Hydrocarbons, compounds containing only carbon and hydrogen, are important in fuels. The heat of combustion of cyclopentane, C5H10, is 786.6 kcal/mol. Write a balanced equation for the complete combustion of cyclopentane. How much energy is released during the complete combustion of 416 grams of cyclopentane

4664.54  kcal of energy is produced on the complete combustion of 416 grams of cyclopentane

Explanation:

Combustion is the process by which hydrocarbons react with oxygen to heat to produce heat energy.

The heat energy produced when one mole of an hydrocarbon is completely burnt or combusted in air is called the heat of combustion

The balanced equation for the complete combustion of cyclopentane (C5H10) is given below:

             2C₅H₁₀ + 15O₂ → 10CO₂ + 10H₂O

                                                             ΔH combustion = 786.6 kcal/mol

What the above equation means is that each time one mole of cyclopentane is completely burnt, 786.6kcal of energy is released.

Hence we need to calculate the number of moles of cyclopentane in 416grams; therefore

No of moles cyclopentane = mass of cyclopentane / molar mass of cycopentane  

                                             = 416 g / 70.1 g/mol

                                             = 5.9343moles

                                             ≅ 5.93 moles of cyclopentane in 416grams

From the question, since the  cyclopentane is completely combusted, it implies that the energy released would be

    1 mole of cyclopentane     = 786.6 kcal of energy

   5.93 moles of cyclopentane would produce    

                                                = 5.93 moles x 786.6kcal/mol

                                                = 4664.54  kcal of energy

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