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Chemical Quantities

Chemical Quantities . 10.1 The Mole: A Measurement of Matter. Do Now What is 4.2 x 10 5 x 6 Objective – Counting and the Mole HW Pg. 296 # 9-15. Measuring Matter. Common methods of measuring Count Mass Volume. What is a Dozen?. What is Dozen?. A dozen is 12 of something

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Chemical Quantities

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  1. Chemical Quantities 10.1 The Mole: A Measurement of Matter

  2. Do Now What is 4.2 x 105x 6 • Objective – Counting and the Mole • HW Pg. 296 # 9-15

  3. Measuring Matter • Common methods of measuring • Count • Mass • Volume

  4. What is a Dozen?

  5. What is Dozen? • A dozen is 12 of something we need to start thinking of the something as a representative particle

  6. What is a Mole?

  7. What is a Mole? • A mole = 6.02 x 1023 representative particles • A mole of any substance contains Avogadro’s Number of representative particles.

  8. Converting with the mole • How many dozen eggs is 136 eggs?

  9. Converting with the mole • How many dozen eggs is 136 eggs? 136 eggs * 1 dozen = 11.33 dozzen 12 eggs

  10. Converting with the mole • How many dozen eggs is 136 eggs? 136 eggs * 1 dozen = 11.33 dozzen 12 eggs • How many mole is 2.80 x 1024 atoms of silicon?

  11. Converting with the mole • How many dozen eggs is 136 eggs? 136 eggs * 1 dozen = 11.33 dozzen 12 eggs • How many mole is 2.80 x 1024 atoms of silicon? 2.80 x 1024atoms * 1 mole = 4.65 mol Si 6.02 x 1023atoms

  12. The Mass of a Mole of an Element

  13. 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.

  14. The Mass of a Mole of a Compound • What is the mass of a mole of H2O2?

  15. The Mass of a Mole of a Compound • What is the mass of a mole of H2O2? H + H + O + O 1.01 + 1.01 + 16.00 + 16.00 = 34.02grams

  16. Chemistry and Snow

  17. 10.2 Mole to Mass and Volume • The Mole Mass Relationship Mass (g) = number of moles x mass (g) 1 mole

  18. The Mole Mass Relationship Mass (g) = number of moles x mass (g) 1 mole What is the mass of 3 moles of NaCl?

  19. Mass (g) = number of moles x mass (g) 1 mole Mass (g) = 3.00 moles NaClx 58.5 (g) 1 mole NaCl = 176 g

  20. The Mole Volume Relationship At STP, 1 mole or 6.02 x 1023 representative particles, of any gas occupies a volume of 22.4L Molar Volume = 22.4 L

  21. 10.1 Homework Review • Pg. 296 #9-15 9. By count, mass, and volume 10. One mole of any substance contains Avogadro’s number (6.02 x 1023) representative particles 11. The molar mass on any element is its atomic mass expressed in grams 12. Add together the masses, expressed in grams, of each element in one mole of the compound 13. 2.49 x 10-1mol NH3 14. 5.27 x 1024 atoms 15. 136.2 grams/mole

  22. 10.1 and 10.2 Practice • Calculate the molar mass of the following a. Br b. H3PO4 • How many moles are in 15.5 g of SiO2? • Find the mass of 7.00 mole of H2O2. • Calculate the volume of 7.6 moles of Ar gas at STP. • Find the mass, in grams, of a single molecule of aspirin ( C9H8O4). • Find the number of atoms in 5,78 mol NH4NO3.

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