2. Review:
A voltaic cell is created consisting of a solid nickel electrode in contact with a solution of Ni2+ ions and a solid copper electrode in contact with a solution of Cu2+ ions.
Calculate the standard cell potential.
After the cell operates for 30 minutes, the mass of the Ni electrode decreases by 1.69 grams. What quantity of charge, in Coulomb’s, passes through the cell?
Calculate the current, in amperes.

3. Eocell under non-standard conditions:
Electrochemical cells may start out at standard conditions, but don’t last that way for very long.
In the real world, cells seldom operate under standard conditions, they are tailored for optimal voltage/amps, etc.

4. Eocell under non-standard conditions:
As the reaction approaches equilibrium, the voltage slowly decreases to Ecell = 0

5. Eocell and Free Energy:
Positive cell voltages mean the cell is spontaneous in the direction written ( - ∆G )
There is an equation that relates the two quantities.

6. Eocell and Free Energy:

7. Eocell and Free Energy:
The standard cell potential, Eocell, for the reduction of silver ions with copper metal is V at 25oC. Calculate ∆Grxn
GENERAL TREND: MORE POSITIVE ECELL IS MORE SPONTANEOUS, MORE PRODUCT FAVORED

8. Eocell and Free Energy:
On your own:
Calculate the equilibrium constant for the reaction: Fe + Cd2+  Fe Cd
(assume standard conditions)

14. Quantitative Stuff with Electrochemical Cells