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Given the following information, find the lattice enthalpy (kJ/mol) of NaCl(s).   ΔHf (NaCl) = -411 kJ/mol ΔHsublimation (Na) = 107 kJ/mol IE1 (Na) = 496 kJ/mol Bond Energy (Cl-Cl) = 244 kJ/mol EA1 (Cl) = -349 kJ/mol

Given the following information, find the lattice enthalpy (kJ/mol) of NaCl(s).   ΔHf (NaCl) = -411 kJ/mol ΔHsublimation (Na) = 107 kJ/mol IE1 (Na) = 496 kJ/mol Bond Energy (Cl-Cl) = 244 kJ/mol EA1 (Cl) = -349 kJ/mol

Chemistry & Chemical Reactivity
Chemistry & Chemical Reactivity
9th Edition
ISBN:9781133949640
Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel
Chapter12: The Solid State
Section12.3: Bonding In Ionic Compounds: Lattice Energy
Problem 1RC
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Given the following information, find the lattice enthalpy (kJ/mol) of NaCl(s).

 

ΔHf (NaCl) = -411 kJ/mol

ΔHsublimation (Na) = 107 kJ/mol

IE1 (Na) = 496 kJ/mol

Bond Energy (Cl-Cl) = 244 kJ/mol

EA1 (Cl) = -349 kJ/mol

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