Home
Class 11
CHEMISTRY
a) Define lattice enthalpy of an ionic c...

a) Define lattice enthalpy of an ionic compound.
b) What is Born-Haber cycle?

Promotional Banner

Topper's Solved these Questions

  • THE s-BLOCK ELEMENTS

    MAXIMUM PUBLICATION|Exercise EXERCISE|107 Videos

Similar Questions

Explore conceptually related problems

Define ionic compounds?

Lattice enthalpy of an ionic salt is a factor that determine its stability. a) Define the lattice enthalpy. b) Draw the Born-Haber cycle for the calculation of lattice enthalpy of the ionic crystal NaCl.

Born-Haber Cycle is useful to calculate lattice enthalpies of ionic solids. Construct Born-Haber Cycle for NaCl_(s)

a) What is enthalpy of solution? b) What is enthalpy of dilution?

Lattice enthalpy of an ionic salt is a factor that determine its stability. Define the lattice enthalpy.

a) What is meant by enthalpy of formation? b) What is the value of standard enthalpy of formation ( Delta_fH^o ) of an element?

Electron gain enthalpy is an important periodic property. a) What is meant by electron gain enthalpy? b) What are the factors affecting electron gain enthalpy? c) How electron gain enthalpy varies on moving across a period? Justify.

Lattice enthalpy of an ionic salt is a factor that detemines its stability.Draw the Born-Haber cycle for the calculation of lattice enthalpy of the ionic crystal NaCl.

MAXIMUM PUBLICATION-THERMODYNAMICS-EXAMPLE
  1. Thermodynamic process differ based on the manner in which it is carrie...

    Text Solution

    |

  2. a) What are thermochemical equations? b) Give an example for a therm...

    Text Solution

    |

  3. a) Define lattice enthalpy of an ionic compound. b) What is Born-Hab...

    Text Solution

    |

  4. Predict what happens to entropy in the following changes: a) Metal ...

    Text Solution

    |

  5. a) Give the relation between change in enthalpy and change in free ene...

    Text Solution

    |

  6. a) Predict in each of the following whether entropy increses or decrea...

    Text Solution

    |

  7. a) Explain the effect of temperature on the spontaneity of a process b...

    Text Solution

    |

  8. a) Explain the first, second and third laws of thermodynamics. b) Wh...

    Text Solution

    |

  9. U1, q, w, U2 are given. U1 is internal energy, q is absorbed heat, w i...

    Text Solution

    |

  10. a) Predict whether entropy increases or decreases in the following cha...

    Text Solution

    |

  11. In a process, 701 J of heat is absorbed by a system and 394 J of work ...

    Text Solution

    |

  12. The reaction of cyanamide, NH2CN(s) with oxygen was carried out in a b...

    Text Solution

    |

  13. Calculate the number of kJ of heat necessary to raise the temperature ...

    Text Solution

    |

  14. The enthalpy of formation of CO(g), CO2(g) , N2O(g), N2O4(g) are -110,...

    Text Solution

    |

  15. The equilibrium constant for the reaction is 10. Calculate the value o...

    Text Solution

    |

  16. Calculate the entropy change in surrounding when 1.0 mol of H2O(l) is ...

    Text Solution

    |

  17. Comment on the thermodynamic stability of NO(g) and NO2(g) given : f...

    Text Solution

    |

  18. a) State Hess's Law of constant heat summation. b) The equilibrium c...

    Text Solution

    |

  19. A system in thermodynamics refers to that part of the universe in whic...

    Text Solution

    |

  20. Lattice enthalpy of an ionic salt is a factor that determine its stabi...

    Text Solution

    |