emf generated by the cell is 0.40 V.
Oxidation: [tex]2Al + 6e^{-}[/tex]→[tex]2Al^{3+}[/tex]
Reduction: [tex]3I_{2} + 6e^{-}[/tex]→[tex]6I^{-}[/tex]
Overall: [tex]2Al + 3I_{2}[/tex]→[tex]2Al^{3+} + 6I^{-}[/tex]
Nernst equation for this cell reaction at 25-degree celsius:
[tex]E_{cell} = E^{0}_{cell} - \frac{0.059}{n} log[Al^{3+}]^{2} [I^{-}]^{6}[/tex]
where n is the number of electrons exchanged during cell reaction, [tex]E^{0}_{cell}[/tex] is standard cell emf, [tex]E_{cell}[/tex] is cell emf, [tex][Al^{3+}][/tex] is the concentration of [tex]Al^{3+}[/tex] , and [tex][I^{-}][/tex] is the concentration of [tex]I^{-}[/tex].
Plug in all the given values in the above equation -
[tex]E_{cell} = 2.20 - \frac{0.059}{6} [(4.0 * 10^{-3})^{2}*(0.15)^{6}][/tex]
=0.40 V
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