Problem: Using the table of half-cell reactions, calculate the ΔG° for cell reaction below. (Make sure you find n for the reaction.)I- (aq)  |  I2  | |  Fe+2 (aq)  |  Fe1) -200 kJ2) +200 kJ3) -100 kJ4) +100 kJ

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We’re being asked to calculate the ΔG° for cell reaction below:

I(aq)  |  I2  ||  Fe+2 (aq)  |  Fe


We will have to calculate for the  ΔG° using the following steps:

Step 1: Identify the anode and the cathode in the reaction and write the overall reaction
Step 2: 
Calculate the cell potential of the reaction.
Step 3Calculate  ΔG°.

G°=-nFE°cell

ΔG° = Gibbs Free Energy, J
n = # of e- transferred
F = Faraday’s constant = 96485 J/(mol e-)
cell = standard cell potential, V

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Problem Details

Using the table of half-cell reactions, calculate the ΔG° for cell reaction below. (Make sure you find n for the reaction.)

I(aq)  |  I2  | |  Fe+2 (aq)  |  Fe

1) -200 kJ

2) +200 kJ

3) -100 kJ

4) +100 kJ

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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.