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Nernst equation gives the variation of p...

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))`, ?

A

0.02 V

B

0.03 V

C

0.06 V

D

0.01 V

Text Solution

Verified by Experts

The correct Answer is:
A
`E_1 = E^(0) + (0.06)/(3) logC , E_2 = E^(0) +(0.06)/(3) log ((C)/(10))`
` (E_2 -E_1) = (0.06)/(3) [log""((C)/(60))-logC] = 0.02 log((C)/(10) xx (1)/(C)) = 0.02 xx log 10^(-1) = -0.02V`
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Knowledge Check

  • 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`

  • What is the potential of half-cell consisting of zinc electrode in 0.01 M ZnSO_(4) solution at 25^(@)C(E_(o x)^(@)=0.763V)

    A
    0.8221 V
    B
    8.221 V
    C
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  • E^@Cu^(2+)//Cu is + 0.34V At which one of the following concentrations of Cu^(2+) , reduction potential of copper electrode becomes zero

    A
    `1.76 xx 10^(-6)M`
    B
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    C
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    D
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    The driving force DeltaG diminishes to zero on the way to equilibrium, just as in any other spontaneous process. Both DeltaG and the corresponding cell potential (E = (DeltaG)/(nF)) zero when the redox reaction comes to equilibrium. The Nernst equation for the redox process of the cell may be given as : E= E^(@) -(0.059)/( n) log Q The key to the relationship is the standard cell potential E^(@) , derived from the standard free energy change as : E^(@)=-(DeltaG^(@))/(nF) . At equilibrium, the Nernst equation is given as : E^(@) = -(0.059)/(n) log K On the basis of information available for the reaction : (4)/(3) Al + O_2 to (2)/(3) Al_2 O_3 , DeltaG = -827kJ// mol of O_2 the minimum emf required to carry out an electrolysis of Al_2O_3 is : ( Given 1 F = 96500 C )

    The Nernst equation , E = E^(0) -(RT)/(nF) . In Q indicates that the equilibrium constant K_(c) will be equal to Q when :

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