The reduction of O_2 to H_2O has a standard reduction potential (E*) of +1.23 V,

Question

The reduction of O_2 to H_2O has a standard reduction potential (E*) of +1.23 V, and proceeds according to the following: O_2(g) + 4 H^+(aq) + 4 e^- rightarrow 2 H_2O(l) Let's call this the O_2/H_2O electrode. In the following, draw the electrochemical cell resulting from the combination of the O_2/H_2O electrode and the standard hydrogen electrode. Make sure to: Label the anode and cathode indicate the flow of the electrons Calculate the resulting voltage, E*_cell Write the balanced chemical equation for the overall redox reaction BONUS: note that the chemical equation of your redox reaction is the same as that of the combustion of hydrogen gas. How do you call these types of electrochemical cells?

Explanation / Answer

The reduction of O_2 to H_2O has a standard reduction potential (E*) of +1.23 V,

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