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Given the following processes and their respective enthalpies in kJ/mol:             Li(s)  -->  Li(g);               DHs = +161             Li(g)  -->  Li+(g) +  e–;     IE1  = +520             F2(g)  -->  2F(g);               BE =

Given the following processes and their respective enthalpies in kJ/mol:             Li(s)  -->  Li(g);               DHs = +161             Li(g)  -->  Li+(g) +  e–;     IE1  = +520             F2(g)  -->  2F(g);               BE =

Chemistry
Chemistry
10th Edition
ISBN:9781305957404
Author:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Publisher:Steven S. Zumdahl, Susan A. Zumdahl, Donald J. DeCoste
Chapter1: Chemical Foundations
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  1. Given the following processes and their respective enthalpies in kJ/mol:

            Li(s)  -->  Li(g);               DHs = +161

            Li(g)  -->  Li+(g) +  e–;     IE1  = +520

            F2(g)  -->  2F(g);               BE = +160

            F(g) + e–  --> F-(g);           EA = -328

            Li+(g) +  F-(g)  -->  LiF(s);   UL =  x

         If the reaction: Li(s)  + ½F2(g)  -->  LiF(s)  has DHf= -616.0 kJ/mol, deduce the value of x for UL (lattice energy in kJ/mol) in LiF. 

         (A) -1129

         (B) -1049

         (C) -183

         (D) -103

 

 

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