Faraday constant: Difference between revisions
imported>Paul Wormer No edit summary |
mNo edit summary |
||
| (One intermediate revision by one other user not shown) | |||
| Line 1: | Line 1: | ||
{{subpages}} | |||
In [[chemistry]] and [[physics]], the '''Faraday constant''' ''F'' is the amount of charge (in absolute value) in one mole of electrons or one mole of monovalent (singly charged) ions. Its value<ref>Obtained from [http://physics.nist.gov/cgi-bin/cuu/Value?f NIST] on December 16, 2007</ref> is | In [[chemistry]] and [[physics]], the '''Faraday constant''' ''F'' is the amount of charge (in absolute value) in one mole of electrons or one mole of monovalent (singly charged) ions. Its value<ref>Obtained from [http://physics.nist.gov/cgi-bin/cuu/Value?f NIST] on December 16, 2007</ref> is | ||
:<math> | :<math> | ||
| Line 12: | Line 13: | ||
==Reference== | ==Reference== | ||
<references /> | <references />[[Category:Suggestion Bot Tag]] | ||
[[Category: | |||
Latest revision as of 12:00, 15 August 2024
In chemistry and physics, the Faraday constant F is the amount of charge (in absolute value) in one mole of electrons or one mole of monovalent (singly charged) ions. Its value[1] is
where NA is Avogadro's constant and e is the charge of an electron.
The constant F must be carefully distinguished from the unit F (the faraday) which is a unit of capacitance.
The constant and the unit are named after the British physicist Michael Faraday.
Before electrons were discovered and a value for Avogadro's number was known, Faraday discovered (1833) that in electrolysis the amount of charge F necessary to deposit one mole of monovalent ions on an electrode (cations on the cathode, anions on the anode) is always the same, irrespective of the kind of ions. For a long time weighing the amount of silver—which in solution is the cation Ag+—deposited during electrolysis was the accepted manner of measuring electric charge and electric current.