Home
Class 12
CHEMISTRY
Calculate the standard cell potentials a...

Calculate the standard cell potentials at `25^(@)C` for the electrochemical cells, `Zn | Zn^(2+)||` reference half-cell and reference half-cell `||Cu^(2+)| Cu`, where the reference half-cell is,
(i) SHE
(ii) Ag` //` AgCl electrode.

Text Solution

Verified by Experts

The correct Answer is:
(i) 0.76 V, 0.34V (ii) 0.98V, 0.12V
Doubtnut Promotions Banner Mobile Dark
|

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    ARIHANT PUBLICATION|Exercise CHAPTER PRACTICE ( LONG ANSWER TYPE QUESTIONS) |3 Videos

  • ELECTROCHEMISTRY

    ARIHANT PUBLICATION|Exercise CHAPTER PRACTICE ( SHORT ANSWER TYPE I QUESTIONS) |10 Videos

  • D-BLOCK ELEMENTS

    ARIHANT PUBLICATION|Exercise Chapter practice (Long answer type questions)|2 Videos

  • ELEMENTS : NITROGEN FAMILY

    ARIHANT PUBLICATION|Exercise CHAPTER PRACTICE ( Long Answer Type Questions ) |11 Videos

Similar Questions

Explore conceptually related problems

Calculate the half cell potential at 25^@C for the cell reaction Cu^(2+)(aq)+2erarrCu , When [Cu^(2+)]=4M and E^@(Cu^(2+)//Cu)=0.34V .

Calculate the standard reduction potential of (Ag^+)/ (Ag) electrode when the cell potential for the cell Cu | Cu^2+ (1M) | | Ag^+(1M) | Ag is 0.46 V .

Knowledge Check

  • The standard cell potential for the cell is , Zn|Zn^(2+)(1M)||Cu^(2+)(1M)|Cu [E^@ for Zn^(2+)//Zn=-0.76V, E^@ for Cu^(2+)//Cu=+0.34V]

    A
    `-0.76+0.34=-0.42V`
    B
    `-0.34-(-0.76)=+0.42V`
    C
    `0.34-(-0.76)=+1.10V`
    D
    `-0.76-(+.34)=-1.10V`

  • The standard cell potential for the cell is , Zn|Zn^(2+)(1M)||Cu^(2+)(1M)|Cu[E^@ for Zn^(2+)//Zn=-0.76,E^@forCu^(2+)//Cu=+0.34]

    A
    `-0.76+0.34=-0.42V`
    B
    `-0.34-(-0.76)=+0.42V`
    C
    `0.34-(-0.76)=+1.10V`
    D
    `-0.76-(+.34)=-1.10V`

    • Similar Questions

    Explore conceptually related problems

    If the standard half cell and reduction potentials are 0.522 V for Cu^+ | Cu and 0.3402V for Cu^(2+) | Cu . Find the standard half cell potential for Cu^(2+) | Cu+ .

    Calculate the standard electrode potential of Ni^(2+) | Ni electrode if emf of the cell, Ni(s) | Ni^(2+) ( 0.01 M ) || Cu^(2+) ( 0.1M) | Cu(s) is 0.059 V. [ Given E_(Cu^(2+) //Cu) ^(@) = + 0.34V

    A cell is prepared by dipping a copper rod in 1 M CuSO_(4) solution and a nickel rod in 1 M NiSO_(4) solution. The standard reduction potentials of copper electrode and nickel electrode are 0.34 V and -0.25V , respectively, (i) What will be the cell reaction? (ii) What will be the standard EMF of the cell? (iii) Which electrode will be positive? (iv) How will the cell be represented?

    What are Electrochemical cells ? What would happen if no salt bridge were used in electrochemical cell like Zn - Cu cell ? Write the Nernst equation to calculate the emf of this cell.

    Calculate the half-cell potential at 298 K for the reaction Cu^(2+) ( aq) + 2e^(-) rarr Cu(s) where [ Cu^(2+) ] is 5.0 M and E^(@) is + 0.34 V

    Give the half-cell and net cell reactions in the following batteries. (i) Leclanche cell (ii) Nickel-metal hydride battery

    Home
    Profile