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Marissa asked in Science & MathematicsChemistry · 1 decade ago

Help with Mass- Volume Gas Law Mole Problem?

How many liters of carbon dioxide are produced when 10.0 ml of ethyl alcohol (C2H5OH) are burned completely in oxygen? the density of ethyl alcohol is 0.789 g/ml

please show the work as best you can... thank you in advance!

4 Answers

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  • 1 decade ago
    Favorite Answer

    0.789 g/mL x 10.0 mL = 7.89g EtOH

    7.89g EtOH x (1 mole EtOH / 40.021g EtOH) = 0.171 moles EtOH

    C2H5OH + 3O2 ==> 2CO2 + 3H2O

    0.171 moles EtOH x (2 moles CO2 / 1 mole EtOH) = 0.343 moles CO2

    Assuming STP

    0.343 moles CO2 x (22.4L CO2 / 1 mole CO2) = 7.68L CO2

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    5 years ago

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    4 years ago

    T temperature to be measured on kelvin scale.. i.e. 19+273 ok and no of moles.. weight divided via molecular weight fee of R 2 b chosen accordin to the instruments used for pressur en volume.. if u use atm-l then the fee of R is 0.0821 if u use pascal-m^3 fee is 8.314 and for calculation of heat or potential in energy, fee of R shud be approximated to 2

  • mass of C2H5OH = 10 mL * 0.789 g/mL = 7.89 g

    Mr C2H5OH = 46

    mol C2H5OH = 7.89 g : 46 g/mol = 0.17 mol

    The reaction :

    C2H5OH + 7/2O2 ---> 2CO2 + 3H2O

    0.17 mol

    mol CO2 = 2 * 0.17 mol

    = 0.34 mol

    volume CO2 (STP) = 0.34 mol * 22.4 L/mol

    = 7.616 L

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