Problem: A galvanic cell is based on the following half-reactions at 25°C:Ag+ + e- → AgH2O2 + 2H+ + 2e- → 2H2OPredict whether Ecell is larger or smaller than E°cell for the following cases.b. [Ag+] = 2.0 M, [H2O2] = 1.0 M, [H+] = 1.0 x 10 -7 M

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FREE Expert Solution

Modified Nernst equation:

Ecell=E°cell-(0.0592n)log[anode][cathode]

Ag+ e- Ag                       E° = +0.80 V
H2O2 + 2H+ + 2e- 2H2O    E° = +1.78 V


In log function: 

  • if anode > cathode → log (anode)/(cathode) = negative value → Ecell is higher than E°cell
  • if cathode > anode → log (anode)/(cathode) = positive value → Ecell is lower than E°cell

For the half reactions:

  • ↓ E° → oxidation → anode
  • ↑ E° → reduction → cathode
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Problem Details

A galvanic cell is based on the following half-reactions at 25°C:

Ag+ e- → Ag
H2O2 + 2H+ + 2e- → 2H2O

Predict whether Ecell is larger or smaller than E°cell for the following cases.

b. [Ag+] = 2.0 M, [H2O2] = 1.0 M, [H+] = 1.0 x 10 -7 M