Batteries

A battery, also called an electric cell, is basically an electric cell that converts chemical energy into electrical energy or electricity as we call it. All cells consist of a liquid, paste, or solid electrolyte and a positive electrode, and a negative electrode. The electrolyte conducts ions; one of the electrodes will react, producing electrons, while the other electrode will accept electrons. When both electrodes are connected to an electric device that is called a load, we have an electrical current flowing where the electrons go from the positive electrode to the negative electrode.

Dry cell batteries are the most common batteries around. It looks like your typical flashlight battery that you use for a flashlight. The electrolyte, which conducts ions, is made of a mixture of ammonium chloride and zinc chloride that’s in a paste-like form. The negative electrode is made of zinc, and the positive electrode is a carbon rod surrounded by a mixture of carbon and manganese dioxide. A typical dry cell battery can produce around 1.5 volts. The dry cell battery was invented in the 1860’s by a chemist named Georges Leclanché.

Thomas Edison developed the alkaline cell battery or nickel-iron battery in the early 1900’s. It has a negative electrode that consists of iron, the positive electrode is of nickel oxide, and the electrolyte is a potassium hydroxide solution. This battery is used mainly used industries for stressful usage. The Alkaline battery has an approximate life of ten years and produces about 1.15 volts.

In 1859 a physicist named Gaston Planté invented the rechargeable battery. This type of battery works in the same sort of way as an equilibrium reaction. After the battery has been discharged, the chemicals can be regained by passing an electric current through them except, through the opposite direction that a normal cell would operate which is in some ways like a reversible type of reaction. The electrolyte is a dilute solution of sulfuric acid; the negative electrode consists of lead, and the positive electrode of lead dioxide. In operation, the negative lead electrode turns into free electrons and positive lead ions.