Steps to Calculate the Empirical and Molecular Formulas
Step 1: Given
A compound contains:
Hydrogen — 4.07%
Carbon – 24.27%
Chlorine – 71.65%
Molar Mass Is 98.96G
Step 2: Evaluating Empirical Formulae
The empirical formula for each atom is created by first dividing the percentages of atoms by the molecular masses of the atoms.
Hydrogen — 4.07/1 = 4.07
Carbon – 24.27/12 = 2.02
Chlorine — 71.65/35.5 = 2.01
Divide all the values now by the result that was the lowest.
Hydrogen — 4.07/2.01 = 2
Carbon –2.02/2.01 = 1
Chlorine — 2.01/2.01 = 1
Therefore, the empirical formula is CH2Cl
Step 3: Calculation of Molecular Formulae
From the empirical formula, we can write
CH2Cl = 12 + 2 x 1 + 35.5
The molecular weight of 98.96 is twice as great as the empirical weight.
Hence, the molecular formula is C2H4Cl2
A compound contains 4.07% Hydrogen, 24.27% Carbon, and 71.65% of Chlorine. Its molar mass Is 98.96G. What are its empirical and molecular formulas?
4.07% Hydrogen, 24.27% Carbon, and 71.65% Chlorine are all present in a molecule. It has a 98.96G molar mass. The empirical formula is CH2Cl, and the molecular formula is C2H4Cl2. Here the molecular weight is two times higher than the empirical weight