But thank you, the video was very helpful, Thanks for the help. I am a junior in high school and this just taught me more in two minutes than my chemistry teacher did in 24 weeks!!! Pingback: How do Batteries Work? Send us a photo of what you made to editor mocomi.
Great and superrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrrr awesome shiz. This helped me a lot with the research for my science fair project. Thanks I needed this!!! At the other electrode, the electron is used by the lead dioxide in a reaction with the hydrogen and sulfate ions in the acid to form lead sulfate 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 ratio and so are useful in laptop computers and space applications. The future of batteries 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. You must be logged in to post a comment. How do Batteries Work? How does a battery produce electricity? Contents How does a battery produce electricity?
Imagine a world without batteries. Luckily, we do have batteries. Back in BC in Mesopotamia, the Parthian culture used a device known as the Baghdad battery, made of copper and iron electrodes with vinegar or citric acid. Archaeologists believe these were not actually batteries but were used primarily for religious ceremonies. The invention of the battery as we know it is credited to the Italian scientist Alessandro Volta, who put together the first battery to prove a point to another Italian scientist, Luigi Galvani.
In , Galvani had shown that the legs of frogs hanging on iron or brass hooks would twitch when touched with a probe of some other type of metal. He experimented with stacks of layers of silver and zinc interspersed with layers of cloth or paper soaked in saltwater, and found that an electric current did in fact flow through a wire applied to both ends of the pile. Volta also found that by using different metals in the pile, the amount of voltage could be increased.
He described his findings in a letter to Joseph Banks, then president of the Royal Society of London, in It was a pretty big deal Napoleon was fairly impressed! A battery is a device that stores chemical energy, and converts it to electricity. This is known as electrochemistry and the system that underpins a battery is called an electrochemical cell.
A battery can be made up of one or several like in Volta's original pile electrochemical cells. Each electrochemical cell consists of two electrodes separated by an electrolyte. So where does an electrochemical cell get its electricity from? To answer this question, we need to know what electricity is. Most simply, electricity is a type of energy produced by the flow of electrons. In an electrochemical cell, electrons are produced by a chemical reaction that happens at one electrode more about electrodes below!
To understand this properly, we need to have a closer look at the cell's components, and how they are put together. To produce a flow of electrons, you need to have somewhere for the electrons to flow from , and somewhere for the electrons to flow to. The electrons flow from one electrode called the anode or negative electrode to another electrode called the cathode the positive electrode.
These are generally different types of metals or other chemical compounds. He stacked lots of these cells together to make the total pile and crank up the voltage. But where does the anode get all these electrons from in the first place? And why are they so happy to be sent off on their merry way over to the cathode? There are a couple of chemical reactions going on that we need to understand. At the anode, the electrode reacts with the electrolyte in a reaction that produces electrons.
These electrons accumulate at the anode. Meanwhile, at the cathode, another chemical reaction occurs simultaneously that enables that electrode to accept electrons. The technical chemical term for a reaction that involves the exchange of electrons is a reduction-oxidation reaction, more commonly called a redox reaction.
The entire reaction can be split into two half-reactions, and in the case of an electrochemical cell, one half-reaction occurs at the anode, the other at the cathode. Reduction is the gain of electrons, and is what occurs at the cathode; we say that the cathode is reduced during the reaction.
Oxidation is the loss of electrons, so we say that the anode is oxidised. Each of these reactions has a particular standard potential. Standard potentials for half-reactions Below is a list of half reactions that involve the release of electrons from either a pure element or chemical compound. E 0 is measured in volts.
So, if you take lithium and fluoride, and manage to combine them to make a battery cell, you will have the highest voltage theoretically attainable for an electrochemical cell. This list also explains why in Volta's pile, the zinc was the anode, and silver the cathode: the zinc half-reaction has a lower more negative E 0 value Any two conducting materials that have reactions with different standard potentials can form an electrochemical cell, because the stronger one will be able to take electrons from the weaker one.
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