Hydrocarbons, compounds containing only carbon and hydrogen, are important in fuels. The heat of combustion of cyclobutane, C4H8, is 650.3 kcal/mol. Write a balanced equation for the complete combustion of cyclobutane. How much energy is released during the complete combustion of 331 grams of cyclobutane

1. C4H8 + 6O2  > 4CO2 + 4H20

2. 3836.77 kcal

Explanation:

1. Balanced equation for the complete combustion of cyclobutane:

C4H8 + 6O2  > 4CO2 + 4H20

2. Heat of combustion of cyclobutane = 650.3 kcal/mol

    Molecular weight of cyclobutane, C4H8 = 56.1 g/mol

   Mole of C4H8 : mass of cyclobutane/Molecular weight of cyclobutane

  Mole of C4H8 = 331/56.1 = 5.9 mol

Energy released during combustion =  5.9 mol × 650.3 kcal/mol = 3836.77kcal

Therefore the energythat  is released during the complete combustion of 331 grams of cyclobutane is 3836.77kcal