Home
Class 12
CHEMISTRY
Calculte the standard free energy change...

Calculte the standard free energy change for the reaction occurring in a Daniell cell `(E_("cell")^(@)=1.10V)`.
`Zn(s)+Cu^(2+)(aq)rarrZn^(2+)(aq)+Cu(s)`

Text Solution

Verified by Experts

`{:("Anode reaction: "Zn(s)" "rarr" "Zn^(2+)(aq)+2e),("Cathode reaction : "Cu^(2+)(aq)+2e" "rarr" "Cu(s)),(bar(" Cell reaction: "Zn(s)+Cu^(2+)(aq)" "rarr" "Zn^(2+)(aq)+Cu(s))):}`
As 2 mol electrons are involved in the cell reaction, n = 2.
Therefore, the standard free energy change,
`DeltaG^(@)=-nFE^(@)`
`=-(2xx96500xx1.10)=-212300J,C-212300J`
`=-212.3" kJ "[because "1 volt - coulomb = 1 joule"]`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    CHHAYA PUBLICATION|Exercise PROBLEM|7 Videos

  • ELECTROCHEMISTRY

    CHHAYA PUBLICATION|Exercise WARM UP EXERCISE|62 Videos

  • D - AND F - BLOCK ELEMENTS

    CHHAYA PUBLICATION|Exercise PRACTICE SET 8 (Answer the following questions)|10 Videos

  • ENVIRONMENTAL CHEMISTRY

    CHHAYA PUBLICATION|Exercise PRACTICE SET 14(Answer the following questions)|6 Videos

Similar Questions

Explore conceptually related problems

Determine DeltaG^(@) and the value of the equilibrium constant for the following reaction occurring in an electrochemical cell at 25^(@)C . Cu(s)+2Ag^(+)(aq)rarr Cu^(2+)(aq)+2Ag(s) Given that, E_(Cu^(2+)|Cu)^(@)=0.34V and E_(Ag^(+)|Ag)^(@)=0.80V

Calculate the value of equilibrium constant of the reaction occurring in Deniell cell at 25^(@)C . Given : E_(Zn^(2+)|Zn)^(@)=-0.76V and E_(Cu^(2+)|Cu)^(@)=+0.34V

Determine DeltaG^@ and the value of the equlibrium constant for the following reaction occurring in an electrochemical cell at 25^@C . Cu (s) + 2Ag^+ (aq) rarr Cu^(2+)(aq)+2Ag(s) Given that E_(Cu^(2+)//Cu)^@=0.34 V and E_(Ag^+//Ag)^@ =0.80V

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

Calculate the EMF of the electrochemical cell for which the following cell reaction is given below- Zx(S) + ni^(2_+)(aq) rarr Zn^(+2)(aq) + Ni(S) Given E_(zn^2//zn)^@ = - 0.76 V E_(Ni^(2+) // Nl) = - 0.25 V.

Calculate the standard cell potential of the galvanic cell in which the following reaction takes place: Fe%(2+)(aq)+Ag^(+)(aq)rarrFe^(3+)(aq)+Ag(s) Calculate the Delta_(r)G^(@) and equilibrium constant of the reaction also. (E_(Ag^(+)|Ag)^(@)=0.80V, E_(Fe^(3+)|Fe^(2+))^(@)=0.77V)

Calculate the standard cell potentials of the galvanic cells in which the following reactions take place : Fe^(2+)(aq)+Ag^(+)(aq)rarr Fe^(3+)(aq)+Ag(s) Calculate Delta_(r )G^(0) , equilibrium constant of the reactions.

Write the anode and cathode reactions for the given cell reactions. S_(2)O_(8)^(2-)(aq)+2I^(-)(aq)rarr2SO_(4)^(2-)(aq)+I_(2)(s)

Calculate the standard emf of the cell having the standard free energy change of the cell reaction is -64.84 kJ for 2 electrons transfer.

Under standard conditions, the following reactions occur spontaneously : (i) Zn(s)+2Ag^(+)(aq)rarrZn^(2+)(aq)+2Ag(s) (ii) Fe(s)+Cu^(2+)+(aq)rarrCu(s)+Fe^(2+)(aq) (iii) Cu(s)+2Ag^(+)(aq)rarr Cu^(2+)(aq)+2Ag(s) (iv) Zn(s)+Cu^(2+)(aq)rarrCu(s)+Zn^(2+)(aq) (v) Zn(s)+Fe^(2+)(aq)rarr Fe(s)+Zn^(2+)(aq) (vi) Fe(s)+2Ag^(+)(aq)rarr Fe^(2+)(aq)+2Ag(s) If E_(Zn^(2+)|Zn)^(@), E_(Fe^(2+)|Fe)^(@), E_(Ag^(+)|Ag)^(@) and E_(Cu^(2+)|Cu)^(@) have value of x, y, z and p volt respectively, then -