An experimental fuel cell has been designed that uses carbon monoxide as fuel. The overall reaction is 2CO(g) + O2(g) → 2CO2(g) The two half cell reactions are
CO + O2- → CO2 + 2e-
O2 + 4e– → 2O2-
The two half reactions are carried out in separate compartments connected with a solid mixture of CeO2 and Gd2O3. Oxide ions can move through this solid at high temperatures (about 800oC). ΔG for the overall reaction at 800oC under certain concentration conditions is –380 kJ. Calculate the cell potential for this fuel cell at the same temperature and concentration conditions.