Conceivably the most popular
application for lead-acid batteries is as the power source for the starter in
an automobile. In stationary storage applications, lead-acid batteries are also
used to provide uninterruptible power supply (UPS) service to datacenters and
even island grid support for small scale distributed renewable energy
applications. There are an estimated 95,000 lead-acid battery arrays deployed
in the US at utility substations to provide blackout and black start grid
support (Eyer & Corey, 2010) . First invented in 1859 by Gaston Planté,
lead-acid batteries are the most prevalent form of energy storage today (EPRI, 2003) .
Lead-acid
batteries consist of alternating plates of lead (Pb) and lead oxide (PbO2),
that form the electrodes. The electrodes are submerged in a liquid or gel
electrolyte solution of sulfuric acid (H2SO4). During
discharge the lead anode gives up electrons that the lead oxide cathode
accepts. This creates the flow of electricity (Figure 1).
During discharge both plates begin to accumulate lead sulfate (PbSO4) (Hammack,
2012) .
Figure 1 basic diagram of a lead-acid battery during
discharge.
While charging, the electron flow is
reversed and sulfate returns to the electrolyte making it stronger and
increasing the charge of the battery (EPRI, 2003) . The overall
chemical reaction is:
![](https://blogger.googleusercontent.com/img/b/R29vZ2xl/AVvXsEhcfHlH4U5bKQczOlYv6NGHmQ8HvCcoHgB0maWhY4hVbSdrZDh4hU8kURUqPMSi8w74FW10x4MvvLNiFBr8evdn9qEb2lGkB2EMUKT89E9pMt_aFRh-yqBVLwtlW66RfEQJd5dzdikk8z5l/s1600/equation_for_lead_acid_battery.png)
The buildup of lead sulfate on the electrodes can limit the ability for the battery to recharge. For this reason lead-acid batteries to be used in deep discharge applications (common for energy storage) must be designed with larger electrodes that are spaced further apart and must also include a reservoir to capture sulfate debris
Though
lead is considered poisonous to humans, its density makes it easy to separate
from other materials when a battery is recycled. This ability to easily isolate
lead, coupled with the fact that lead-acid batteries are so pervasive, makes
lead-acid battery recycling a profitable endeavor such that 96% of all lead-acid
batteries are recycled. Even the spent electrolyte is recaptured through acid
reclamation. 60% to 80% of each new battery contains recycled lead or plastic (US EPA, 2012) .
Works Cited
Baxter, R. (2006). Energy Storage; A Nontechnical
Guide. Tulsa, Oklahoma: PennWell Corporation.
EPRI. (2003). EPRI-DOE Handbook of Energy Storage
for Transmission & Distribution Applications. Washington DC: EPRI,
Palo Alto, CA, and the U.S. Department of Energy.
Eyer, J., & Corey, G. (2010). Energy Storage
for the Electricity Grid: Benefits and Market Potential Assessment Guide.
Albuquerque, New Mexico: Sandia National Laboratories.
Hammack, B. (2012, July 3). How a Lead-Acid
Battery Works. Retrieved January 6, 2013, from Engineer Guy:
http://www.youtube.com/watch?v=rhIRD5YVNbs&feature=youtube_gdata_player
US EPA. (2012, November 19). Batteries.
Retrieved January 6, 2013, from US EPA: http://www.epa.gov/osw/conserve/materials/battery.htm
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