reaction yield lesson 6
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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. - PowerPoint PPT PresentationTRANSCRIPT
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 reactants products
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
The Haber Process is used to make ammonia.
N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a high yield
The Haber Process is used to make ammonia.
N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a high yield
low temperature
The Haber Process is used to make ammonia.
4 2N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a high yield
low temperature
The Haber Process is used to make ammonia.
4 2N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a high yield
low temperaturehigh pressure
The Haber Process is used to make ammonia.
4 2N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a high yield
low temperaturehigh pressureremove NH3
The Haber Process is used to make ammonia.
4 2N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a high yield
low temperaturehigh pressureremove NH3
add N2 and H2
The Haber Process is used to make ammonia.
N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a reasonable rate
The Haber Process is used to make ammonia.
N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a reasonable rate
high temperature
The Haber Process is used to make ammonia.
N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a reasonable rate
high temperaturecatalysts Os & Ur
The Haber Process is used to make ammonia.
N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a reasonable rate
high temperaturecatalysts Os & Uradd N2 & H2
The Haber Process is used to make ammonia.
N2(g) + 3H2(g) ⇌ 2NH3(g) + energy
To ensure a reasonable rate
high temperature- 500 oCcatalysts Os & Uradd N2 & H2
high pressure
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the yield.
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the yield.
low temperature
1 2
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the yield.
low temperature
1 2
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the yield.
low temperaturelow pressure
1 2
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the yield.
low temperaturelow pressureadd N2O4
remove NO2
1 2
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the rate.
1 2
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the rate.
high temperature
1 2
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the rate.
high temperatureadd a catalyst
1 2
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the rate.
high temperatureadd a catalysthigh pressure
1 2
N2O4(g) ⇋ 2NO2(g) + 59 KJ
Describe four ways of increasing the rate.
high temperatureadd a catalysthigh pressureadd N2O4
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.
reactants products
1. What conditions will produce the greatest yield?
P2O4(g) ⇋ 2PO2(g) ∆H = -28 kJ
A. high temperature & high pressureB. low temperature & low pressureC. high temperature & low pressureD. low temperature & high pressure
1. What conditions will produce the greatest yield?
P2O4(g) ⇋ 2PO2(g) + 28kJ
A. high temperature & high pressureB. low temperature & low pressureC. high temperature & low pressureD. low temperature & high pressure
1. What conditions will produce the greatest yield?
P2O4(g) ⇋ 2PO2(g) + 28kJ
A. high temperature & high pressureB. low temperature & low pressureC. high temperature & low pressureD. low temperature & high pressure
2. What conditions will produce the greatest rate?
Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)
A. high Zn surface area, low [HCl], low temperatureB. low Zn surface area, high [HCl], high temperatureC. high Zn surface area, high [HCl], high temperatureD. high Zn surface area, high [HCl], low temperature
2. What conditions will produce the greatest rate?
Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)
A. high Zn surface area, low [HCl], low temperatureB. low Zn surface area, high [HCl], high temperatureC. high Zn surface area, high [HCl], high temperatureD. high Zn surface area, high [HCl], low temperature
3. What increases the rate?
Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)
A. removing H2
B. removing ZnCl2(aq)
C. lowering pressureD. adding HCl
3. What increases the rate?
Zn(s) + 2HCl(aq) → H2(g) + ZnCl2(aq)
A. removing H2
B. removing ZnCl2(aq)
C. lowering pressureD. adding HCl
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
1. Increase Temperature
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
1. Increase Temperature
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
1. Increase Temperature
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
1. Increase Temperature
[N2O4]
[NO2]
2x
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
1. Increase Temperature
[N2O4]
[NO2]
2x
x
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
2. Decrease Volume
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
2. Decrease Volume- all concentrations go up!
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
2. Decrease Volume- all concentrations + pressure goes up!
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
2. Decrease Volume- all concentrations + pressure goes up!
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
2. Decrease Volume- all concentrations + pressure goes up!
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
2. Decrease Volume- all concentrations + pressure goes up!
[N2O4]
[NO2] 2x
x
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
3. Adding N2O4
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
3. Adding N2O4
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
3. Adding N2O4
[N2O4]
[NO2]
x
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
3. Adding N2O4
[N2O4]
[NO2]2x
x
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
4. Removing NO2
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
4. Removing NO2
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
4. Removing NO2
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
4. Removing NO2
[N2O4]
[NO2]
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
4. Removing NO2
[N2O4]
[NO2]
2x
Graphing Equilibrium N2O4(g) ⇋ 2NO2(g) + 59 KJ
4. Removing NO2
[N2O4]
[NO2]
2x
x