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Solved: Use the Born-Haber cycle outlined in Section 9.3
Chapter 9, Problem 25P(choose chapter or problem)
Use the Born-Haber cycle outlined in Section 9.3 for LiF to calculate the lattice energy of NaCl. [The heat of sublimation of Na is 108 kJ/mol and \(\Delta H_\mathrm f^\circ(\mathrm{NaCl})=-411\mathrm{\ kJ/mol}\). Energy needed to dissociate \(\frac{1}{2}\) mole of \(\mathrm{Cl_2}\) into CI atoms = 121.4 kJ.]
Questions & Answers
QUESTION:
Use the Born-Haber cycle outlined in Section 9.3 for LiF to calculate the lattice energy of NaCl. [The heat of sublimation of Na is 108 kJ/mol and \(\Delta H_\mathrm f^\circ(\mathrm{NaCl})=-411\mathrm{\ kJ/mol}\). Energy needed to dissociate \(\frac{1}{2}\) mole of \(\mathrm{Cl_2}\) into CI atoms = 121.4 kJ.]
ANSWER:
Step 1 of 4
“Born-Haber cycle” assists in the ionic compound’s lattice energy predictions.
It involves several theoretical steps to calculate the ionic solid’s formation enthalpy change from its constituent elements in their standard states. It assists in the ionic compound’s stability prediction based on the energy involved in the crystal lattices’ formation.