Problem: Sketch the galvanic cells based on the following half-reactions. Show the direction of electron flow, show the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation, and determine E° for the galvanic cells. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm.a. H2O2 + 2H+ + 2e- → 2 H2O        E° = 1.78 V    O2 + 2H+ + 2e- → H2O2             E° = 0.68 V

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Identify the cathode and anode:

Smaller (↓) E° → oxidation → anode

Larger (↑) E° → reduction → cathode

H2O2 + 2 H+ + 2 e- → 2 H2O        E° = 1.78 V → cathode

O2 + 2 H+ + 2 e- → H2O2             E° = 0.68 V → anode


Write the overall balanced equation:

Reduction:    H2O2 + 2 H+ + 2 e- → 2 H2O

Oxidation:                           H2O2 → O2 + 2 H+ + 2 e- 
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Overall:    2 H2O2(aq) → O2(g) + 2 H2O(l)


Calculate the E°cell for the galvanic cell:

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Problem Details

Sketch the galvanic cells based on the following half-reactions. Show the direction of electron flow, show the direction of ion migration through the salt bridge, and identify the cathode and anode. Give the overall balanced equation, and determine E° for the galvanic cells. Assume that all concentrations are 1.0 M and that all partial pressures are 1.0 atm.

a. H2O2 + 2H+ + 2e- → 2 H2O        E° = 1.78 V
    O2 + 2H+ + 2e- → H2O2             E° = 0.68 V