40
End Show Slide 1 of 39 chemistry
| Date post: | 14-Dec-2015 |
| Category: |
Documents |
| Upload: | lionel-roberts |
| View: | 213 times |
| Download: | 0 times |
End Show
Slide 1 of 39
chemistry
End Show© 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
End Show© 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
End Show
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
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 5 of 39
End Show
10.5
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 6 of 39
End Show
10.5
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 7 of 39
End Show
10.5
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 8 of 39
End Show
10.5
© Copyright Pearson Prentice Hall
Slide 9 of 39
End Show
Practice Problems for Sample Problem 10.5
Problem Solving 10.16 Solve Problem 16 with the help of an interactive guided tutorial.
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 10 of 39
End Show
10.6
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 11 of 39
End Show
10.6
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 12 of 39
End Show
10.6
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 13 of 39
End Show
10.6
© Copyright Pearson Prentice Hall
Slide 14 of 39
End Show
Practice Problems for Sample Problem 10.6
Problem Solving 10.18 Solve Problem 18 with the help of an interactive guided tutorial.
End Show© 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
End Show
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
End Show
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
End Show
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
End Show
Slide 19 of 39
© Copyright Pearson Prentice Hall
Mole–Mass and Mole–Volume Relationships
> The Mole–Volume Relationship
Calculating Volume at STP
10.2
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 20 of 39
End Show
10.7
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 21 of 39
End Show
10.7
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 22 of 39
End Show
10.7
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 23 of 39
End Show
10.7
© Copyright Pearson Prentice Hall
Slide 24 of 39
End Show
Practice Problems for Sample Problem 10.7
Problem Solving 10.20 Solve Problem 20 with the help of an interactive guided tutorial.
End Show
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
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 26 of 39
End Show
10.8
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 27 of 39
End Show
10.8
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 28 of 39
End Show
10.8
© Copyright Pearson Prentice Hall
SAMPLE PROBLEM
Slide 29 of 39
End Show
10.8
© Copyright Pearson Prentice Hall
Slide 30 of 39
End Show
Practice Problems for Sample Problem 10.8
Problem Solving 10.22 Solve Problem 22 with the help of an interactive guided tutorial.
End Show© Copyright Pearson Prentice Hall
Slide 31 of 39
Mole–Mass and Mole–Volume Relationships
> The Mole Road Map10.2
End Show© Copyright Pearson Prentice Hall
Slide 32 of 39
Mole–Mass and Mole–Volume Relationships
> The Mole Road Map10.2
End Show© Copyright Pearson Prentice Hall
Slide 33 of 39
Mole–Mass and Mole–Volume Relationships
> The Mole Road Map10.2
End Show© Copyright Pearson Prentice Hall
Slide 34 of 39
Mole–Mass and Mole–Volume Relationships
> The Mole Road Map
The Mole Road Map
10.2
End Show© 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.
End Show© 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.
© Copyright Pearson Prentice Hall
Slide 37 of 39
End Show
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
Slide 38 of 39
End Show
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
Slide 39 of 39
End Show
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
END OF SHOW
