00:01
In this question, we're going to be looking at the electrochemical cell.
00:03
Let's take a look at some of the details.
00:07
First of all, this cell is made up of copper in a copper solution, and then lead in a lead solution.
00:13
And so we need to draw those containers.
00:15
So we'll start off with our two containers.
00:19
And in one of the half cells, we'll draw one piece of metal, and then in the other half cell we'll draw the other piece of metal.
00:27
This is going to be in a solution.
00:29
So i usually like to draw some kind of squiggly line indicating that it's a little.
00:32
Liquid.
00:33
Now we're going to label the one on the left as the lead.
00:37
So we'll go ahead and label that as lead as pb.
00:40
And the one on the right, we're going to label that as the copper.
00:43
Now, technically, it doesn't really matter which side each one is.
00:47
But i tend to like to put the anode on the left and the cathode on the right, but we'll get to that eventually.
00:54
Now, the lead is going to be in a solution of lead nitrate.
00:58
And typically we would just bother putting the ion.
01:02
So, so it's lead with a positive 2.
01:04
And it doesn't hurt to put in a little a q, indicating that that's dissolved in solution.
01:11
Now, of course, the copper is going to be submerged in a solution of copper sulfate.
01:17
And so we'll pick out the copper ion and put in the aq.
01:20
So that's a good starting point.
01:23
Now, the other thing is that these have to be connected.
01:26
So we'll go ahead and change color for the wire.
01:28
They're going to be connected and some kind of resistor in between.
01:32
Sometimes you'll see a little light bulb.
01:36
I like to just say that it's a volt meter of some sort.
01:39
So a wire connects one electrode to the other electrode and with some kind of resistor.
01:47
Now this would not be enough in order to have the cell operate because this is an open circuit.
01:55
So one of the last components, which is very important, is to put in what we call a salt bridge.
02:01
What that's going to allow is that, as this reaction is proceeding, i have that a little bit wider, sorry.
02:08
As this reaction is proceeding, it's going to allow the charge to be balanced out.
02:15
And so we're just going to label this as a salt bridge.
02:19
And that's very critical in order for this reaction to proceed within the cell.
02:25
Okay, so typically if you want to add in something, typically you'd have a sodium ion, and you might have a nitrate ion that's in there.
02:34
So we'll go ahead and put no3 minus.
02:37
But you want to have something that's not going to form a precipitate with each of your ions in solution.
02:45
But typically we can just label that as a salt bridge.
02:48
Okay, so that's the critical parts.
02:50
Now we need to think of which one is the anode and which one is the cathode.
02:56
So i'm going to label this side as the anode and this side as the cathode.
03:01
Now a couple details about that.
03:04
One is that the anode is where oxidation occurs.
03:08
And if we look at our value, the voltages that are given, the oxidation is the losing of electrons...