Wet cell 1595221 218914528 2008-06-12T19:09:21Z K Eliza Coyne 7008937 external link A '''wet cell''' is a galvanic [[electrochemical cell]] with a liquid [[electrolyte]]. A [[dry cell]], on the other hand, is a cell with a pasty electrolyte. Wet cells were a precursor to dry cells and are commonly used as a learning tool for [[electrochemistry]]. It is often built with common laboratory supplies, like [[beaker (glassware)|beakers]], for demonstrations of how electrochemical cells work. A particular type of wet cell known as a [[concentration cell]] is important in understanding [[corrosion]]. Wet cells may be [[primary cell]]s (non-rechargeable) or [[secondary cell]]s (rechargeable). While a dry cell's electrolyte is not truly completely free of moisture and must contain some moisture to function, when it was first developed it had the advantage of containing no sloshing liquid that might leak or drip out when inverted or handled roughtly, making it highly suitable for small portable electric devices. By comparison, the first wet cells were typically fragile glass containers with lead rods hanging from the open top, and needed careful handling to avoid spillage. An inverted wet cell would almost certainly leak, while a dry cell would not. Wet-cell [[Lead-acid batteries]] would not achieve the safety and portability of the dry cell, until the development of the [[Gel Battery]]. ==Primary wet cells== ===Daniell cell=== :''main article: [[Daniell cell]] The most famous wet cell is the Daniell cell, which is sometimes referred to as a crowfoot or gravity cell. The Daniell cell was developed in 1836 by the British chemist (and meteorologist) [[John Frederic Daniell]]. ===Other primary wet cells=== * [[Leclanche cell]] * [[Grove cell]] * [[Bunsen cell]] * [[Chromic acid cell]] * [[Clark cell]] * [[Weston cell]] ==Secondary wet cells== A [[Battery (electricity)|battery]] is a collection of several [[galvanic cell]]s connected in series to produce a greater [[voltage]] than a single cell could. [[Car batteries]] are wet cells and give a good example of the pros and cons of such systems. A standard 12-V car battery consists of 6 lead [[acid]] cells that each produce 2 volts. The most commonly used [[lead-acid battery]] consists of a [[lead]] metal anode and a [[lead oxide]] cathode, both of which are immersed in a solution of [[sulfuric acid]]. As seen in car batteries, a disadvantage of such a system is that it is extremely heavy. On the plus side, however, the [[redox]] reaction that occurs is readily reversible allowing it to have a long, reliable, and useful life. In a car battery, the cell is recharged by the car's [[alternator]]. ==External links== * [http://www.magnet.fsu.edu/education/tutorials/java/electricalcell/index.html Interactive Java Tutorial on a Simple Electrical Cell] National High Magnetic Field Laboratory [[Category:Electrochemistry]] [[Category:Electric batteries]]