Equilibrium
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what is equilibrium
Equilibrium can be defined as a state reached of a reversible reaction, in which the rate of the forward and backward reactions equal.
examples of equilibrium
• water cycle - closed water bottle
features of the equilibrium state
• dynamic (ever changing, f and r reaction occurring at equal rate) • closed system (no change of matter with the surroundings) • concentration of products and reacts constant at equilibrium • no macroscopic change in properties (no visible change at blind eye) • can be reached from either direction
what is the equilibrium constant expression
Kc= [C]^c[D]^d/[A]^a[B]^b or products/reactants
what does Kc indicate
the extent of the reaction under the conditions used - it has no units
High Kc
a lot of products
low Kc
small amount of reactants converted to products
kc= 1
reaction at equilibrium
kc
reaction hardly goes
kc> 10^10
reaction complete
kc= 0.01
reactants predominate
kc= 100
products predominate
whats it the reaction quotients
Q= the Kc calculations when you don have concentration values/reaction isn’t at equilibrium
what is Le Chatelier principle
• when a system at equilibrium is disturbed, the equilibrium position will shift in the direction which tends to minimize, or counteract, the effect of the disturbance LIKE DIFFUSION
how do catalysts affect equilibrium position
• they don’t. But it does affect the speed at which the reaction reaches equillibiurm