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26 April, 05:28

How many liters of C7H16 would be required to form 20.0 g of h2o

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  1. 26 April, 07:23
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    0.0215 L

    Explanation:

    The combustion of C₇H₁₆ is given by the balanced equation;

    C₇H₁₆ + 11O₂ → 7CO₂ + 8H₂O

    From the question we are given;

    Mass of H₂O that would be formed as 20.0 g

    We are required to determine the number of liters of C₇H₁₆ that would produce 20.0 g of water.

    We are going to use the following steps;

    Step 1: Calculate the number of moles of H₂O

    Number of moles = Mass : Molar mass

    Molar mass of H₂O = 18.02 g/mol

    = 20.0 g : 18.02 g/mol

    = 1.1099 moles

    Step 2: Moles of C₇H₁₆

    From the equation, 1 mole of C₇H₁₆ produces 8 moles of H₂O

    Therefore, the mole ratio of C₇H₁₆ to H₂O is 1 : 8

    Thus, the moles of C₇H₁₆ = Moles of water : 8

    = 1.1099 moles : 8

    = 0.139 moles

    Step 3: Calculate the mass of C₇H₁₆

    Mass = Number of moles * Molar mass

    Molar mass of C₇H₁₆ = 100.21 g/mol

    Therefore;

    Mass = 0.139 moles * 100.21 g/mol

    = 13.929 g

    Step 4 : Volume of C₇H₁₆ in liters

    Density of Heptane is 648 Kg/m³ or 0.648 g/mL

    Therefore; since Volume = Mass : Density

    Then; Volume of heptane = 13.929 g : 0.648 g/mL

    = 21.495 mL

    but, 1000 mL = 1 L

    Therefore, the volume of heptane = 0.021495 L

    = 0.0215 L

    The volume of Heptane required will be 0.0215 L
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