Now Faraday's constant represents the charge which we use capital C in Coulombs of 1 mole of electrons and is named after British scientist Michael Faraday. Now here we're going to say the charge that passes through the cell equals the moles of electrons times Faraday's constant. So if we have an electrochemical cell, we can determine that its charge is equal to moles of electrons N times Faraday's constant F.

Beyond this, we can save. The conversion factor between coulombs and joules is that one coulomb is equal to 1 Joule per Volt. So by incorporating Faraday's constant, it's possible for us to go between coulombs to joules or kilojoules, or vice versa. Now here we're going to say that Faraday's constant, remember, is 96,485 coulombs per mole of electrons.

And we just learned about this conversion factor. So here we want to get rid of coulomb, so we put on the bottom 1 coulomb, and on the top we're going to say that's equal to 1 Joule per Volt. Coulomb's cancel out, so it's still going to be the same 96,485 joules over volts times moles of electrons because the volts are denominated here. So they're staying a denominator here. Moles of electrons never got cancelled out, so they remain a denominator as well.

So just remember, by remembering this conversion factor, we can basically interchange between coulombs to joules or kilojoules, right? So this is all the things that we need to know in terms of Faraday's constant.