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Chapter 10: Chemical Quantities (Topic pre-viewed in lab)

Chapter 10: Chemical Quantities (Topic pre-viewed in lab). The mole : A measurement of matter TB section 10.1 Mole-Mass and Mole-Volume relationships: TB section 10.2 Percent Composition and Chemical Formula TB section10.3. Activities

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Chapter 10: Chemical Quantities (Topic pre-viewed in lab)

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  1. Chapter 10: Chemical Quantities (Topic pre-viewed in lab) The mole: A measurement of matter TB section 10.1 Mole-Mass and Mole-Volume relationships: TB section 10.2 Percent Composition and Chemical Formula TB section10.3 • Activities • In-class workshops calculation of molar mass (gram-formula mass) • Open-notes evaluations • Quizes and tests • Homework • Lab activities • Mole ratios lab – Qualitative Lab 5 • Mole labs – Quantitative Labs 6 , 8, 9 • Na2CO3 + CaCl2 yields CaCO3 and 2 NaCl • NaHCO3 and HCl yields CO2 + H2O + NaCl • Percent composition of water in a hydrate

  2. 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 term representative particle refers to the species present in a substance: usually atoms, molecules, or formula units. • The number of representative particles in a mole, 6.02  1023, is called Avogadro’s number.

  3. 10.1 What is a Mole?

  4. 10.2

  5. 10.2

  6. 10.1 What is a Mole? • Converting Moles to Number of Particles

  7. 10.3 • Read the question CAREFULLY. What do you need to find? • Hints: • How many molecules of propane are in one mole of propane? • How many atoms are there in one molecule of propane?

  8. 10.3

  9. 10.3

  10. 10.3

  11. for Sample Problem 10.3

  12. 10.1 The Mass of a Mole of an Element • The Mass of a Mole of an Element (use Periodic Table) • How is the atomic mass of an element related to the molar mass 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 (gram-formula mass).

  13. 10.1 The Mass of a Mole of an Element • One molar mass of carbon, sulfur, mercury, and iron are shown.

  14. 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? • 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.

  15. 10.1 The Mass of a Mole of a Compound • One SO3 molecule has a mass of 80.1 amu. Substitute the unit grams for atomic mass units. Thus 1 mol of SO3 has a mass of 80.1 g. One mole of SO3 molecules has a mass of 80.1 grams

  16. 10.1 The Mass of a Mole of a Compound • Molar Masses of Glucose, Water, and Paradichlorobenzene

  17. 10.4

  18. 10.1 Section Quiz. • 10.1.

  19. 10.1 Section Quiz. • 2. A mole of hydrogen gas, H2(g), contains 6.02 x 1023 • molecules. • atoms. • amu. • grams.

  20. 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.

  21. 10.1 Section Quiz. • 4. Calculate the molar mass of ammonium nitrate. • 45.02 g • 80.05 g • 60.06 g • 48.05 g

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