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Reaction Yield Lesson 6

Reaction Yield Lesson 6. 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. N 2(g) + 3H 2(g) ⇌ 2NH 3(g) + energy.

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Reaction Yield Lesson 6

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  1. Reaction Yield Lesson 6

  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 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 Os and Ur

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

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

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

  14. Graphing Equilibrium N2O4(g)⇋ 2NO2(g) + 59 KJ [NO2] [N2O4] 3. Decrease Volume- all concentrations + pressure goes up! 2x x

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