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19 February, 10:48

what is the molecular formula for a compund that is 82.76% C has a molecular mass of 58.1 grams per mole, and is composed solely of carbon and hydrogen

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Answers (2)
  1. 19 February, 12:20
    0
    C4H10.

    Explanation:

    The % of Hydrogen = 100 - 82.76 = 17.24%

    Dividing by the atomic masses

    C = 82.76 / 12.011 = 6.89

    H = 17.24 / 1.008 = 17.1

    C: H = 1:2.48

    = 2:5

    So the empirical formula is C2H5 = 2*12.011 + 5.04 = 29.05 g

    Now the molecular mass is 58.1 g which is 2 * 29.05 so the molecular formula is

    2 * (C2H5) = C4H10.
  2. 19 February, 13:40
    0
    Molecular formula for the compound is: C₄H₁₀

    Explanation:

    We analyse the data given.

    82.76% means, that in 100g of compound 82.76 g are C

    We have the molar mass which is 58.1 g/mol, so let's determine the mass of C, and then, its moles. Therefore we make this rule of three:

    In 100 g of compound we have 82.76 g of C

    In 58.1 g of compound we may have (85.1. 82.76) / 100 = 48 g of C

    If we convert the mass to moles: 48 g. 1mol / 12g = 4 moles of C

    we notice that the compound has 4 moles of C

    Molar mass of compound is 58.1 g/mol

    48 g of compound are C, therefore (58 - 48) = 10 g are from H

    If we convert the mass to moles → 10 g. 1 mol/1 g = 10 moles

    Molecular formula for the compound is: C₄H₁₀

    Notice: Centesimal composition for H in the compound

    (10g / 58 g). 100 = 17.24 %

    17.24 % + 82.76% = 100%
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