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2. Zinc–carbon battery - Wikipedia

   en.wikipedia.org/wiki/Zinc–carbon_battery

   In Europe, battery disposal is controlled by the WEEE Directive and Battery Directive regulations, and as such zinc–carbon batteries must not be thrown out with domestic waste. In the EU, most stores that sell batteries are required by law to accept old batteries for recycling .

3. Nickel–zinc battery - Wikipedia

   en.wikipedia.org/wiki/Nickel–zinc_battery

   Nickel–zinc batteries have a charge–discharge curve similar to 1.2 V NiCd or NiMH cells, but with a higher 1.6 V nominal voltage. [5]Nickel–zinc batteries perform well in high-drain applications, and may have the potential to replace lead–acid batteries because of their higher energy-to-mass ratio and higher power-to-mass ratio – as little as 25% of the mass for the same power. [6]

4. Rechargeable battery - Wikipedia

   en.wikipedia.org/wiki/Rechargeable_battery

   Battery manufacturers' technical notes often refer to voltage per cell (VPC) for the individual cells that make up the battery. For example, to charge a 12 V lead-acid battery (containing 6 cells of 2 V each) at 2.3 VPC requires a voltage of 13.8 V across the battery's terminals.

5. Battery eliminator circuit - Wikipedia

   en.wikipedia.org/wiki/Battery_eliminator_circuit

   In battery-powered equipment, a battery eliminator circuit (BEC) is an electronic voltage regulator used to power a subsystem at a different voltage without the need for a supplemental battery. BECs are commonly used in radio-controlled models , which need separate voltages to power the motor and the R/C equipment.

6. Battery room - Wikipedia

   en.wikipedia.org/wiki/Battery_room

   Batteries often used in battery rooms are the flooded lead-acid battery, the valve regulated lead-acid battery or the nickel–cadmium battery. Batteries are installed in groups. Several batteries are wired together in a series circuit forming a group providing DC electric power at 12, 24, 48 or 60 volts (or higher).

7. History of the battery - Wikipedia

   en.wikipedia.org/wiki/History_of_the_battery

   A lead-acid cell consists of a lead anode and a lead dioxide cathode immersed in sulfuric acid. Both electrodes react with the acid to produce lead sulfate, but the reaction at the lead anode releases electrons whilst the reaction at the lead dioxide consumes them, thus producing a current. These chemical reactions can be reversed by passing a ...