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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.