Unit 13 Chemical Reactions

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Unit 13 Chemical Reactions

  1. 1. Unit 13:CHEMICAL REACTIONS<br />Reactants: Zn + I2<br />Product: Zn I2<br />
  2. 2. Unit 13 Learning Objectives:<br /><ul><li> Explore the nature of chemical reactions, including catalysts and reactants.</li></li></ul><li>Unit 13 Learning Objectives:<br /><ul><li> Explore the nature of chemical reactions, including catalysts and reactants.
  3. 3. Law of conservation of mass and energy.</li></li></ul><li>Unit 13 Learning Objectives:<br /><ul><li> Explore the nature of chemical reactions, including catalysts and reactants.
  4. 4. Law of conservation of mass and energy.
  5. 5. Write and balance chemical equations.</li></li></ul><li>Unit 13 Learning Objectives:<br /><ul><li> Explore the nature of chemical reactions, including catalysts and reactants.
  6. 6. Law of conservation of mass and energy.
  7. 7. Write and balance chemical equations.
  8. 8. Learn to classify the different reaction types.</li></li></ul><li>A Little Review of the Terms <br /><ul><li>Chemical Reaction: when two or more substances come together to form a NEW substance, this is a chemical reaction!
  9. 9. Substances can be Atoms, Molecules, or Compounds</li></ul>Reactants<br />Products<br />Chemical reaction is occurring<br />
  10. 10. A Little Review of the Terms <br /><ul><li>Chemical Reaction: when two or more substances come together to form a NEW substance, this is a chemical reaction!
  11. 11. Substances can be Atoms, Molecules, or Compounds
  12. 12. Reactants are the things being brought together to react
  13. 13. Products are the new stuff that is made in the reaction!</li></ul>Reactants<br />Products<br />Chemical reaction is occurring<br />
  14. 14. Identifying chemical reactions<br />The release of heat and/or light<br />The formation of a solid when two liquids are mixed together (precipitate)<br />
  15. 15. Identifying chemical reactions<br />The change in color when two liquids are poured together<br />The formation of a gas from a <br />liquid solution<br />
  16. 16. Chemical Equations<br />Because of the principle of the <br /> conservation of matter<br />The chemical equation must be balanced<br />It must have the same number of atoms of the same kind on both sides.<br />C3H8 + O2 CO2 + H2O<br />C = 3 H = 8 O =2 C = 1 H = 2 O = 3<br />
  17. 17. Balancing Equations<br />C3H8 + O2 CO2 + H2O<br /> 3C 8H<br />C3H8 + O2 CO2 + H2O<br />
  18. 18. Balancing Equations<br />C3H8 + O2 CO2 + H2O<br />C3H8 + O23CO2 + 4H2O<br /> 10 O = 6 O + 4 O<br />
  19. 19. Balancing Equations<br />C3H8 + O2 CO2 + H2O<br />C3H8 + O23CO2 + 4H2O<br /> 10 O <br />
  20. 20. Balancing Equations<br />C3H8 + O2 CO2 + H2O<br />C3H8 + 5O23CO2 + 4H2O<br /> 10 O <br />
  21. 21. Which one of the following is a balanced equation?<br />Ca (s) + O2 (g) -> 2CaO (s)<br />B. 2Ca (s) + O2 (g) -> 2CaO (s)<br />C. 3Ca (s) + O2 (g) -> CaO (s)<br />D. 6Ca (s) + O2 (g) -> 2CaO (s)<br />Secret Question<br />
  22. 22. Which one of the following is a balanced equation?<br />Ca (s) + O2 (g) -> 2CaO (s)<br />B. 2Ca (s) + O2 (g) -> 2CaO (s)<br />C. 3Ca (s) + O2 (g) -> CaO (s)<br />D. 6Ca (s) + O2 (g) -> 2CaO (s)<br />Secret Question<br />
  23. 23. Which one of the following is a balanced equation?<br />Ca (s) + O2 (g) -> 2CaO (s)<br />B. 2Ca (s) + O2 (g) -> 2CaO (s)<br />C. 3Ca (s) + O2 (g) -> CaO (s)<br />D. 6Ca (s) + O2 (g) -> 2CaO (s)<br />2O<br />2Ca and 2O<br />2Ca<br />Secret Question<br />
