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Balancing equations
 

Balancing equations

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    Balancing equations Balancing equations Presentation Transcript

    • Balancing Chemical Equations
    • Law of Conservation of Matter
      • “ Matter is neither created nor destroyed, only changed from one form to another.”
    • 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!
    • 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
    • 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???
    • these are the diatomics
    • 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
    • Sample Problems
    • 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
    • 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
    • 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
    • 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
    • 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
    • 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