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Chemistry10.1

Chemistry10.1. 10.1. The Mole: A Measurement of Matter.

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Chemistry10.1

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  1. Chemistry10.1

  2. 10.1 The Mole: A Measurement of Matter • You could measure the amount of sand in a sand sculpture by counting each grain of sand, but it would be much easier to weigh the sand. You’ll discover how chemists measure the amount of a substance using a unit called a mole, which relates the number of particles to the mass.

  3. 10.1 Measuring Matter • Measuring Matter • What are three methods for measuring the amount of something?

  4. 10.1 Measuring Matter • You often measure the amount of something by one of three different methods—by count, by mass, and by volume.

  5. 10.1

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  8. 10.1

  9. for Sample Problem 10.1

  10. 10.1 What is a Mole? • What Is a Mole? • How is Avogadro’s number related to a mole of any substance?

  11. 10.1 What is a Mole? • A mole of any substance contains Avogadro’s number of representative particles, or 6.02  1023 representative particles. • The term representative particle refers to the species present in a substance: usually atoms, molecules, or formula units.

  12. 10.1 What is a Mole? • Converting Number of Particles to Moles • One mole (mol) of a substance is 6.02  1023 representative particles of that substance and is the SI unit for measuring the amount of a substance. • The number of representative particles in a mole, 6.02  1023, is called Avogadro’s number.

  13. 10.1 What is a Mole?

  14. 10.2

  15. 10.2

  16. 10.2

  17. 10.2

  18. for Sample Problem 10.2

  19. 10.1 What is a Mole? • Converting Moles to Number of Particles

  20. 10.3

  21. 10.3

  22. 10.3

  23. 10.3

  24. for Sample Problem 10.3

  25. 10.1 The Mass of a Mole of an Element • The Mass of a Mole of an Element • How is the atomic mass of an element related to the molar mass of an element?

  26. 10.1 The Mass of a Mole of an Element • The atomic mass of an element expressed in grams is the mass of a mole of the element. • The mass of a mole of an element is its molar mass.

  27. 10.1 The Mass of a Mole of an Element • One molar mass of carbon, sulfur, mercury, and iron are shown.

  28. 10.1 The Mass of a Mole of a Compound • The Mass of a Mole of a Compound • How is the mass of a mole of a compound calculated?

  29. 10.1 The Mass of a Mole of a Compound • To calculate the molar mass of a compound, find the number of grams of each element in one mole of the compound. Then add the masses of the elements in the compound.

  30. 10.1 The Mass of a Mole of a Compound • Substitute the unit grams for atomic mass units. Thus 1 mol of SO3 has a mass of 80.1 g.

  31. 10.1 The Mass of a Mole of a Compound • Molar Masses of Glucose, Water, and Paradichlorobenzene

  32. 10.4

  33. 10.4

  34. 10.4

  35. 10.4

  36. for Sample Problem 10.4

  37. 10.1 Section Quiz. • 10.1.

  38. 10.1 Section Quiz. • 1. Three common ways of measuring the amount of something are by count, by mass, and • by temperature. • by volume. • by area. • by density.

  39. 10.1 Section Quiz. • 2. A mole of hydrogen gas, H2(g), contains 6.02 x 1023 • molecules. • atoms. • amu. • grams.

  40. 10.1 Section Quiz. • 3. The atomic mass of fluorine is 19.0 amu, so the molar mass is • 19.0 amu. • 19.0 g. • 6.02 x 1023 amu. • 6.02 x 1023 g.

  41. 10.1 Section Quiz. • 4. Calculate the molar mass of ammonium nitrate. • 45.02 g • 80.05 g • 60.06 g • 48.05 g

  42. END OF SHOW

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