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10 December, 10:23

determine the empirical formula of a compound containing 48.38 grams of carbon, 8.12 grams of hydrogen, and 53.5 of oxygen. in an experiment, the molar mass of the compound was determined to be 180.15 g/mol. what is the molecular formula of the compound?

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  1. 10 December, 12:26
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    The molecular mass of this compound is 180 g/mol and could be Glucose

    Explanation:

    Step 1: Calculate moles

    mole = mass / Molar mass

    ⇒ mole Carbon = 48.38 g/12 g/mol = 4.0317 moles

    ⇒ mole Hydrogen 8.12 g/1 g/mol = 8.12 moles

    ⇒ mole Oxygen 53.5 g/16 g/mol = 3.34375 moles

    Step 2: Calculate the ratio

    the smallest amount of moles is 3.34375 (oxygen), so we divide all by this number

    ⇒C = 4.0317/3.34375 = 1.206 ≈ 1

    ⇒H = 8.12.1 / 3.34375 = 2.425 ≈ 2

    ⇒O = 3.3437575/3.34375 = 1.00

    Therefore; the empirical formula = CH2O

    This has a molar mass of 30 g/mol

    Now to find the molecular formula we divide 180.15 / 30 = 6

    This means we have to multiply all numbers of elements by 6

    The molecular formule = C6H12O6, which is glucose (or fructose, ...) and has a molar mass of 180g/mol
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