6. An unknown compound is analyzed and found to consist of 49% carbon, 2.7 % hydrogen, and 48.2 % chlorine. If the molecular mass of the compound is 150,
what is the molecular formula of the compound?

Molecular formula = C₆H₄Cl₂

Explanation:

Given data:

Percentage of hydrogen = 2.7%

Percentage of carbon = 49%

Percentage of chlorine = 48.2%

Molar mass of compound = 150 g/mol

Molecular formula = ?

Solution:

Number of gram atoms of H = 2.7 / 1.01 = 2.67

Number of gram atoms of Cl = 48.2 / 16 = 1.36

Number of gram atoms of C = 49 / 12 = 4.08

Atomic ratio:

            C                      :           H             :           Cl

           4.08/ 1.36         :     2.67/1.36       :       1.36/1.36

            3                      :        2                 :        1

C : H : Cl = 3 : 2 : 1

Empirical formula is C₃H₂Cl.

Molecular formula:

Molecular formula = n (empirical formula)

n = molar mass of compound / empirical formula mass

Empirical formula mass = 12×3 + 1.01 ×2 + 35.5 = 73.52 g/mol

n = 150 / 73.52

n = 2

Molecular formula = n (empirical formula)

Molecular formula = 2 (C₃H₂Cl)

Molecular formula = C₆H₄Cl₂

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