1. Chapter 10 Chemical Quantities 10.1 The Mole: A Measurement of Matter
10.2 Mole-Mass and Mole-Volume Relationships
10.3 Percent Composition and Chemical Formulas
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2. What ways can you quantify how much you have of something?
What Is a Mole?
What ways can you quantify how much you have of something?
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3. This is similar to using
What Is a Mole?
The ‘mole’ is a unit of measurement used to count the number of particles found within a substance.
This is similar to using
Dozen (12)
Pair (2)
Ream (500)
Gross (144)
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4. What Is a Mole?
1 mole = × 1023 of ANYTHING
6.02 × 1023 is called Avogadro’s number in honor of the person who started working with it.
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5. Representative particle
What Is a Mole?
representative particle - species present in a substance, usually atoms, molecules, or formula units.
Representative particle
Example
Element
Atom
Copper
Molecular Compound
Molecule
H2O
Ionic Compound
Formula Unit
NaCl
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6. 1 mole = 6.02 × 1023 representative particles
What Is a Mole?
The mole can be used as a conversion factor
1 mole = × 1023 representative particles
1 mole × 1023 of something
6.02 × 1023 of something 1 mole
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7. How many molecules are in 6.3 moles of methane (CH4)?
Sample Problem 10.3
Converting Moles to Number of Molecules
How many molecules are in 6.3 moles of methane (CH4)?
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8. How many molecules are in 6.3 moles of methane (CH4)?
Sample Problem 10.3
Converting Moles to Number of Molecules
How many molecules are in 6.3 moles of methane (CH4)?
3.79 x 1024 molecules of CH4
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9. How many atoms are in 6.3 moles of methane (CH4)?
Sample Problem 10.3
Converting Moles to Atoms
How many atoms are in 6.3 moles of methane (CH4)?
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10. How many atoms are in 6.3 moles of methane (CH4)?
Sample Problem 10.3
Converting Moles to Atoms
How many atoms are in 6.3 moles of methane (CH4)?
1.89 x atoms
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11. Molar Mass Mass of a mole of an element
For elements, this is the atomic mass given in the periodic table, expressed in grams.
Also called molecular weight or molecular mass(in case of molecules which is the sum of atomic masses of all the atoms they are composed of)
Element
Molar Mass
Carbon
12.0 g
Hydrogen
1.0 g
Chlorine
35.5 g
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12. The Mass of a Mole of an Element
Molar Mass
The Mass of a Mole of an Element
1 mol of sulfur atoms = 32.1 g
1 mol of carbon atoms = 12.0 g
1 mol of iron atoms = 56.0 g
This figure shows one mole of carbon, sulfur, and iron.
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13. Molar Mass
The mass of a mole of a compound is the sum of the masses of all the atoms in the compound.
Example
Molar mass SO3 = molar mass S + molar mass O3
= 32.1g g x 3
= 80.1 g
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14. Finding the Molar Mass of a Compound
Sample Problem 10.4
Finding the Molar Mass of a Compound
Calculate the molar mass of the following compounds.
NaCl
N2O3
Fe(OH)2
Be3(PO4)2
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15. Finding the Molar Mass of a Compound
Sample Problem 10.4
Finding the Molar Mass of a Compound
Calculate the molar mass of the following compounds.
NaCl – 58.5g
N2O3 – 76.0 g
Fe(OH)2 – 89.8 g
Be3(PO4)2 – 217 g
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16. END OF 10.1
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