If the $E ^ { \circ }$ of the galvanic cell is 0.98 V and the $E ^ { \circ }$ of the copper anode is -0.34 V, what is the $E ^ { \circ }$ of the hydrogen cathode?

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Quizplus · Accepted Answer

The overall cell reaction is Cu + H2 → Cu2+ + 2H+. The standard potential of the cell is the difference between the standard potentials of the cathode and anode: E°cell = E°cathode - E°anode. Thus, 0.98 V = E°cathode - (-0.34 V), or E°cathode = 0.98 V - (-0.34 V) = 1.32 V. Since the cathode is the reduction half-reaction (in this case, H+ + e- → H2), the standard potential of the hydrogen electrode (cathode) is E° = 1.32 V - 0.94 V = 0.64 V.

If The E∘E ^ { \circ }E∘ Of the Galvanic Cell Is 0

If The $E ^ { \circ }$ Of the Galvanic Cell Is 0