A primary battery (non-rechargeable) often used in electronics applications requiring heavy currents for long periods of time (e.g. CD players and radios). Alkaline cells overcome some of the problems with carbon-zinc batteries by using potassium hydroxide in place of ammonium chloride in the electrolyte. Potassium hydroxide is a base or alkaline material, hence "alkaline" batteries.
Alkaline batteries have a much longer shelf life and perform better under drain and in cold weather than their carbon-zinc counterparts. They also avoid the use of the zinc-corroding ammonium ions and do not produce any gaseous products. Typically, they can deliver 50-100% more total energy than carbon-zinc batteries of the same size; hence their popularity in consumer applications.
Thursday, December 30, 2010
Alkaline Batteries.
In the simplest explanation, a battery is "Two conductors of Electricity separated by a dielectric constant" In the case of an Alkaline Battery the dielectric constant or electrolyte is Alkaline.
The alkaline battery gets its name because it has an alkaline electrolyte of potassium hydroxide although some people generalize the term alkaline battery referring to batteries of the same size and closely the same voltage, but have a different chemical makeup such as Carbon Zinc or Mercury.
The world’s energy needs are ever greater and more varied as time goes on. One source of energy has developed as a convenient way to power electronic devices, and that is the alkaline battery. Batteries are essentially small containers that hold chemicals which react to produce electricity. The alkaline battery is the most common and versatile type of battery used, and it gets its name because of the alkaline electrolyte potassium chloride, which is one of the chemicals it contains.
Each alkaline battery has two ends, or terminals -- a positive and a negative terminal. Inside the battery, a chemical reaction produces electrons, which gather at the negative terminal of the battery. However, unless the negative terminal is connected to the positive terminal, the chemical reaction stops and no more electricity is produced. This is the reason that an alkaline battery can sit in a drawer or on a shelf for a long time and still have plenty of power when it is needed. If it is not used, the battery does not wear out in a short period of time. Usually, the battery is used by connecting some sort of device to it, such as a motor, the light bulb in a flashlight, or a radio, for example. The electrons flow out of the negative terminal of the battery, through a wire to the device. There they power the device before flowing back to the positive terminal. This completes a circuit, allowing the chemical reaction to continue, and the battery to produce more electrons. When the device is switched off, the circuit is broken so that electrons can no longer flow in a complete circle. The battery then stops producing electrons, since the terminals are no longer connected.The alkaline battery is one of the more modern types of battery used, having been introduced first in the 1960s. The very first battery was created by scientist Alessandro Volta in 1800. Volta made his battery by stacking alternating layers of zinc, salt water-soaked blotting paper, and silver. The higher the stack, the higher the voltage produced by this arrangement. This type of battery was known as the voltaic pile. The modern alkaline battery still uses the same fundamental principles as the voltaic pile, namely two different types of metal, separated by a liquid which conducts electricity, with a negative and a positive terminal
.
The alkaline battery gets its name because it has an alkaline electrolyte of potassium hydroxide although some people generalize the term alkaline battery referring to batteries of the same size and closely the same voltage, but have a different chemical makeup such as Carbon Zinc or Mercury.
The world’s energy needs are ever greater and more varied as time goes on. One source of energy has developed as a convenient way to power electronic devices, and that is the alkaline battery. Batteries are essentially small containers that hold chemicals which react to produce electricity. The alkaline battery is the most common and versatile type of battery used, and it gets its name because of the alkaline electrolyte potassium chloride, which is one of the chemicals it contains.
Each alkaline battery has two ends, or terminals -- a positive and a negative terminal. Inside the battery, a chemical reaction produces electrons, which gather at the negative terminal of the battery. However, unless the negative terminal is connected to the positive terminal, the chemical reaction stops and no more electricity is produced. This is the reason that an alkaline battery can sit in a drawer or on a shelf for a long time and still have plenty of power when it is needed. If it is not used, the battery does not wear out in a short period of time. Usually, the battery is used by connecting some sort of device to it, such as a motor, the light bulb in a flashlight, or a radio, for example. The electrons flow out of the negative terminal of the battery, through a wire to the device. There they power the device before flowing back to the positive terminal. This completes a circuit, allowing the chemical reaction to continue, and the battery to produce more electrons. When the device is switched off, the circuit is broken so that electrons can no longer flow in a complete circle. The battery then stops producing electrons, since the terminals are no longer connected.The alkaline battery is one of the more modern types of battery used, having been introduced first in the 1960s. The very first battery was created by scientist Alessandro Volta in 1800. Volta made his battery by stacking alternating layers of zinc, salt water-soaked blotting paper, and silver. The higher the stack, the higher the voltage produced by this arrangement. This type of battery was known as the voltaic pile. The modern alkaline battery still uses the same fundamental principles as the voltaic pile, namely two different types of metal, separated by a liquid which conducts electricity, with a negative and a positive terminal
.
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