1 / 39

Mole–Mass and Mole–Volume Relationships

10.2. Mole–Mass and Mole–Volume Relationships.

rpoore
Télécharger la présentation

Mole–Mass and Mole–Volume Relationships

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. 10.2 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.

  2. 10.2 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?

  3. 10.2 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. Coversion Factor: 1mole = molar mass

  4. 10.5

  5. 10.5

  6. 10.5

  7. 10.5

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

  9. 10.6

  10. 10.6

  11. 10.6

  12. 10.6

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

  14. 10.2 The Mole–Volume Relationship • The Mole–Volume Relationship • What is the volume of a gas at STP?

  15. 10.2 The Mole–Volume Relationship • Avogadro’s hypothesis states that equal volumes of gases at the same temperature and pressure contain equal numbers of particles.

  16. 10.2 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).

  17. 10.2 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.

  18. 10.2 The Mole–Volume Relationship • Calculating Volume at STP Conversion Factor: 1 mole = 22.4 L at STP

  19. 10.7

  20. 10.7

  21. 10.7

  22. 10.7

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

  24. 10.2 The Mole–Volume Relationship • Calculating Molar Mass from Density

  25. 10.8

  26. 10.8

  27. 10.8

  28. 10.8

  29. for Sample Problem 10.8 Problem Solving 10.22 Solve Problem 22 with the help of an interactive guided tutorial.

  30. 10.2 The Mole Road Map

  31. 10.2 The Mole Road Map

  32. 10.2 The Mole Road Map

  33. 10.2 The Mole Road Map • The Mole Road Map

  34. Simulation 10 • Simulation 10 • Use the mole road map to convert among mass, volume, and number of representative particles.

  35. 10.2 Section Quiz. 10.2.

  36. 10.2 Section Quiz. • 1. Calculate the mass in grams of a sample containing 1.85 x 1034 molecules of water. • 3.07 x 1010 g • 5.53 x 1011 g • 188 g • 8.46 x 103 g

  37. 10.2 Section Quiz. • 2. Calculate the number of moles in a spoonful of table sugar (C12H22O11) having a mass of 10.5 g. • 32.6 mol • 3.59  103 mol • 3.07  10–3 mol • 1.85  1022 mol

  38. 10.2 Section Quiz. • 3. What is the volume of 0.35 mol of oxygen gas at STP? • 32 L • 64 L • 7.8 L • 16 L

  39. END OF SHOW

More Related