Calculate the lattice energy for LiF(s) given the following:
sublimation energy for Li(s) = +166 KJ/mol
delta Hf for F(g) = +77 KJ/mol
first ionization energy of Li(g) = +520 KJ/mol
electron affinity of F(g) = -328 KJ/mol
enthalpy of formation of LiF(s) = -617 KJ/mol
Calculate the lattice energy for LiF(s) given the following: sublimation energy for Li(s) = +166 KJ/mol...
Consider the following information. The lattice energy of LiCl is ΔH lattice = −834 kJ/mol. The enthalpy of sublimation of Li is ΔH sub = 159.3 kJ/mol. The first ionization energy of Li is IE 1 = 520 kJ/mol. The electron affinity of Cl is ΔH EA = -349 kJ/mol. The bond energy of Cl2 is BE = 243 kJ/mol. Determine the enthalpy of formation, ΔHf, for LiCl(s).
Given the following information, calculate the lattice energy of CaF2 The enthalpy of formation of CaF2 -1228 kJ/mol Heat of sublimation of Ca 177.8 kJ/mol Bond dissociation energy of F2 159 kJ/mol First ionization energy of Ca 589.8 kJ/mol Second ionization energy of Ca 1145.4 kJ/mol . Electron affinity of F -328 kJ/mot [ Answer : -2644 KJİ I
Using the thermodynamic quantities shown below: construct a Born-Haber cycle for the following reaction: Li(s) + 1/2 F2(g) LiF(s); calculate the lattice energy of LiF. Vaporization of Li(s): +159 F2 bond enthalpy: +155 Li ionization energy: +520 F- electron affinity: +328 LiF(s) heat of formation: -616
Consider the following information. The lattice energy of NaCl is ΔH lattice=−788 kJ/mol The enthalpy of sublimation of Na is ΔHsub=107.5 kJ/mol The first ionization energy of Na is IE1=496 kJ/mol. The electron affinity of Cl is ΔHEA=−349 kJ/mol. The bond energy of Cl2 is BE=243 kJ/mol. Determine the enthalpy of formation, ΔHf, for NaCl(s). ΔHf= kJ/mol
Consider the following information. • The lattice energy of NaCl is AHlattice = –788 kJ/mol. • The enthalpy of sublimation of Na is AHsub = 107.5 kJ/mol. • The first ionization energy of Na is IE1 = 496 kJ/mol. • The electron affinity of Cl is AHEA = -349 kJ/mol. • The bond energy of Cl, is BE = 243 kJ/mol. Determine the enthalpy of formation, AHf, for NaCl(s). AH= kJ/mol
Consider the following information. • The lattice energy of KCl is AHlattice = -701 kJ/mol. • The enthalpy of sublimation of K is AHsub = 89.0 kJ/mol. • The first ionization energy of K is IE1 = 419 kJ/mol. • The electron affinity of Cl is AHEA = -349 kJ/mol. • The bond energy of Cl, is BE = 243 kJ/mol. Determine the enthalpy of formation, AHf, for KCl(s). AHư= kJ/mol
3. Draw the Bom Haber Cycle and calculate the lattice energies for LiF, MgO, and CaC12 using the data provided in the table below. This can be done on a separate page if you are working off this template. AH (1/2 B.E.) Electon Affinity Ionization Sublimation AH EA Energy Ionic Compoud F 80 kJ/mol 328 kJ/mol Li 520 kJ/mol 155 kJ/mol LiF -594 kJ/mol 0 249.4 kJ/mol 141 kJ/mol (15) . Mg 738 kJ/mol (19) 148 kJ/mol MgO -601 kJ/mol...
2. Use the following data to calculate the lattice energy (U) of NaCl(s) from sodium me chlorine: Enthalpy of formation (4H) for NaCl(s) - -411 kJ/mol Enthalpy of sublimation (4Hub) of Na 107.3 kJ/mol The first ionization energy of Na (E,)-495.8 kJ/mol The bond dissociation energy (D) of Clh- 243 kJ/mol The electron affinity of Cl (Eea)- 348.6 kJ/mol.
b) Given the following data, calculate the lattice energy for silver iodide. Enthalpy of sublimation of silver = +286 kJmol Enthalpy of sublimation of iodine : +107 kJmol.' Enthalpy of dissociation of iodine : +151 kJmol Ionisation energy of silver : +730 kJmol? Electron affinity of iodine : -295 kJmol Enthalpy of formation of AgI : -62 kJ moll