Electrochemical Energy Conversion and Storage

The most important function of electrochemistry is the storage and conversion of energy.  Galvanic cell converts chemical energy to work; equivalently, an electrolytic cell converts electrical work into chemical free energy. Appliances that carry out these conversions are known as batteries. In ordinary batteries the chemical elements are contained within the device itself. If the reactants are endowed from an external source as they are consumed, the device is called a fuel cell. A secondary battery is able of being recharged; its electrode reactions can proceed in either direction. At the time of charging, electrical work is done on the cell to provide the free energy needed to force the reaction in the non-spontaneous direction. A primary battery, as exemplified by a normal flashlight battery which cannot be recharged with any efficiency, so the bulk of energy it can deliver is limited to that obtainable from the reactants that were placed in it at the time of production. Lithium batteries are the batteries that have lithium as an anode. They stand apart from other batteries in their high charge quantity (long life) and high cost per unit. Depending on the design and chemical compounds used, lithium cells can generate voltages from 1.5 V comparable to a zinc–carbon or alkaline battery to about 3.7 V. A flow battery, or redox flow battery is a type of rechargeable battery where rechargeability is provided by two chemical elements dissolved in liquids contained within the system and separated by a membrane

  • Fuel cells
  • Primary and secondary batteries
  • Lithium Batteries
  • Microbial fuel cells
  • Direct carbon fuel cells 
  • Rechargeable metal-air batteries
  • Flow batteries

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