moles notes. 1. atomic mass unit amu – atomic mass unit, used to describe the mass of an atom...

Moles Notes

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Moles Notes

1. Atomic Mass Unitamu – atomic mass unit, used to describe the mass of an atom

Conversion factor: 1 amu = 1.66 x 10-24 g

Equivalence statement: 1 amu or 1.66x10-24 g

1.66x10-24g 1 amu

Example:How many amu are in 27.0 grams of mercury?

x ________________amu Hg

1.66 x 10-24

g Hg

27.0 g Hg= 1.63 x 1025 amu Hg

Page 3: Moles Notes. 1. Atomic Mass Unit amu – atomic mass unit, used to describe the mass of an atom Conversion factor: 1 amu = 1.66 x 10 -24 g Equivalence statement:

2. The Mole

mole (mol) – indicates a quantity of a substance that has a mass in grams numerically equal to its atomic mass.

****Round the atomic mass on the periodic table to the TENTHS PLACE.****

Example:1 mol of copper = ______________ g1 mol of calcium = ______________ g1 mol of chromium = ______________ g

63.5

40.152.0

Page 4: Moles Notes. 1. Atomic Mass Unit amu – atomic mass unit, used to describe the mass of an atom Conversion factor: 1 amu = 1.66 x 10 -24 g Equivalence statement:

3. Molar Massmolar mass (g/mol) – indicates the mass of one

mole of a compound– 1st determine type of bond and write correct formula– 2nd add up the masses of each atom in the formula

Example:

Calculate the molar mass of sodium chloride

Calculate the molar mass of silver phosphate

Calculate the molar mass of barium hydroxide

NaClNa = 1 x 23.0 = 23.0Cl = 1 x 35.5 = 35.5

58.5 g/mol

Ag3PO4

Ag = 3 x 107.9 = 323.7 P = 1 x 31.0 = 31.0 418.7 g/mol O = 4 x 16.0 = 64.0

Ba = 1 x 137.3 = 137.3

O = 2 x 16.0 = 32.0 H = 2 x 1.0 = 2.0

Ba(OH)2

171.3 g/mol

Page 5: Moles Notes. 1. Atomic Mass Unit amu – atomic mass unit, used to describe the mass of an atom Conversion factor: 1 amu = 1.66 x 10 -24 g Equivalence statement:

4. Avogadro’s Number

Avogadro’s number – indicates the number of atoms molecules or particles in a mole.

Conversion factor: 1 mol = 6.022 x 1023 units of a substance

(atoms, molecules, particles)

Equivalence statement: 1 amu _ or 6.022x1023atoms 6.022x1023atoms 1 amu

Page 6: Moles Notes. 1. Atomic Mass Unit amu – atomic mass unit, used to describe the mass of an atom Conversion factor: 1 amu = 1.66 x 10 -24 g Equivalence statement:

Examples:

Mole Mass

What is the mass of 5.0 mol of sulfur?

Mass Mole

How many moles are in 17.0 g of bromine,Br2?

x ______________g S

32.1

mol S5.0 mol S = 160 g S

x ____________mol Br2

159.8

g Br2

17.0 g Br2 = 0.106 mol Br2

Br = 2 x 79.9 = 159.8 g/mol

Page 7: Moles Notes. 1. Atomic Mass Unit amu – atomic mass unit, used to describe the mass of an atom Conversion factor: 1 amu = 1.66 x 10 -24 g Equivalence statement:

Mole Atoms (molecules or particles)

How many atoms are in 2.3 moles of copper?

Atoms (molecules or particles) Mole

How many moles are in 1.24 x 1024 molecules of carbon dioxide?

x __________________atoms Cu

6.02 x 1023

mol Cu2.3 mol Cu = 1.4 x 1024 atoms Cu

x ____________________mol CO2

6.02 x 1023

molecules CO2

1.24 x 1024 molecules CO2 =

2.06 mol CO2

Page 8: Moles Notes. 1. Atomic Mass Unit amu – atomic mass unit, used to describe the mass of an atom Conversion factor: 1 amu = 1.66 x 10 -24 g Equivalence statement:

Atoms (molecules or particles) Grams

How many grams are in 2.4 x 1025 particles of KCl?

Grams Atoms (molecules or particles)

How many atoms are in 514 g of Pb?

x ______________g KCl

mol KCl

74.6

x ____________________mol KCl

6.02 x 1023

particles KCl

2.4 x 1025 particles KCl =

3.0 x 103 g KCl

K 1 x 39.1 = 39.1

Cl 1 x 35.5 = 35.5

74.6 g/mol

x __________________atoms Pb

mol Pb

6.02 x 1023

x ______________mol Pb

207.9

g Pb

514 g Pb=

1.49 x 1024 atoms Pb

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