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Write Nernst equation for the following ...

Write Nernst equation for the following cell reaction :
`Zn(s) | Zn^(2+)(aq)|| Cu^(2+)(aq) | Cu(s)`

Text Solution

Verified by Experts

`E_(cell) = E_(cell)^(Theta) - (2.303 RT)/(6 F) log ([Al^(3+)]^(2))/([Fe^(2+)]^(3))`
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Knowledge Check

  • The correct representation of Nernst equation for half-cell ,reaction Cu^(2+) (aq) + e^(-) to Cu^(+) (aq) is

    A
    `E_(cu^(+),cu^(2+))^(@) = E_(cu^(+),cu^(2+))^(@) - (0.0592)/(2) log .([Cu^(+)])/([Cu^(2+)])`
    B
    `E_(cu^(+),cu^(2+))^(@) = E_(cu^(+),cu^(2+))^(@) - (0.0592)/(1) log .([Cu^(+)])/([Cu^(2+)])`
    C
    `E_(cu^(+),cu^(2+))^(@) = E_(cu^(+),cu^(2+))^(@) - (0.0592)/(2) log .([Cu^(+)])/([Cu^(2+)])`
    D
    `E_(cu^(+),cu^(2+))^(@) = E_(cu^(+),cu^(2+))^(@) - (0.0592)/(1) log .([Cu^(+)])/([Cu^(2+)])`

  • What is the Gibbs energy of the following reaction? Zn(s)+Cu^(2+) (aq) rarr Zn^(2+)(aq)+Cu^(2+) (s), E_("cell")^(@)=1.1 V

    A
    `106135.75 J mol^(-1)`
    B
    `21227 J mol^(-1)`
    C
    `-212.27 kJ mol^(-1)`
    D
    `21227 J mol^(-1)`
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