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17 July, 08:07

Liquid octane CH3CH26CH3 will react with gaseous oxygen O2 to produce gaseous carbon dioxide CO2 and gaseous water H2O. Suppose 73. g of octane is mixed with 105. g of oxygen. Calculate the minimum mass of octane that could be left over by the chemical reaction. Be sure your answer has the correct number of significant digits.

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  1. 17 July, 08:30
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    The minimum mass of octane that could be left over is 43.0 grams

    Explanation:

    Step 1: Data given

    Mass of octane = 73.0 grams

    Mass of oxygen = 105.0 grams

    Molar mass octane = 114.23 g/mol

    Molar mass oxygen = 32.0 g/mol

    Step 2: The balanced equation

    2C8H18 + 25O2 → 16CO2 + 18H2O

    Step 3: Calculate the number of moles

    Moles = mass / molar mass

    Moles octane = 73.0 grams / 114.23 g/mol

    Moles octane = 0.639 moles

    Moles O2 = 105.0 grams / 32.0 g/mol

    Moles O2 = 3.28 moles

    Step 4: Calculate the limiting reactant

    For 2 moles octane we need 25 moles O2 to produce 16 moles CO2 and 18 moles H2O

    O2 is the limiting reactant. It will completely be consumed. (3.28 moles). There will react 3.28 / 12.5 = 0.2624 moles. There will remain 0.639 - 0.2624 = 0.3766 moles octane

    Step 5: Calculate mass octane remaining

    Mass octane = moles * molar mass

    Mass octane = 0.3766 moles * 114.23 g/mol

    Mass octane = 43.0 grams

    The minimum mass of octane that could be left over is 43.0 grams
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