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3. The heat of formation (enthalpy) for the LiF ionic solid is -617 kJ mol?¹, as in the following reaction: Li(s) + ½F?(g) ? LiF(s) The following information has been given: ?Hsub(Li) = +161 kJ mol?¹ (energy of sublimation or atomization) ?HIE(Li) = +520 kJ mol?¹ (first ionization energy) ?Hdissoc(F) = +77 kJ mol?¹ (energy of dissociation or atomization) ?HEA(F) = -328 kJ mol?¹ (energy of electron affinity) Calculate the lattice energy for the formation of ionic LiF.

          3. The heat of formation (enthalpy) for the LiF ionic solid is -617 kJ mol?¹, as in the following reaction: Li(s) + ½F?(g) ? LiF(s) The following information has been given:
?Hsub(Li) = +161 kJ mol?¹ (energy of sublimation or atomization)
?HIE(Li) = +520 kJ mol?¹ (first ionization energy)
?Hdissoc(F) = +77 kJ mol?¹ (energy of dissociation or atomization)
?HEA(F) = -328 kJ mol?¹ (energy of electron affinity)
Calculate the lattice energy for the formation of ionic LiF.

3. The heat of formation (enthalpy) for the LiF ionic solid is -617 kJ mol?¹, as in the following reaction: Li(s) + ½F?(g) ? LiF(s) The following information has been given:
?Hsub(Li) = +161 kJ mol?¹ (energy of sublimation or atomization)
?HIE(Li) = +520 kJ mol?¹ (first ionization energy)
?Hdissoc(F) = +77 kJ mol?¹ (energy of dissociation or atomization)
?HEA(F) = -328 kJ mol?¹ (energy of electron affinity)
Calculate the lattice energy for the formation of ionic LiF.

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