Problem: 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 V2 IO3-(aq) + 10 e- <=> 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


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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

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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.