lectrochemistry: Using Standard Cell Potentials 


Calculating the Cell Potential:The net reaction of a voltaic cell constructed from a standard zinc electrode and a standard copper electrode is obtained by adding the two halfreactions together:
How do we know which metal will become oxidized and which metal ion reduced? By looking at a table of standard reduction potentials! One of the halfreactions must be reversed to yield an oxidation. Reverse the halfreaction that will yield the highest (positive) net emf for the cell. Remember that when one reverses a reaction, the sign of Eº (+ or –) for that reaction is also reversed. Consider again the following table of standard reduction potentials:
Let's calculate the potential generated in by a cell constructed from standard Zr and I_{2} electrodes: From the table, we write a balanced reduction halfreaction for each electrode and copy down the reduction potentials:
Reversing which reaction will yield most positive standard reduction potential? Let's try both! Case 1: reversing the iodine reduction: Eº_{net} = Eº_{ox}(I_{2}) + Eº_{red}(Zr) Eº_{net} = (– 0.54) + (– 1.53) Eº_{net} = – 2.07 V Case 2: reversing the zirconium reduction: Eº_{net} = Eº_{red}(I_{2}) + Eº_{ox}(Zr) Eº_{net} = ( 0.54) + ( 1.53) Eº_{net} = 2.07 V
The highest positive potential is found by using the Zr oxidation halfreaction. The cell would therefore proceed spontaneously in Case 2. Notice that we did not multiply the value for the reduction potential of I_{2} by a factor of 2, even though the iodine reduction equation would be multiplied by this factor to balance the number of electrons produced and consumed. Review: On a sheet of paper, derive the balanced net equation for this voltaic cell. When finished, click the question mark to reveal the answer. Use the previous table of standard reduction potentials to calculate the voltage generated by the following voltaic cells at standard conditionstwo decimal places, please!:
Nicely done! A negative voltage represents a nonspontanous reaction! Try again. 0.86 (mercury electrode, reduction) + 0.00 (hydrogen electrode, oxidation) = ? 1.53 (zirconium electrode, reduction) + 2.93 (rubidium electrode, oxidation) = ? 2.93 (rubidium electrode, oxidation) + 0.86 (mercury electrode, reduction)= ? Before moving to the next page, you should how to calculate the net potential of a voltaic cell by using a table of standard reduction potentials. 
