Although Fig. 1 indicates that chromium (Cr) is more active than iron (Fe), chro

Question

Although Fig. 1 indicates that chromium (Cr) is more active than iron (Fe), chrome plating is nevertheless a very effective procedure to prevent the corrosion (i.e., oxidation) of iron. Provide an explanation for a layer of chrome being able to protect iron despite being a more active metal. Galvanization is a process of protecting iron from corrosion by coating the metal with a layer of zinc. Although Z_n is more active than Fe, Z_n reacts with atmospheric gases to form zinc carbonate (Z_nCO_3), a hard, durable substance which shields the remaining Z_n and the underlying Fe. Suggest a series of reactions involving common atmospheric gases which could converted Z_n into Z_nCO_3. If the Z-nCO_3/Z_n coating of galvanized iron is broken and the underlying iron begins to corrode (i.e., oxidize), a chemical reaction intervenes and converts the corrosion products back to iron. Suggest a reaction which could account for this chemical protection of the iron

Explanation / Answer

Note that even though this is more active than Iron, the corrosion typically takes up more TIME, that is, evne though it will oxidize easier than Iron, this does not means it is faster.

Oxidation is a process in which we care --> which reduced/oxidized and how much it takes...

Also, there are pleny of other species added to the chrome layer... but the basis of the chrome plating is that of kinetics.

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