Use bond energies (table 3-3), values of electron affinities (table 2-7), and the ionization energy of hydrogen (1312 kJ/mol) to estimate ∆E for each of the following reactions.a.  HF(g) → H+(g) + F−(g)b.  HCl(g) → H+(g) + Cl−(g)c.  HI(g) → H+(g)+I−(g)d.  H2O(g) → H+(g) + OH−(g)(Electron affinity of OH(g) = −180. kJ/mol.)

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Use bond energies (table 3-3), values of electron affinities (table 2-7), and the ionization energy of hydrogen (1312 kJ/mol) to estimate ∆E for each of the following reactions.
a.  HF(g) → H+(g) + F(g)
b.  HCl(g) → H+(g) + Cl(g)
c.  HI(g) → H+(g)+I(g)
d.  H2O(g) → H+(g) + OH(g)
(Electron affinity of OH(g) = −180. kJ/mol.)

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