# Problem: Calculate E°(cell) for the reaction, 10 Fe3+(aq) + I2(aq) &lt;=&gt; 2 IO3-(aq) + 10 Fe2+(aq) given the reductionpotentials:Fe3+(aq) + e- &lt;=&gt; Fe2+(aq) , E° = 0.87 V2 IO3-(aq) + 10 e- &lt;=&gt; I2(aq), E° = 1.10 V

###### FREE Expert Solution

We’re being asked to calculate the cell potential given the half-reactions.

We go through the following steps to solve the problem:

Step 1. Write the two half-cell reactions
Step 2. Identify the oxidation half-reaction (anode) and the reduction half-reaction (cathode)
Step 3. Determine the half-cell potentials (refer to the Standard Reduction Potential Table)
Step 4. Calculate E°cell.

Step 1Write the two half-cell reactions

Fe3+(aq) + e-  ↔  Fe2+(aq)           E° = 0.87 V

2 IO3-(aq) + 10 e ↔ I2(aq)          E° = 1.10 V

89% (220 ratings) ###### Problem Details

Calculate E°(cell) for the reaction, 10 Fe3+(aq) + I2(aq) <=> 2 IO3-(aq) + 10 Fe2+(aq) given the reductionpotentials:

Fe3+(aq) + e- <=> Fe2+(aq) , E° = 0.87 V

2 IO3-(aq) + 10 e- <=> I2(aq), E° = 1.10 V