Home
Class 12
CHEMISTRY
Calculate the emf of the cell Cu(s) | Cu...

Calculate the emf of the cell
`Cu(s) | Cu^(2+) (aq) || Ag^(+)(aq) | Ag(s)`
Given,
`E_((Cu^(2+))//(Cu))=+ 0.34 V, E_((Ag^(+))//( Ag)) = 0.80 V`

A

+ 0.46V

B

+1.14V

C

+ 0.57V

D

-0.46V

Text Solution

Verified by Experts

The correct Answer is:
A
Given, `E_((Cu^(2+))//(Cu))=+ 0.34 V` and `E_((Ag^(+))//( Ag)) = 0.80V`
`E_(cell)^@=E_(cathode)^@-E_(anode)^@= E_((Ag^(+))//( Ag))- E_((Cu^(2+))//( Cu))`
`therefore` emf of the cell, `E_(cell)^@=0.80-0.35=+0.46V`
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • EAMCET-2019 (TS) SHIFT-1

    SIA PUBLICATION|Exercise CHEMISTRY|30 Videos

  • ENVIRONMENTAL CHEMISTRY

    SIA PUBLICATION|Exercise PROBLEM|16 Videos

Similar Questions

Explore conceptually related problems

Calculate the EMF of the cell Cu//Cu^(2+)(0.1M)"//"Cl^(-) (0.01)// 1/2 Cl_(2) , Pt E^(@) Cu^(2+)//Cu = +0.33V E^(@) 1/2 Cl_(2)//Cl^(-) = +1.36V

Write the cell reaction taking plce in the cell CU_((s))|Cu_((aq))^(+2)||Ag _((aq))^(+) |Ag _((s))

Knowledge Check

  • The cell reaction of the galvanic cell, Cu(s) // Cu^(2+)(aq) // Hg^(2+) (aq) // Hg (l) is

    A
    `Hg + Cu^(2+) to Hg^(2+) + Cu`
    B
    `Hg + Cu^(2+) to Hg^(+) + Cu^(+)`
    C
    `Hg + Cu^(+) to CuHg`
    D
    `Cu + Hg^(2+) to Cu^(2+) + Hg `

  • E.M.F of the cell reaction, 2Ag^(+) + Cu rarr 2Ag + Cu^(2+) is 0.46V. If E_(Cu^(2+)//Cu)^(@) is +0.34V, E_(Ag^(+)//Ag)^(@) is

    A
    0.80 V
    B
    0.12 V
    C
    0.40 V
    D
    1.60 V

  • E.M.F of the cell reaction , 2Ag^(+) + Cu to 2Ag + Cu^(2+) is 0.46 V . If E_(Cu^(2+) // Cu)^(0) is | 0.34 V , E_(Ag^(+)//Ag)^(0) is

    A
    `0.80`
    B
    `0.12 V `
    C
    `0.40 V `
    D
    `1.60 V `

    • Similar Questions

    Explore conceptually related problems

    Define emf. Calculat the emf of the following galvanic cell : Zn_((s))+Cu_((aq))^(+2)to Zn_((aq))^(+2)+Cu_((s)) E_(zn^(+2//Zn))^(0) =0.76V(anode) ,E_(cu^(+3//Cu))^(0)=+0.34 (Cathode)

    Which metal will dissolve if the cell works Cu|Cu^(2+)||Ag^(+)|Ag

    E_("red")^(0) (Standard reduction potential ) of different half-cells are given E_(Cu^(+2)//Cu)^(0) = 0.34 V E_(Zn^(+2)//Zn)^(0) = -0.76 V , E_(Ag^(+) // Ag)^(0) = 0.80 V , E_(Mg^(2+) // Mg)^(0) = -2.37 V . In which cell DeltaG^(@) is most negative ?

    The standard reduction potentials for the two half-cell reactions are given below : Cd^(2+) (aq) + 2e^(-) to Cd(s) , E^(0) = -0.40 V " "Ag^(+)(aq) + e^(-) to Ag(s) , E^(0) = 0.80 V The standard free energy change for the reaction 2Ag_((aq))^(+) + Cd_((s)) + Cd_((aq))^(2+) is given by

    Consider the systems having liquid-solid interface, (a) copper wire in silver nitrate solution and (b) silver wire in copper sulphate solution. Predict which interface will show spontaneous reaction, if E_(Cu^(2+)//Cu)^(@)=0.34V and E_(Ag^(+)//Ag)^(@)= 0.80V ?

    Home
    Profile