# 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

###### FREE Expert Solution

Modified Nernst equation:

$\overline{){{\mathbf{E}}}_{{\mathbf{cell}}}{\mathbf{=}}{\mathbf{E}}{{\mathbf{°}}}_{{\mathbf{cell}}}{\mathbf{-}}\mathbf{\left(}\frac{\mathbf{0}\mathbf{.}\mathbf{0592}}{\mathbf{n}}\mathbf{\right)}{\mathbf{log}}\frac{\left[\mathrm{anode}\right]}{\left[\mathrm{cathode}\right]}}$

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
97% (409 ratings) ###### 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