AP Chemistry: Equilibrium

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55 Terms

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chemical equilibrium (dynamic equilibrium)
two exactly opposite reactions are occuring simultaneously with the same rates of reaction
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equilibrium constant (Kc, Kp)
the reaction quotient at equilibrium
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reactant quotient (Q)
fraction relating the products ad reactants
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at equilibrium are the concentrations of the chemical species equal
not necessiraly, they are constant
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what states of matter are not included in an equilibrium equation
liquids and solids
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if the K value is large
there are more products than reactants; reaction lies to the right
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if the K value is small
there are more products than reactants; reaction lies to the left
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Le Châtelier’s principle
if a chemical system at equilibrium is stressed, it will reestablish equilibrium by shifting the reactions involved
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what are examples of stressors on equilibrium
changes in concentration, pressure, and temperature
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are changes in pressure significant in all equilibrium reactions
no, only if gases are involved
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if the volume a container decreases, how will the equilibrium system shift?
to the side with less moles of gas
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if the volume a container increases, how will the equilibrium system shift?
to the side with more moles of gas
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what factor changes the value of the equilibrium constant
temperature
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heterogeneous equilibria
equilibria that involve more than one phase
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homogeneous equilibria
* systems in the gas phase, where all reactants and products are gases

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what shift occurs when Q=K
no shift
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what shift occurs when Q>K
shift right to left
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what shift occurs when Q
shift left to righ
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saturated solutions are at
equilibrium
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shift right meaning
there are not enough products, so the system will shift to consume reactants and produce more products
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shift left meaning
there are not enough reactants, so the system will shift to consume products and produce more reactants
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what type of solution is at equilibrium
a saturated solution
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if K >1, what side of the reaction is favored
products (forward reaction) is favored
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if K is very large, describe the reaction
reaction goes essentially to completion
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if K
reactants (reverse reaction) are favored at equilibrium
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if K is very small, describe the reaction
reaction barely proceeds at all
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relate the K of the reverse reaction to that of the forward reaction
it is the reciprocal
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when the equation of reaction is multipled by *n,* what happens to K
K is put to the nth power
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when elementary steps are added together, the K of the overall reaction is
the product of the K’s of the elementary steps
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if the pressure is increased, how will the equilibrium system shift?
to the side with less gas moles
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if the pressure is decreased, how will the equilibrium system shift?
to the side with more gas moles
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if an inert gas is added, how will the equilibrium system shift?
no effect
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if heat is added to an endothermic reaction, how does K change?
K increases (K>1)
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if heat is added to an endothermic reaction, how does the equilibrium system shift?
to the right (forward direction)
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if heat is added to an exothermic reaction, how does K change?
K decreases (K
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if heat is added to an exothermic reaction, how does the equilibrium system shift?
shift to the left (reverse direction)
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when concentration changed, the system will always shift away from
the added component
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diluting always shifts towards which type of species
aqueous species
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concentrating always shifts towards which type of species
less aqueous species
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if the amount of a liquid or solid is changed in a system, how does the system react?
no change
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how does adding a catalyst affect the equilibrium system?
no change
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Ksp
solubility product constant
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how does having more anions and cations affect the Ksp value?
the Ksp value is increased
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solubility (s)
concentration of solid that dissolves
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how does solubility affect the value of the equilbrium constant?
it has no effect, the attainment of equilibrium can be affected however
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the Ksp of two salts can only be compared with
salts that fall into the same number of ions
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a bigger Ksp value means
more soluble
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when tow salts have a different number of ions, how can their solubilities be compared
by solving for solubility
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what happens when Q is greater than the Ksp
precipitation
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when happens when Q is less than the Ksp
no precipitate
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common-ion effect
when a solid is dissolved in a solution with either the cation or anion already present, less solid will dissolve
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how does the common-ion effect affect the Ksp?
no change
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how does increasing pH affect the solubility of a salt?
decreases the solubility
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how does decreasing pH affect the solubility of a salt?
increases the solubility
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adding a substance that is not in the equilibrium equaiton increases the change of
a reaction with the substance