A hydrogen–oxygen fuel cell with an alkaline electrolyte (such as aqueous potassium hydroxide) produces electricity.
What is the half-equation for the reaction that occurs at the anode?
O2(g)+2H2O(l)+4e−→4OH−(aq)\text{O}_2(\text{g}) + 2\text{H}_2\text{O}(\text{l}) + 4\text{e}^- \rightarrow 4\text{OH}^-(\text{aq})O2(g)+2H2O(l)+4e−→4OH−(aq)
2H2(g)+4OH−(aq)→4H2O(l)+4e−2\text{H}_2(\text{g}) + 4\text{OH}^-(\text{aq}) \rightarrow 4\text{H}_2\text{O}(\text{l}) + 4\text{e}^-2H2(g)+4OH−(aq)→4H2O(l)+4e−
2H2(g)→4H+(aq)+4e−2\text{H}_2(\text{g}) \rightarrow 4\text{H}^+(\text{aq}) + 4\text{e}^-2H2(g)→4H+(aq)+4e−
O2(g)+4H+(aq)+4e−→2H2O(l)\text{O}_2(\text{g}) + 4\text{H}^+(\text{aq}) + 4\text{e}^- \rightarrow 2\text{H}_2\text{O}(\text{l})O2(g)+4H+(aq)+4e−→2H2O(l)