Explain: Corrosion of $Fe$ is a galvanic cell-like arrangement.

(N/A) Corrosion of iron $(Fe)$ is an electrochemical process that acts like a galvanic cell.
$1$. At the anodic site,iron atoms lose electrons to form $Fe^{2+}$ ions: $2Fe(s) \rightarrow 2Fe^{2+}(aq) + 4e^-$.
$2$. At the cathodic site,oxygen and water react with the electrons released by iron to form hydroxide ions: $O_2(g) + 2H_2O(l) + 4e^- \rightarrow 4OH^-(aq)$.
$3$. The $Fe^{2+}$ ions further react with oxygen to form hydrated ferric oxide $(Fe_2O_3 \cdot xH_2O)$,which is known as rust.
$4$. The overall reaction is: $2Fe(s) + O_2(g) + 4H^+(aq) \rightarrow 2Fe^{2+}(aq) + 2H_2O(l)$.