| specific energy | (1.692, 4.932 MJ/kg) |
|---|---|
| energy density | (5.328-35.21 MJ/L) |
| specific power | 100 W/kg[3][4] |
| Nominal cell voltage | 1.65 V |
Zinc–air batteries (non-rechargeable), and zinc–air fuel cells, (mechanically-rechargeable) are electro-chemical batteries powered by oxidizing zinc with oxygen from the air. These batteries have high energy densities and are relatively inexpensive to produce. Sizes range from very small button cells for hearing aids, larger batteries used in film cameras that previously used mercury batteries, to very large batteries used for electric vehicle propulsion.
In operation, a mass of zinc particles forms a porous anode, which is saturated with an electrolyte. Oxygen from the air reacts at the cathode and forms hydroxyl ions which migrate into the zinc paste and form zincate (Zn(OH)2−
4), releasing electrons to travel to the cathode. The zincate decays into zinc oxide and water returns to the electrolyte. The water and hydroxyls from the anode are recycled at the cathode, so the water is not consumed. The reactions produce a theoretical 1.65 volts, but this is reduced to 1.4–1.35 V in available cells.
Zinc–air batteries have some properties of fuel cells as well as batteries: the zinc is the fuel, the reaction rate can be controlled by varying the air flow, and oxidized zinc/electrolyte paste can be replaced with fresh paste. A future possibility is to power electric vehicles.
Contents |
The effect of oxygen was known early in the 19th century when wet-cell Leclanche batteries absorbed atmospheric oxygen into the carbon cathode current collector. In 1878 a porous platinized carbon air electrode was found to work as well as the manganese dioxide (MnO2) of the Leclanche cell. Commercial products began to be made on this principle in 1932 when George W. Heise and Erwin A. Schumacher of the National Carbon Company built cells,[5] treating the carbon electrodes with wax to prevent flooding. This type is still used for large zinc–air cells for navigation aids and rail transportation. However, the current capacity is low and the cells are bulky.
Large primary zinc–air cells such as the Thomas A. Edison Industries Carbonaire type were used for railway signaling, remote communication sites, and navigation buoys.These were long-duration, low-rate applications. Development in the 1970s of thin electrodes based on fuel-cell research allowed application to small button and prismatic primary cells for hearing aids, pagers, and medical devices, especially cardiac telemetry.[6]
Here are the chemical equations for the zinc–air cell[2]:
Zinc–air batteries have higher capacity-to-volume (and weight) ratio than other types of battery because air from the atmosphere is one of the battery reactants. The air is not packaged with the battery, so that a cell can use more zinc in the anode than a cell that must also contain, for example, manganese dioxide. This increases capacity for a given weight. As a specific example, a zinc–air battery of 11.6 mm diameter and height 5.4 mm from one manufacturer has a capacity of 620mAh and weight 1.9g; various silver oxide and alkaline cells of the same size supply 150-200 mAh and weigh 2.3-2.4 g.[7]
Zinc–air cells have long shelf life if sealed to keep air out; even miniature button cells can be stored for up to 3 years at room temperature with little capacity loss if their seal is not removed. Industrial cells stored in a dry state have an indefinite storage life.
The operating life of a zinc–air cell is a critical function of its interaction with its environment. The electrolyte loses more water in conditions of high temperature and low humidity. Because the potassium hydroxide electrolyte is deliquescent, in very humid conditions excess water accumulates in the cell, flooding the cathode and destroying its active properties. Potassium hydroxide also reacts with atmospheric carbon dioxide; carbonate formation eventually reduces electrolyte conductivity. Miniature cells have high self-discharge once opened to air; the cell's capacity is intended to be used within a few weeks.[6]
Because the cathode does not change properties during discharge, terminal voltage is quite stable until the cell approaches exhaustion.
Power capacity is a function of several variables: cathode area, air availability, porosity, and the catalytic value of the cathode surface. Oxygen entry into the cell must be balanced against electrolyte water loss; cathode membranes are coated with hydrophobic material (Teflon) to limit water loss. Low humidity increases water loss; if enough water is lost the cell fails. Button cells have a limited current drain; for example an IEC PR44 cell has a capacity of 600 milliamp-hours (mAh) but a maximum current of only 22 milliamps (mA). Pulse load currents can be much higher since some oxygen remains in the cell between pulses.[6]
Low temperature reduces primary cell capacity but the effect is small for low drains. A cell may deliver 80% of its capacity if discharged over 300 hours at 0 °C (32 °F), but only 20% of capacity if discharged at a 50 hour rate at that temperature. Lower temperature also reduces cell voltage.
Zinc–air batteries cannot be used in a sealed battery holder since some air must come in; the oxygen in 1 liter of air is required for every ampere-hour of capacity used.
