Module 5 - Section 2 [Factors on Equilibrium] Flashcards
State Le Chatelier’s Principle
Le Chatelier’s Principle (LCP) states when a change disturbs an equilibrium system, the equilibrium shifts to counteract the change
Recall conditions that affect the position of equilibrium
Equilibrium is affected by changes of:
- Concentration
- Volume/Pressure → Inversely proportional Boyle’s Law
- Temperature
Recall limitations (per se) of equilibrium
Limitations:
- Changes in concentration of solids or liquids have no effect on the equilibrium
- Changes in pressure only affect gaseous molecules
- Use of a catalyst does not shift the equilibrium as the rate of the forward and reverse reaction changes
- Addition of an inert gas does not shift the equilibrium as although the total pressure of the system changes, the partial pressures do not
Identify for what changes does the molar ratio have to be stated
Dilution and pressure/volume changes
Recall industrial considerations of the Industrial Manufacture of Ammonia – The Haber Process
Considerations:
- Temperature
- Pressure
- Kinetic factors
State the thermodynamic reaction for the Industrial Manufacture of Ammonia – The Haber Process
Nitrogen Gas + Hydrogen Gas → Ammonia Gas [-ΔH]
Account for the considerations in temperature of the Industrial Manufacture of Ammonia – The Haber Process
Temperature has to be in a “Goldilocks Zone”
Conflict between activation energy and exothermic nature of reaction
Account for the considerations in pressure of the Industrial Manufacture of Ammonia – The Haber Process
Pressure is high as economic and safety considerations allow
No conflict between rate of reaction and gaseous molar ratio
Account for the considerations in kinetic factors of the Industrial Manufacture of Ammonia – The Haber Process
Use of catalyst in a fine powder (surface area)
Constant removal of ammonia through liquefaction shifts equilibrium to the right
Using Le Chatelier’s Principle, account for the addition of aqueous reactant in an equilibrium system
Using Le Chatelier’s Principle, account for the addition of aqueous product in an equilibrium system
Using Le Chatelier’s Principle, account for changes in volume/pressure in an equilibrium system
Considering an exothermic reaction, using Le Chatelier’s Principle, account for changes in temperature in an equilibrium system
Considering an endothermic reaction, using Le Chatelier’s Principle, account for changes in temperature in an equilibrium system
Using collision theory, account for the addition of aqueous reactant in an equilibrium system
