Question

In the reaction, \( \text{O}_{2(g)} + 4\text{H}^+_{(aq)} + 4\text{e}^- \rightarrow 2\text{H}_2\text{O}_{(l)} \), the quantity of electricity required to reduce one mole of gaseous oxygen is ( \( E^\circ = 1.23\,\text{V} \) )

Hint:

Always read the stoichiometry directly from the balanced equation. If a question asks for charge, you don't need voltage ($E^\circ$). Voltage is needed to calculate energy ($\Delta G = -nFE$). Don't let extra numbers distract you.

Answer 1