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Unit 2: Equilibrium - Coggle Diagram
Unit 2: Equilibrium
Lesson 6 Energy and Equilibrium
Entropy(Δs)
A measure of the disorder of system
Law of Disorder
Systems tend to go from a state of low disorder to a state of maximum disorder spontaneously.
Entropy in the universe tends to increase.
Spontaneous reactions
Release free energy and are said to be exergonic.
Nonspontaneous reactions
Absorb free energy and are said to be endergonic.
Nonspontaneous reactions can be made spontaneous by increasing the temperature or linking it to a spontaneous reaction that produces a large amount of free energy
Free Energy(ΔG ) Calculations
ΔG = Δ H - Δ TΔS
Free Energy
ΔG° = -RT lnK
R is 8.313 J/K mol.
Lesson 2 Equilibrium Law
Equilibrium constants (Keq)
Indicate if the reverse reaction will favor reactants or products at equilibrium.
Keq = products concentration/reactants concentration
Keq > 1 products favoured
Keq < 1 reactants favoured
Keq = 1 the reaction is at equilibrium
Equilibrium Constant
The value of the equilibrium constant changes when the temperature changes.
Homogeneous equilibria: the reactants and products are in the same phase
Heterogeneous equilibria: the reactants and products are in a different phase.
Lesson 1 Dynamic Equilibrium in Closed Systems
Dynamic equilibrium
The balance between the forward and reverse process occurring at the same rate and no macroscopic change is observed.
Solubility equilibrium
Phase equilibrium
Chemical equilibrium
Catalyst Effect
No effect on the equilibrium.
Reversible Reactions
favour the reactants
favour the products
achieve notable equilibrium conditions
Calculating Equilibrium
A + B ↔ C
Initial concentration: a/V + b/V ↔ 0/V
Equilibrium concentration: (a-x)/V (b-x)/V ↔ 2x/V
Lesson 5 Quantitative Changes in the equilibrium systems
Reaction quotient
Q = [R]c [S]d/ [P]a[Q]b
Q = K then the system is at equilibrium.
Q < K the system will shift towards the product
Q > K the system will shift to the reactant
ICE table
500 law
If the smallest initial concentration is divided by the equilibrium concentration over 500, we can use 500 law.
Lesson 4 The Habor Process
Lesson 3 Qualitative Changes in Equilibrium Systems
Le Châtelier’s Principle
If a stress is applied to a system at equilibrium, the equilibrium will shift to relieve the stress.
Concentration Change
Increase [reactant] = shift right
Increase [product] = shift left
Decrease [reactant] = shifts left
Decrease [product] = shifts right
Temperature Change
Increase = favors the endothermic direction
Decreasing = favours the exothermic direction.
Pressure/Volume Change
Increasing pressure or decreasing volume favors fewer gas molecules.
Decreasing pressure or increasing volume favors more gas molecules.
Catalysts
No effect.
Jerry Zou
