A. In the 1860s, George Leclanche of France developed what would be the forerunner of the world's first widely used battery—the zinc carbon cell. The anode was a zinc- and mercury-alloyed rod (zinc, the anode in Volta's original cell, proved to be one of the best metals for the job). The cathode was a porous cup of crushed manganese dioxide and some carbon. Into the mix was inserted a carbon rod to act as the current collector. Both the anode and the cathode cup were plunged into a liquid solution of ammonium chloride, which acted as the electrolyte. The system was called a "wet cell.” Though Leclanche's cell was rugged and inexpensive, it was eventually replaced by the improved "dry cell" in the 1880s. The anode became the zinc can containing the cell, and the electrolyte became a paste rather than a liquid—basically the zinc carbon cell that is known today.
A.MBatteries may seem simple, but the delivery of packaged power is a complicated electrochemical process. Electric current in the form of electrons begins to flow in the external circuit when the device—a light bulb for example—is turned on. At that time, the anode material, zinc, gives up two electrons per atom in a process called oxidation, leaving unstable zinc ions behind. After the electrons do their work powering the light bulb, they re-enter the cell at the cathode, where they combine with the active material, manganese dioxide, in a process called reduction. The combined processes of oxidation and reduction couldn’t occur in a power cell without an internal way to carry electrons back to the anode, balancing the external flow of current. This process is accomplished by the movement of negatively charged hydroxide ions present in the water solution called the electrolyte. Every electron entering the cathode reacts with the manganese dioxide to form MnOO-. Then, MnOO- reacts with water from the electrolyte. In that reaction, the water splits, releasing hydroxide ions into the electrolyte and hydrogen ions that combine with MnOO- to form MnOOH. The internal circuit is completed when the hydroxide ions produced in this reaction at the cathode flow to the anode in the form of ionic current. There, they combine with unstable zinc ions, which were formed at the anode when the electrons were originally given up to the external circuit. This produces zinc oxide and water. This completes the circuit (which is necessary to have a constant flow of electricity) and powers your flashlight.
A. No, different batteries provide different lengths of life and power output depending on the type and amount of chemicals used to compose them...
A.Carefully follow instructions on your equipment regarding proper insertion of batteries, ensuring that the + (plus) and – (minus) terminals are aligned correctly. CAUTION: Some equipment using three or more batteries may appear to work properly even if one battery is inserted incorrectly; such usage may lead to battery leakage or rupture that could result in equipment damage.
A.We recommend storing batteries at room temperature in a dry environment. Extreme heat or cold reduces battery performance. You'll want to avoid putting battery-powered devices in very warm places. In addition, refrigeration is not necessary or recommended.
A.All rechargeable batteries should be recycled. Other batteries can and should be recycled as well. Refer to our Care and Disposal section to get all the details on this topic.
A. Chargers switch to a trickle charge when the normal charge is complete. You should unplug your charger when charging is complete or when it is not in use.
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