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Balancing equations
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Transcript

  • 1. Balancing Chemical Equations
  • 2. Law of Conservation of Matter
    • “ Matter is neither created nor destroyed, only changed from one form to another.”
  • 3. LCM continued
    • Every reaction that takes place in nature or in the laboratory must have the same number of atoms on both sides of the equation, or is BALANCED!
  • 4. ANATOMY OF AN EQUATION
    • Letter in parenthesis tells state of matter
    • notice H and O with their subscripts…
    • why???
    H 2 (g) + O 2 (g) H 2 O(l) reactants yield products
  • 5. DIATOMIC ELEMENTS
    • In nature, diatomic elements contain two atoms bonded together, hence di- prefix.
    • When written by themselves , always get a subscript 2.
    • Which ones are diatomic???
  • 6. these are the diatomics
  • 7. BALANCING EQUATIONS
    • Atom inventory of the whole equation
    • Balance atoms by adding coefficients!
    • You cannot add or change subscripts!!!
    RULES: (1) save O and H till the end (2) use least common multiple to get numbers equal (3) start with oddest combination or biggest difference
  • 8. Sample Problems
  • 9. Cu(s) + O 2 (g) Cu 2 O(s) Cu O 1 2 2 1 2 1 2 1 2 2 balanced!!! 4 4 4
  • 10. K(s) + N 2 (g) K 3 N(s) K N 1 2 3 1 3 1 3 2 1 2 6 6 6 BALANCED
  • 11. Al(s) + HCl(aq) AlCl 3 (aq) + H 2 (g) Al H Cl 1 1 1 1 2 3 3 1 3 3 6 3 6 6 6 2 6 2 2 2 BALANCED
  • 12. Co(s) + O 2 (g) Co 2 O 3 (s) Co O 1 2 2 3 2 1 2 3 2 6 6 4 4 4 BALANCED
  • 13. Al 2 O 3 (s) + C(s) Al(s) + CO 2 (g) Al O C 2 3 1 1 2 1 2 2 2 3 6 6 4 3 3 3 4 BALANCED 4
  • 14. AgNO 3 (aq) + H 2 S(aq) Ag 2 S(s) + HNO 3 (aq) Ag N O H S 1 1 3 2 1 2 1 3 1 1 2 2 2 6 2 2 2 6 1 1 BALANCED