Home
Class 12
CHEMISTRY
The standard potential of a cell using t...

The standard potential of a cell using the reaction is `1.12`. The heat of the reaction is `-504.2kJ mol ^(-1)` at `25^(@)C`. Calculate the entropy change.

Text Solution

Verified by Experts

`2Ni(s)+4H_(2)Orarr 2Ni(OH)_(2)+4H^(o+)+4e^(-)`
`4H^(o+)+O_(2)+4e^(-)rarr2H_(2)O`
`DeltaG^(c-)=-nFE^(c-)=-4xx96500xx1.12=-432320J`
`DeltaG^(c-)=DeltaH^(c-)-TDeltaS^(c-)`
`:. DeltaS^(c-)=(DeltaH^(c-)-DeltaG^(c-))/(T)`
`=-(504.2xx10^(3)J-(-432320))/(298)`
`=-241.2JK^(-1)mol^(-1)`
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 emf of the cell reaction Zn(s) +Cu^(2+) (aq) rarr Zn^(2+) (aQ) +Cu(s) is 1.1V . Calculate the free enegry change for the reaction. If the enthalpy of the reaction is -216.7 kJ mol^(-1) , calculate the entropy change for the reaction.

The standard potential of a cell using the reaction +3HgO(s)+2(overset(c-)(O)H) (aq) is 0.489V at 25^(@)C . What is the equilibrium constant of the reaction ?

At 27^@C latent heat of I^- fusion of a compound is 2.7xx10^3 J mol^(-1) . Calculate the entropy change during fusion.

The standard free energy change for a reaction is -213.3 KJ mol^(-1) "at" 25^(@)C . If the enthalpy change of the reaction is -217.77 KJ "mole"^(-1) . Calculate the magnitude of entropy change for the reaction in Joule "mole"^(-1)

Cells use the hydrolysis of adenosine triphosphate, abbreviated as ATP, as a source of energy. Symbolically, this reaction can be written as where ADP represents adenosine diphosphate. For this reaction, "deltaG^(@) is 30 kJ/mol and delta H^0 is -30 kJ/mol at 27^(@)C . Calculate the entropy change.

The activation energy of exothermic reaction ArarrB is 80 kJ "mol"^(-1) . The heat of reaction is 200 kJ "mol"^(-1) . The activation energy for the reaction Brarra ( in kJ/mol) will be :

If the enthalpy change for the transition of liquid water to steam is 300kJ mol^(-1)" at "27^(@)C , the entropy change for the proces would be

Zinc reacts with dilute hydrochloric acid to give hydrogen at 17^(@)C . The enthalpy of the reaction is -12.00 kJ mol^(-1) of zinc and entropy change equals 50 J K^(-1) mol^(-1) for the reaction. Calculate the free enegry change and predict whether the reaction is spontaneous or not.

If the enthalpy change for the transition of liquid water to steam is 30 kJ mol^(-1)" at " 27^@C the entropy change for the process would be

The standard emf of a galvanic cell involving cell reaction with n = 2 is found to be 0.295 V at 25^(@)C . The equilibrium constant of the reaction would be (Given F=96,500 C mol^(-1), R = 8.314 JK^(-1) mol^(-1) ):

CENGAGE CHEMISTRY ENGLISH-ELECTROCHEMISTRY-Solved Examples (Electrochemical Cell)
  1. A graph is plotted between E(cell) and log .([Zn^(2+)])/([Cu^(2+)]) . ...

    Text Solution

    |

  2. Given : NO(3)^(-) rarrNO(2)( acidic medium ), " "E^(-)=0.8V N...

    Text Solution

    |

  3. The standard potential of a cell using the reaction is 1.12. The heat...

    Text Solution

    |

  4. The standard potential of a cell using the reaction +3HgO(s)+2(overse...

    Text Solution

    |

  5. The EMF of the cell : Ag|AgCl,0.1 MKCl||0.1 M AgNO(3)|Ag is 0.45V. 0...

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |

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

    Text Solution

    |