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 -
Overall: 2 H2O2(aq) → O2(g) + 2 H2O(l)
Calculate the E°cell for the galvanic cell:
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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What scientific concept do you need to know in order to solve this problem?
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Based on our data, we think this problem is relevant for Professor Bloxton's class at TEMPLE.
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Our data indicates that this problem or a close variation was asked in Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition. You can also practice Chemistry: An Atoms First Approach - Zumdahl Atoms 1st 2nd Edition practice problems.