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Consult the table on standard electrode ...

Consult the table on standard electrode potentials and suggest three substance that can oxidise ferrous ions under suitable conditions.

Text Solution

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`Fe^(2+)` (ferrous) ions gets oxidised to `Fe^(3+)` (farriec) ion as follows
`Fe^(2+) to Fe^(3+)+e^(-)E_(0x)^(0)=-0.77V`
Only those substances can oxidise `Fe^(2+)` ions to `Fe^(3+)` ions which can accept electrons released during oxidation or are placed above iron in electrochemical series. Three such substances
are `Cl_(2)(g), Br_(2)(g) and F_(2)(g).`
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Knowledge Check

  • Which defines the standard reduction electrode potential of Zn^(2+) ions?

    A
    `Zn_((aq))^(2+) + 2e to Zn_((s)) , [Zn^(2+)] = 1 M`
    B
    `Zn_((g)) to Zn^(2+) + 2e , [Zn^(2+)] = 1M `
    C
    `Zn_((aq))^(2+) to Zn_((s)) + 2e , [Zn^(2+) ] = 1M `
    D
    `Zn_((g))^(2+) to Zn_((s)) - 2e , [Zn^(2+)] = 1M`

  • Oxidation is de-electronation whereas reduction is electronation. Oxidants are the substances which oxidise others and reduced themselves. On the other hand reductants are the substances which reduce others and oxidised themselves. The oxidation number of an element in a compound decides its nature to act as oxidant or reductant. Oxidation-reduction occur simultaneously and the overall chemical change is called redox reaction. Redox reactions are of three types: (i) Intermolecular redox reactions, (ii) Autoredox or disproportionation reaction, and (iii) Intramolecular redox reactions. Select the species which can act as oxidant and reductant both : (1) H_2SO_3 (II) H_2 O_2 (III) O_3 (IV) HNO_3 (V) CI_2

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