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Mole Calculations 1

Mole Calculations 1. Chemical Calculations. Atoms and molecules are extremely small. If they are so small and so light, how can we weigh them?. We weigh large numbers of them. Avogadro took 1.00 g of the smallest atom (H) and determined how many H atoms there are in 1.00 g of H .

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Mole Calculations 1

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  1. Mole Calculations 1

  2. Chemical Calculations Atoms and molecules are extremely small. If they are so small and so light, how can we weigh them? We weigh large numbers of them.

  3. Avogadro took 1.00 g of the smallest atom (H) and determined how many H atomsthere are in 1.00 g of H. He found that: 1.00 g H = 6.02 x 1023 atoms = 1.00 mole This is called Avogadro’s number

  4. 1 dozen donuts = 12 donuts 1 century = 100 years 1 millennium = 1000 years 1.00 mole = 6.02 x 1023 particles

  5. The mole is a large number of particles Particle Atom element Cu 6.02 x 1023 at 1 mole Molecule covalent CH4 6.02 x 1023 molecules 1 mole Formula Unit ionic NaCl6.02 x 1023 FUs 1 mole

  6. 1. Convert 2.5 x 1025 at C to moles 2.5 x 1025 at x 1 mole = 42 moles C 6.02 x 1023 at

  7. 2. Convert 16.3 moles CO2 to molecules 16.3 moles x 6.02 x 1023 molecules = 9.81 x 1024 molecules 1mole

  8. 3. Convert 8.9 x 1024 molecules CO2 to moles x 1 mole 8.9 x 1024 molecules = 15 moles CO2 6.02 x 1023 molecules

  9. 4. Convert 28 moles NaCl to Formula Units x 6.02 x 1023 FU 28 moles = 1.7 x 1025 FUs 1mole

  10. Determining Avogadro’s Number

  11. Electrolysis Apparatus Ampmeter Power Supply Stop Watch

  12. Determining Avogadro’s Number Produce a volume of hydrogen gas while measuring the time and electrical current. Volume of H210.0 mL Time 80.7 s Current0.913 amp

  13. Background information 1 amp is defined as the number of coulombs per second. There are 6.24 x 1018 electrons in a coulomb. The density of H2 is 0.07871 g/L. It takes 1 electron to make 1 H atom

  14. 1. Calculate the number of atoms of H, starting with the time. 80.7 s x 0.913 coul x 6.24 x 1018 el x 1 at H = 4.5976 x 1020 at s 1 coul 1 el

  15. 2. Calculate the number of grams H starting with the volume of H. 10.0 mL x 1 L x 0.07871 g = 7.871 x 10-4 g H 1000 mL 1 L

  16. 3. Divide the atoms of H by the grams of H to get the number of H atoms in a gram which is Avogadro’s number. 4.5976 x 1020 at 7.871 x 10-4 g H = 5.84 x 1023 at/ 1 gram H = 5.84 x 1023 at/ 1 mole Avogadro Facts The Mole Song

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