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18 February, 22:02

Calculate the number of pounds of CO2 released into the atmosphere when a 15.0-gallon tank of gasoline is burned in an automobile engine. Assume that gasoline is primarily octane, C8H18, and that the density of gasoline is 0.692 g·mL-1 (this assumption ignores additives). Also assume complete combustion.

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  1. 19 February, 00:16
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    266.997 pounds

    Explanation:

    The balanced equation for the combustion of octane is;

    2C₈H₁₈ (l) + 25O₂ (g) → 16CO₂ (g) + 18H₂O (g)

    Assuming that gasoline is purely octane:

    Amount of gasoline available is 15.0 gallon

    We are required to calculate the amount of CO₂ released to the atmosphere;

    This can be done in several steps;

    Step 1: Mass of octane in grams

    Amount of octane = 15.0 gallons

    But, 1 gallon = 3785.41 ml

    Therefore;

    15 gallon is equivalent to;

    = 15 * 3785.41 ml

    = 56,781.15 ml

    We are given the density of octane (0.692 g/ml) and thus we can calculate the mass of octane.

    Mass = density * volume

    = 0.692 g/ml * 56,781.15 ml

    = 39,292.56 g

    Step 2: Number of moles of octane

    Number of moles = Mass / Molar mass

    Molar mass of octane = 114.23 g/mol

    Number of moles of Octane = 39,292.56 g : 114.23 g/mol

    = 343.978 moles

    Step 3: Moles of carbon dioxide released

    From the equation;

    2 moles of octane completely burns in air to yield 16 moles of CO₂

    Therefore;

    343.978 moles of octane produces;

    = (343.978 moles/2) 16

    = 2751.824 moles of CO₂

    Step 4: Mass of CO₂ in pounds

    1 mole of CO₂ has 44.01 g

    Therefore;

    2751.824 moles contains;

    = 2751.824 moles * 44.01 g/mol

    = 121,107.77 g

    But, 1 pound = 453.592 g

    Therefore;

    Mass of CO₂ in pounds = 121,107.77 g : 453.592 g

    = 266.997 pounds

    Therefore, the mass of CO₂ released to the atmosphere is 266.997 pounds
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