1. Molecular Formula

2. The percent by mass of each element in a compound
Percent Composition
The percent by mass of each element in a compound

3. To find percent composition, take molar mass of element divided by molar mass of compound and multiply by 100.

4. What is the percent composition of H in water.
(2.02 g H ÷ g water) X 100 = 11.2% H

5. What is the percent composition of O in Glucose (C6H12O6).
(96 g O ÷ g Glucose) X 100 = 53.28% O

6. Empirical Formula
The formula of a compound with the smallest whole number mole ration of the elements.

7. To find empirical formula, take the grams of each element and convert to moles by dividing each element by their molar mass. Then take each mole and divided by the smallest mole. This gives you the subscript for each empirical formula.

8. What is the empirical formula with 40.05g S and 59.95g O.
40.05g S ÷ 32.07g/mol S = mol S
59.95gO÷16g/mol O=3.747mol O
1.249 mol S/1.249 = 1 mol S
3.747 mol O/1.249 = 3 mol O
SO3

9. What is the empirical formula with 35.98g Al and 64.02g S.
64.02g S÷32.07g/molS=1.99molS
35.98gAl÷26.98g/molAl=1.33molAl
1.33 mol Al/1.33 = 1 mol Al
1.99 mol S/1.33 = 1.5 mol S
Al2S3

10. Molecular Formula
It specifies the actual number of atoms of each element in one molecule or formula unit of the substance.

11. To find the molecular formula, take the experimental mass and divided by the mass of the empirical formula. Take this ratio and multiply by empirical formula to find molecular formula.

12. What is the molecular formula of a compound with empirical formula of CH and exp. mass of g/mol.
26.04 g/mol ÷ g/mol = 2
C2H2

13. What is the molecular formula of a compound with empirical formula of CH and exp. mass of g/mol.
78.12 g/mol ÷ g/mol = 6
C6H6