Home
Class 12
CHEMISTRY
Calculate the standard Gibbs energy chan...

Calculate the standard Gibbs energy change for the redox reaction of Daniel cell .

Text Solution

Verified by Experts

Cell reaction in Daniel cell is
`Zn+Cu^(2+) aq) rarr Zn^(2+) (aq) +Cu`
The standard electrode potential, `E_("cell")^(@)` is 1.1 V.
The standard free energy change, `DeltaG^(@)= -nFE_("cell")^(@)`
` = - 2xx1.1xx96500=-21.3 "kJ mol"^(-1)`.
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTRY

    AAKASH SERIES|Exercise Subjective Exercise -1 (Short Answer Questions)|7 Videos

  • ELECTROCHEMISTRY

    AAKASH SERIES|Exercise Subjective Exercise -1 ( Very Short Answer Questions)|3 Videos

  • ELECTROCHEMISTRY

    AAKASH SERIES|Exercise PRACTICE SHEET -5 (INTEGER ANSWER TYPE QUESTIONS )|6 Videos

  • DILUTE SOLUTIONS

    AAKASH SERIES|Exercise EXERCISE - 1.2|55 Videos

  • ELEMENTS OF D - BLOCK

    AAKASH SERIES|Exercise EXERCISE - 5.2|33 Videos

Similar Questions

Explore conceptually related problems

The cell in which the following cell reaction occurs, 2Fe _((aq))^(3+)+2I_((aq))^(-)to 2Fe _((aq))^(2+)+I_(2(s)) has E_(cell)^(0)=0.236V at 298 K. Calculate the standard Gibbs energy and the equilibrium costant of the cell reaction.

The cell in which the following reaction occurs: 2Fe^(3+)(aq) + 2I^(-)(aq) to 2Fe^(2+) (aq) + I_(2)(s) has E_("cell")^(0)= 0.236 V at 298 K. Calculate the standard Gibbs energy and the equilibrium constant of the cell reaction .

The standard emf of Deniell cell is 1.1 V. Calculate the standard Gibbs energy for the cell reactions: Zn_((s))+Cu_((aq))^(2+)to Zn _((aq))^(2+)+Cu_((s))

Write the electrode reactions in a Daniel cell.

At 60^@C dinitrogen tetroxide is fifty percent dissociated. Calculate the standard free energy change at this temperature and at one atmosphere.

Which one is not a redox reaction?

AAKASH SERIES-ELECTROCHEMISTRY -PROBLEM
  1. What is the ratio of (a) gram atoms and (b) weights of the metals libe...

    Text Solution

    |

  2. During the electrolysis of fused potassium chloride at platinum electr...

    Text Solution

    |

  3. A 200 W, 110 V in candescent lamp is connected in series with cells co...

    Text Solution

    |

  4. An oxide of metal (at . Wt = 112) contains 12.5% of oxygen by weight. ...

    Text Solution

    |

  5. E^@ of zinc electrode is -0.762V. Calculate the single electrode poten...

    Text Solution

    |

  6. At what concentration of copper sulphate solution, the potential of Cu...

    Text Solution

    |

  7. At 25^(@)C, the reduction potential of hydrogen electrode is -0.118 V...

    Text Solution

    |

  8. E^(@) values of Ni^(2+), Ni and Cl(2), Cl^(-) are respectively -0.25V...

    Text Solution

    |

  9. A cell is constructed Pb^(2+) Pb and Ni^(2+), Ni electrodes. If E^(@) ...

    Text Solution

    |

  10. Calculate the standard Gibbs energy change for the redox reaction of D...

    Text Solution

    |

  11. E("cell")^(@) for the redox reation 2Ag((aq))^(+)Cu rarr Cu((aq))^(...

    Text Solution

    |

  12. Represent the cell in which the following reaction takes place Mg(s)...

    Text Solution

    |

  13. Lithinum is the strogest reductant in aqueous solutions. Why ?

    Text Solution

    |

  14. Calculate the solubility product of Ag(2)CrO(4) at 298k, if the EMF o...

    Text Solution

    |

  15. What are the limitations of fuel cells?

    Text Solution

    |

  16. What happens when lead storage battery is subjected to charging ?

    Text Solution

    |

  17. Potash solution is not recommended in a hydrocarbon-oxygen fuel cell. ...

    Text Solution

    |

  18. A long iron rod is partially dipped in common salt solution. What happ...

    Text Solution

    |

  19. Concentrated nitric acid can be transported in vessels of aluminium or...

    Text Solution

    |

  20. Highly conducting solutions favour rapid corrosion. Explain.

    Text Solution

    |