Home
Class 12
CHEMISTRY
Calculate the E.M.F. of the zinc - silve...

Calculate the E.M.F. of the zinc - silver cell at `25^(@)C` when `[Zn^(2+)]=0.10M and [Ag^(+)]=10M.[E^(@) " cell at "25^(@)C="1.56 volt"]`

Text Solution

Verified by Experts

The cell reaction in the zinc - silver cell would be
`2Ag^(+)+Zn hArr 2Ag+Zn^(2+)`
The Nernst equation for the above all reaction may be written as :
`E_("cell")=E_("cell")^(@)-(RT)/(nF)ln([Ag]^(2)[Zn^(2+)])/([Ag^(+)]^(2)[Zn])`
(since concentrations of solids are taken as unity)
`=E_("cell")^(@)-ln.([Zn^(2+)])/([Ag^(+)]^(2))`
Substituting the various values in Nernst equation, we have
`E_("cell")=1.56-(2.303xx8.314xx298)/(2xx96495)log""(0.1)/((10)^(2))`
`="1.648 volts."`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY - II

    NCERT GUJARATI|Exercise SELF EVALUATION((B) Answer in one or two sentences :)|2 Videos

  • ELECTROCHEMISTRY - II

    NCERT GUJARATI|Exercise SELF EVALUATION((D) Solve the problems :)|11 Videos

  • ELECTRO CHEMISTRY - I

    NCERT GUJARATI|Exercise SELF EVALUATION((D) Solve the problems :)|6 Videos

  • ETHERS

    NCERT GUJARATI|Exercise SELF EVALUATION ((D) Answer not exceeding sixty words :)|2 Videos

Similar Questions

Explore conceptually related problems

Calculate the voltage E of the cell at 25^(@)C Mn(s) |Mn(OH_(2))(s)|Mn^(2+)(x,M)OH^(-) (1.00 xx 10^(-4)M)||Cu^(2+) (0.675M)|Cu(s) given that K_(sp) = 1.9 xx 1-^(-13) for Mn(OH)_(2)(s) E^(@) (Mn^(2+)//Mn) =- 1.18 V, E^(@) (Cu^(+2)//C) = +0.34V

Calculate the cell e.m.f. and DeltaG for the cell reaction at 298K for the cell. Zn(s) | Zn^(2+) (0.0004M) ||Cd^(2+) (0.2M)|Cd(s) Given, E_(Zn^(2+)//Zn)^(@) =- 0.763 V, E_(Cd^(+2)//Cd)^(@) = - 0.403 V at 298K . F = 96500 C mol^(-1) .

For a cell reaction involving a two-electron change, the standard e.m.f. of the cell is found to be 0.295V at 25^(@)C . The equilibrium constant of the reaction at 25^(@)C will be:

Calculate the EMF of a Daniel cell when the concentartion of ZnSO_(4) and CuSO_(4) are 0.001M and 0.1M respectively. The standard potential of the cell is 1.1V .