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Given the overall formation constant of ...

Given the overall formation constant of the `[Fe(CN)_(6)]^(4-)` ion as `10^(35)` and the standard potentials for the half reaction,
`Fe^(3+)+e^(-) hArr Fe^(2+) , E^(@)=0.77 V`
`[Fe(CN)_(6)]^(3-)+e^(-)hArr [Fe(CN)_(6)]^(4-) , E^(@)=0.36 V`
Calculate the overall formation constant of the`[Fe(CN)_(6)]^(3-)` ion.

A

`8.59xx10^(41)`

B

`7.59xx10^(41)`

C

`5.59xx10^(41)`

D

`9.59xx10^(41)`

Text Solution

Verified by Experts

The correct Answer is:
C

(A) Let `K_(f)` be the formation constant of `[Fe(CN)_(6)]^(3-)` ion.
`Fe^(2+)+6CN^(-)hArr[Fe(CN)_(6)]^(4-),K_(f)=10^(35)`,
`Delta G_(1)^(@)=-2.303RT log K_(f)=-199704.69 J`
`Fe^(3+)+e^(-)hArr Fe^(2+), E^(@)=0.77V` ,
`Delta G_(2)^(@)=-96500xx0.77=-74305 J`
`Delta G_(3)^(@)=+96500xx0.36=34740 J`
`[Fe(CN)_(6)]^(4-) hArr [Fe(CN)_(6)]^(3-)+e^(-)`,
`E^(@)=-0.36 V`,
`bar(Fe^(3+)+6CN^(-)hArr [Fe(CN)_(6)]^(3-)`,
`Delta G_(4)^(@)=Delta G_(1)^(@)+Delta G_(2)^(@)+Delta G_(3)^(@)=-239269.69 J`
`Delta G_(4)^(@)=-2.303RT log K _(f) therefore K _(f)=8.59xx10^(41)`
`2Fe^(3+)+2e^(-)rarr 2Fe^(2+)` or
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Find the oxidation state of Fe in Fe_(4)[Fe(CN)_(6)]_(3) .

The overall formation constant for the reaction of 6 mole of CN^(-) with cobalt (II) is 1 xx 10^(19) . The standard reduction potential for the reaction [Co(CN)_(6)]^(3-) +e^(-) rarr Co(CN)_(6)^(4-) is -0.83V . Calculate the formation constant of [Co(CN)_(6)]^(3-) Given Co^(3+) +e^(-) rarr Co^(2+) , E^(@) = 1.82V

Knowledge Check

  • [Fe(CN)_(6)]^(4-) is

    A
    inner complex
    B
    outer complex
    C
    square planar
    D
    trigonal bipyramidal
  • IUPAC name of [Fe(CN)_(6)]^(3-) ion is

    A
    hexacyanoferrate (II) ion
    B
    hexacyanoferrate (III) ion
    C
    hexacyanide iron (III) ion
    D
    iron (III) hexacyanide ion
  • The shape of [Fe(CN)_(6)]^(4-) ion is

    A
    Hexagonal
    B
    Pyramidal
    C
    Octahedral
    D
    Octagonal
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    The name of the complex ion, [Fe(CN)_(6)]^(3-) is :