00:01
The standard free energy change of an electrochemical reaction can be computed as negative n times f times e -cell knot, where delta g -not is the standard free energy change of the reaction, and is the number of electrons transferred.
00:16
F is the pyridus constant, and e -not cell is the cell potential.
00:20
In this problem, we are going to first write half -reactions by simply rewriting the retricions such that we collect those common terms.
00:30
So such as n i 2 plus with n i and then you have your f e 2 plus with f a 3 plus and then we will we will make sure that this reaction is balanced by putting this appropriate number of electrons on the side that needs the decrease in the number of electrons so for the first for the first reaction we need to put two minus two electrons in order to reduce the charge on the left side so two electrons on the left side, and on the right side, we need to put two electrons on the next reaction.
01:10
Rather, we need to put two electrons on the right side to reduce the charge there.
01:15
So as the electrons on the first reaction is shown in the reactant side, that means electrons are gained, and so this is reduction reaction.
01:26
The other reaction will be oxidation as electrons are lost.
01:29
That means electrons are found in the product side.
01:32
So let us compute the cell potential for this.
01:36
And that's going to be the difference between the reduction potential of the reduction reaction and the reduction potential of the species in the oxidation reaction...