Home
Class 12
CHEMISTRY
DeltaG is the available energy (energy p...

`DeltaG` is the available energy (energy produced) during the electochemical reaction in galvanic cell which can be converted into useful work. In the light of second law of thermodynamics, in the cell, the change in electrode potential with temperature will be equal to:

A

`DeltaS)/(nF)`

B

`(nF)/(DeltaS)`

C

`-2.303` RT log `K_(c)`

D

`(-2.303 RT)/(nF)`

Text Solution

Verified by Experts

The correct Answer is:
A
Promotional Banner

Topper's Solved these Questions

  • ELECTROCHEMISTY

    GRB PUBLICATION|Exercise Faraday s Laws and Electrolysis|87 Videos

  • ELECTROCHEMISTY

    GRB PUBLICATION|Exercise Conductance and Kohlrausch s law|40 Videos

  • ELECTROCHEMISTY

    GRB PUBLICATION|Exercise Batteries|10 Videos

  • D-BLOCK ELEMENTS

    GRB PUBLICATION|Exercise Subjective Type|18 Videos

  • ENVIRONMENTAL CHEMISTRY

    GRB PUBLICATION|Exercise Straight objective type|40 Videos

Similar Questions

Explore conceptually related problems

Photoelectric cell is a device in which the light energy is converted into

Write equation for the reaction between free energy change and standard cell potential.

What is the relationship between Gibbs free energy of the cell reaction in a galvanic cell and the emf of the cell ? When will the maximum work be obtained froma galvanic cell ?

Photo cell is a device in which light energy is converted into

The cell potential (E) and the free energy change (Delta G) accompanying an electrochemical reaction are related by

Solar cell is a photoelectric cell, which converts light energy into electrical energy.

The emf of a galvanic cell is positive when free energy change of reaction is

GRB PUBLICATION-ELECTROCHEMISTY-Thermodynamics in Electrochemistry
  1. DeltaG^(@) of the cell reaction AgCl(s) + 1/2H(2) rightarrow Ag(s) +...

    Text Solution

    |

  2. The emf of the cell Zn|ZnCl(2) (0.05M) | AgCl(s),Ag is 1.015 V at 298 ...

    Text Solution

    |

  3. The Gibbs energy for the decomposition of Al(2)O(3) at 500^(@)C is as...

    Text Solution

    |

  4. Calculate the cell EMF in mV for Pt|H(2)(1atm)|HCl(0.01M)||AgCl(s)|A...

    Text Solution

    |

  5. What is cell entropy change of the following cell? Pt(s)|H(2)(g)|CH(3)...

    Text Solution

    |

  6. At 298 K the standard free energy of formation of H(2)O(l) is -237.20 ...

    Text Solution

    |

  7. The potential of the Daniel cell, Zn |(ZnSO(4))||(CuSO(4)|Cu was repor...

    Text Solution

    |

  8. Using the data in the preceding problem, calcualte the equilibrium con...

    Text Solution

    |

  9. DeltaG = DeltaH - TDeltaS and DeltaG + T[(d(DeltaG))/(dT)](p) then ((d...

    Text Solution

    |

  10. DeltaG is the available energy (energy produced) during the electochem...

    Text Solution

    |

  11. At 298 K the standard free energy of formation of H(2)O (l) is -237.20...

    Text Solution

    |

  12. DeltaG^(@) of the cell reaction AgCl(s) + 1/2H(2) rightarrow Ag(s) +...

    Text Solution

    |

  13. The EMF of an electrolytic cell does not depend upon:

    Text Solution

    |

  14. For the reaction: C(3)H(8)(g) + 5O(2)(g) rightarrow 3CO(2)(g) + 4H(2...

    Text Solution

    |

  15. Ag^(aq) + e^(-) rightarrow Ag(s) E69@) = 0.80 V Mg^(2+)(aq) + 2e^(-)...

    Text Solution

    |

  16. What is the DeltaG^(@) value for the electrochemical cell below? Cu(...

    Text Solution

    |

  17. 10Cl^(-)(aq) + 2MnO(4)^(-)(aq) + 16H^(+)(aq) rightarrow 5Cl(2)(g) + 2M...

    Text Solution

    |

  18. The standard potential for the reaction, Cl(2)(g) + 2Br^(-)(aq) righ...

    Text Solution

    |

  19. What is the approximate value of the equilibrium constant, K(eq), at 2...

    Text Solution

    |

  20. 3Ni^(2+) + 2Al rightarrow 2Al^(3+) + 3Ni, E^(@0 = 1.41 V For the rea...

    Text Solution

    |