# Problem: The equation ΔG° = -nFE° also can be applied to half-reactions. Use standard reduction potentials to estimate ΔG°f for Fe2+(aq) and Fe3+(aq). (ΔG°f for e- = 0.)

###### FREE Expert Solution

ΔG° can be calculated from the cell potential using the following equation:

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

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

ΔG°f for Fe2+(aq):

Fe2+(aq) + 2 e- → Fe(s)       E° = -0.447 V

n = 2 mol e-
F = 96485 C/(mol e-)
E° = -0.447 V

ΔG°rxn = 86257.59 J

ΔG°rxn = 86.26 kJ

ΔG˚f, Fe2+–86.26 kJ/mol Fe2+

ΔG°f for Fe3+(aq):

87% (363 ratings) ###### Problem Details

The equation ΔG° = -nFE° also can be applied to half-reactions. Use standard reduction potentials to estimate ΔG°f for Fe2+(aq) and Fe3+(aq). (ΔG°for e- = 0.)

Frequently Asked Questions

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.

What professor is this problem relevant for?

Based on our data, we think this problem is relevant for Professor Guiton's class at UK.

What textbook is this problem found in?

Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.