00:01
In this video, we want to fill in this table for some redox reactions, oxidation and reduction.
00:09
And we have to figure out which species is going to be oxidized, which is going to be reduced by comparing the reduction potentials.
00:18
So first, let's fill in the reduction potentials for each species.
00:22
So copper is positive 0 .34 volts because that's indicated in here.
00:26
And then zinc is negative 0 .76 volts.
00:30
The rest of them we can look up.
00:33
So for lead, the reduction potential is negative 0 .13 volts.
00:39
That shows up a lot, luckily, so we don't have to look up many values.
00:52
All right, then we want silver is going to be positive 0 .80.
01:01
And then magnesium is negative 2 .37.
01:11
Okay, so writing them both as reduction potentials, the species that has a higher reduction potential will be the cathode.
01:18
I'll just put c and a.
01:20
So in this case, the cathode is going to be copper because that's the one that has a higher reduction potential.
01:25
So we have cu2 plus plus two electrons makes copper.
01:30
And then the anode will reverse it.
01:32
So it's going to be lead turning into lead 2 plus plus two electrons.
01:41
And then our e cell is going to be the value for the cathode, which is 0 .34, minus the value of the anode reduction potential.
01:53
We're flipping the sign because oxidation means flip the sign of the reduction potential.
01:58
So it's 0 .34 plus 0 .13 is 0 .47.
02:06
All right, for our next example, silver is going to be reduced because the reduction potential is higher...