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 =

1. Given the following processes and their respective enthalpies in kJ/mol:

            Li(s)  -->  Li(g);               DH_s = +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);   U_L =  x

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

         (A) -1129

         (B) -1049

         (C) -183

         (D) -103