1. For the fluorination of methane (first reaction) one C–H and a F–F bond are broken, while C–F and H–F bonds are formed. The sum of the standard energies of the broken bonds is 99 + 36.6 = 135.6, and that of the formed bonds is 116 + 135 = 251. In practice, ΔHº is calculated by subtracting the energy of the bonds formed by the products from that of the bonds broken in the reactants. In this case, 135.6 - 251 = -115.4. If the resulting ΔHº is negative the reaction is exothermic, if positive it is endothermic. 2. For the iodination of methane, ΔHº = reactants (99 + 36) - products (51 + 71) = +13. 3. For propene hydrogenation, ΔHº = reactants (63 + 104) - products (99 + 99) = -31. (63 is the difference between C–C bond energy and C=C bond energy) 4. For bromine addition to propene, ΔHº = reactants (63 + 46) - products (68 + 68) = -27. 5. For hydrogen addition to propyne, ΔHº = reactants (54 + 104) - products (99 + 99) = -40. 6. For tautomerization, ΔHº = reactants (63 + 111) - products (99 + 91) = -16. (91 is the difference between C–O bond energy and C=O bond energy) 7. For the dehydration of 2-propanol, ΔHº = reactants (85.5 + 99) - products (63 + 111) = +10.5. Note that the addition of hydrogen to propene (#3) and propyne (#4), and the dehydration of 2-propanol (#7) require catalysts, and in the last case heat.
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This script written by William Reusch, Dept. of Chemistry, Michigan State University. Please send comments and corrections to whreusch@msu.edu.