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20 February, 23:34

Combustion of 1.000 g of an organic compound known to contain only carbon, hydrogen, and oxygen produces 2.360 g of carbon dioxide and 0.640 g of water. What is the empirical formula of the compound?

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  1. 20 February, 23:42
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    The empirical formula is C3H4O

    Explanation:

    Step 1: Data given

    Mass of the compound = 1.000 grams

    The compound contains:

    - Carbon

    - hydrogen

    - oxygen

    The combustion of this compound gives:

    2.360 grams of CO2

    0.640 grams of H2O

    Step 2: Calculate moles CO2

    Moles CO2 = mass CO2 / molar mass CO2

    Moles CO2 = 2.360 grams / 44.01 g/mol

    Moles CO2 = 0.05362 moles

    In CO2 we have 1 mol

    This means for 1 mol CO2 we have 1 mol C

    For 0.05362 moles CO2 we have 0.05362 moles C

    We have 0.05362 moles of C in the compound

    Step 3: Calculate mass of C

    Mass C = moles C * molar mass C

    Mass C = 0.05362 moles * 12.0 g/mol

    Mass C = 0.643 grams

    Step 4: Calculate moles of H2O

    Moles H2O = 0.640 grams / 18.02 g/mol

    Moles H2O = 0.0355 moles H2O

    For 1 mol H2O we have 2 moles of H

    For 0.0355 moles H2O we have 2*0.0355 = 0.071 moles H

    Step 5: Calculate mass of H

    Mass H = moles H * molar mass H

    Mass H = 0.071 moles * 1.01 g/mol

    Mass H = 0.072 grams

    Step 6: Calculate mass of O

    Mass of O = Mass of compound - mass of C - mass of H

    Mass of O = 1.000 g - 0.643 - 0.072 = 0.285 grams

    Step 7: Calculate moles of O

    Moles O = 0.285 grams / 16.0 g/mol

    Moles O = 0.0178 moles

    Step 8: Calculate mol ratio

    We divide by the smallest amount of moles

    C: 0.05362 / 0.0178 = 3

    H: 0.071 / 0.0178 = 4

    O: 0.0178/0.0178 = 1

    The empirical formula is C3H4O
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