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What does the high negative value of standard reduction potential of an electrode indicate?

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Knowledge Check

  • Which cell will measure standard electrode potential of copper electrode ?

    A
    `Pt(s)|H_(2)("g, 0.1 bar")|H^(+)(aq, 1M)|Cu^(2+)(aq, 1M)|Cu(s)`
    B
    `Pt(s)|H_(2)("g, 1bar")|H^(+)(aq, 1M)|Cu^(2+)("aq, 2M")|Cu(s)`
    C
    `Pt(s)|H_(2)("g, 1bar")|H^(+)(aq, 1M)|Cu^(2+)("aq, 1M)|Cu(s)`
    D
    `Pt(s)|H_(2)("g, 1bar")|H^(+)(aq, 0.1M)|Cu^(2+)("aq, 1M")|Cu(s)`

  • Which cell will measure standard electrode potential of copper electrode -

    A
    `Pt(s)|H_(2)"(g, 0.1 bar)"|H^(+)"(aq, 1M)"||Cu^(2+)"(aq, 1M)"|Cu`
    B
    `Pt(s)|H_(2)"(g, 1 bar)"|H^(+)"(aq, 1M)"||Cu^(2+)"(aq, 1M)"|Cu`
    C
    `Pt(s)|H_(2)"(g, 1 bar)"|H^(+)"(aq, 1M)"||Cu^(2+)"(aq, 1M)"|Cu`
    D
    `Pt(s)|H_(2)"(g, 1bar)"|H^(+)"(aq, 0.1M)"||Cu^(2+)"(aq, 1M)"|Cu`

  • 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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