1. Using Chemical Formulas

2. H2O The chemical formula for water is H2O.
How many atoms of hydrogen and oxygen are there in one water molecule?
H2O
1 oxygen atom
2 hydrogen atoms
How might you calculate the mass of a water molecule, given the atomic masses of hydrogen and oxygen?
In this section, you will learn how to carry out these and other calculations for any compound.

3. Using Chemical Formulas
As well as indicating the elements and the relative numbers of atoms or ions of each element in a compound, chemical formulas can also be used to calculate formula mass, molar mass, and the percent composition of a compound.

4. Formula Mass
The formula mass of any molecule, formula unit, or ion is the sum of the average atomic masses of all the atoms represented in its formula.
The units for formula mass are atomic mass units (amu).
The mass of a water molecule, H2O, can be referred to as a molecular mass.
The mass of one formula unit of an ionic compound, such as NaCl, is not a molecular mass.

5. Example: Find the formula mass for H2O.
H2O has 2 hydrogen atoms and 1 oxygen atom.
Atomic mass of hydrogen = 1.01 amu
Atomic mass of oxygen = amu
2 hydrogen atoms x 1.01 amu =
1 oxygen atom x amu =
2.02 amu
16.00 amu
Total
18.02 amu
Formula mass of H2O

6. Molar Masses
The molar mass of a substance is equal to the mass in grams of one mole, or 6.02 x 1023 particles, of the substance.
Units for molar mass are g/mol.
The molar mass of a compound is calculated by summing the masses of the elements present in a mole of the molecules or formula units that make up that compound.
A compound’s molar mass is numerically equal to its formula mass.

7. Example: Find the molar mass for KClO3.
KClO3 has 1 potassium (K) atom, 1 chlorine atom (Cl), and 3 oxygen (O) atoms.
Atomic mass of potassium = amu
Atomic mass of chlorine = amu
Atomic mass of oxygen = amu
1 potassium atom x amu =
1 chlorine atom x amu =
3 oxygen atoms x amu =
39.10 amu
35.45 amu
48.00 amu
Total
amu

8. Since a compound’s molar mass is numerically equal to its formula mass (KClO3 = amu) the molar mass of KClO3 would be
Numerically equivalent to formula mass but units are different.
g/mol
This tells us that if we have one mole of KClO3 we would have g of KClO3 or
6.02 x 1023 formula units of KClO3.

9. Molar Mass as a Conversion Factor
The molar mass of a compound can be used as a conversion factor to relate an amount in moles to a mass in grams for a given substance.
To convert moles to grams, multiply the amount in moles by the molar mass.
Amount in moles x molar mass (g/mol) = mass in grams

10. Example:
What is the mass in grams of 2.50 mol of oxygen (O2) gas?
Given: mol O2
Unknown: mass of O2 in grams
Solution: mol O2 → grams O2

11. Determine the molar mass of O2.
O2 has 2 oxygen atoms.
Atomic mass of O is amu.
2 oxygen atoms x = amu
Remember that molar mass is numerically equal to the formula mass so the molar mass of O2 = g/mol.
32.00
g O2
80.0
g O2
2.50 mol O2 x = 1
mol O2

12. Ibuprofen, C13H18O2, is the active ingredient in many nonprescription pain relievers. Its molar mass is g/mol.
a. If the tablets in a bottle contain a total of 33 g of ibuprofen, how many moles of ibuprofen are in the bottle? 1
mol
C13H18O2
33 g C13H18O2 x =
0.16
mol C13H18O2
206.31 g
C13H18O2

13. b. How many molecules of ibuprofen are in the bottle
b. How many molecules of ibuprofen are in the bottle? Remember we have 0.16 mol.
6.02 x 1023
molecules
0.16 mol C13H18O2 x =
9.6 x 1022 1
mol
molecules
C13H18O2

14. c. What is the total mass in grams of carbon in 33 g of ibuprofen?
To start, determine the number of moles of carbon per 1 mole of C13H18O2. There are 13 moles of carbon per 1 mole of C13H18O2.
Two conversion factors are needed to solve problem: number of moles of carbon per mole of C13H18O2 and the molar mass of carbon.
13 moles C
12.01 g C
1 mol C13H18O2
1 mol C

15. How many moles are present in the sample? 13
mol C
12.01
g C
0.16 mol C13H18O2 x x 1
mol C 1
mol C13H18O2 25
g C =
Problem:
Consider a sample of 10.0 g of the gaseous hydrocarbon C3H4 to answer the following questions.
How many moles are present in the sample?
How many molecules are present in the C3H4 sample?
What is the total mass in grams of carbon in the sample?

16. Additional Problems:
How many molecules of aspirin, C9H8O4, are there in moles of aspirin?
If we have 6.54 x 108 molecules HCN, how many moles of HCN are there?
What is the total mass of nitrogen in 1.25 moles of Zn(NO3)2?

17. Percent Composition
It is often useful to know the percentage by mass of a particular element in a compound.
For example, suppose the compound potassium chlorate, KClO3, were to be used as a source of oxygen. It would be useful to know the percentage of oxygen in the compound.
To find the mass percentage of an element in a compound, the following equation can be used.

18. The mass percentage of an element in a compound is the same regardless of the sample’s size.
The percentage of an element in a compound can be calculated by determining how many grams of the element are present in one mole of the compound.
The percentage by mass of each element in a compound is known as the percentage composition of the compound.

19. Percentage Composition of Iron Oxides

20. Example: Find the percentage composition of copper(I) sulfide, Cu2S.
1) Find the molar mass of the compound.
Cu2S has 2 copper atoms and 1 sulfur atom.
The atomic mass of copper is amu and the atomic mass of sulfur is amu.
2 copper atoms x amu =
1 sulfur atom x amu =
127.1 amu
32.07 amu
The formula mass of Cu2S = amu.
The molar mass of Cu2S = g/mol.

21. 2) Use the mass of each element present in one mole of the compound to calculate the mass percentage of each element.
2 atoms of Cu = g
1 atom of S = g
Molar mass of Cu2S = g.
A good check is to see if the results add up to about 100%. (Because of rounding, the total may not always be exactly 100%).