A simple explanation of the way the batteries that we use in our laptop computers, mobile phones and mp3 players work.
With some understanding of oxidation and reduction reactions and of electrochemistry we can appreciate how the batteries that we use everyday produce electricity. Batteries contain chemicals, some of them hazardous, which is why we should be careful to recycle them.
The chemicals in the battery (Dell latitude d505 battery info) react together in a redox reaction to produce electrons. These electrons are made available so that when a circuit is attached to both terminals of the battery, electricity will flow. Our question needs to be: what types of reactions produce electrons and how are they contained in a way which will make them useful?
A battery or cell is made up of pairs of compartments. The compartments are kept apart from each other but there is an electrical connection between them. At one electrode (the anode) an oxidation reaction can occur and electrons made available. This will not happen unless the electrode can take the electrons by pumping them through the circuit. At the other electrode (the cathode) a reduction reaction can occur if free electrons are available. These free electrons can come from the anode to the cathode through the electrical circuit.
In the lab a simple experiment can be set up to demonstrate what is going on. An electrode is placed in a beaker containing a solution of silver nitrate and a piece of copper metal is used as an electrode in a beaker containing copper nitrate. The two beakers are connected with a “salt bridge” which can be a piece of filter paper soaked in another solution. When the two electrodes are connected via a bulb, the bulb lights up, the copper electrode is eaten away and the other electrode becomes covered with silver.
What is happening? Well, at the copper electrode the copper is oxidised to copper ions, and electrons are released into the circuit. The electrons are taken to the other electrode where they are taken up by silver ions in the solution to make silver metal. This is a very simple cell and other reactions are used in other types of cells.
Lead-Acid Batteries in Cars
The chemicals used in batteries depend on the purpose of the battery (Dell studio 1735 Battery) and the size required for the purpose. Car batteries contain sulphuric acid as the electrolyte in connected compartments with electrodes of lead and lead dioxide in different compartments. The lead combines with the sulphate ions in the acid to form lead sulphate and an electron is released to the circuit. At the other electrode the electron is used by the lead dioxide in a reaction with the hydrogen and sulphate ions in the acid to form lead sulphate and water. This reaction is reversible, so applying an electric current to the battery will recharge it.
In solid batteries the electrolyte is a paste surrounding the electrodes which react until there is no more electrolyte in contact with the electrodes. Each reaction pair produces a fixed voltage, so differing electrodes and electrolytes can be used to produce different voltages. Also some reactions produce electrons quickly, for example batteries based on lithium and lithium chloride are used for digital cameras because they need to provide power surges to charge the flash. Other reactions are used because they have a good power-to-weight ration and so are useful in laptop computers and space applications.
The future of batteries (IBM thinkpad r51 battery) and cells looks interesting. There are more and more applications in which portable electricity supplies are necessary and new technologies are being developed in the search for these sources.