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16 February, 18:56

a sample of a compound that contains only the elements C, H and N is completely burned in O2 to produce 44g of CO2, 45g of H2O, and some NO2. A possible empirical formula of the compound is A. CH2N B. CH5N C. C2H5N D. C3H3N2

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  1. 16 February, 19:37
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    B. CH₅N

    Explanation:

    The combustion reaction of a compound CₐHₓNₙ with O₂ is:

    CₐHₓNₙ + O₂ → a CO₂ + X/2 H₂O + n NO₂

    Where 1 mole of CₐHₓNₙ with an excess of O₂ produce a moles of CO₂, X/2 moles of H₂O and n moles of NO₂

    Thus, you need to convert the mass of CO₂ and H₂O to moles to find the C:H ratio and determine a possible empirical formula thus:

    Moles CO₂ (Molar mass 44g/mol):

    44g ₓ (1mol / 44g) = 1 mole CO₂ = 1 mole C

    Mole of H₂O (Molar mass 18g/mol):

    45g ₓ (1 mol / 18g) = 2.5 moles H₂O = 5 moles H

    Thus, in the compound you have 5 moles of H per mole of C, and a possible empirical formula is:

    B. CH₅N

    The only structure that meet this C:H ratio
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