Home
Class 11
CHEMISTRY
The enthalpy and entropy change for the ...

The enthalpy and entropy change for the reaction,
`Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g)`
are `30KJmol^(-1)` and `105JK^(-1)mol^(-1)` respectively. The temperature at which the raction will be in equilibrium is:

A

300 K

B

285.7 K

C

273 K

D

450 K

Text Solution

Verified by Experts

The correct Answer is:
B
`DeltaG=DeltaH-T Delta S`
Promotional Banner

Topper's Solved these Questions

  • THERMODYNAMICS

    NARAYNA|Exercise Level -II (C.W)|41 Videos

  • THERMODYNAMICS

    NARAYNA|Exercise Level -III|64 Videos

  • THERMODYNAMICS

    NARAYNA|Exercise C.U.Q|122 Videos

  • STRUCTURE OF ATOM

    NARAYNA|Exercise EXERCISE - IV EXEMPLAR PROBLEMS|24 Videos

Similar Questions

Explore conceptually related problems

The enthalpy and entropy change for the reaction, Br_(2)(l)+Cl_(2)(g)rarr2BrCl(g) are 30KJmol^(-1) and 105JK^(-1)mol^(-1) respectively. The temperation at which the raction will be in equilibrium is:

The enthalpy and entropy change for the reaction Br_(2)(I) + CI_(2)(g) rightarrow 2BrCI(g) are 40 kJ mol^(-1) and 110 JK^(-1) mol ^(-1) repectively. The temperature at which the reaction will be in equilibrium is

The enthalpy and entropy change for the reaction: Br_(2)(l) + Cl_(2)(g) to 2BrCl(g) are 30 kJ mol–1 and 105 JK–1 mol–1 respectively. The temperature at which the reaction will be in equilibrium is:-

The enthalpy and entropy change for the reaction, Br_2(l) + Cl_2(g) - 2BrCl(g) are 7.1 kcal mol^-1 and 25 cal K^-1 mol^-1 respectively. This reaction will be spontaneous at

DeltaH and DeltaS for Br_(2)(l) +CI_(2)(g) rarr 2BrCI(g) are 29.00 kJ mol^(-1) and 100.0 J K^(-1) mol^(-1) respectively. Above what temperature will this reaction become spontaneous?

DeltaH and DeltaS for the reaction Br_(2)(l)+Cl_(2)(g)to2BrCl(g) are 29.37 kJ and 104.7J" "K^(-1) respectively. Above what temperature will this reaction become spontaneous?

NARAYNA-THERMODYNAMICS-Level -I (C.W)
  1. Human body requires 2370 k.cal of energy daily. If the heat of combusi...

    Text Solution

    |

  2. Energy required to dissociate 4 gms of H(2)(g) into free atoms is 208 ...

    Text Solution

    |

  3. The enthalpy change when 1.00 g of water freezes at 0^(@)C and 1.00 at...

    Text Solution

    |

  4. Deltax is given by : Deltax= ("hydration energy")+("lattice energy")...

    Text Solution

    |

  5. The bond energy of an O -H bond is 109 K. cal "mole"^(-1). When a mole...

    Text Solution

    |

  6. The heat of atomisation of PH(3) is 228 K cal/mol and that os P(2)H(4)...

    Text Solution

    |

  7. When enthalpy and entropy change for a chemical reaction are -2.5 xx10...

    Text Solution

    |

  8. The enthalpy and entropy change for the reaction, Br(2)(l)+Cl(2)(g)r...

    Text Solution

    |

  9. If Delta H("vap") of pure water at 100^(@)C is 40.627 kJ mol^(-1). The...

    Text Solution

    |

  10. The temperature at which the reaction Ag(2)O(s) rarr 2Ag(s) +1/2 O(2...

    Text Solution

    |

  11. The latent heat of fusion of ice is 5.99 kJ/mol at its melting point. ...

    Text Solution

    |

  12. The entropy change for the conversion of 1 mole of alpha-" tin" (at 13...

    Text Solution

    |

  13. DeltaH (vap) for water is 40.7 kJ mol^(-1). The entropy of vapourisati...

    Text Solution

    |

  14. Following data is known about melting of a compound AB.DeltaH=9.2kJmo...

    Text Solution

    |

  15. Combustion of hydrogen in a fuel cell at 300 K is represented as 2H(2(...

    Text Solution

    |

  16. What will be the value of Delta G^(@). If equilibrium constant for a r...

    Text Solution

    |

  17. Zn((s))+Cu((aq))^(+2) rarr Cu((s))+Zn((aq))^(+2) given that Delta(f)...

    Text Solution

    |

  18. CO((g))+1/2 O(2) (g) rarr CO(2(g)) DeltaH=-67.37 K.cal at 25^(@)C th...

    Text Solution

    |

  19. The standard Gibb's free energy change, DeltaG^(@) is related to equil...

    Text Solution

    |

  20. What is the free energy change, 'DeltaG' When 1.0 mole of water at 100...

    Text Solution

    |