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Write the cell representation for the galvanic cell used for measuring standard electrode potential of iron having `E_(Fe^(2+)//Fe)^(@) = -0.44V`

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Knowledge Check

  • A galvanic cell with electrode potential of zinc=+0.76 and of copper =0.34V . The E.M.F is

    A
    0.76V
    B
    0.34V
    C
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    D
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  • Copper from copper sulphate solution can be displaced by ………….The standared reduction potentials of some electrodes are given below: E^@(Fe^(2+),Fe) =-0.44V E^@(Zn^(2+),Zn)=-0.76 V E^@(Cu^(2+),Cu) =+0.34V E^@(Cr^(3+),Cr)=-0.74V E^@(H^+,1/2 H_2)=-0.00 V

    A
    `H_2`
    B
    Zn
    C
    Cr
    D
    All

  • Copper from copper sulphate solution can be displaced by ………….The standared reduction potentials of some electrodes are given below: E^@(Fe^(2+),Fe) =-0.44V E^@(Zn^(2+),Zn)=-0.76 V E^@(Cu^(2+),Cu) =+0.34V E^@(Cr^(3+),Cr)=-0.74V E^@(H^+,1/2 H_2)=-0.00 V

    A
    `H_2`
    B
    Zn
    C
    Cr
    D
    All

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    A cell is set up between ‘Zn’ and ‘Cu’ electrode. If the two half cells work under standard condition, calculate the cell potential. Given E^@(Zn^(2+)//Zn)=-0.76V and E^@(Cu^(2+)//Cu)=+0.34V .

    What is electrode potential ? Write the expression for the emf of a cell in terms of oxidation potential.

    For the zinc electrode the standard oxidation potential is +0.76V. then what is its standard reduction potential?

    A copper silver cell is setup. The copper ion concentration is 0.10 M.The concentration of silver ion is not known. The cell potential when measured was 0.422 V . Determine the concentration of silver ions in the cell . [Given E_(Ag^(+)//Ag)^(@) = 0.80 V, E_(cu^(2+)//Cu)^(@) = + 0.34 V ]

    A cell has e.m.f.E.A potentiometer measures potential difference V , then

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