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25 September, 07:50

What is the empirical formula of a compound containing 5.03 grams carbon, 0.42 grams hydrogen, and 44.5 grams chlorine?

C2H3Cl

C2H2Cl

CHCl4

CHCl3

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  1. 25 September, 08:19
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    The right choice is CHCl₃

    Explanation:

    To find the empirical formula firstly, change the mass to moles.

    For Carbon:

    no. of moles = (mass / molar mass) = (5.03 g / 12 g/mol) = 0.42 mol

    For Hydrogen:

    no. of moles = (mass / molar mass) = (0.42 g / 1 g/mol) = 0.42 mol

    For Chlorine:

    no. of moles = (mass / molar mass) = (44.5 g / 35.5 g/mol) = 1.25 mol

    The ratio for Carbon and Hydrogen is 1 : 1

    0.42 mol / 042 mol = 1.00

    Then find a ratio between the moles.

    The ratio of Chlorine to both Carbon and Hydrogen is 3:1

    1.25 mol / 0.42 mol = 2.98 ≅ 3

    So the ratio is 1 C : 1 H : 3 Cl.

    So, the right choice is CHCl₃

    Carbon usually forms four bonds one to Hydrogen and 3 to Chlorine atoms.

    Chlorine usually forms one bond to Carbon atom.

    Hydrogen usually forms one bond Carbon atom.
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