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2010 Balancing Equations


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2010 Balancing Equations

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