Large zinc–air batteries, with capacities up to 2,000 ampere–hours per cell, are used to power navigation instruments and marker lights, oceanographic experiments, and railway signals.
Primary zinc–air cells are made in button format to about 1 Ah. Prismatic shapes for portable devices are manufactured with capacities between 5 and 30 Ah. Hybrid cells have manganese dioxide added to the cathodes to allow high peak currents. Button cells are highly effective, but it is difficult to extend the same construction to larger sizes due to air diffusion performance, heat dissipation, and leakage problems. Prismatic and cylindrical cell designs address these problems. Stacking prismatic cells requires air channels in the battery and may require a fan to force air through the stack.[6]
Rechargeable zinc–air cells are a difficult design problem since zinc precipitation from the water-based electrolyte must be closely controlled. The problems are dendrite formation, non-uniform zinc dissolution and limited solubility in electrolytes. Electrically reversing the reaction at a bi-functional air cathode, to liberate oxygen from discharge reaction products, is difficult; membranes tested to date have low overall efficiency. Charging voltage is much higher than discharge voltage, producing cycle energy efficiency as low as 50%. Providing charge and discharge functions by separate uni-functional cathodes, increases cell size, weight, and complexity.[6] A satisfactory electrically recharged system potentially offers low material cost and high specific energy, but none has yet reached the market.[8]
Rechargeable systems may mechanically replace the anode and electrolyte, essentially operating as a refurbishable primary cell, or may use zinc powder or other methods to replenish the reactants. Mechanically-recharged systems were investigated for military electronics uses in the 1960s because of the high energy density and easy recharging. However, primary lithium batteries offered higher discharge rates and easier handling.
Mechanical recharging systems have been researched for decades for use in electric vehicles. Some approaches use a large zinc–air battery to maintain charge on a high discharge–rate battery used for peak loads during acceleration. Zinc granules serve as the reactant. Vehicles exchange used electrolyte and depleted zinc for fresh reactants at a service station to recharge.
The term zinc–air fuel cell usually refers to a zinc–air battery in which zinc metal is added and zinc oxide is removed continuously. Zinc electrolyte paste or pellets are pushed into a chamber, and waste zinc oxide is pumped into a waste tank or bladder inside the fuel tank. Fresh zinc paste or pellets are taken from the fuel tank. The zinc oxide waste is pumped out at a refueling station for recycling. Alternatively, this term may refer to an electrochemical system in which zinc is a co-reactant assisting the reformation of hydrocarbons at the anode of a fuel cell.
Metallic zinc could be used as an alternative fuel for vehicles, either in a zinc–air battery [9] or to generate hydrogen near the point of use. Zinc's characteristics have motivated considerable interest as an energy source for electric vehicles. Gulf General Atomic demonstrated a 20 kW vehicle battery. General Motors conducted tests in the 1970s. Neither project led to a commercial product.[10]
Solid zinc cannot be moved as easily as a liquid. An alternative is to form pellets that are small enough to be pumped. Fuel cells using it would be able to quickly replace zinc-oxide with fresh zinc metal.[11] The spent material can be recycled. The zinc–air "battery" cell is a primary cell (non-rechargeable); recycling is required to reclaim the zinc; much more energy is required to reclaim the zinc than is usable in a vehicle.
One advantage of utilizing zinc–air batteries for vehicle propulsion is that the availability of zinc metal is 100 times greater than that of lithium, per unit of battery energy. Current yearly global zinc production is sufficient to produce enough Zinc-Air batteries to power over one billion electric vehicles, whereas current lithium production is only sufficient to produce ten million lithium-ion powered vehicles.[12] Approximately 35% of the world's supply, or 1.8 gigatons of zinc reserves are in the United States,[13] whereas the U.S. holds only 0.38% of known lithium reserves.[14]
Attempts to address zinc–air's limitations include[15]
Vent holes allow any pressure build-up to be released. Zinc corrosion can produce hydrogen. Manufacturers caution against hydrogen build-up in enclosed areas. A short-circuited cell gives relatively low current. Deep discharge below 0.5 V/cell may result in electrolyte leakage; there is little useful capacity below 0.9 V/cell.
Older designs used mercury amalgam amounting to about 1% of the weight of a button cell, to prevent zinc corrosion. Newer types have no added mercury. Zinc is relatively low in toxicity. Mercury-free designs require no special handling when discarded or recycled.[6]
In United States waters, environmental regulations now require proper disposal of primary batteries removed from navigation aids. Formerly, discarded zinc–air primary batteries were dropped into the water around buoys, which allowed mercury in the cells to escape to the environment.[16]
|
||||||||