# 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

###### FREE Expert Solution

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°.

$\overline{){\mathbf{∆}}{\mathbf{G}}{\mathbf{°}}{\mathbf{=}}{\mathbf{-}}{\mathbf{nFE}}{{\mathbf{°}}}_{{\mathbf{cell}}}}$

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