The reaction below shows the corrosion process of iron. Calculate E°cell for the corrosion process and state whether you would predict that this is a spontaneous or nonspontaneous process.

2 Fe (s) + O2 (g) + 4 H+ (aq) → 2 Fe2+ (aq) + 2 H2O (l)

Look up Eo couples for Fe to Fe^+2 and O2 + H^+ to H2O. Calculate Ecell. If it is positive it is spontaneous; if negative it is not spontaneous.

To calculate E°cell for the corrosion process, we need to use standard reduction potentials. The given balanced equation involves the reduction of oxygen and the oxidation of iron.

Step 1: Find the half-reactions
Oxidation half-reaction: 2 Fe → 2 Fe2+ + 4 e-
Reduction half-reaction: O2 + 4 H+ + 4 e- → 2 H2O

Step 2: Lookup the standard reduction potentials
We can find the reduction potentials for the half-reactions in a standard reduction potential table. The values we need are:
E°red(O2/H2O) = +1.23 V (reduction potential of O2)
E°red(Fe2+/Fe) = -0.44 V (reduction potential of Fe2+)

Step 3: Calculate E°cell using the formula
E°cell = E°red(Reduction half) - E°red(Oxidation half)

E°cell = [E°red(O2/H2O) - E°red(Fe2+/Fe)]

E°cell = [1.23 V - (-0.44 V)]
E°cell = 1.67 V

Step 4: Determine whether the process is spontaneous or nonspontaneous
For a spontaneous process, E°cell must be positive. In this case, the calculated E°cell is 1.67 V, which is positive. Hence, we predict that the corrosion process of iron is a spontaneous process.