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24 March, 05:27

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 1.0 kg of octane burned. (Hint: Begin by writing a balanced equation for the combustion reaction.)

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  1. 24 March, 06:49
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    3.09kg

    Explanation:

    First, let us write a balanced equation for the reaction. This is illustrated below:

    2C8H18 + 25O2 - > 16CO2 + 18H2O

    Molar Mass of C8H18 = (12x8) + (18x1) = 96 + 18 = 114g/mol

    Mass of C8H18 from the balanced equation = 2 x 114 = 228g

    Converting 228g of C8H18 to kg, we obtained:

    228/1000 = 0.228kg

    Molar Mass of CO2 = 12 + (2x16) = 12 + 32 = 44g/mol

    Mass of CO2 from the balanced equation = 16 x 44 = 704g

    Converting 704g of CO2 to kg, we obtained:

    704/1000 = 0.704kg

    From the equation,

    0.228kg of C8H18 produced 0.704kg of CO2.

    Therefore, 1kg of C8H18 will produce = 0.704/0.228 = 3.09kg of CO2
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