00:01
So we're asked to calculate the standard cell potential and equilibrium constant for the following reaction.
00:06
We have the first one, copper solid plus two moles of silver ions and going to copper two ions plus two moles of silver solid.
00:28
So we can clearly see that in this copper is the anode and silver is the cathode because the oxidation number of copper goes from zero to plus two.
00:37
That's an increase.
00:38
That's oxidation.
00:40
But that of silver goes from plus one to zero.
00:46
That's a reduction.
00:47
So the e standard of this will be the electrode potential of the cathode, which is ag plus ag minus that of the anode, which is cu2 plus cu.
01:00
And of course, the standard values for the electrode potential for that of silver, the value, the standard potential for silver is 0 .80.
01:16
While that of copper is 0 .80.
01:26
Like i said, that of copper, copper two is 0 .34.
01:31
So what we have is 0 .80 minus 0 .34.
01:37
And this will give you 0 .46 volt.
01:46
That is it.
01:48
Then for the equilibrium constant, the e theta cell standard is 0 .0592 over n log of k, where n is the number of moles of electrons.
02:01
That's two.
02:03
So 0 .46 equals to 0 .0592 divided by two log of k.
02:11
This would mean that the log of k is two multiplied by 0 .46 divided by 0 .0592.
02:21
And that would give us 15 .5.
02:27
So which means that k is the antilog of 15 .54.
02:39
And that would give us, so the value of k would be, so k is 3 .47 times 10 to the power of 15.
02:49
That's the value of k.
02:52
Okay...