Consider the following equation that describes the complete combustion of propane, c3h8. the bond energies are: c h 416 kj/mol; c c 356 kj/mol; oo 498 kj/mol; co 803 kj/mol; h o 467 kj/mol. which is the amount of energy gained on making all the bonds in carbon dioxide and water according to the equation?

8,554 kJ/mol

Explanation:

The equation of the complete combustion of propane is:

C₃H₈ +  5O₂ → 3CO₂ + 4H₂O

The molecule of carbon dioxide is OCO, so there are 2 CO bonds, and the molecule of water is HOH, so there are two H O bonds in the molecule.

The total bond energy is the sum of the energy of each bond. Because there are 3 moles of CO₂ and 4 moles of H₂O, the energy gained is:

3*2*803 + 4*2*467 = 8,554 kJ/mol

the answer is d. 74.02