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2010 Balancing Equations
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2010 Balancing Equations

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  • Transcript

    • 1. Balancing Equations February 2, 2010
    • 2. Objectives
      • Balance both sides of a chemical equation by making the number of atoms equal
      • Use coefficients to balance the number of atoms on each side of a chemical equation
      • Explain the Law of Conservation of Mass in a chemical equation
    • 3. CHEMICAL REACTIONS Reactants: Zn + I 2 Product: Zn I 2
    • 4. Chemical Equations
      • Depict the kind of reactants and products and their relative amounts in a reaction.
      • 4 Al (s) + 3 O 2 (g) ---> 2 Al 2 O 3 (s)
      • The letters (s), (g), and (l) are the physical states of compounds.
    • 5.
      • Reaction of charcoal and oxygen
        • C (s) + O 2 (g)  CO 2 (g)
    • 6.
      • Because of the principle of the conservation of matter ,
      • an equation must be balanced .
      • It must have the same number of atoms of the same kind on both sides.
      Chemical Equations Lavoisier, 1788
    • 7.
        • When balancing a chemical reaction you may add coefficients in front of the compounds to balance the reaction, but you may
        • not
        • change the subscripts.
    • 8. Subscripts vs. Coefficients
      • The subscripts tell you how many atoms of a particular element are in a compound. The coefficient tells you about the quantity, or number, of molecules of the compound.
    • 9. Chemical Equations
      • 4 Al (s) + 3 O 2(g) ---> 2 Al 2 O 3 (s)
      • means
      • 4 Al atoms + 3 O 2 molecules ---produces--->
      • 2 molecules of Al 2 O 3
    • 10.