The metal that forms a self-protecting film of oxide to prevent corrosion is

Given the half-cell reactions:
$2H^+ + \frac{1}{2}O_2 + 2e^- \to H_2O(l), E^o = 1.23 \ V$
$Fe^{2+} + 2e^- \to Fe(s), E^o = -0.44 \ V$
Calculate the value of $\Delta G^o$ in $kJ$ for the overall corrosion reaction.

In the galvanizing process,iron is coated with zinc. The resulting chemical protection is most similar to that provided when

Corrosive sublimate is

The metal used in the galvanizing of iron is

Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are