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Types of Reactions: Double Replacement and Combustion

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Types of Reactions: Double Replacement and Combustion

  1. 1. Classifying Equations The Five Types of Chemical Equations Chapter 11.2
  2. 2. Objectives <ul><li>Describe the five types of chemical equations. </li></ul><ul><li>Predict the products of the five types of chemical equations. </li></ul>
  3. 3. Preview of the Five Reaction Types <ul><li>using the terminology of your Chemistry Reference Tables/EOC (it may not match with the book) </li></ul><ul><li>1) Synthesis </li></ul><ul><li>2) Decomposition </li></ul><ul><li>3) Single Replacement </li></ul><ul><li>4) Double Replacement </li></ul><ul><li>5) Combustion </li></ul><ul><li>Found on p. 6 of your Chemistry Reference Tables </li></ul>
  4. 4. Double Replacement Reactions <ul><li>Swapping cations </li></ul>
  5. 5. Double Replacement Reactions <ul><li>Swapping cations </li></ul>
  6. 6. Double Replacement Reactions <ul><li>Swapping cations </li></ul><ul><li>Na 2 S (aq) + Cd(NO 3 ) 2 (aq) ---> CdS (s) + 2 Na(NO 3 ) (aq) </li></ul>
  7. 7. Double Replacement Reactions <ul><li>Swapping cations </li></ul><ul><li>Na 2 S (aq) + Cd(NO 3 ) 2 (aq) ---> CdS (s) + 2 Na(NO 3 ) (aq) </li></ul><ul><li>IDENTITY BADGE : Two compounds ---> two compounds. </li></ul>
  8. 8. Precipitation <ul><li>precipitate : any solid product from a chemical reaction </li></ul>
  9. 9. Precipitation <ul><li>precipitate : any solid product from a chemical reaction </li></ul><ul><li>Especially common in double replacement reactions. </li></ul>
  10. 10. Precipitation <ul><li>precipitate : any solid product from a chemical reaction </li></ul><ul><li>Especially common in double replacement reactions. </li></ul><ul><li>Usually do not list the other product. </li></ul>
  11. 11. Precipitation <ul><li>precipitate : any solid product from a chemical reaction </li></ul><ul><li>Especially common in double replacement reactions. </li></ul><ul><li>Example question: Calcium bromide reacts with silver nitrate to produce silver bromide as a precipitate. </li></ul><ul><li>Usually do not list the other product. </li></ul>
  12. 12. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul>
  13. 13. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na </li></ul>
  14. 14. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na B = OH </li></ul>
  15. 15. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na B = OH C = Fe </li></ul>
  16. 16. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na B = OH C = Fe D = NO 3 </li></ul>
  17. 17. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na + B = OH C = Fe D = NO 3 </li></ul>
  18. 18. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na + B = OH - C = Fe D = NO 3 </li></ul>
  19. 19. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na + B = OH - C = Fe 3+ D = NO 3 </li></ul>
  20. 20. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na + B = OH - C = Fe 3+ D = NO 3 - </li></ul>
  21. 21. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na + B = OH - C = Fe 3+ D = NO 3 - </li></ul><ul><li>AD = Na + & NO 3 - </li></ul>
  22. 22. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na + B = OH - C = Fe 3+ D = NO 3 - </li></ul><ul><li>AD = NaNO 3 </li></ul>
  23. 23. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na + B = OH - C = Fe 3+ D = NO 3 - </li></ul><ul><li>AD = NaNO 3 CB = Fe 3+ & OH - </li></ul>
  24. 24. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>A = Na + B = OH - C = Fe 3+ D = NO 3 - </li></ul><ul><li>AD = NaNO 3 CB = Fe(OH) 3 </li></ul>
  25. 25. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>AD = NaNO 3 CB = Fe(OH) 3 </li></ul><ul><li>Skeleton: Na(OH) (aq) + Fe(NO 3 ) 3 (aq) ---> Na(NO 3 ) (aq) + Fe(OH) 3 (s) </li></ul>
  26. 26. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>Skeleton: Na(OH) (aq) + Fe(NO 3 ) 3 (aq) ---> Na(NO 3 ) (aq) + Fe(OH) 3 (s) </li></ul><ul><li>Balanced: 3Na(OH) (aq) + Fe(NO 3 ) 3 (aq) ---> 3Na(NO 3 ) (aq) + Fe(OH) 3 (s) </li></ul>
  27. 27. Double Replacement Try It <ul><li>Write the balanced equation for Na(OH) (aq) + Fe(NO 3 ) 3 (aq). [Note: Iron (III) hydroxide is going to be a precipitate.] </li></ul><ul><li>Skeleton: Na(OH) (aq) + Fe(NO 3 ) 3 (aq) ---> Na(NO 3 ) (aq) + Fe(OH) 3 (s) </li></ul><ul><li>Balanced: 3Na(OH) (aq) + Fe(NO 3 ) 3 (aq) ---> 3Na(NO 3 ) (aq) + Fe(OH) 3 (s) </li></ul>
