please need help.. no attachments thankyou 1. A sample of a chemical compound has 2.96g carbon, 0.414g hydrogen, 0.675g oxyg

Question

please need help..
no attachments thankyou

1. A sample of a chemical compound has 2.96g carbon, 0.414g hydrogen, 0.675g oxygen and 2.96 sulphur.
calculate it’s empirical formula.

2.if it’s mass was 972g, determine its molecular formula.​

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Trung Dũng 4 years 2021-08-16T10:16:42+00:00 1 Answers 39 views 0

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  1. ngocdiep
    0
    2021-08-16T10:18:02+00:00
    Reply

    Answer:

    1. The empirical formula => C₆H₁₀OS₂

    2. Molecular formula => C₃₆H₆₀O₆S₁₂

    Explanation:

    1. Determination of the empirical formula.

    Carbon (C) = 2.96 g

    Hydrogen (H) = 0.414 g

    Oxygen (O) = 0.675 g

    Sulphur (S) = 2.96 g

    Divide by their molar mass

    C = 2.96 / 12 = 0.247

    H = 0.414 / 1 = 0.414

    O = 0.675 / 16 = 0.042

    S = 2.96 / 32 = 0.0925

    Divide by the smallest

    C = 0.247 / 0.042 = 6

    H = 0.414 / 0.042 = 10

    O = 0.042 / 0.042 = 1

    S = 0.0925 /0.042 = 2

    Therefore, the empirical formula is

    C₆H₁₀OS₂

    2. Determination of the molecular formula.

    Molar mass of compound = 972 g/mol

    Empirical formula => C₆H₁₀OS₂

    Molecular formula =>?

    Molecular formula = [C₆H₁₀OS₂]ₙ

    Molecular formula = molar mass of compound

    Thus,

    [C₆H₁₀OS₂]ₙ = 972

    [(12×6) + (10×1) + 16 + (32×2)]n = 972

    [72 + 10 + 16 + 64]n = 32

    162n = 972

    Divide both side by 162

    n = 972 / 162

    n = 6

    Molecular formula = [C₆H₁₀OS₂]ₙ

    Molecular formula = [C₆H₁₀OS₂]₆

    Molecular formula = C₃₆H₆₀O₆S₁₂

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