, and solid state, all of which offer their own distinct advantages and disadvantages. Nonetheless, efficiency of lithium–air batteries is still limited by incomplete discharge at the cathode, charging overpotential exceeding discharge overpotential, and component stability. During discharge of lithium–air batteries, the superoxide ion (O2−) formed will react with the electrolyte or other cell components and will prevent the battery from being rechargeable.
Sodium–air batteries were proposed with the hopes of overcoming the battery instability associated with superoxide in lithium–air batteries. Sodium, with an energy density of 1605 Wh/kg, does not boast as high an energy density as lithium. However, it can form a stable superoxide (NaO2) as opposed to the superoxide undergoing detrimental secondary reactions. Since NaO2 will decompose reversibly to an extent back to the elemental components, this means sodium–air batteries have some intrinsic capacity to be rechargeable. Sodium–air batteries can only function with aprotic, anhydrous electrolytes. When a DMSO electrolyte was stabilized with sodium trifluoromethanesulfonimide, the highest cycling stability of a sodium–air battery was obtained (150 cycles).
Potassium–air batteries were also proposed with the hopes of overcoming the battery instability associated with superoxide in lithium–air batteries. While only two to three charge-discharge cycles have ever been achieved with potassium–air batteries, they do offer an exceptionally low overpotential difference of only 50 mV.
- No article; see also Calcium: chemical properties for some air (oxygen) reactions.
Iron–air rechargeable batteries are an attractive technology with the potential of grid-scale energy storage. The main raw-material of this technology is iron oxide (rust) which is abundant, non-toxic, inexpensive and environmentally friendly. Most of the batteries being developed right now utilize iron oxide (mostly powders) to generate/store hydrogen via the Fe/FeO reduction/oxidation (redox) reaction (Fe + H2O ⇌ FeO + H2). In conjunction with a fuel cell this enables the system to behave as a rechargeable battery creating H2O/H2 via production/consumption of electricity. Furthermore, this technology has minimal environmental impact as it could be used to store energy from intermittent solar and wind power sources, developing an energy system with low carbon dioxide emissions.
The way the system works can start by using the Fe/FeO redox reaction, then the hydrogen created during the oxidation of iron can be consumed by a fuel cell in conjunction with oxygen from the air to create electricity. When electricity must be stored, hydrogen generated from water by operating the fuel cell in reverse is consumed during the reduction of the iron oxide to metallic iron. The combination of both of these cycles is what makes the system operate as an iron–air rechargeable battery.
Limitations of this technology come from the materials used. Generally, iron oxide powder beds are selected, however, rapid sintering and pulverization of the powders limit the ability to achieve a high number of cycles resulting in a lower capacity. Other methods currently under investigation, such as 3D printing and freeze-casting, seek to enable the creation of architecture materials to allow for high surface area and volume changes during the redox reaction.
- Calculated from the specific energy density (including oxygen) value and 39.1 and 16 atomic weight data for K and O respectively for KO2.
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