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The standard electrode potential of Cu^(...

The standard electrode potential of `Cu^(2+)|Cu` half cell is `+0.34V`. What does it mean?

Text Solution

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It means that at `25^(@)C`, when a copper rod remains in contact with a solution of `Cu^(2+)` ions at 1 M concentration, the electrical potential developed by the formation of oppositely charged electrical double layer, at the interface of copper rod and solution is `+0.34V`.
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The standard electrode potential of Daniell cell is 1.1V. Calculate the standard Gibbs energy for the reaction : Zn(s)+Cu^(2+)(aq)rarr Zn^(2+)(aq)+Cu(s)

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Knowledge Check

  • Consider the following four electrodes : P=Cu^(2+)"(0.001 M)|Cu(s) Q=Cu^(2+)("(0.1 M)"|Cu(s) R=Cu^(2+)"(0.01 M)"|Cu(s) S=Cu^(2+)"(0.001)"|Cu(s) If the standard electrode potential of Cu^(2+)|Cu is +0.34V , the reduction potential in volts of the above electrodes follows the order-

    A
    `P gt S gt R gt Q`
    B
    `S gt R gt O gt P`
    C
    `R gt S gt O gt P`
    D
    `Q gt R gt S gt P`

  • The positive value of the standard electrode potential of Cu^(2+)|Cu indicates that -

    A
    this redox couple is a stronger reducing agent than the `H^(+)|H_(2)` couple
    B
    this redox couple is stronger oxidising agent than `H^(+)|H_(2)`
    C
    `Cu` can displace `H_(2)` from acid
    D
    `Cu` cannot displace `H_(2)` from acid

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