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Chapter #3   Lecture Part 1[1]
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Chapter #3 Lecture Part 1[1]

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Transcript

  • 1. Stoichiometry
    • Stoichiometry = “Chemical Arithmetic”
    • Stoichiometry of Elements
    • Stoichiometry of Compounds
    • Stoichiometry of Chemical Reactions
  • 2. Atomic mass is the mass of an atom in atomic mass units (amu) Micro World atoms & molecules Macro World grams
  • 3. The mole (mol) is the amount of a substance that contains as many elementary entities as there are atoms in exactly 12.00 grams of 12 C
  • 4. Molar mass is the mass of 1 mole of in grams eggs shoes marbles atoms 1 mole 12 C atoms = 6.022 x 10 23 atoms = 12.00 g 1 12 C atom = 12.00 amu 1 mole 12 C atoms = 12.00 g 12 C 1 mole lithium atoms = 6.941 g of Li
  • 5.  
  • 6. Lecture Problem
    • Calculate the mass, in grams, of 4.50 moles of calcium atoms.
  • 7. Lecture Problem
    • Calculate the number of moles of calcium atoms in 612 grams of calcium.
    • Calculate the number of calcium atoms in 612 grams of calcium.
  • 8. Molecular mass (or molecular weight) is the sum of the atomic masses (in amu) in a molecule. SO 2
  • 9. Molar Mass Problem
    • Calculate the molar mass of sucrose, C 12 H 22 O 11 .
  • 10. Percent composition of an element in a compound = n is the number of moles of the element in 1 mole of the compound 52.14% + 13.13% + 34.73% = 100.0% n x molar mass of element molar mass of compound x 100% C 2 H 6 O %C = 2 x (12.01 g) 46.07 g x 100% = 52.14% %H = 6 x (1.008 g) 46.07 g x 100% = 13.13% %O = 1 x (16.00 g) 46.07 g x 100% = 34.73%
  • 11. Empirical Formula
    • Identifies the elements present and shows the simplest whole-number ratio of the atoms in a substance.
  • 12. Data Utilized To Determine An Empirical Formula
    • Weight of each element present in a given sample of the compound.
    • Weight percentage of each element in a compound.
    • Weight of products generated from a reaction involving the compound of interest.
  • 13. Empirical Formula Problem
    • Determine the empirical formula of a compound containing 11.66 grams of iron and 5.01 grams of oxygen.
  • 14. Empirical Formula Problem
    • Determine the empirical formula of a compound containing 62.1% carbon, 5.21% hydrogen, 12.1% nitrogen, and 20.7% oxygen.
  • 15. Molecular Formula
    • Identifies the elements present and shows the exact number of atoms of each element present per molecule.
  • 16. Data Utilized To Determine A Molecular Formula
    • Empirical Formula
    • &
    • Molar Mass of Compound
  • 17. Molecular Formula Problem
    • Cadaverine, a foul smelling substance produced by the action of bacteria on meat, contains 58.55% carbon, 13.81% hydrogen and 27.40% nitrogen. The molar mass of the compound is 102.2 grams/mole. Determine the molecular formula of cadaverine.

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