Using a table of standard reduction potentials calculate the standard cell potential (electromotive force)?

Question

Using a table of standard reduction potentials calculate the standard cell potential (electromotive force) in volts

for the following cell.


Fe + F2 = Fe2+ + 2F−

2) Calculate the standard free energy change in kJ/mol for the above cell reaction.

Enter a numeric answer only

Answer 1

I'm using the values from:http://www.northland.cc.mn.us/Chemistry/standard_reduction_potentials.htm

E0 (Fe2+/Fe) = -0.447 V
E0 (F2/F-) = +2.866 V

So for the reaction Fe + F2 <=> Fe2+ +2F-

E0 = E0(F2/F-) - E0(Fe2+/Fe) = 2.866-(-0.447) = + 3.313 V

ΔG0 = -nFE0 = -2*96485*3.313 = -639309 = -639.3 kJ/mol

Answer 2

(Fe2+)+2e->Fe -0.44
F2+2e>2F- +2.87
from your equation
E=0.44+2.87=3.31

Answer 3

use equation Ecell=Eredu-Eoxi

Ecell=2.87-(-.44)
=3.31