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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

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© 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

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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

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

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

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

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

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© 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.

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© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 9 of 39 10.6

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

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

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

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© 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.

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© 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

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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

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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

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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

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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

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

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

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

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

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© 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.

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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

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© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 25 of 39 10.8

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

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

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

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© 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.

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

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

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

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

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© 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.

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© 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.

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© 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

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© 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

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© 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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