Problem: 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).

FREE Expert Solution

We’re being asked to determine the standard cell potential (E°cellof the reaction occurring in an electrochemical cell. To calculate for the standard cell potential, use the following equation:


E°cell = E°cathode - E°anode


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
.

View Complete Written Solution
Problem Details

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).