1. Reaction Yield
Lesson 6

3. reactants products ⇌ ⇌ The Yield of a Reaction
The yield is the amount of products.
Low yield
High yield
reactants
products ⇌
reactants
products ⇌

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

5. The Haber Process is used to make ammonia
N2(g) H2(g) ⇌ 2NH3(g) energy
To ensure a high rate
high temperature C
high pressure Kpa
add N2 and H2
add catalysts Os and Ur

6. 1 2
N2O4(g) ⇋ NO2(g) KJ
Increasing the yield
low temperature
low pressure
remove NO2
add N2O4

7. 1 2
N2O4(g) ⇋ NO2(g) KJ
Increasing the rate
high temperature
high pressure
add N2O4
add a catalyst

8. 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.

9. 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 KJ
B. low temperature & low pressure

10. 2. What conditions will produce the greatest rate?
Zn(s) HCl(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

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

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

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

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

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