 # © Copyright Pearson Prentice Hall Slide 1 of 39 Mole–Mass and Mole–Volume Relationships How can you guess the number of jelly beans in a jar? You estimate.

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© Copyright Pearson Prentice Hall Slide 1 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

© Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > Slide 2 of 39 The Mole–Mass Relationship How do you convert the mass of a substance to the number of moles of the substance? 10.2

Slide 3 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 Coversion Factor: 1mole = molar mass

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 4 of 39 10.5

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 5 of 39 10.5

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 6 of 39 10.5

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 7 of 39 10.5

© Copyright Pearson Prentice Hall Slide 8 of 39 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 9 of 39 10.6

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 10 of 39 10.6

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 11 of 39 10.6

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 12 of 39 10.6

© Copyright Pearson Prentice Hall Slide 13 of 39 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 > Slide 14 of 39 The Mole–Volume Relationship What is the volume of a gas at STP? 10.2

Slide 15 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

Slide 16 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

Slide 17 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Volume Relationship At STP, 1 mol or, 6.02  10 23 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

Slide 18 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Volume Relationship Calculating Volume at STP 10.2 Conversion Factor: 1 mole = 22.4 L at STP

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 19 of 39 10.7

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 20 of 39 10.7

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 21 of 39 10.7

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 22 of 39 10.7

© Copyright Pearson Prentice Hall Slide 23 of 39 Practice Problems for Sample Problem 10.7 Problem Solving 10.20 Solve Problem 20 with the help of an interactive guided tutorial.

Slide 24 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 25 of 39 10.8

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 26 of 39 10.8

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 27 of 39 10.8

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 28 of 39 10.8

© Copyright Pearson Prentice Hall Slide 29 of 39 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 Slide 30 of 39 Mole–Mass and Mole– Volume Relationships > The Mole Road Map 10.2

© Copyright Pearson Prentice Hall Slide 31 of 39 Mole–Mass and Mole– Volume Relationships > The Mole Road Map 10.2

© Copyright Pearson Prentice Hall Slide 32 of 39 Mole–Mass and Mole– Volume Relationships > The Mole Road Map 10.2

© Copyright Pearson Prentice Hall Slide 33 of 39 Mole–Mass and Mole– Volume Relationships > The Mole Road Map 10.2

© Copyright Pearson Prentice Hall Slide 34 of 39 Mole–Mass and Mole– Volume Relationships > Simulation 10 Use the mole road map to convert among mass, volume, and number of representative particles.

© Copyright Pearson Prentice Hall Slide 35 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 36 of 39 10.2 Section Quiz. 1. Calculate the mass in grams of a sample containing 1.85 x 10 34 molecules of water. a.3.07 x 10 10 g b.5.53 x 10 11 g c.188 g d.8.46 x 10 3 g

© Copyright Pearson Prentice Hall Slide 37 of 39 10.2 Section Quiz. 2. Calculate the number of moles in a spoonful of table sugar (C 12 H 22 O 11 ) having a mass of 10.5 g. a.32.6 mol b.3.59  10 3 mol c.3.07  10 –3 mol d.1.85  10 22 mol

© Copyright Pearson Prentice Hall Slide 38 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

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