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//Chapter-4,Example 7,Page 94
clc;
close;
delta_H1= 104 //for reaction.. H2(g)---> 2H(g)
delta_H2= 120/2 //for reaction.. (1/2)O2(g)---> O(g)
delta_H3= -58 //for reaction.. H2(g) + (1/2)O2(g)---> H2O(g)
delta_H=delta_H1 + delta_H2 - delta_H3
//there are two O-H bonds
//therefore for one bond required heat energy is half of delta_H
printf('the O-H bond energy is %.f Kcal',delta_H/2)
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