1 / 16

Industrial Applications of Equilibrium Principles Lesson 4

Industrial Applications of Equilibrium Principles Lesson 4. The Yield of a Reaction. products. reactants. reactants. products. The yield is the amount of products. Low yield. High yield. ⇌. ⇌. The Haber Process is used to make ammonia. 4 2.

gustav
Download Presentation

Industrial Applications of Equilibrium Principles Lesson 4

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. Industrial Applications of Equilibrium Principles Lesson 4

  2. The Yield of a Reaction products reactants reactants products The yield is the amount of products. Lowyield High yield ⇌ ⇌

  3. TheHaber Processis used to make ammonia 42 N2(g) + 3H2(g)⇌ 2NH3(g) +energy To ensure a high yield- Think: what will drive the rxn to products side? low temperature high pressure remove NH3 add N2 and H2

  4. TheHaber Processis used to make ammonia 42 N2(g) + 3H2(g)⇌ 2NH3(g) +energy To ensure a high rate high temperature- 600 0C high pressure- 20000 Kpa add N2 and H2 add catalysts

  5. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Increasing the yield low temperature low pressure remove NO2 add N2O4

  6. 1 2 N2O4(g)⇋ 2NO2(g)+ 59 KJ Increasing the rate high temperature high pressure add N2O4 add a catalyst

  7. Know the difference betweenRateandYield! Rate is how fast you get to equilibrium. Yield is the amount of productrelative toreactants at equilibrium.

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

  9. 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 D. high Zn surface area, high [HCl], low temperature C. high Zn surface area, high [HCl], high temperature

  10. 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

  11. Graphing Equilibrium Graphing changes imposed on the system

  12. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 1. Adding [N2O4] [N2O4] [NO2] x 2x

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

  14. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ 3. Increase Temperature [N2O4] [NO2] x 2x

  15. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ [NO2] [N2O4] 4. Decrease Volume- all concentrations + pressure goes up! 2x x

  16. Page 55 Questions 27 + 28

More Related