We’re being asked to determine the standard cell potential (E°cell) of the reaction occurring in an electrochemical cell. To calculate for the standard cell potential, use the following equation:
When a balanced reaction is given, identify the anode and the cathode half-reactions by determining the changes in oxidation states of each species based on the given reaction:
Balanced reaction: Fe(s) + 2 Fe3+(aq)→ 3 Fe2+(aq)
We will do the following steps:
Step 1: Write the two half-cell reactions
Step 2. Identify the reduction half-reaction (cathode) and the oxidation half-reaction (anode)
Step 3: Determine the half-cell potentials (refer to the Standard Reduction Potential Table)
Step 4. Calculate E°cell.
Using standard reduction potentials (Appendix E in the textbook), calculate the standard emf for each of the following reactions.
Fe(s) + 2Fe3 + (aq) → 3Fe2 + (aq).