Discussion
In the reaction, O2(g) + 4H+(aq) + 4 e- →2H2O(l) , the quantity of electricity needed to reduce one mole of gaseous oxygen is (E°cell = 1.23V)
Answer: A
The quantity of electricity is 386000 Coulombs.
The equation shows 4 electrons for each O2, so reducing one mole of oxygen needs 4 moles of electrons, that is 4 faradays:
\[ Q = 4F = 4 \times 96500 = 386000\ \text{C} \]
The cell potential of 1.23 V is not needed; it would be used to find the energy, not the charge. 96500 C is one faraday, enough for only a quarter of a mole of O2.
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