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Chemistry Lesson 10.1

Chemistry Lesson 10.1. “The Mole”. I. Measuring Matter. A. 3 ways… 1. counting (#’s) 2. mass (gram, pound…) 3. volume (liter, gallon…) B. Units of measurement… 1. pair = 2. dozen = 3. ream =. 2. 12. 500. II. What is a mole?.

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Chemistry Lesson 10.1

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  1. ChemistryLesson 10.1 “The Mole”

  2. I. Measuring Matter A. 3 ways… 1. counting (#’s) 2. mass (gram, pound…) 3. volume (liter, gallon…) B. Units of measurement… 1. pair = 2. dozen = 3. ream = 2 12 500

  3. II. What is a mole? A. Def – the S.I. unit that measures an amount or quantity. 1. similar to others: dozen (12), ream (144), bakers dozen (13), gross (144), hour (60 min), day (24 hr)… B. 1 mole = 1. 2. 602,000,000,000,000,000,000,000 2. called Avogadro’s number 3. Usually refers to atoms, molecules, or compounds (Fe, H2O, CaCl2) 6.02 x 1023particles

  4. C. Why such a big number? 1. Atoms are smaller than microscopic 2. We need to be precise in chemistry

  5. D. Problems 1. How many moles of iron do you have with 2.41 x 1024 atoms? = 4.00 moles of iron 2. I have 3.3 x 1022 formula units of NaCl. How many moles is this? =0.055 moles of NaCl 3. I have 9.76 x 1025 molecules of N2. How many moles is this? =162 moles

  6. 4. How many molecules are in 2.12 mol of propane (C3H8)? 2.12 mol x (6.02 x 1023) propane molecules 1 1 mol =1.28 x 1024 propane molecules 5. How many atoms of propane are found in 1.28 x 1024 molecules of propane? 1.28 x 1024 molecules x 11 atoms 1 1 molecule (C3H8) =1.41 x 1025 atoms

  7. 7. With a partner create a question similar to others used today and answer it. Then write the same question down and trade it with another group. Grade it when they are done.

  8. Assignment 10.1 • How many atoms are in 4.10 mol of C6H12O6? • How many molecules are in 0.750 mol of H2O? • How many C atoms are in 0.890 mol of C6H12O6? • How many H atoms are in 1.23 mol of C6H12O6? • How many mol are found in 6.02 x 1027 molecules of H2O? 5.92 x 1025 atoms 4.52 x 1023 molecules 3.21 x 1024 Carbon atoms 8.89 x 1024 Hydrogen atoms 1.00 x 104 mol of water

  9. III. How much does a mole weigh? A. Molar Mass (single elements) 1. Def – how much 1 mole of an element weighs in grams. 2. Ex: Carbon = 3. Others: P = K = Ag = Fe = Ar = Li = 12.01 g 30.97 39.10 107.87 55.85 39.95 6.94

  10. B. Molar Mass (molecule – covalent) 1. Def – the mass of one mole of a molecular compound. 2. Use atomic values and add together 3. Ex: SO3 S = 32.06 O = 16.00 (3) 32.06 + 48.00 = 80.06 g

  11. 4. Examples PO4 C8H18 H2O SO4 PCl3 N2O5 94.97 114.26 18.02 96.06 137.32 108.02

  12. C. Molar Mass (compound – ionic) 1. Def – the mass of one mole of an ionic compound. 2. Examples CaI2Na3PO4 Li3N AlCl3 Fe2O3 Al(OH)3 163.94 293.88 133.33 34.83 159.70 78.01

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