History Of Battery
An electrical battery is an amalgamation of single or more electronic cells, which is used to convert the hoarded energy into electrical energy. After the first invention of Voltaic pile in the year 1800 by Volta Alessandro, batteries have become the major power source for many industrial applications and household, and currently, is a multi-billion dollar industry. However, batteries might be used once, or recharged for as in standby power appliances. Miniature cells are been used to power devices like portable electronic devices and wristwatches: batteries which are larger provide standby power for computer data centers and telephone exchanges (MacDonald, 2003)
Categories and types of batteries
According to Sparks, A. and Clinton, C, (2000), batteries are categorized into two, each type with advantages and disadvantages.
Primary batteries; irreversibly convert chemical energy to electrical energy. After the initial supply of reactants become exhausted, the energy cannot be enthusiastically restored to the battery by electrical way. The widespread types of disposable batteries are alkaline batteries and zinc-carbon batteries. These have an elevated energy density than rechargeable batteries, although disposable batteries don’t perform well under high-drain applications with loads fewer than 75 ohms (75 ).
Secondary batteries; they can be recharged. This means that their chemical reactions can be reversed by supplying electrical energy to the cell, reinstating their initial means. The older form of rechargeable battery is the lead-acid battery. It’s very heavy, low manufacturing cost and has a high surge current (over approximately 10Ah). Example of a lead battery is the modern car battery; it’s very heavy and can deriver a peak current of 450 amperes. The valve regulated lead acid (VRLA) battery uses an immobilized sulfuric acid electrolyte, decreasing the possibilities of leakage and prolonging shelf life. Moreover, their electrolyte is immobilized by two means, that’s “Gel batteries” (or gel cell) and “Absorbed Glass Mat” (AGM). Other manageable rechargeable batteries are dry cell types. They are used in cell phones and laptops computers. They include nickel-cadmium (NiCd), hydride (NiMH), nickel metal and lithium (Li-ion) cells.
In times goes by, some primary batteries used, for instance, for telegraph circuits, were reinstated to maneuver by substituting the components of the battery guzzled by the chemical reaction. However, secondary batteries aren’t indefinitely rechargeable because of dissipation of the active materials, internal corrosion and loss of electrolyte. (William, 2005)
Battery cell types
There’s a lot of electrochemical cells, they depends on design chosen and chemical processes applied. The variation includes electrolytic cells, voltaic piles, galvanic cells, and flow cells.
Wet cell (flooded cell or vented cell)
It has a liquid electrolyte, used as a learning tool for electrochemistry. Wet cell might either be primary cells (non-rechargeable) or secondary cells (rechargeable). Initially all practical primary batteries like the Daniel cell were constructed as open-topped glass jar wet cells. Others are Grove cell, Chromic acid cell, Leclanche cell, Weston cell, and Clark cell.
Dry cell
It has the electrolyte immobilized as a paste, amid only sufficient moisture in the paste to permit current to flow. Unlike wet cell, the dry cell can be functioned in any random locations, and wouldn’t spill its electrolyte if overturned. Example of a dry cell is the zinc-carbon battery, which have a similar voltage with alkaline battery (1.5 volts), both uses zinc-manganese dioxide amalgamation. These batteries are known as high power batteries. (William, 2005)
Molten salt
This is a primary or secondary battery that draws on a molten salt as its electrolyte. Moreover, their power density and energy density makes them potentially constructive for electric vehicles, although they have to be cautiously insulted to preserve heat.
Reserve
This type of battery can be stored for a long duration of time and is activated when its interior parts (electrolytes) are brought together. For example, a battery for an electronic fuse can be stimulated by the impact of firing a gun, flouting a capsule of electrolyte to stimulate the battery and power the fuse’s circuits. Holding back batteries are normally designed for a short service existence (minutes or seconds) after long existence (years)
Battery cell performance
Batteries characteristics might differ over load cycle, charge cycle and over life time because of many factors including current drain, internal chemistry and temperature.
Conclusion
Battery is a combination of single or more electronic cells that are used to convert the stored energy into electrical energy. After its invention, it has become a major source of power to domestics and industrial users. There two types of batteries, that are primary (non-rechargeable) and secondary (rechargeable).
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