You may find the section on current in the physics tutorial helpful.
Redox reactions have many important uses. One of these is electrolysis, the conversion of electrical energy to chemical energy.
Do you remember this table? (From the electrodes segment)
In electrolysis, oxidation still occurs at the anode, and reduction still occurs at the cathode,
but the polarity of the electrodes is different.
Faraday's constant is the charge carried by one mole of electrons.
There are 6.02214e23 electrons per mole of electrons. (Avogadro's number)
Each electron has a charge of 1.602177e-19 coulombs per electron.
So Faraday's constant is 1.602177e-19 coulombs per electron * 6.02214e23 electrons per mole of electrons = 9.64853e4 coulombs / mole of electrons.
This constant is useful to us when we are doing problems in electrolysis.
Let's work a problem.
A current of .01 amperes is passed through a solution of AgNo3 for eight hours.
What mass of silver accumulates on the cathode?