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Calculate the standard reduction potenti...

Calculate the standard reduction potential of `Ag^(+)|Ag` electrode when the cell potential for the cell ,
`Cu (s) |Cu^(2+) (1 M) || Ag^(+) (1 M) Ag` is 0.46 V . Given that `Cu^(2+) |Cu = 0.34` V

Text Solution

Verified by Experts

The correct Answer is:
0.80 V
`E_(Cell)^(Theta) = E_((Ag^(+) |Ag))^(Theta) - E_((Cu^(2+) |Cu))^(Theta)`
`0.46 = E_(Ag^(+) |Ag)^(Theta) = -0.34`
`therefore E_((Ag^(+)|Ag))^(Theta) = 0.80 V`
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Knowledge Check

  • Calculate the emf of the following cell: Cu(s)|Cu^(2+) (aq)||Ag^(+) (aq)| Ag(s) Given that, E_(Cu^(2+)//Cu)^(@)=0.34 V, E_(Ag//Ag^(+))^(@)=-0.80 V

    A
    0.046 V
    B
    0.46 V
    C
    0.57 V
    D
    `-0.46 V`

  • If the standard electrode poten tial of Cu^(2+)//Cu electrode is 0.34V. What is the electrode potential of 0.01 M concentration of Cu^(2+) ?

    A
    0.399V
    B
    0.281V
    C
    0.222V
    D
    0.176V

  • The standard cell potential for the cell Zn|Zn^(2+) (1 M)|| Cu^(2+) (1 M)| Cu Given E_(Cu^(2+)//Cu)^(@) = 0.34 V and E_(Zn^(2+)//Zn)^(@) = - 0.76 V is

    A
    1.10 V
    B
    ` - 0.42 V `
    C
    `-1.10 V`
    D
    None of these
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