A compound analyzed as 18.0% carbon, 2.26% hydrogen, and 79.7% chlorine. calculate the empirical formula of the compound.

To answer this item, our basis is 100g. We solve for the masses of the given elements in this item,

carbon: (0.18) (100 g) = 18 g

hydrogen: (0.0226) (100 g) = 2.26 g

chlorine: (0.797) (100 g) = 17.7 g

Then, we calculate for the number of moles by dividing the masses by the molar masses of the given elements.

Number of moles:

carbon = (18 g) x (1 mol / 12 g) = 1.5 moles

hydrogen = (2.26 g) x (1 mol / 1.01 g) = 2.23 moles

chlorine = (79.7 g) x (1 mol / 35.45 g) = 2.25 moles

We get the ratio of the number of moles by dividing them with the lowest value, 1.5.

Carbon = 1.5 moles / 1.5 = 1

Hydrogen = 2.23 moles / 1.5 = 1.48

Chlorine = 2.25 / 1.5 = 1.5

The empirical formula is,

C1H1.5CL1.5

Simplifying,

C2H3Cl3