le chatelier's principle and equilibrium
DESCRIPTION
By: Shelby Toler. Le Chatelier's Principle and Equilibrium. 2 SO 3 (g) ↔ 2 SO 2 (g) + O 2 (g) ΔH° = 197.78 kJ. Increasing the temperature of the reaction. Right. 2 SO 3 (g) ↔ 2 SO 2 (g) + O 2 (g) ΔH° = 197.78 kJ. Increasing the pressure on the reaction. Left. - PowerPoint PPT PresentationTRANSCRIPT
![Page 1: Le Chatelier's Principle and Equilibrium](https://reader033.vdocuments.us/reader033/viewer/2022061614/5681300b550346895d957d22/html5/thumbnails/1.jpg)
Le Chatelier's Principle and Equilibrium
By: Shelby Toler
![Page 2: Le Chatelier's Principle and Equilibrium](https://reader033.vdocuments.us/reader033/viewer/2022061614/5681300b550346895d957d22/html5/thumbnails/2.jpg)
2 SO3(g) ↔ 2 SO
2 (g) + O
2 (g)
ΔH° = 197.78 kJ
Increasing the temperature of the reaction.
Right
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2 SO3(g) ↔ 2 SO
2 (g) + O
2 (g)
ΔH° = 197.78 kJ
Increasing the pressure on the reaction.
Left
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2 SO3(g) ↔ 2 SO
2 (g) + O
2 (g)
ΔH° = 197.78 kJAdding more O2 when the reaction is at
equilibrium
Left
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2 SO3(g) ↔ 2 SO
2 (g) + O
2 (g)
ΔH° = 197.78 kJRemoving O2 from the system when
the reaction is at equilibrium
Right
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N2O
4(g) ↔ 2NO
2
ΔH° = 58.0 kJ
Adding more NO2 when the reaction is at equilibrium.
Left
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N2O
4(g) ↔ 2NO
2
ΔH° = 58.0 kJ
Increasing the pressure
Left
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N2O
4(g) ↔ 2NO
2
ΔH° = 58.0 kJ
Increase the volume
Right
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N2O
4(g) ↔ 2NO
2
ΔH° = 58.0 kJ
Increasing the temperature.
Right
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3H2(g) + N
2(g) ↔ 2NH
3(g)
ΔH° = -92.38 kJIncreasing the temperature of the reaction.
Left
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3H2(g) + N
2(g) ↔ 2NH
3(g)
ΔH° = -92.38 kJAdding more N2 when the reaction is at
equilibrium
Right
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3H2(g) + N
2(g) ↔ 2NH
3(g)
ΔH° = -92.38 kJRemoving H2 when the reaction is at
equilibrium.
Left
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3H2(g) + N
2(g) ↔ 2NH
3(g)
ΔH° = -92.38 kJIncreasing the pressure
Right
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3H2(g) + N
2(g) ↔ 2NH
3(g)
ΔH° = -92.38 kJ Increasing the volume.
Left
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2CO (g) + O2 (g) ↔ 2CO
2 (g)
Increasing the pressure on the reaction.
Right
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2CO (g) + O2 (g) ↔ 2CO
2 (g)
Adding more O2 when the reaction is at equilibrium
Right
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2CO (g) + O2 (g) ↔ 2CO
2 (g)
Adding another reactant to the reaction
Right
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2CO (g) + O2 (g) ↔ 2CO
2 (g)
Increasing the volume.
Left
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N2 (g) + O
2 (g) ↔ 2NO (g)
Increasing the pressure on the reaction
No Shift
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N2 (g) + O
2 (g) ↔ 2NO (g)
Adding more O2 when the reaction is at equilibrium
Right
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N2 (g) + O
2 (g) ↔ 2NO (g)
Adding another reactant to the reaction
Right
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N2 (g) + O
2 (g) ↔ 2NO (g)
Increasing the Volume
No Shift
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PCl3(g) + Cl
2(g) <----> PCl
5(g)
What could you do to increase Pcl5?
Increase the pressureDecrease the volume
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PCl3(g) + Cl
2(g) <----> PCl
5(g)
What could you do to increase Cl2?
Decrease the pressureIncrease the volume
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N2 (g) + 3H
2 (g) <---> 2NH
3 (g)
What could you do to increase NH3?
Increase the pressureDecrease the volume
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N2 (g) + 3H
2 (g) <---> 2NH
3 (g)
What could you do to decrease N2?
Increase the pressureDecrease the volume