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Question: The potential difference needed for the electrolytic reduction of aluminum oxide \[\left( {A{l_2}{O_...

The potential difference needed for the electrolytic reduction of aluminum oxide (Al2O3)\left( {A{l_2}{O_3}} \right) at 500∘C500^\circ C is at least:
A. 4.5 V4.5{\text{ }}V
B. 3.0 V3.0{\text{ }}V
C. −5.0  V - 5.0\,\,V
D. −2.5  V - 2.5\,\,V

Explanation

Solution

Electrode potential is a measure of tendency of an electrode in a half cell to lose or gain electrons. The oxidation potentials give the tendency to lose electrons and reduction potentials give the tendency to gain electrons.
Formula used: ΔG∘=−nFEcell∘\Delta G^\circ = - nFE{^\circ _{cell}}
Where ΔG∘=\Delta G^\circ = Gibbs free energy change
n=n = Number of electrons change
F=F = Faraday
Ecell∘=E{^\circ _{cell}} = Potential difference

Complete answer:
Relationship between Gibbs free energy change and the cell potential is given below
ΔG∘=−nF Ecell∘\Delta G^\circ = - nF\,E{^\circ _{cell}}………………….(i)
Where DG∘=DG^\circ = Gibbs free energy change
n=n = number of electron transferred
F=F = Faraday
Ecell∘=E{^\circ _{cell}} = potential difference
We know that electrolytic reduction of aluminum oxide
23Al2O3→42Al+O2   ΔG∘=+960KJ/mol\dfrac{2}{3}A{l_2}{O_3}\xrightarrow{{}}\dfrac{4}{2}Al + {O_2}\,\,\,\Delta G^\circ = + 960KJ/mol
Number of electrons gain by metal =4 = 4 electrons
F=96500 C.F = 96500\,C.
Substitute the value in Equation (1), we get
960×1000=−4×96500×Ecell∘960 \times 1000 = - 4 \times 96500 \times E{^\circ _{cell}}, solve the equation and find the potential difference
Ecell∘=−9600004×96500E{^\circ _{cell}} = - \dfrac{{960000}}{{4 \times 96500}}
=−2.48V= - 2.48V
So, potential difference is −2.5V - 2.5V
Hence, the correct option is D.

Note: The decrease in free energy of the system in a spontaneous redox reaction is equal to the electrical work - done by the system on the surroundings. In thermodynamics, the Gibbs free energy is thermodynamics potential that can be used to calculate the maximum of reversible work that may be performed by a thermodynamics system at a constant temperature and pressure.In a galvanic cell the Gibbs free energy related to potential by: ΔG∘=−nFEcell∘\Delta G^\circ = - nFE{^\circ _{cell}} if E∘E^\circ cell greater than zero, then the process is spontaneous (galvanic cell). If E∘E^\circ cell less than zero, then the process is nonspontaneous (electrolytic cell).