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).
Frequently Asked Questions
What scientific concept do you need to know in order to solve this problem?
Our tutors have indicated that to solve this problem you will need to apply the Cell Potential concept. If you need more Cell Potential practice, you can also practice Cell Potential practice problems.
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