Equilibrium Flashcards
physical equilibrium
the equilibrium of a substance from one phase to another
chemical equilibrium
bond equilibrium = the equilibrium of 2 substances ( products and reagents)
equilibrium
the state of a reaction system where the forward reaction rate = the reverse reaction rate
is there a change in concentration in equilibrium
there is no net change
dynamic equilibrium
at chemical equilibrium with constant, opposing reactions occurring at the microscopic level while maintaining macroscopic qualitative properties
what is required for a dynamic equilibrium
closed system and constant temperature
what is K
= the equilibrium constant = the ratio of equilbrium concentrations for a chemical system at a certain temperature
what are factors affecting equilibrium
- concentration of reactants -> determines frequency of collisions ([low]-> few collisions, [high] ->many collisions)
- temperature -> determines energy of reaction
what is homogenous equilibrium
all components of the reaction are the same physical state
what is heterogenous equilibrium
physical states of components differ -> use activity for k
k = 1
[products] = [reactants]
very large K (>10^10)
Reaction has a strong tendency to go to completion with mixture containing almost only products at equilibrium
mixture has mostly only products at equilibrium
equilibrium lies far towards products
very small K
no tendency to occur, with high concentration of reactants at equilibrium -> lies towards reactants
K at equilibrium
remains constant, same with amounts of reactants and products
le chatelier’s principle
if an equilibrium is disrupted, the system shifts in response to re-establish equilibrium
increasing reactant concentration
shifts reaction towards products
increasing product concentration
shifts reaction towards reactants
decreasing volume/increasing pressure
shifts to direction that produces fewer moles of gas
increasing v/decreasing p
shifts to direction that produces more moles of gas
increasing temperature
shifts reaction towards direction of endothermic reactions
decreasing temperature
shifts reaction towards exothermic reaction
Q<K
reaction shifts to the right towards the product as reaction is using more reactants
Q>K
reaction shifts to left towards reactants as reaction is using more products
adding a catalyst
does not change equilibrium
adding an inert gas at constant volume
increases pressure -> shifts to side with fewer moles of gas
