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Reaction Yield Lesson 6

Reaction Yield Lesson 6. Increasing the Yield of a Reaction The yield is the amount of products . The greater the yield the more products there are at equilibrium Chemists use LeChatelier’s Principle to maximize the equilibrium yield for a reaction. High Yield. products.

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Reaction Yield Lesson 6

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  1. Reaction Yield Lesson 6

  2. Increasing the Yield of a Reaction The yield is the amount of products. The greater the yield the more products there are at equilibrium Chemists use LeChatelier’s Principle to maximize the equilibrium yield for a reaction. High Yield products reactants

  3. Increasing the Yield of a Reaction The yield is the amount of products. The greater the yield the more products there are at equilibrium Chemists use LeChatelier’s Principle to maximize the equilibrium yield for a reaction. Low Yield reactants products

  4. The Haber Process is used to make ammonia. N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a high yield

  5. The Haber Process is used to make ammonia. N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a high yield low temperature

  6. The Haber Process is used to make ammonia. 4 2 N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a high yield low temperature

  7. The Haber Process is used to make ammonia. 4 2 N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a high yield low temperature high pressure

  8. The Haber Process is used to make ammonia. 4 2 N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a high yield low temperature high pressure remove NH3

  9. The Haber Process is used to make ammonia. 4 2 N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a high yield low temperature high pressure remove NH3 add N2 and H2

  10. The Haber Process is used to make ammonia. N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a reasonable rate

  11. The Haber Process is used to make ammonia. N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a reasonable rate high temperature

  12. The Haber Process is used to make ammonia. N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a reasonable rate high temperature catalysts Os & Ur

  13. The Haber Process is used to make ammonia. N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a reasonable rate high temperature catalysts Os & Ur add N2 & H2

  14. The Haber Process is used to make ammonia. N2(g) + 3H2(g)⇌ 2NH3(g) + energy To ensure a reasonable rate high temperature- 500 oC catalysts Os & Ur add N2 & H2 high pressure

  15. N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the yield.

  16. N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the yield. low temperature

  17. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the yield. low temperature

  18. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the yield. low temperature low pressure

  19. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the yield. low temperature low pressure add N2O4 remove NO2

  20. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the rate.

  21. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the rate. high temperature

  22. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the rate. high temperature add a catalyst

  23. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the rate. high temperature add a catalyst high pressure

  24. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Describe four ways of increasing the rate. high temperature add a catalyst high pressure add N2O4

  25. Know the difference between Rate and Yield! Rate is how fast you get to equilibrium. Yield is the amount of product relative to reactants at equilibrium. products reactants

  26. 1. What conditions will produce the greatest yield? P2O4(g)⇋ 2PO2(g) ∆H = -28 kJ A. high temperature & high pressure B. low temperature & low pressure C. high temperature & low pressure D. low temperature & high pressure

  27. 1. What conditions will produce the greatest yield? P2O4(g)⇋ 2PO2(g) + 28kJ A. high temperature & high pressure B. low temperature & low pressure C. high temperature & low pressure D. low temperature & high pressure

  28. 1. What conditions will produce the greatest yield? P2O4(g)⇋ 2PO2(g) + 28kJ A. high temperature & high pressure B. low temperature & low pressure C. high temperature & low pressure D. low temperature & high pressure

  29. 2. What conditions will produce the greatest rate? Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq) A. high Zn surface area, low [HCl], low temperature B. low Zn surface area, high [HCl], high temperature C. high Zn surface area, high [HCl], high temperature D. high Zn surface area, high [HCl], low temperature

  30. 2. What conditions will produce the greatest rate? Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq) A. high Zn surface area, low [HCl], low temperature B. low Zn surface area, high [HCl], high temperature C. high Zn surface area, high [HCl], high temperature D. high Zn surface area, high [HCl], low temperature

  31. 3. What increases the rate? Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq) A. removing H2 B. removing ZnCl2(aq) C. lowering pressure D. adding HCl

  32. 3. What increases the rate? Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq) A. removing H2 B. removing ZnCl2(aq) C. lowering pressure D. adding HCl

  33. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 1. Increase Temperature [N2O4] [NO2]

  34. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 1. Increase Temperature [N2O4] [NO2]

  35. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 1. Increase Temperature [N2O4] [NO2]

  36. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 1. Increase Temperature [N2O4] [NO2] 2x

  37. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 1. Increase Temperature [N2O4] [NO2] x 2x

  38. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 2. Decrease Volume [N2O4] [NO2]

  39. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 2. Decrease Volume- all concentrations go up! [N2O4] [NO2]

  40. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 2. Decrease Volume- all concentrations + pressure goes up! [N2O4] [NO2]

  41. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 2. Decrease Volume- all concentrations + pressure goes up! [N2O4] [NO2]

  42. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 2. Decrease Volume- all concentrations + pressure goes up! [N2O4] [NO2]

  43. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 2. Decrease Volume- all concentrations + pressure goes up! [N2O4] [NO2] x 2x

  44. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 3. Adding N2O4 [N2O4] [NO2]

  45. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 3. Adding N2O4 [N2O4] [NO2]

  46. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 3. Adding N2O4 [N2O4] [NO2] x

  47. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 3. Adding N2O4 [N2O4] [NO2] x 2x

  48. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 4. Removing NO2 [N2O4] [NO2]

  49. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 4. Removing NO2 [N2O4] [NO2]

  50. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 4. Removing NO2 [N2O4] [NO2]

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