1. Percent Composition and Chemical Formulas
Prentice-Hall Chapter 10.3
Dr. Yager

2. Objectives
Describe how to calculate the percent of mass of an element in a compound.
Interpret an empirical formula.
Distinguish between empirical and molecular formulas.

3. Percent Composition of a Compound
The percent by mass of an element in a compound is the number of grams of the element divided by the mass in grams of the compound, multiplied by 100%.

4. Percent Composition from Mass Data
The relative amounts of the elements in a compound are expressed as the percent composition or the percent by mass of each element in the compound.

7. Percent Composition from the Chemical Formula

10. Percent Composition as a Conversion Factor
You can use percent composition to calculate the number of grams of any element in a specific mass of a compound.

11. Propane (C3H8) is 81. 8% carbon and 18% hydrogen
Propane (C3H8) is 81.8% carbon and 18% hydrogen. You can calculate the mass of carbon and the mass of hydrogen in an 82.0 g sample of C3H8.

12. Ethyne (C2H2) is a gas used in welder’s torches
Ethyne (C2H2) is a gas used in welder’s torches. Styrene (C8H8) is used in making polystyrene.
These two compounds of carbon have the same empirical formula (CH) but different molecular formulas.

13. Empirical Formulas
The empirical formula of a compound shows the smallest whole-number ratio of the atoms in a compound.

17. Molecular Formula Compared to Empirical Formula
The molecular formula of a compound is either the same as its experimentally determined empirical formula, or it is a simple whole-number multiple of its empirical formula.

18. Methonal, ethanoic acid, and glucose all have the same empirical formula - CH2O.

22. 1. Calculate the percent by mass of carbon in cadaverine, C5H14N2, a compound present in rotting meat.
67.4% C
58.8% C
51.7% C
68.2% C

23. 1. Calculate the percent by mass of carbon in cadaverine, C5H14N2, a compound present in rotting meat.
67.4% C
58.8% C
51.7% C
68.2% C

24. 2. Which of the following is NOT an empirical formula?
H2N CH
C3H6

25. 2. Which of the following is NOT an empirical formula?
H2N CH
C3H6

26. 3. Determine the molecular formula of a compound that contains 40
3. Determine the molecular formula of a compound that contains 40.0 percent C, 6.71 percent H, and percent O and has a molar mass of g.
C2H4O2
CH2O
C2H3O
C2H4O

27. 3. Determine the molecular formula of a compound that contains 40
3. Determine the molecular formula of a compound that contains 40.0 percent C, 6.71 percent H, and percent O and has a molar mass of g.
C2H4O2
CH2O
C2H3O
C2H4O