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The Nernst equation giving dependence of...

The Nernst equation giving dependence of electrode potential on concentration is

A

`E=E^(@) + (2.303RT)/(nF) log. ([M])/([M^(n+)])`

B

`E=E^(@) + (2.303RT)/(nF) log. ([M^(n+)])/([M]) `

C

`E=E^(@) -(2.303RT)/(nF) log. ([M^(n+)])/([M]) `

D

`E=E^(@) - (2.303RT)/(nF) log [M^(n+)]`

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Knowledge Check

  • The electrode potential of an electrode is

    A
    The potential applied to the electrode
    B
    The ionization potential of the material of the electrode
    C
    The tendency of the electrode to loose or gain electrons when it is in contact with its ions
    D
    The potential energy of the electrons in an electrode.

  • The relationship between free energy and electrode potential is

    A
    `DeltaG = nFE`
    B
    `DeltaG = nFE`
    C
    `DeltaG = (nFE)/(R)`
    D
    `DeltaG = (DeltaH)/(nFE)`

  • Nernst equation gives the variation of potential of an electrode based on activity of ions temperature and pressure. The equation is E=E^(@) -(2.303RT)/(nF) logQ (or) E=E^@ - (0.0591)/(n) log Q E^@ = Standard potential and 'Q' is the reaction quotient. Which cell has least potential ?

    A
    `ZN// underset(1M)(Zn^(+2))// underset(1M)(Cu^(+2))//Cu`
    B
    `Zn// underset(0.1M)(Zn^(+2))// // underset(0.1M)(Cu^(+2))// Cu`
    C
    `Zn // underset(0.1M)(Zn^(+2))// underset(1M)(Cu^(+2))// Cu`
    D
    `Zn// underset(1M)(Zn^(+2))// underset(0.1M)(Cu^(+2))// Cu`

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    The Nernst equation for the reduction potential of a non metal A when [A^(n-)] = C is given by

    Nernst equation gives the variation of potential of an electrode based on activity of ions temperature and pressure. The equation is E=E^(@) -(2.303RT)/(nF) logQ (or) E=E^@ - (0.0591)/(n) log Q E^@ = Standard potential and 'Q' is the reaction quotient. What is the reduction potential of a hydrogen electrode in an aqueous solution containing 0.1 M NH_4OH,(Kb=10^(-5)) , ?

    If the standard electrode protential of Cu^(2+)// Cu electrode is 0.34 V , what is the electrode potential at 0.01 M concentration of Cu^(2+) ? (T = 298^(@) K)

    Stopping potential depends on

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