The combustion of gasoline produces carbon dioxide and water. assume gasoline to be pure octane (c8h18) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.7 kg of octane burned. (hint: begin by writing a balanced equation for the combustion reaction.)

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Khloe Burton

Chemistry

25 May, 15:23

The combustion of gasoline produces carbon dioxide and water. assume gasoline to be pure octane (c8h18) and calculate the mass (in kg) of carbon dioxide that is added to the atmosphere per 1.7 kg of octane burned. (hint: begin by writing a balanced equation for the combustion reaction.)

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Elmo · Answer 1

The balanced equation for combustion of octane is given below

2C₈H₁₈ + 25O₂ - - - > 16CO₂ + 18H₂O

stoichiometry of octane to carbon dioxide is 2:16

number of moles of octane burnt - 1700 g / 114.2 g/mol = 14.88 mol

For every 2 mol of octane - 16 mol of CO₂ is formed

Therefore for 14.88 mol of octane - 16/2 x 14.88 mol = 119.0 mol of CO₂

Mass of CO₂ formed - 119.0 mol x 44 g/mol = 5236 g

mass of CO₂ formed - 5.236 kg