  24. 24. Symbols Used in Equations<br />Solid (s)<br />Liquid (l)<br />Gas (g)<br />Aqueous solution (aq)<br />Catalyst H2SO4<br />Change of temperature () Delta<br />
  25. 25. Chemical Equations<br />Reactants and Products<br />Al (s) + O2 (g) ---&gt; Al2O3 (s)<br />Stoichiometry:<br />
  26. 26. Chemical Equations<br />Reactants and Products<br />Al (s) + O2 (g) ---&gt; Al2O3 (s)<br />Stoichiometry:<br />2Al<br />2<br />
  27. 27. Chemical Equations<br />Reactants and Products<br />Al (s) + O2 (g) ---&gt; Al2O3 (s)<br />Stoichiometry:<br />3O<br />2 times what equals 3?<br />
  28. 28. Chemical Equations<br />Reactants and Products<br />Al (s) + O2 (g) ---&gt; Al2O3 (s)<br />Stoichiometry:<br />3O<br />2 times what equals 3? 1.5<br />but, that is not a whole number…<br />So, what do we do?<br />
  29. 29. Chemical Equations<br />Reactants and Products<br />Al (s) + O2 (g) ---&gt; 2Al2O3 (s)<br />Stoichiometry:<br />6O<br />2 times what equals 6?<br />
  30. 30. Chemical Equations<br />Reactants and Products<br />Al (s) + 3O2 (g) ---&gt; 2Al2O3 (s)<br />Stoichiometry:<br />6O<br />2 times what equals 6?<br />
  31. 31. Chemical Equations<br />Reactants and Products<br />Al (s) + 3O2 (g) ---&gt; 2Al2O3 (s)<br />Stoichiometry:<br />4Al<br />2 times what equals 6?<br />
  32. 32. Chemical Equations<br />Reactants and Products<br />4Al (s) + 3O2 (g) ---&gt; 2Al2O3 (s)<br />Stoichiometry: is the part of chemistry that studies amounts of substances that are involved in reactions. <br />
  33. 33. Chemical Equations<br />Fe2O3 = rust<br />Aluminum powder<br />What happens when you mix rust and aluminum? <br />Thermite Reaction<br />
  34. 34. Chemical Equations<br />Fe2O3 + 2Al -> 2Fe + Al2O3<br />Thermite Reaction<br />http://www.youtube.com/watch?v=sjLgzgflCk8&feature=related<br />
  35. 35. Chemical Equations<br />Fe2O3 + 2Al -> 2Fe + Al2O3<br />Thermite Reaction<br />This reaction needs a lot of heat to get started, but produces far more heat afterwards (&gt; 2000°F)<br />
  36. 36. Classifying Reactions<br />Five main types: <br />Synthesis<br />Combustion<br />Decomposition<br />Single displacement<br />Double displacement <br />
  37. 37. Synthesis Reaction<br />Two or more substances combine to form another substance. <br />For example: A + B  AB <br />2H2+ O2 2H2O<br />2 or more simpler substances  one more complex substance<br />
  38. 38. Decomposition Reactions<br />Opposite of synthesis. <br />One substance breaks down into 2 or more other substances. <br />AB  A + B <br />One compound 2 or more simpler substances<br />2H2O 2H2+ O2<br />electricity<br />
  39. 39. Single Replacement Reaction<br />One element replaces another element in a compound <br />A + BC  AC + B <br />Element + compound  new element + new compound<br />Zn + CuSO4  ZnSO4 + Cu<br />
  40. 40. Double Replacement Reactions<br />Positive ion of one compound replaces the positive ion of the other <br />AB + CD  AD + CB <br />2 compounds 2 new compounds<br />Forms precipitate, covalent compound, or gas<br />AgNO3 (aq) + NaCl (aq) -> AgCl (s) + NaNO3 (aq)<br />
  41. 41. Combustion<br />Reaction of a substance with oxygen and a flame <br />If it is combustion of a hydrocarbon, you always get CO2 and H2O (both gases)<br />Oxygen (O2) is always a reactant. <br />C3H8 + 5 O2 -> 3 CO2 + 4 H2O + heat<br />

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