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If /\G^(@) for the half cell MnO4^(-)"|"...

If `/_\G^(@)` for the half cell `MnO_4^(-)"|"MnO_2` in an acid solution is -xF then find the value of x.(Given:`E_(MnO_4^(-)"|"Mn^(2+))^(@)=1.5V,E_(MnO_2"|"Mn^(2+))^(@)=1.25V`)

Answer

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If DeltaG^(@) for the half cell MnO_(4)^(-) | MnO_(2) in an acid solution is xF then find the value of x. (Given: E_(MnO_(4)^(-) | Mn^(2+))^(@) = 0.34 V, E_(Sn^(4+)|Sn^(2+))^(@) = 0.15 V )

What is the standard electrode potential for the electrode, MnO_4^-//MnO_2 in an acid solution? E_(MnO_4^-,Mn^(2+))^@=1.51 V, E_(MnO_2,Mn^(2+))^@=1.23V

Knowledge Check

  • The oxidation number of Mn in MnO_(4)^(-1) is

    A
    `+6`
    B
    `-5`
    C
    `+7`
    D
    `+5`

  • Calcualte DeltaG^(@) for Mn^(+2) + MnO_(2) overset(H^(+))to 2Mn^(+3) + H_(2)O Given: E_(Mn^(+3)//Mn^(+2))^(@) = 1.51V , V, E_(MnO_(2)//Mn^(+3))^(@) = 0.95 V.

    A
    237.39 kJ
    B
    54 kJ
    C
    `-54kJ`
    D
    `-237.39kJ`

  • The oxidation state of Mn in MnO_4^(2-) is

    A
    `+8`
    B
    `+6`
    C
    `+7`
    D
    `+5`

    • Similar Questions

    Explore conceptually related problems

    What is the standard electrode potential for the electrode MnO_(4)^(-)//MnO_(2) in solution ? ("Given: "E_(MnO_(4)^(-)//Mn^(2+))^(@)=1.51" volt," E_(MnO_(2)//Mn^(2+))^(@)=1.23"volt")

    Find the standard electrode potential of MnO_(4)^(c-)|MnO_(2). The standard electrode potential of MnO_(4)^(c-)|Mn^(2+)=1.51V and MnO_(2)|MnO_(2)|Mn^(2+)=1.23V .

    Find out the value of n in: MnO_(4)^(-) + 8H^(+) + "ne" rarr Mn^(2+) + 4H_(2)O

    If electrode potential of following cell: Pt_(s)|Fe_(aq)^(2+),Fe_(aq)^(3+)||MnO_(4(aq))^(-),Mn_(aq)^(2+),H_(aq)^(+)|Pt_(s) is X then calculate value of 20X. [Given: E_(MnO_(4)^(-)|Mn^(2+) = 1.51 V, E_(Fe^(3+)|Fe^(2+))^(@) = 0.78 V, (2.303 RT)/F = 0.06]

    Oxidation number of Mn in K_(2)MnO_(4) is

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