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Understanding Moles in Chemistry: Counting Particles with Precision

Discover how chemists use moles to count particles in this detailed guide, including interesting facts and key historical milestones. Learn about Avogadro's contribution, the Law of Conservation of Mass, and conversion methods between moles and particles.

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Understanding Moles in Chemistry: Counting Particles with Precision

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  1. So what unit do chemists use to count particles? Particles are so tiny, chemists use the unit of moles. A mole contains 6.02 x 1023 atoms. 602, 000, 000, 000, 000, 000, 000, 000

  2. 602,000,000,000,000,000,000,000 • One mole of popcorn would cover every dry surface of the Earth to a depth of six miles • One mole of stacked pennies would reach to the moon and back 16 times • One mole of marshmallows would cover the US to a depth of 650 miles

  3. 1811- Avogadro- equal volumes of gases at the same temperature and pressure contained equal number of molecules • 1861- Cannizzaro- developed atomic weights for known elements • 1865- Loschmidt- determined the number of atoms present in given volume of air • 1971- true value 6.02 x 1023 found

  4. Recall the Law of Conservation of Mass Mass of reactants = mass of products Mass of starting substances = mass of ending substances 2 hydrogen atoms + 1 oxygen atom  1 water molecule

  5. Law of Definite Proportions • Regardless of amount, a compound will always be composed of the same elements in the same proportions by mass • For example, two hydrogen atoms will always combine with one oxygen atom to produce one molecule of water

  6. x 6.02 x 1023 Moles Particles Atoms, molecules ÷ 6.02 x 1023 Moles ↔ Particles Conversion

  7. Convert 3.5 moles to atoms

  8. Convert 18.06x1023 atoms to moles

  9. Convert from moles to particles • 2.7 moles of lithium • 1.8 moles of sodium chloride

  10. Convert from moles to particles • 5.3 moles of bromine • 4.7 moles of potassium oxide

  11. particles  moles • 4.32 x 1024 atoms of calcium

  12. particles  moles • 2.7 x 1020 atoms of copper

  13. particles  moles • 2.5 x 1024 molecules of sodium chloride • 5.32 x 1023 molecules of calcium chloride

  14. You try these… • 25 moles to particles • 4.08 x 104 particles to moles • 0.002 moles to particles • 2.3 x 1016 particles

  15. Moles to particles 2.7 moles 1.8 moles 5.3 moles 4.7 moles Particles to moles 4.32 X 1024 2.70 X 1020 2.50 X 1024 5.32 X 1023 HomeworkComplete on another sheet of paper showing your work!

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