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Explain how rusting of iron is envisaged...

Explain how rusting of iron is envisaged as setting up of an electroCHMemical cell.

Text Solution

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Formation of carbonic acid takes place on the surface of iron:
`H_(2)O(l)+CO_(2)(g)rarrH_(2)CO_(3)hArr2H^(+)+CO_(3)^(2-)`
In presence of `H^(+)` ion, oxidation of iron takes place
`Fe(s)rarrFe^(2+)(aq)+2e^(-)`
The electrons are used at other spot where reduction takes place:
`O_(2)(g)+4H^(+)(aq)=4e^(-)rarr2H_(2)O(l)`
Overall reaction is:
`2Fe(s)+O_(2)(g)+4H^(+)(aq)hArr2Fe^(2+)(aq)+2H_(2)O(l)`
Thus, an electrochemical cell is established on the surface.
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Explain how rusting of iron is envisaged as setting up of an electrochemical cell.

Explain how rusting of iron is envisaged as setting up of an electrochemical cell.

Knowledge Check

  • Rusting of iron involves

    A
    oxidation
    B
    reduction
    C
    decompositions
    D
    displacement
  • During rusting of iron it gets

    A
    oxidised
    B
    reduced
    C
    Oxidised and hydrated
    D
    hydrated
  • The rusting of iron is catalysed by

    A
    Fe
    B
    `O_(2)`
    C
    `H^(+)`
    D
    Zn
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