Chapter10 section02 Mole–Mass and Mole–Volume Relationships By Hamdy Karim

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Hamdy Karim

Students will learn how they calculate the number of moles of a substance and the mol of a gas at STP!

Education Technology

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Mole–Mass and Mole–Volume
Relationships
How can you guess the number of
jelly beans in a jar? You estimate
the size of a jelly bean and then
estimate the dimensions of the
container to obtain its volume. In a
similar way, chemists use the
relationships between the mole and
quantities such as mass, volume,
and number of particles to solve
chemistry problems.
10.2

© Copyright Pearson Prentice Hall
Mole–Mass and Mole–
Volume Relationships
>
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The Mole–Mass Relationship
The Mole–Mass Relationship
How do you convert the mass of a
substance to the number of moles of the
substance?
10.2

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© Copyright Pearson Prentice Hall
Mole–Mass and Mole–
Volume Relationships
> The Mole–Mass Relationship
Use the molar mass of an element
or compound to convert between
the mass of a substance and the
moles of a substance.
10.2

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SAMPLE PROBLEM
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10.5

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SAMPLE PROBLEM
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10.5

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SAMPLE PROBLEM
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10.5

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SAMPLE PROBLEM
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10.5

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Practice Problems for Sample Problem 10.5
Problem Solving 10.16 Solve
Problem 16 with the help of an
interactive guided tutorial.

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SAMPLE PROBLEM
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10.6

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10.6

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10.6

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10.6

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Practice Problems for Sample Problem 10.6
Problem Solving 10.18 Solve
Problem 18 with the help of an
interactive guided tutorial.

© Copyright Pearson Prentice Hall
Mole–Mass and Mole–
Volume Relationships
>
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The Mole–Volume Relationship
The Mole–Volume Relationship
What is the volume of a gas at STP?
10.2

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© Copyright Pearson Prentice Hall
Mole–Mass and Mole–
Volume Relationships
> The Mole–Volume Relationship
Avogadro’s hypothesis states that equal
volumes of gases at the same temperature
and pressure contain equal numbers of
particles.
10.2

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© Copyright Pearson Prentice Hall
Mole–Mass and Mole–
Volume Relationships
> The Mole–Volume Relationship
The volume of a gas varies with temperature
and pressure. Because of these variations,
the volume of a gas is usually measured at a
standard temperature and pressure.
Standard temperature and pressure (STP)
means a temperature of 0°C and a pressure
of 101.3 kPa, or 1 atmosphere (atm).
10.2

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© Copyright Pearson Prentice Hall
Mole–Mass and Mole–
Volume Relationships
> The Mole–Volume Relationship
At STP, 1 mol or, 6.02 × 1023
representative particles, of any gas
occupies a volume of 22.4 L.
The quantity 22.4 L is called the
molar volume of a gas.
10.2

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© Copyright Pearson Prentice Hall
Mole–Mass and Mole–
Volume Relationships
> The Mole–Volume Relationship
Calculating Volume at STP
10.2

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SAMPLE PROBLEM
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10.7

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SAMPLE PROBLEM
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10.7

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SAMPLE PROBLEM
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10.7

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SAMPLE PROBLEM
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10.7

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Practice Problems for Sample Problem 10.7
Problem Solving 10.20 Solve
Problem 20 with the help of an
interactive guided tutorial.

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© Copyright Pearson Prentice Hall
Mole–Mass and Mole–
Volume Relationships
> The Mole–Volume Relationship
Calculating Molar Mass from Density
10.2

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SAMPLE PROBLEM
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10.8

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SAMPLE PROBLEM
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10.8

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SAMPLE PROBLEM
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10.8

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SAMPLE PROBLEM
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10.8

© Copyright Pearson Prentice Hall
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Practice Problems for Sample Problem 10.8
Problem Solving 10.22 Solve
Problem 22 with the help of an
interactive guided tutorial.

© Copyright Pearson Prentice Hall
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Mole–Mass and Mole–
Volume Relationships
> The Mole Road Map10.2

© Copyright Pearson Prentice Hall
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Mole–Mass and Mole–
Volume Relationships
> The Mole Road Map10.2

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Mole–Mass and Mole–
Volume Relationships
> The Mole Road Map10.2

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Mole–Mass and Mole–
Volume Relationships
> The Mole Road Map
The Mole Road Map
10.2

© Copyright Pearson Prentice Hall
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Mole–Mass and Mole–
Volume Relationships
> Simulation 10
Simulation 10
Use the mole road map to convert among
mass, volume, and number of representative
particles.

© Copyright Pearson Prentice Hall
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Section Quiz
-or-
Continue to: Launch:
Assess students’ understanding
of the concepts in Section
10.2 Section Quiz.
10.2.

