CHAPTER 3

CHAPTER 3 - 3 Chemical Equations & Reaction Stoichiometry...

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3 Chemical Equations & Reaction Stoichiometry
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2 Chapter Three Goals 1. Chemical Equations 2. Calculations Based on Chemical Equations 3. The Limiting Reactant Concept 4. Percent Yields from Chemical Reactions 5. Sequential Reactions 6. Concentrations of Solutions 7. Dilution of solutions 8. Using Solutions in Chemical Reactions 9. Synthesis Question
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3 Chemical Equations Symbolic representation of a chemical reaction that shows: 1. reactants on left side of reaction 2. products on right side of equation 3. relative amounts of each using stoichiometric coefficients
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4 Chemical Equations Attempt to show on paper what is happening at the laboratory and molecular levels.
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5 Chemical Equations Look at the information an equation provides: Fe O + 3 CO 2 Fe + 3 CO 2 3 2  →
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6 Chemical Equations Look at the information an equation provides: reactants yields products Fe O + 3 CO 2 Fe + 3 CO 2 3 2  →
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7 Chemical Equations Look at the information an equation provides: reactants yields products 1 formula unit 3 molecules 2 atoms 3 molecules Fe O + 3 CO 2 Fe + 3 CO 2 3 2  →
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8 Chemical Equations Look at the information an equation provides: reactants yields products 1 formula unit 3 molecules 2 atoms 3 molecules 1 mole 3 moles 2 moles 3 moles Fe O + 3 CO 2 Fe + 3 CO 2 3 2  →
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9 Chemical Equations Look at the information an equation provides: reactants yields products 1 formula unit 3 molecules 2 atoms 3 molecules 1 mole 3 moles 2 moles 3 moles 159.7 g 84.0 g 111.7 g 132 g Fe O + 3 CO 2 Fe + 3 CO 2 3 2  →
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10 Chemical Equations Law of Conservation of Matter There is no detectable change in quantity of matter in an ordinary chemical reaction. Balanced chemical equations must always include the same number of each kind of atom on both sides of the equation. This law was determined by Antoine Lavoisier. • Propane,C 3 H 8 , burns in oxygen to give carbon dioxide and water. O H 4 CO 3 O 5 H C 2 2 2 8 3 + → +
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11 Law of Conservation of Matter • NH 3 You do it! You do it!
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12 Law of Conservation of Matter • NH 3 O H 6 + NO 4 O 5 + NH 4 correctly or O H 3 + NO 2 O + NH 2 2 2 3 2 2 2 5 3 → →
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13 Law of Conservation of Matter • C 7 H 16 burns in oxygen to form carbon dioxide and water. You do it! You do it!
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14 Law of Conservation of Matter • C 7 H 16 burns in oxygen to form carbon dioxide and water. O H 8 + CO 7 O 11 + H C 2 2 2 16 7 →
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15 Law of Conservation of Matter • C 7 H 16 burns in oxygen to form carbon dioxide and water. Balancing equations is a skill acquired only with lots of practice work many problems O H 8 + CO 7 O 11 + H C 2 2 2 16 7 →
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Calculations Based on Chemical Equations Can work in moles, formula units, etc. Frequently, we work in mass or weight
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This note was uploaded on 04/16/2011 for the course CHEM 1211 taught by Professor Atwood during the Spring '07 term at UGA.

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CHAPTER 3 - 3 Chemical Equations & Reaction Stoichiometry...

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