End Show Slide 1 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Mass Relationship Mole-mass relationship: How do you convert the mass of a substance to the number of moles of the substance? 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

End Show Slide 2 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole Road Map 10.2

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 3 of 39 End Show 10.5

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

for Sample Problem 10.5

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 6 of 39 End Show 10.6

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 7 of 39 End Show 10.6

© Copyright Pearson Prentice Hall Slide 8 of 39 End Show Practice Problems for Sample Problem 10.6

End Show © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > Slide 9 of 39 The Mole–Volume Relationship What is the volume of a mole of a gas at STP? of O 2 (g)? of H 2 (g)? of He (g)? 10.2

End Show Slide 10 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 11 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 kPa, or 1 atmosphere (atm). 10.2

End Show Slide 12 of 39 © Copyright Pearson Prentice Hall Mole–Mass and Mole– Volume Relationships > The Mole–Volume Relationship At STP, 1 mol or, 6.02  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 © Copyright Pearson Prentice Hall Slide 13 of 39 Mole–Mass and Mole– Volume Relationships > The Mole Road Map 10.2

End Show Slide 14 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 15 of 39 End Show 10.7

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 16 of 39 End Show 10.7

© Copyright Pearson Prentice Hall Slide 17 of 39 End Show Practice Problems for Sample Problem 10.7

End Show Slide 18 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 19 of 39 End Show 10.8

© Copyright Pearson Prentice Hall SAMPLE PROBLEM Slide 20 of 39 End Show 10.8

© Copyright Pearson Prentice Hall Slide 21 of 39 End Show Practice Problems for Sample Problem 10.8

End Show © Copyright Pearson Prentice Hall Slide 22 of 39 Mole–Mass and Mole– Volume Relationships > The Mole Road Map 10.2

End Show © Copyright Pearson Prentice Hall Slide 23 of 39 Section Quiz -or- Continue to: Launch: Assess students’ understanding of the concepts in Section 10.2 Section Quiz

© Copyright Pearson Prentice Hall Slide 24 of 39 End Show 10.2 Section Quiz. 1. Calculate the mass in grams of a sample containing 1.85 x molecules of water. a.3.07 x g b.5.53 x g c.188 g d.8.46 x 10 3 g

© Copyright Pearson Prentice Hall Slide 25 of 39 End Show 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  mol

© Copyright Pearson Prentice Hall Slide 26 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