Galvanic Cells: Difference between revisions

Revision as of 23:00, 5 December 2015

Currently, it is not possible the potential difference between a strip of metal and a solution where the metal is dipped in. This arrangement is known as a galvanic cell and the situation can be represented as an oxidation-reduction (redox) reaction equation. A typical call consists of two strips of metal (one zinc and the other copper) and they are usually dipped in a solution containing salt from the corresponding metal. The two sides are separated by a porous barriers; this is because it avoids the two mixers from mixing at a fast rate but still allows the ions to diffuse from both sides. The set up can be seen in the picture.

The Main Idea

Oxidation – reduction reactions are very useful when it comes to calculating electrical energy in batteries. A basic electrochemical cell can be made with copper and zinc metals and solutions of their sulfates. During this reaction, the electrons from the zinc will be transferred to the copper through an electric conducting path (electric current). The more basic version of a galvanic cell is called an electrochemical cell; the difference is that galvanic cells can generate electric current.

Half cell reaction in its simplest form consists of an electrode (solid metal) which is immersed in a solution that has cations from the metal and anions to neutralize the charges. A galvanic cell has two-half cells; where one of the half cells is composed of metal A and the electrode of the other half-cell is composed of metal B; the equation would be:

A^n+ + ne- --> A

B^m+ + me- --> B

The two electrodes are connected with a metal wire which conduct the electrons that participate. The electrode are connected with a metal wire in order to allow the electrons to transfer and participate in the reaction.

History

Examples

External links

http://www.chem1.com/acad/webtext/elchem/ec2.html

References

http://www.sparknotes.com/chemistry/electrochemistry/galvanic/section2/page/2/

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 B^m+ + me- --> B
+The two electrodes are connected with a metal wire which conduct the electrons that participate. The electrode are connected with a metal wire in order to allow the electrons to transfer and participate in the reaction.
+[[File:galcel.jpg]]
 ==History==
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 ==Examples==
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 ===External links===
-[http://www.scientificamerican.com/article/bring-science-home-reaction-time/]
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 ==References==
-This section contains the the references you used while writing this page
+http://www.sparknotes.com/chemistry/electrochemistry/galvanic/section2/page/2/
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