1.

Corrosion of iron is essentially an electrochemical phenomenon where the cell reactions are

Answer»

Fe is oxidised to `Fe^(2+)` and dissolved oxygen in WATER is reduced to `overset(THETA)(OH)`
Fe is oxidised to `Fe^(3+)` and `H_(2)O` is reduced to`O_(2)^(2-)`
Fe is oxidised to `Fe^(2+)` and `H_(2)O` is reduced to`O_(2)^(-)`
Fe is oxidised to `Fe^(2+)` and `H_(2)O` is reduced to`O_(2)`

Solution :`FetoFe^(2+)+2e` (anode rection)
`O_(2)+2H_(2)O+4eto4OH^(-)` (cathode reaction) The overall reaction is
`2FE + O_(2) + 2H_(2)O to 2Fe(OH)_(2)`
`Fe(OH)_(2)` may be dehydrated to iron OXIDE FeO, or further oxidised to `Fe(OH)_(3)` and then dehydrated NTO iron rust, `Fe_(2) O_(3)`


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