© Copyright Pearson Prentice Hall
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10.2 Section Quiz.
1. Calculate the mass in grams of a sample
containing 1.85 x 1034
molecules of water.
a. 3.07 x 1010
g
b. 5.53 x 1011
g
c. 188 g
d. 8.46 x 103
g

© Copyright Pearson Prentice Hall
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10.2 Section Quiz.
2. Calculate the number of moles in a spoonful
of table sugar (C12H22O11) having a mass of
10.5 g.
a. 32.6 mol
b. 3.59 × 103
mol
c. 3.07 × 10–3
mol
d. 1.85 × 1022
mol

© Copyright Pearson Prentice Hall
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10.2 Section Quiz.
3. What is the volume of 0.35 mol of oxygen gas
at STP?
a. 32 L
b. 64 L
c. 7.8 L
d. 16 L

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Chapter10 section02 Mole–Mass and Mole–Volume Relationships By Hamdy Karim

1. Slide 1 of 39 chemistry

2. © Copyright Pearson Prentice Hall Slide 2 of 39 Mole–Mass and Mole–Volume Relationships How can you guess the number of jelly beans in a jar? You estimate the size of a jelly bean and then estimate the dimensions of the container to obtain its volume. In a similar way, chemists use the relationships between the mole and quantities such as mass, volume, and number of particles to solve chemistry problems. 10.2

3. © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > Slide 3 of 39 The Mole–Mass Relationship The Mole–Mass Relationship How do you convert the mass of a substance to the number of moles of the substance? 10.2

4. Slide 4 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Mass Relationship Use the molar mass of an element or compound to convert between the mass of a substance and the moles of a substance. 10.2

9. © Copyright Pearson Prentice Hall Slide 9 of 39 Practice Problems for Sample Problem 10.5 Problem Solving 10.16 Solve Problem 16 with the help of an interactive guided tutorial.

14. © Copyright Pearson Prentice Hall Slide 14 of 39 Practice Problems for Sample Problem 10.6 Problem Solving 10.18 Solve Problem 18 with the help of an interactive guided tutorial.

15. © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > Slide 15 of 39 The Mole–Volume Relationship The Mole–Volume Relationship What is the volume of a gas at STP? 10.2

16. Slide 16 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Volume Relationship Avogadro’s hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles. 10.2

17. Slide 17 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Volume Relationship The volume of a gas varies with temperature and pressure. Because of these variations, the volume of a gas is usually measured at a standard temperature and pressure. Standard temperature and pressure (STP) means a temperature of 0°C and a pressure of 101.3 kPa, or 1 atmosphere (atm). 10.2

18. Slide 18 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Volume Relationship At STP, 1 mol or, 6.02 × 1023 representative particles, of any gas occupies a volume of 22.4 L. The quantity 22.4 L is called the molar volume of a gas. 10.2

19. Slide 19 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Volume Relationship Calculating Volume at STP 10.2

24. © Copyright Pearson Prentice Hall Slide 24 of 39 Practice Problems for Sample Problem 10.7 Problem Solving 10.20 Solve Problem 20 with the help of an interactive guided tutorial.

25. Slide 25 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Volume Relationship Calculating Molar Mass from Density 10.2

30. © Copyright Pearson Prentice Hall Slide 30 of 39 Practice Problems for Sample Problem 10.8 Problem Solving 10.22 Solve Problem 22 with the help of an interactive guided tutorial.

34. © Copyright Pearson Prentice Hall Slide 34 of 39 Mole–Mass and Mole– Volume Relationships > The Mole Road Map The Mole Road Map 10.2

35. © Copyright Pearson Prentice Hall Slide 35 of 39 Mole–Mass and Mole– Volume Relationships > Simulation 10 Simulation 10 Use the mole road map to convert among mass, volume, and number of representative particles.

36. © Copyright Pearson Prentice Hall Slide 36 of 39 Section Quiz -or- Continue to: Launch: Assess students’ understanding of the concepts in Section 10.2 Section Quiz. 10.2.

37. © Copyright Pearson Prentice Hall Slide 37 of 39 10.2 Section Quiz. 1. Calculate the mass in grams of a sample containing 1.85 x 1034 molecules of water. a. 3.07 x 1010 g b. 5.53 x 1011 g c. 188 g d. 8.46 x 103 g

38. © Copyright Pearson Prentice Hall Slide 38 of 39 10.2 Section Quiz. 2. Calculate the number of moles in a spoonful of table sugar (C12H22O11) having a mass of 10.5 g. a. 32.6 mol b. 3.59 × 103 mol c. 3.07 × 10–3 mol d. 1.85 × 1022 mol

39. © Copyright Pearson Prentice Hall Slide 39 of 39 10.2 Section Quiz. 3. What is the volume of 0.35 mol of oxygen gas at STP? a. 32 L b. 64 L c. 7.8 L d. 16 L

40. END OF SHOW

Editor's Notes

These aluminum satellite dishes at the National Radio Astronomy Observatory near Soccoro, New Mexico are naturally protected from corrosion by the formation of a thin film of aluminum oxide (Al2O3).
Rust weakens an iron chain.
In each container, the volume occupied by the gas molecules is small compared with the container’s volume, so the molecules are not tightly packed. a) The molecules in this container are small. b) This container can accommodate the same number of larger molecules.
This box, with a volume of 22.4 L, holds one mole of gas at STP.
The map shows the conversion factors needed to convert among volume, mass, and number of particles. Interpreting Diagrams How many conversion factors are needed to convert from the mass of a gas to the volume of a gas at STP?
The map shows the conversion factors needed to convert among volume, mass, and number of particles. Interpreting Diagrams How many conversion factors are needed to convert from the mass of a gas to the volume of a gas at STP?
The map shows the conversion factors needed to convert among volume, mass, and number of particles. Interpreting Diagrams How many conversion factors are needed to convert from the mass of a gas to the volume of a gas at STP?
The map shows the conversion factors needed to convert among volume, mass, and number of particles. Interpreting Diagrams How many conversion factors are needed to convert from the mass of a gas to the volume of a gas at STP?

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