Home
Class 12
CHEMISTRY
Estimate the E^(@) reduction for Cu|CuS ...

Estimate the `E^(@)` reduction for `Cu|CuS` electrode.
Given `: K_(sp) ` of `CuS=8.0 xx 10^(-36),E^(@)._((Cu|Cu^(2+)))=-0.34V`

Text Solution

Verified by Experts


`E^(c-)._(CuS|Cu)=x`
`E^(c-)._(Cu|Cu^(2+))=-0.34V`
`E^(c-)._(cell)=x-0.34V`

Cell is in equilibrium
`:. E_(cell)=0`
`:. E_(cell)=E^(c-)._(cell)-(0.059)/(2)log[Cu^(2+)][S^(2-)]`
`E^(c-)._(cell)=(0.059)/(2)log K_(sp)`
`=(0.059)/(2)log(8.5xx10^(-36))=01.04V`
Since `E^(c-)._(cell)=x-0.34`
`:. x=-.34=-1.04Vimplies x=-0.70V`
`:. E^(c-)._(CuS|Cu)=-0.70V`
or standard reduction potential for `Cu|CuS=-0.70V.`
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Solved Examples(Electrolysis And Electrolytic Cells)|12 Videos

  • ELECTROCHEMISTRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Ex 3.1 (Objective)|28 Videos

  • ELECTROCHEMISTRY

    CENGAGE CHEMISTRY ENGLISH|Exercise Archieves Subjective|35 Videos

  • D AND F BLOCK ELEMENTS

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives Subjective|29 Videos

  • GENERAL PRINCIPLES AND PROCESS OF ISOLATION OF ELEMENTS

    CENGAGE CHEMISTRY ENGLISH|Exercise Archives (Subjective)|14 Videos

Similar Questions

Explore conceptually related problems

The standard potential E^(@) for the half reactions are as : Zn rarr Zn^(2+) + 2e^(-), E^(@) = 0.76V Cu rarr Cu^(2+) +2e^(-) , E^(@) = -0.34 V The standard cell voltage for the cell reaction is ? Zn +Cu^(2) rarr Zn ^(2+) +Cu

If excess of Zn is added to 1.0M solution of CuSO_(4) , find the concentration of Cu^(2+) ions at equilibrium. Given :E^(c-)._((Zn^(2+)|Zn))=-0.76V E^(c-)._(cell)=(E^(c-)._((Cu^(2+)|Cu))=0.34V

The solubility of CuS in pure water at 25^(@)C is 3.3 xx 10^(-4)g L^(-1) . Calculate K_(sp) of CuS . The accurate value of K_(sp) of CuS was found to be 8.5 xx 10^(-36) at 25^(@)C .

What is E^(c)._(red) for the reaction : Cu^(2+)+2e^(-) rarr Cu in the half cell Pt_(S^(2)|CuS|Cu) . if E^(c-)._(Cu^(2+)|Cu) is 0.34V and K_(sp) of CuS=10^(-35) ?

Calculate the standard free energy change in kJ for the reaction Cu^(+) +I^(-) to CuI Given: CuI + e to Cu+I^(-) E^(0)=-0.17V Cu^(+)+e to Cu E^(0)=0.53V

The 0.1M copper sulphate solution in which copper electrode is dipped at 25^(@)C . Calculate the electrode potential of copper electrode. [Given : E^(0) Cu^(+2)//Cu = 0.34V]

Find the equilibrium constant for the reaction Cu^(2+)+ 1n^(2+) Cu^(+) + 1n^(3+) Given that E_(CU^(2+)//CU^(+))^(@) = 0.15V, E_(In^(2+)//1n^(+)) = -0.4V E_(1n^(3+)//1n^(+))^(@) = - 0.42V

Cu^(+) ion is not stable in aqueous solution because because of dispropotionation reaction. E^(@) value of disproportionation of Cu^(+) is [E_(Cu^(2+)//Cu^(+))^(@)=+ 0.15 V, E_(Cu^(2+)//Cu)^(@)=0.34 V]

Calculate the DeltaG^(@) and equilibrium constant of the reaction at 27^(@)C Mg+ Cu^(+2) hArr Mg^(+2) + Cu E_(Mg^(2+)//Mg)^(@) = -2.37V, E_(Cu^(2+)//Cu)^(@) = +0.34V

CENGAGE CHEMISTRY ENGLISH-ELECTROCHEMISTRY-Solved Examples (Electrochemical Cell)
  1. The EMF of the cell : Ag|AgCl,0.1 MKCl||0.1 M AgNO(3)|Ag is 0.45V. 0...

    Text Solution

    |

  2. Calculate the potential corresponding to the following cell. Given P...

    Text Solution

    |

  3. Estimate the E^(@) reduction for Cu|CuS electrode. Given : K(sp) of...

    Text Solution

    |

  4. Knowing that K(sp) for AgCl is 1.0 xx 10^(-10), calculate E for a silv...

    Text Solution

    |

  5. Consider the following half reactions : PbO(2)(s)+4H^(o+)(aq)+SO(4)...

    Text Solution

    |

  6. The e.m.f of cell Ag|AgI((s)),0.05M KI|| 0.05 M AgNO(3)|Ag is 0.788 V....

    Text Solution

    |

  7. For the cell Zn|ZnCl(2)(m)|AgCl,E is 1.24V at 25^(@)C and 1.260V at 35...

    Text Solution

    |

  8. A saturated calomel electrode is coupled through a salt bridge with a ...

    Text Solution

    |

  9. Two weak acid solutions HA(1) and HA(2) with the same concentration an...

    Text Solution

    |

  10. Find the solubility of AgCl in 0.1 M CaCl(2). E^(c-).(Ag^(o+)|Ag)=0.79...

    Text Solution

    |

  11. The EMF of the cell : Ag|Ag(2)CrO(4)(s),K(2)CrO(4)(0.1 M)||AgNO(3)(0...

    Text Solution

    |

  12. The EMF of a galvanic cell Pt|H(2)(1 atm)|HCl(1M)|Cl(2)(g)|Pt is 1.29V...

    Text Solution

    |

  13. Calculate the potential of silver electrode in a saturated solution of...

    Text Solution

    |

  14. A solution of Fe^(2+) is titrated potentiaometrically using Ce^(4+) so...

    Text Solution

    |

  15. Find the EMF of the cell at 25^(@)C. E^(c-).(red("quinhydrone elec...

    Text Solution

    |

  16. Construct a cell using given electrodes at 298K and also calculate its...

    Text Solution

    |

  17. The EMF of the following cell is observed to be 0.118V at 25^(@)C: ...

    Text Solution

    |

  18. Find the standard electrode potential of I(2)|2I^(c-) if the equilibri...

    Text Solution

    |

  19. A silver electrode dipping in AgNO(3) solution (0.1M) is combined salt...

    Text Solution

    |

  20. The EMF of a galvanic cell composed of two hydrogen electrodes is 177 ...

    Text Solution

    |