The rusting of iron is formulated as Fe_2O_3 | vedclass

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(C) The rusting of iron is an electrochemical process. At the anode,iron is oxidized to ferrous ions: $2Fe(s) \rightarrow 2Fe^{2+}(aq) + 4e^-$. At the

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$Fe(OH)_2$

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(C) The rusting of iron is an electrochemical process. At the anode,iron is oxidized to ferrous ions: $2Fe(s) \rightarrow 2Fe^{2+}(aq) + 4e^-$. At the cathode,oxygen is reduced in the presence of $H^+$ ions: $O_2(g) + 4H^+(aq) + 4e^- \rightarrow 2H_2O(l)$. The $Fe^{2+}$ ions further react with oxygen to form $Fe^{3+}$ ions,which form hydrated ferric oxide,$Fe_2O_3 \cdot xH_2O$. During this process,$Fe(OH)_2$ is formed initially,which is then further oxidized to $Fe(OH)_3$ and finally dehydrated to form rust $(Fe_2O_3 \cdot xH_2O)$.

The rusting of iron is formulated as $Fe_2O_3 \cdot xH_2O$. This process involves the formation of which of the following as an intermediate product?

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