  28. 28. Double Replacement Try It 2 <ul><li>Write the balanced equation for: H 3 (PO 4 ) (aq) + K(OH) (aq). </li></ul>
  29. 29. Double Replacement Try It 2 <ul><li>Write the balanced equation for: H 3 (PO 4 ) (aq) + K(OH) (aq). </li></ul><ul><li>Skeleton: H 3 (PO 4 ) (aq) + K(OH) (aq) ---> H(OH) (l) + K 3 (PO 4 ) </li></ul>
  30. 30. Double Replacement Try It 2 <ul><li>Write the balanced equation for: H 3 (PO 4 ) (aq) + K(OH) (aq). </li></ul><ul><li>Skeleton: H 3 (PO 4 ) (aq) + K(OH) (aq) ---> H(OH) (l) + K 3 (PO 4 ) </li></ul><ul><li>Balanced: H 3 (PO 4 ) (aq) + 3K(OH) (aq) ---> 3H(OH) (l) + K 3 (PO 4 ) </li></ul>
  31. 31. Double Replacement Try It 2 <ul><li>Write the balanced equation for: H 3 (PO 4 ) (aq) + K(OH) (aq). </li></ul><ul><li>Skeleton: H 3 (PO 4 ) (aq) + K(OH) (aq) ---> H(OH) (l) + K 3 (PO 4 ) </li></ul><ul><li>Balanced: H 3 (PO 4 ) (aq) + 3K(OH) (aq) ---> 3H(OH) (l) + K 3 (PO 4 ) </li></ul>
  32. 32. Combustion Reactions <ul><li>Flame! Fire! Burning! </li></ul>
  33. 33. Combustion Reactions <ul><li>Flame! Fire! Burning! </li></ul><ul><li>Hydrocarbon + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul>
  34. 34. Combustion Reactions <ul><li>Flame! Fire! Burning! </li></ul><ul><li>Hydrocarbon + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul><ul><li>hydro carbon = compound that contains hydrogen </li></ul>
  35. 35. Combustion Reactions <ul><li>Flame! Fire! Burning! </li></ul><ul><li>Hydrocarbon + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul><ul><li>hydro carbon = compound that contains hydrogen </li></ul><ul><li>hydro carbon = compound that contains carbon </li></ul>
  36. 36. Combustion Reactions <ul><li>Flame! Fire! Burning! </li></ul><ul><li>Hydrocarbon + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul><ul><li>hydro carbon = compound that contains hydrogen </li></ul><ul><li>hydro carbon = compound that contains carbon </li></ul><ul><li>hydrocarbon = contains H and C </li></ul>
  37. 37. Combustion Reactions <ul><li>CH 4 (g) + 2 O 2 (g) ---> CO 2 (g) + 2 H 2 O (g) </li></ul><ul><li>IDENTITY BADGE : always produces CO 2 (g) + H 2 O (g) ONLY </li></ul>
  38. 38. Combustion Try It <ul><li>Write the balanced equation for the complete combustion of formic acid (HCOOH). </li></ul>
  39. 39. Combustion Try It <ul><li>Write the balanced equation for the complete combustion of formic acid (HCOOH). </li></ul><ul><li>Skeleton: hydrocarbon (aq) + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul>
  40. 40. Combustion Try It <ul><li>Write the balanced equation for the complete combustion of formic acid (HCOOH). </li></ul><ul><li>Skeleton: hydrocarbon (aq) + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul><ul><li>Skeleton: HCOOH (aq) + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul>
  41. 41. Combustion Try It <ul><li>Write the balanced equation for the complete combustion of formic acid (HCOOH). </li></ul><ul><li>Skeleton: HCOOH (aq) + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul><ul><li>Balanced: 2 HCOOH (aq) + O 2 (g) ---> 2 H 2 O (g) + 2 CO 2 (g) </li></ul>
  42. 42. Combustion Try It <ul><li>Write the balanced equation for the complete combustion of formic acid (HCOOH). </li></ul><ul><li>Skeleton: HCOOH (aq) + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul><ul><li>Balanced: 2 HCOOH (aq) + O 2 (g) ---> 2 H 2 O (g) + 2 CO 2 (g) </li></ul>
  43. 43. Combustion Try It 2 <ul><li>Write the balanced equation for the complete combustion of glucose (C 6 H 12 O 6 ). </li></ul>
  44. 44. Combustion Try It 2 <ul><li>Write the balanced equation for the complete combustion of glucose (C 6 H 12 O 6 ). </li></ul><ul><li>Skeleton: C 6 H 12 O 6 (s) + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul>
  45. 45. Combustion Try It 2 <ul><li>Write the balanced equation for the complete combustion of glucose (C 6 H 12 O 6 ). </li></ul><ul><li>Skeleton: C 6 H 12 O 6 (s) + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul><ul><li>Balanced: C 6 H 12 O 6 (s) + 6 O 2 (g) ---> 6 H 2 O (g) + 6 CO 2 (g) </li></ul>
  46. 46. Combustion Try It 2 <ul><li>Write the balanced equation for the complete combustion of glucose (C 6 H 12 O 6 ). </li></ul><ul><li>Skeleton: C 6 H 12 O 6 (s) + O 2 (g) ---> H 2 O (g) + CO 2 (g) </li></ul><ul><li>Balanced: C 6 H 12 O 6 (s) + 6 O 2 (g) ---> 6 H 2 O (g) + 6 CO 2 (g) </li></ul>

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