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 ΔH lattice=−788 kJ/mol The enthalpy of...
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 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 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
calculate the lattice energy of NaCl based on the given information : ΔH°f[NaCl(s)] = -411 kJ/mol ΔH°f [Clg] = 121.5 kJ/mol ΔH°sublimation [Na] = 109 kJ/mol IE1 (Na) = 496 kJ/mol EA1 (Cl) = -349 kJ/mol
The enthalpy of formation of MX is ΔHf° = –527 kJ/mol. The enthalpy of sublimation of M is ΔHsub = 139 kJ/mol. The ionization energy of M is IE = 475 kJ/mol. The electron affinity of X is ΔHEA = –309 kJ/mol. (Refer to the hint). The bond energy of X2 is BE = 223 kJ/mol.
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...
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 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...
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.
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