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What is corrosion ? Describe the role of...

What is corrosion ? Describe the role of zinc in cathodic protection of iron. Can we use tin in place of zinc for this purpose ? Give reason.

Text Solution

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Corrosion is a process in which a metal reacts with substances present in the atmosphere to form compounds at its surface.
Role of zinc : Zn acts as anode. It loses electrons in preference to iron because it is more reactive than Fe.
`Zn to Zn^(2+) + 2e^(-)`
If any `Fe^(2+)` ions are formed, they gain electrons to form iron back.
`Fe^(2+) + 2e^(-) to Fe`
Tin cannot be used to protect iron because it is lesser reactive than Fe.
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Knowledge Check

  • Zinc is used to protect corrosion of iron because

    A
    `E_("oxi") ` of `ZnltE_("oxi")` of iron
    B
    `E_("red")` of `ZnltE_("red")` of iron
    C
    `Zn` is cheaper than iron
    D
    `Zn` is abundantly available

  • Zinc is used to protect corrosion of iron because

    A
    `E_("oxi")" of" Zn ltE_("oxi")" of iron"`
    B
    `E_("red")" of"Zn lt E_("red")" of iron"`
    C
    Zn is cheaper than iron
    D
    Zn is abundantly available

  • Zinc is used to protect iron from rusting because

    A
    `E_(red)^@ of Zn gt E_(red)^@` of Fe
    B
    `E_(OX)^@ of Zn gt E_(OX)^@` of Fe
    C
    zinc does not melt easily
    D
    zinc is cheap.

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