A) metallic iron is oxidised to \[F{{e}^{3+}}\]ions
B) metallic iron is reduced to \[F{{e}^{2-}}\] ions
C) oxygen gas is reduced to oxide ion
D) yellowish-brown product is formed
Correct Answer: B
Solution :
In the presence of \[{{O}_{2}}\] and \[{{H}_{2}}O\] rusting of iron takes place. \[{{H}^{+}}\] ions act as a catalyst. It is believed that oxidation of \[Fe\] into \[F{{e}^{2+}}\] occurs at a place which act as anode, \[Fe\xrightarrow{{}}F{{e}^{2+}}+2e{{~}^{-}}\] (oxidation) (at anode) In the presence of \[{{H}^{+}}\] ions \[{{O}_{2}}\] is reduced into \[{{H}_{2}}O\] at a place which acts as cathode \[{{O}_{2}}+4{{H}^{+}}+4{{e}^{-}}\xrightarrow{{}}2{{H}_{2}}O\] (reduction) \[F{{e}^{2+}}\] formed at anode are oxidised into \[F{{e}^{3+}}\] by air. \[4F{{e}^{2+}}+{{O}_{2}}+4{{H}_{2}}O\xrightarrow{{}}2F{{e}_{2}}{{O}_{3}}+8{{H}^{+}}\]
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