1. 598 kJ/mol
2. -11 kJ/mol
3. 598 kJ/mol - (-11 kJ/mol) = +609 kJ/mol
4. Endothermic
5. True
Use the information above to complete the calculations and answer the questions below. Column A 1. How much energy must be absorbed to break the bonds of the 2 molecules of HI? : How much energy must be absorbed to break the bonds of the 2 molecules of HI? 2. How much energy is released when the bonds of H2 and I2 form in the products? : How much energy is released when the bonds of H2 and I2 form in the products? 3. What is the total energy of the reaction? (Use the formula: Total bond energies of reactants - Total bond energies of products) : What is the total energy of the reaction? (Use the formula: Total bond energies of reactants - Total bond energies of products) 4. Based on the value of the total energy of the reaction, is this reaction endothermic or exothermic?: Based on the value of the total energy of the reaction, is this reaction endothermic or exothermic? 5. True or False - It takes more energy to break the two H–I bonds than is released when forming the H–H and I-I bonds. : True or False - It takes more energy to break the two H–I bonds than is released when forming the H–H and I-I bonds. Column B a.True b.299 kJ/mol c.False d.-11 kJ/mol e.587 kJ/mol f.+ 1185 kJ/mol g.598 kJ/mol h.Endothermic i.+11 kJ/mol j.Exothermic
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