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THE MOLE

THE MOLE. Lesson 1: The Mole and Avogadro’s Number. Unit 8 – Moles and Stoichiometry. What is the Mole?. It’s a counting number. Like :. 1 dozen =. 12. 144. 1 gross =. 1 ream =. 500. VERY. A large amount!!!!. What is the Mole?. Avogadro’s number (N A )

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THE MOLE

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  1. THE MOLE

  2. Lesson 1:The Mole and Avogadro’s Number Unit 8 – Moles and Stoichiometry

  3. What is the Mole? It’s a counting number Like: 1 dozen = 12 144 1 gross = 1 ream = 500

  4. VERY A large amount!!!! What is the Mole? • Avogadro’s number (NA) • 1 mol = 6.02  1023 representative particles

  5. Avogadro’s Number 6.02 x 1023 is called “Avogadro’s Number” in honor of the Italian chemist Amadeo Avogadro (1776-1855). I didn’t discover it. Its just named after me! Amadeo Avogadro

  6. HOW LARGE IS IT??? A. What is the Mole? • 1 mole of pennies would cover the Earth 1/4 mile deep! • 1 mole of hockey pucks would equal the mass of the moon! • 1 mole of basketballs would fill a bag the size of the earth!

  7. What is the Mole? • 1 mol = 6.02  1023 representative particles • Representative particle refers to the species present in a substance: particles, atoms, molecules, or formula units.

  8. Converting Between Amount in Moles and Number of Particles

  9. Converting Moles to Number of representative particles 1. How many molecules are in 2.50 moles of C12H22O11? 6.02  1023 molecules 1 mol 2.50 mol = 1.51  1024 molecules C12H22O11

  10. How many atoms of lithium are in 3.50 moles of lithium? 3.50 mol Li 6.02 x 1023 atoms Li = atoms Li 2.11 x 1024 1 mol Li

  11. Converting Number of Representative Particles to mole Calculate the moles of Aluminum Oxide in 2.0 x1024 molecules 2.0 x 1024 molecules 1 mole = 3.32 mole of Aluminum Oxide 6.02  1023 molecules

  12. What does Atomic Mass tell us? • Atomic mass tells the mass of 1 mole of an element • atomic mass units per atom (amu) • round to 2 decimal places

  13. The Mass of a Mole of an Element 12.01 amu 26.98 amu 65.39 amu • carbon • aluminum • zinc

  14. What is Formula Mass? The sum of the atomic masses of all atoms in a compound • water • sodium chloride • H2O • 2(1.01) + 16.00 = 18.02 amu • NaCl • 22.99 + 35.45 = 58.44 amu

  15. Why the Mole? amu is too small to measure in most labs The mole establishes a relationship between amu and grams.

  16. What is Molar Mass? The mass in grams of one mole of atoms is numerically the same as the mass in Atomic mass units of one of those atoms amu = g/mol Formula Mass unit = amu Molar Mass unit = g/mol

  17. Molar Mass Examples • sodium bicarbonate • sucrose • NaHCO3 • 22.99 + 1.01 + 12.01 + 3(16.00) = 84.01 g/mol • C12H22O11 • 12(12.01) + 22(1.01) + 11(16.00) = 342.34 g/mol

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