Home
Class 12
CHEMISTRY
The values of DeltaH and Delta S of a ce...

The values of `DeltaH and Delta S` of a certain reaction are `-400 kJ mol^-1 and -20 kJ mol^-1 K^-1` respectively. The temperature below which the reaction is spontaneous is _________.

A

100 K

B

`20^@` C

C

20 K

D

`120^@` C

Text Solution

Verified by Experts

The correct Answer is:
C
Promotional Banner

Topper's Solved these Questions

  • CHEMICAL THERMODYNAMICS AND ENERGETICS

    TARGET PUBLICATION|Exercise EVALUATION TEST|25 Videos
  • CHEMICAL THERMODYNAMICS AND ENERGETICS

    TARGET PUBLICATION|Exercise CRITICAL THINKING|95 Videos
  • CHEMICAL KINETICS

    TARGET PUBLICATION|Exercise Evaluation test|13 Videos
  • CHEMISTRY IN EVERYDAY LIFE

    TARGET PUBLICATION|Exercise 7|3 Videos

Similar Questions

Explore conceptually related problems

The value of DeltaH and DeltaS for a reaction are respectively 30 kJ mol^(-1) and 100JK^(-1)mol^(-1) . Then temperature above which the reaction will become spontaneous is:

The values of Delta H and Delta S for the reaction are 170 kJ and 170 J K^(-1) , respectively. This reaction will be spontaneous at

For a reaction, DeltaH=10000" kJ "mol^(-1) and DeltaS=25" kJ "k^(-1)mol^(-1) . The minimum temperature, above which the reaction would be spontaneous is

The DeltaH^(@) and DeltaS^(@) value for a particular reaction are -60.0 kJ and -0.200 kJ . K^(-1) respectively, Under what reaction spontaneous?

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?

For a certain reaction X rarr Y the value of DeltaH and DeltaS are 50.50KJ mol^(-1) and 100.03JK^(-1) respectively. The temperature at which DeltaG=0 is

DeltaH and DeltaS for a reaction are +30.558 kJ mol^(-1) and 0.66 kJ mol^(-1) at 1 atm pressure. The temperature at which free energy is equal to zero and the nature of the reaction below this temperature are

TARGET PUBLICATION-CHEMICAL THERMODYNAMICS AND ENERGETICS -COMPETITIVE THINKING
  1. Adsorpton of gases on solid surface is generally exothermic because :

    Text Solution

    |

  2. Ice and water are at equilibrium at 0^@C , DeltaH=4 kJ/mol for the pro...

    Text Solution

    |

  3. Which of the following statements of correct for the spontaneous adsop...

    Text Solution

    |

  4. The correct thermodnamic conditions for the spontaneous reaction at al...

    Text Solution

    |

  5. An endotthermic reaction is non-spontaneous at freezing point of water...

    Text Solution

    |

  6. The standard enthalpy or the decomposition of N2 O5 to NO2 is 58.04 kJ...

    Text Solution

    |

  7. For the reaction Ag(2)O(s)rarr 2Ag(s)+1//2O(2)(g) the value of Delta H...

    Text Solution

    |

  8. At what temperature, a reaction will be at equilibrium at 1 atm if Del...

    Text Solution

    |

  9. The values of DeltaH and Delta S of a certain reaction are -400 kJ mol...

    Text Solution

    |

  10. Which of the following statements is correct for a reversible process ...

    Text Solution

    |

  11. If K gt 1.0, then the value of DeltaG^@ will be .

    Text Solution

    |

  12. Using the Gibbs energy change, Delta G^(@)=+ 63.3 kJ, for the followin...

    Text Solution

    |

  13. For the reaction: X(2)O(4)(l)rarr2XO(2)(g) DeltaU=2.1 cal , DeltaS...

    Text Solution

    |

  14. Entropy of a perfect crystalline solid at absolute zero is

    Text Solution

    |

  15. Which law of thermodynamics helps in calculating the absolute entropie...

    Text Solution

    |

  16. A heat engine absorbs heat Q(1) at temperature T(1) and Q(2) at temper...

    Text Solution

    |

  17. What is the free energy change in dissolving one mole of NaCl with its...

    Text Solution

    |

  18. For the reaction X2 Y(4(l)) to 2XY(2(g)) at 300 K the values of DeltaU...

    Text Solution

    |

  19. The heats of vaporization of H2 O, C2 H5 OH "and" CS2 "are 40.6 kJ" mo...

    Text Solution

    |

  20. The entropy change involved in the isothermal reversible expansion of ...

    Text Solution

    |