00:01
All right, so here we have, we're told that an aqueous solution of magnesium chloride solution is electrolyzed under one bar pressure using platinum electrodes.
00:13
We're to write the half reactions predicted to occur at the anode and the cathode based on the cell potential.
00:21
Okay, so let's look at it.
00:24
At anode, two reactions are possible.
00:27
We're talking about, before we're talking about magnesium chloride and what we have present are magnesium ions, chloride ions, and water, right, and water.
00:44
And of course, the water we can split that is hydrogen ions and hydroxide ions, but we're just going to use that.
00:51
At the cathode, two particular reactions are possible at a cathode.
00:58
At a cathode, we could have the magnesium ion, right, in an electrolytic cell.
01:04
The cathode is the negative electrode.
01:07
The magnesium ions may be reduced and you have magnesium.
01:13
The electrode potential value for this is minus 2 .370.
01:20
Or you could have water itself.
01:25
You can have it reduced, that equation there, and you have production of hydrogen gas and hydroxide ion and nitroxide ion.
01:37
And the ethanol value for that is minus 0 .828.
01:44
Now, the preferred reaction at a cathode, the preferred reaction is going to be the one with a lower negative electrode potential, sort of like what you have with the reverse of electrochemical cells, right, or galvanic cells.
02:00
So this is the preferred equation at the cathode.
02:04
This is going to be the equation.
02:05
Water will be reduced.
02:09
However, at the anode, at the anode, at the anode, we also have two reactions that are possible.
02:17
We have chlorine gas.
02:19
The chlorine, chloride ion may be discharged and undergo oxidation...