A Compound Contains 4.07% Hydrogen, 24.27% Carbon And 71.65% Of Chlorine. Its Molar Mass Is 98.96G. What Are It's Empirical And Molecular Formulas?

Given data

Hydrogen — 4.07%

Carbon–24.27%

Chlorine—71.65%

Molar Mass Is 98.96G

To Calculate Empirical Formulae, first, we have to divide the given percentages of atoms by their molecular masses.

Hydrogen — 4.07 / 1 = 4.07

Carbon–24.27 / 12 = 2.02

Chlorine—71.65 / 35.5 = 2.01

Now we have to divide all the values with the lowest obtained value.

Hydrogen — 4.07 / 2.01 = 2

Carbon–2.02 / 2.01 = 1

Chlorine— 2.01 / 2.01 = 1

Therefore, the empirical formula is CH2Cl

To Calculate Molecular Formulae, we need to find the weight of the empirical formula

CH2Cl

12 + 2*1 + 35.5

= 49.5

The molecular weight- 98.96 is double of empirical weight. Therefore molecular formula is

C2H4Cl2

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