“Equilibrium” What does it mean? What word does it look like? What does it mean? What word does it look like?
Aim: How can we look at systems at equilibrium? Equilibrium: a state of balance Dynamic Equilibrium: when overall rates of forward and reverse reactions are equal This is a Reversible Equilibrium and is indicated by a double arrow Equilibrium: a state of balance Dynamic Equilibrium: when overall rates of forward and reverse reactions are equal This is a Reversible Equilibrium and is indicated by a double arrow
Physical Equilibrium Physical Equilibrium is balance in physical processes Phase equilibrium: equilibrium between phases Physical Equilibrium is balance in physical processes Phase equilibrium: equilibrium between phases
Solution Equilibrium Solution Equilibrium: dissolving & crystallization happening at equal rate liquid-gas liquid-solid
Chemical Equilibrium CH 4 (g) + H 2 O (g) 3 H 2 (g) + CO (g)
Chemical Equilibrium CH 4 (g) + H 2 O (g) 3 H 2 (g) + CO (g)
Homework Finish equilibrium review pages
Remember: Equilibrium is Stability CH 4 + H 2 O 3 H 2 + CO Fwd rxn rate = Rev Rxn rate Using up reactants to make products CH 4 + H 2 O 3 H 2 + CO Fwd rxn rate = Rev Rxn rate Using up reactants to make products
How will a closed system react when a stress if applied? equilibrium stress new equilibrium
Le Chatelier’s Principle Closed systems will adjust to balance stresses Concentration, temperature, pressure Shifts are increased reaction rates in either Fwd (right→) or Rev (left←) directions Closed systems will adjust to balance stresses Concentration, temperature, pressure Shifts are increased reaction rates in either Fwd (right→) or Rev (left←) directions
Concentration Pen/pencil trick, pointing towards shift A + B C Add-Away, Take-Towards Pen/pencil trick, pointing towards shift A + B C Add-Away, Take-Towards
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Concentration Add-Away
Concentration Take-Towards
Le Chatelier’s Principle: Temperature Treat “heat/energy” like any other reactant Adding heat favors reaction Removing heat favors reaction Treat “heat/energy” like any other reactant Adding heat favors reaction Removing heat favors reaction
N H 2 2 NH kJ
12.6 kJ + H 2 + I 2 2 HI
Do Now: Answer the following questions 1. What is Le Chatelier’s Principle? 2. Label the forward and reverse reactions as endothermic or exothermic: CO (g) + 3 H 2 CH 4 (g) + H 2 O (g) + heat 3. In which direction will equilibrium shift if the temperature is increased? 4. In which direction will equilibrium shift if the temperature is decreased? 1. What is Le Chatelier’s Principle? 2. Label the forward and reverse reactions as endothermic or exothermic: CO (g) + 3 H 2 CH 4 (g) + H 2 O (g) + heat 3. In which direction will equilibrium shift if the temperature is increased? 4. In which direction will equilibrium shift if the temperature is decreased?
Pressure Only for gases; count # of molecules on each side If # is equal, pressure has no effect pressure shifts towards fewer molecules pressure shifts towards more molecules Only for gases; count # of molecules on each side If # is equal, pressure has no effect pressure shifts towards fewer molecules pressure shifts towards more molecules
Pressure Example 4 NH (g) + 5 O 2 (g) 4 NO (g) + 6 H 2 O (g) = gas molecules = gas molecules Increase pressure: shift (more to less) 9 10 Decrease pressure: shift (less to more) 9 10 4 NH (g) + 5 O 2 (g) 4 NO (g) + 6 H 2 O (g) = gas molecules = gas molecules Increase pressure: shift (more to less) 9 10 Decrease pressure: shift (less to more) 9 10
N H 2 2 NH 3 Equilibrium shift [N 2 ] [H 2 ] [NH 3 ] # molecules: Increased pressure shifts towards fewer molecules Decreased pressure shifts towards more molecules
H 2 + I 2 2 HI Equilibrium shift [H 2 ] [I 2 ] [HI] # molecules: Increased pressure shifts towards fewer molecules Decreased pressure shifts towards more molecules
Conclusion Questions 1. How does a system at equilibrium respond to a stress? List the factors that can be stresses on an equilibrium system.
Conclusion Questions 2. Given the reaction at equilibrium: N 2 (g) + 3 H 2 (g) 2 NH 2 (g) + heat Which stress would cause the equilibrium to shift to the left? (a) Increasing the temperature (b) Adding N 2 (g) to the system (c) Adding H 2 (g) to the system 2. Given the reaction at equilibrium: N 2 (g) + 3 H 2 (g) 2 NH 2 (g) + heat Which stress would cause the equilibrium to shift to the left? (a) Increasing the temperature (b) Adding N 2 (g) to the system (c) Adding H 2 (g) to the system
Conclusion Questions 2. Given the reaction at equilibrium: N 2 (g) + O 2 (g) 2 NO (g) If the concentration of N 2 (g) is increased, the concentration of O 2 (g) will (a) Decrease (b) Remain the same (c) Increase 2. Given the reaction at equilibrium: N 2 (g) + O 2 (g) 2 NO (g) If the concentration of N 2 (g) is increased, the concentration of O 2 (g) will (a) Decrease (b) Remain the same (c) Increase