During the corrosion of Fe,which species is r | vedclass

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(A) During the corrosion of iron $(Fe)$,the metal acts as an anode and undergoes oxidation: $2Fe(s) \rightarrow 2Fe^{2+}(aq) + 4e^-$. The electrons re

Vedclass · Accepted Answer

$O_2$ in the presence of $H^+$

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(A) During the corrosion of iron $(Fe)$,the metal acts as an anode and undergoes oxidation: $2Fe(s) \rightarrow 2Fe^{2+}(aq) + 4e^-$. The electrons released at the anode move through the metal and are consumed at the cathodic region. In the presence of atmospheric oxygen and moisture (which provides $H^+$ ions),the oxygen is reduced: $O_2(g) + 4H^+(aq) + 4e^- \rightarrow 2H_2O(l)$. Thus,$O_2$ is the species that gets reduced.

During the corrosion of $Fe$,which species is reduced by the electrons produced due to the oxidation of $Fe$?

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