Rusting of iron requires which of the following?

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.

What is the electron movement during the corrosion of $Fe$?

The chemical formula of rust is:

On the basis of the electrochemical theory of aqueous corrosion,the reaction occurring at the cathode is

Metal can be prevented from rusting by