00:01
Hello students, so in this video we have a reaction where the ag plus ion is getting converted to ag and the copper is getting converted to copper 2+.
00:11
The delta g of the reaction is given as minus 88 .66 kj per mole and we have to calculate the standard cell potential of this reaction and we also have to calculate the equilibrium constant of this reaction.
00:33
So we can calculate both of them with the use of delta g.
00:41
So let us, let me write the formula for delta g and the relation between standard cell potential.
00:47
So delta g is actually equals to minus nf e cell or the standard cell potential.
00:56
Here n is the number of electrons transferred in the reaction.
01:03
So here you can see that the reactions can be divided into two half cells which is 2ag plus giving rise to 2ag plus 2 electrons.
01:17
So here ag is getting reduced from plus state to zero state and cu plus 2 electron giving rise to cu2+.
01:29
Here copper is getting oxidized to cu2+.
01:35
So this is the reduction reaction, this is the oxidation reaction.
01:38
So you can see that the number of electrons transferred are two.
01:42
So we can say that the value of n is actually 2 and the value of f is 96485 coulomb per mole and we don't know e cell and the delta g value is minus 88 .66 kilojoule per mole.
02:05
So i will convert this minus 88 .66 to joule per mole by multiplying it with 1000...