00:01
For this reaction, we're given line notation for the couple efe solid efe2 plus on the left hand side, so it's serving as the anode, so oxidation is occurring, so efe solid is going to efe2 plus.
00:16
Then we have, for reduction on the right hand side, the cathode, we have the reduction of fe3 plus to fe2 plus.
00:24
So we have two e2 pluses that are being produced.
00:27
This is the balanced chemical reaction.
00:29
For the next part, it asks you to determine what delta g is for this reaction if you are given e -cell standard of 1 .21 volts.
00:45
Well, delta g standard will be equal to negative n, n is there's one electron transferred, an electron is transferred.
00:55
Now let me back up.
00:57
There's actually two electrons transferred.
00:59
Fruit.
01:00
See, what i neglected was we have an iron going to an iron 2 plus that gives us one of these iron 2 pluses, and then we have two iron 3 pluses going to two more iron 2 pluses.
01:15
So this is our balanced chemical reaction.
01:19
We now have a 6 plus on both sides.
01:22
So delta g will be equal to negative n, f, which is faraday's constant, multiplied by the cell potential standard that is provided 1 .21 volts...