Thermodynamics

• Lattice dissociation enthalpy?

  The energy required to break an ionic lattice into its constituent ions in a gaseous state under standard condtions.
• Lattice formation enthalpy?

  the energy required to form an ionic lattice from it constituent ions in a gaseous state under standard conditions
• Atomisation enthalpy?

  the energy required for the formation of one mole of gaseous atoms under standard conditions
• Enthalpy of electron affinity?

  The enthalpy change when one mole of electrons is added to one mole of gaseous atoms at standard conditions
• Enthalpy of solution?

  The enthalpy change 1 mole of solid ionic is dissolved in water to infinite dilution so the ions no longer interact together under standard conditions
• Enthalpy of hydration?

  The enthalpy change when 1 mole of gaseous ions is dissolved in water to form 1 mole of aqueous ions under standard condition's
• Gibbs free energy?


  ΔG = KJ mol ΔH T=ΔH /ΔS- to find T must convert S to H. ΔS = Jk mol. Jk mol x 1000 = KJmol.
• enthalpy change?

  heat change under constant pressure.