Batteries: Rechargeable vs. Non-rechargeable Batteries
`Rebecca Beam, Mary Kate Wilkin, Jason Kuszynski, and Marcetta Y. Darensbourg
`Texas A&M University, College Station, TX 77843
`
`Abstract
`
`Galvanic Cells
`
`Specific Energy Comparison
`
`Batteries are used to store energy for use when needed by converting chemical energy into
`electrical energy. A simple battery is comprised of multiple cells attached in series. A cell is made
`up of three part: two electrodes (an anode and cathode) in a chemical called an electrolyte. A
`rechargeable battery is capable of reversing the chemical reaction by forcing a current in the
`opposite direction. As society has progressed, rechargeable batteries have been progressively
`replacing non-rechargeable batteries. Laptops, phones, and other electronic, all high drain
`devices, are hosts to a variety of rechargeable batteries, while non-rechargeable batteries are
`prime choice for low drain applications such as alarm clocks or radios. Non-rechargeable
`batteries are known as primary batteries and have some very important uses. Primary batteries
`are used in some pacemakers, remote controls, electronic keys and kids toys. Non Rechargeable
`batteries are often higher capacity and are easily accessible.
`
`● Spontaneous oxidation-reduction
`reaction
`● Oxidation occurs at the anode
`● Reduction occurs at the cathode
`● Electrons flow from the anode to
`the cathode.
`● A salt bridge allows for the flow of
`ions from cathode to anode
`● Since it is spontaneous, it can be
`used in rechargeable or non
`rechargeable batteries.
`
`What Are Batteries?
`
`Electrolytic Cell
`
`Rechargeable Vs. Non-rechargeable
`Batteries
`
`Non-rechargeable:
`
`Rechargeable:
`
`Both:
`
`● Irreversible
`● Galvanic
`● Lower initial
`cost
`
`● Reversible
`● Galvanic and
`Electrolytic
`● Lower cost
`over time
`
`● Chemical Energy
`↓ Electrical Energy
`● Redox Chemistry
`● Electrolyte and
`Electrode
`● Portable
`
`● Anode (-) and cathode (+) in a circuit
`● One metal compound is reduced while the other is oxidized
`● Redox reaction between metals produces an electric potential and leads to a flow of electrons
`from anode to cathode
`● Rechargeable batteries- the electron potential can be reversed by applying an external
`voltage onto the battery, resulting in a reversal of the galvanic discharge that took place
`initially.
`
`The exact energy can be calculated using the following equations:
`● E°cell = E°cathode - E°anode
`● ΔG = -nFE°cell
`
`Examples of Batteries
`
`Battery Uses
`
`Non-Rechargeable:
`● Zinc-Carbon
`● ZnCl
`● LiMnO2
`● Alkaline
`Rechargeable:
`● Lithium Ion
`● Lead-Acid
`● NiCd
`● NiMH
`
`Non-Rechargeable:
`● Alarm clocks
`● Radios
`● Pacemakers
`● Remote controls
`● Electronic keys
`● Kids toys
`
`Rechargeable:
`● Laptops
`● Cell phones
`● Portable devices
`
`● Non-spontaneous
`oxidation-reduction reaction,
`● Used in rechargeable batteries
`● Has a semipermeable
`membranes for the flow of ions.
`● Oxidation occurs at the cathode
`● Reduction occurs at the anode
`
`Zinc-Carbon Battery
`
`Pros
`● Cheap
`● Very long shelf life
`● High
`
`Cons
`● Low storage capacity.
`● Hazardous to environment when
`disposed.
`● Non-rechargeable
`
`Lithium Ion Battery
`
`Pros
`● 5% charge loss per month
`● Stores 150 watt-hours of
`electricity per 1 kg
`● High voltage
`● Rechargeable
`
`Cons
`● Expensive
`● Thermally delicate
`● Class 9 hazardous material
`
`Conclusion
`There are two types of batteries, rechargeable and non-rechargeable. Each type has its
`advantages and disadvantages for example, non rechargeable batteries typically store more
`energy however they can only be used once. Because of the differences, both batteries types
`have specific uses. Most batteries have 3 parts: the anode, cathode and electrolytic solution.
`Current flows between the anode and cathode generating voltage.
`
`Acknowledgments
`
`Special thanks is extended to Marcetta Y. Darensbourg and Zachary Martinez for your guidelines and
`support in this research.
`
`References
`
`BU-106: Advantages of Primary Batteries http://batteryuniversity.com/learn/article/primary_batteries
`(accessed Apr 10, 2017).
`Lithium Ion Battery http://www.cei.washington.edu/education/science-of-solar/battery-technology/
`(accessed Apr 10, 2017).
`American Chemical Society National Historic Chemical Landmarks. Columbia Dry Cell Battery.
`http://www.acs.org/content/acs/en/education/whatischemistry/landmarks/drycellbattery.html (accessed
`April 8, 2017).
`Helmenstine, P. D. A. M. What Is a Galvanic Cell?
`https://www.thoughtco.com/galvanic-cell-definition-604080 (accessed Apr 11, 2017).
`Shriver, D. F.; Weller, M. T.; Overton, T.; Rourke, J.; Armstrong, F. A. Inorganic chemistry; W.H. Freeman
`and Company: New York, 2014.
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