2. Section 7.3 - Percent Composition and Chemical Formulas

3. Calculating the Percent Composition of a compound

4. The relative amounts of each element (Part) in a compound (Whole) are expressed as the Percent Composition or the Percent by Mass of each element in the compound.

6. The percent composition of a compound has as many percent values as there are different elements in the compound.

7. The percent composition of CaCO3 is:

8. To calculate the percent composition of a compound, use the chemical formula to determine which elements and how many moles of each are in the compound.

9. Divide the total mass of one of the elements in the compound by the molar mass of the compound then multiply by 100 to convert to a percent.

10. Remember that the total mass of the element is the molar mass of the element multiplied by its subscript in the formula.

11. Example: What is the percent composition of FeSO4?
= 36.7 %
S =
= 21.1 %
O =
= 42.2 %

12. The Percent By Mass in a compound is the number of grams of the element divided by the number of grams of the compound multiplied by 100.

13. Sample Problem p 189
An 8.20 g piece of magnesium combines with 5.40 g of oxygen to form a compound. What is the Percent Composition (Percent By Mass) of this compound?

14. % Mg =
% Mg =
% O =
% O =

15. Using Percent Composition as a Conversion Factor

16. You can use the percent composition to determine the mass of each element in a sample of a compound.

17. Example: Aluminum makes up 52. 9 % of Al2O3
Example: Aluminum makes up % of Al2O3. Calculate the mass of Aluminum in a 50.0 g sample of Al2O3.

18. We first assume that we have a 100. 0g sample of Al2O3. 52. 9 % of 100
We first assume that we have a 100.0g sample of Al2O % of g is 52.9 g. We can use g divided by g sample as a conversion factor.

20. Calculating Empirical Formula

21. Empirical Formula

22. EMPIRICAL FORMULA
An empirical formula is the smallest whole number ratio of atoms in a formula.

23. EMPIRICAL FORMULA
If the atoms are in a small whole number ratio, then the moles of atoms of each element in the substance will also be in a small whole number ratio.

24. Two Sources of Data From Which to Calculate the Empirical Formula
Experimental Analysis - What is the empirical formula of a compound if a 2.50 gram sample contains g of calcium and 1.60 g of chlorine?

25. Two Sources of Data From Which to Calculate the Empirical Formula
Percentage Composition - A compound has a percentage composition of 40.0% C, 6.71% H, and 53.3% O. What is the empirical Formula?

26. The following is an Example of the Empirical Formula Calculation from Experimental Analysis.

27. What is the empirical formula for a compound if a 2
What is the empirical formula for a compound if a 2.50 g sample contains g of calcium and 1.60 g of chlorine?
Determine the number of moles of each element in the compound.

28. moles Ca
moles Cl

29. The next step is to determine the smallest whole number ratio.
To obtain the smallest whole number ratio, divide both numbers of moles by the smaller number of moles.

31. The mole ratio is 1 mole of Calcium to 2 moles of Chlorine.
The Empirical formula is therefore CaCl2.

32. Example of Empirical Formula Calculation From Percentage Composition:
A compound has a percentage composition of 40.0% C, 6.71% H, and 53.3% O. What is the empirical formula?

33. Example of Empirical Formula Calculation From Percentage Composition
To calculate the ratio of moles of these elements, we assume a 100 g sample % of 100 g is 40.0 g.

34. Example of Empirical Formula Calculation From Percentage Composition
Next we calculate the number of moles of each element present.

35. Example of Empirical Formula Calculation From Percentage Composition
Mol C
3.33
Mol H
6.67
Mol O
3.33

36. Determine the smallest Whole Number Ratio.
The number of moles of each element calculated in step 2 were: 3.33 mol C, 6.64 mol H, and 3.33 mol O. Dividing by the smallest value we obtain the smallest whole number ratio of moles.

37. For C
For H
For O

38. With a ratio of 1-C to 2-H to 1-O
The empirical formula is therefore --- CH2O.

39. What is the empirical formula for a compound if a 40
What is the empirical formula for a compound if a 40.0 g sample contains 29.7 g of sodium and 10.3 g of oxygen?

40. Solution:
Step 1 Determine the number of moles of each element.

42. This will give the smallest whole number ratio.
Step 2 Divide each number of moles by the smallest.
This will give the smallest whole number ratio.

44. The empirical formula is therefore Na2O.
This ratio shows that there are 2 moles of sodium for one mole of oxygen.
The empirical formula is therefore Na2O.

45. Calculating Molecular Formula

46. The Empirical Formula tells us the ratio of each kind of atom present in a compound.
The Molecular Formula tells us the actual number of each kind of atom in a molecule of a compound.

47. If the empirical formula and the molar mass are known, the molecular formula can be calculated.

48. Example:
A certain gas, having a molar mass of 78 g, has an empirical formula of CH. What is the molecular formula?

49. If we multiply the mass of the empirical formula by an integer, the product must equal the molar mass.

50. Where x represents an integer.
(CH)x = 78 g
Where x represents an integer.
(13)x = 78 g
X = 6

51. By multiplying each subscript in the empirical formula by the integer (6), we obtain the molecular formula.
(CH)6 gives C6H6

52. Problem:
The empirical formula of a compound is CHOCl and the molar mass is 129 g. What is the molecular formula?