Home
Class 12
CHEMISTRY
The standard electrode potential for Den...

The standard electrode potential for Deniell cell is `1.1V`. Calculate the standard Gibbs energy for the reaction.
`Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq)+Cu(s)`

Text Solution

Verified by Experts

We know, `DeltaG^(0)=-nFE^(@)`…(i)
n=2 for the given reaction F=96500C, `E^(@)=+1.1V`
`therefore` from (i) `DeltaG^(0)=-2xx96500xx1.1=-212300J`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • ELECTRO CHEMISTRY

    NARAYNA|Exercise W.E-9|1 Videos

  • ELECTRO CHEMISTRY

    NARAYNA|Exercise W.E-10|1 Videos

  • ELECTRO CHEMISTRY

    NARAYNA|Exercise W.E-7|1 Videos

  • 15TH GROUP ELEMENTS

    NARAYNA|Exercise EXERCISE - 4 (NCERT EXEMPLERS/HOTs)|27 Videos

Similar Questions

Explore conceptually related problems

The standard electrode potential for Deniell cell is 1.1V . Calculate the standart Gibbs energy for the reaction. Zn(s) +Cu^(2+)(aq) hArr Zn^(2+)(aq)+Cu(s)

The standard electrode potential for Daniell cell is 1.1 V. Calculate the standard Gibbs energy for the reaction. Zn(s)+Cu^(2+)(aq)rarrZn^(2+)(aq)+Cu(s)

Knowledge Check

  • The standard electrode potential for Daniel cell is 1.1V . Calculate the standard Gibbs energy of the reaction (In KJ/mol) Zn_((s))+Cu_((aq))^(2+)rarrZn_((aq))^(2+)+Cu_((s))

    A
    `106.15`
    B
    `212.3`
    C
    `193`
    D
    `403`

  • The standard electrode potential for Daniel cell is 1.1V . Calculate the standard Gibbs energy of the reaction (In KJ/mol) Zn_((s))+Cu_((aq))^(2+)rarrZn_((aq))^(2+)+Cu_((s))

    A
    `106.15`
    B
    `212.3`
    C
    `193`
    D
    `403`

  • 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)`

    • Similar Questions

    Explore conceptually related problems

    Calculate the standard free enegry change for the reaction: Zn + Cu^(2+)(aq) rarr Cu+Zn^(2+) (aq), E^(Theta) = 1.20V

    Calculate standard Gibbs free energy for the reaction : Zn+Cu^(2+)toZn^(2+)+Cu,E_("cell")^(@)=1.10V

    If the standed electrode potential for a cell is 2 V at 300 K, the equilibrium constant (K) for the reaction Zn(s)+Cu^(2+)(aq) hArrZn^(2+)(aq)+Cu(s) at 300 K is approximately (R=8JK^(-1)mol^(-1),F=96000Cmol^(-1))

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

    Calculate the standard free energy change for the reaction : Zn(s)|Zn^(2+)(1 M)||Cu^(2+)(1 M)|Cu(s) Given E_(cell)^(@)=1.10" V " .

    Home
    Profile