Consider the following information.
The enthalpy of formation of CaO is ΔHf°=-634.9 kJ/mol.
The enthalpy of sublimation of Ca is ΔHsab = 177.8 kJ/mol.
The first and second ionization energies of Ca are IE1 = 590 kJ/mol and IE2 = 1145 kJ/mol.
The first electron affinity of O is ΔHAI=-142 kJ/mol.
The bond energy of O2 is BE = 498 kJ/mol.
The lattice energy of CaO is ΔHatice = -3414 kJ/mol. Determine the second electron affinity of O.
Consider an ionic compound, MX2, composed of generic metal M and generic, gaseous halogen X. The enthalpy of formation of MX2 is ΔHf° = –889 kJ/mol. The enthalpy of sublimation of M is ΔHsub = 161 kJ/mol. The first and second ionization energies of M are IE1 = 613 kJ/mol and IE2 = 1431 kJ/mol. The electron affinity of X is ΔHEA = –329 kJ/mol. (Refer to the Hint). The bond energy of X2 is BE = 239 kJ/mol. Determine...
Consider an ionic compound, MX2, composed of generic metal M and generic, gaseous halogen X.The enthalpy of formation of MX2 is ΔHf° = –915 kJ/mol. The enthalpy of sublimation of M is ΔHsub = 123 kJ/mol. The first and second ionization energies of M are IE1 = 789 kJ/mol and IE2 = 1383 kJ/mol. The electron affinity of X is ΔHEA = –351 kJ/mol. (Refer to the Hint). The bond energy of X2 is BE = 191 kJ/mol.Determine the lattice...
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 an ionic compound, MX,, composed of generic metal M and generic, gaseous halogen X. • The enthalpy of formation of MX, is AH; = -989 kJ/mol. • The enthalpy of sublimation of M is AH sub = 131 kJ/mol. • The first and second ionization energies of M are IE1 = 615 kJ/mol and IE2 = 1392 kJ/mol. • The electron affinity of X is AHEA = -303 kJ/mol. (Refer to the hint). • The bond energy of X,...
Consider an ionic compound, MX2, composed of generic metal M and generic, gaseous halogen X. The enthalpy of formation of MX2 is ΔH∘f=−831 kJ/mol. The enthalpy of sublimation of M is ΔHsub=129 kJ/mol. The first and second ionization energies of M are IE1=691 kJ/mol and IE2=1401 kJ/mol The electron affinity of X is ΔHEA=−307 kJ/mol. The bond energy of X2 is BE=153 kJ/mol. Determine the lattice energy of MX2. ΔHlattice=ΔHlattice= kJ/mol
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
Determine the lattice energy of MX2. Consider an ionic compound, MX2, composed of generic metal M and generic, gaseous halogen X. The enthalpy of formation of MX2 is ΔH∘f=−681 kJ/mol. The enthalpy of sublimation of M is ΔHsub=145 kJ/mol. The first and second ionization energies of M are IE1=607 kJ/mol and IE2=1444 kJ/mol. The electron affinity of X is ΔHEA=−315 kJ/mol. The bond energy of X2 is BE=247 kJ/mol. Determine the lattice energy of MX2. I've been stuck on this question...
Consider an ionic compound, MX2 composed of generic metal M and generic, gaseous halogen ?. The enthalpy of formation of MX2 is 사4°-_653 kJ/mol. The enthalpy of sublimation of M is dHsb = 1 17 kJ/mol. The first and second ionization energies of M are IE1-711 kJ/mol and IEz 1.370 x10 kJ/mol. The electron affinity of X is AHEA-321 kJ/mol. (Refer to the Hint). The bond energy of X2 is BE 173 kJ/mol. Determine the lattice energy of MX2 Number...
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).
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