when the concentrations of the reactants and products stop changing
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the rate of the forward reaction \= the rate of the reverse reaction
at equilibrium, what is equal?
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Keq \= [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ
Keq Formula
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(equilibrium concentrations)
equilibrium constant
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favors the reactants
a small Keq indicates the reaction
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favors the products
a large Keq indicates the reaction
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take the reciprocal
if you reverse a reaction, you \_______________ the Keq
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raise the Keq to the x power
if you multiply a balanced chem equation by a coefficient of x, you \__________________ the Keq
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multiply
if you add two reactions together, you \________________ the Keq
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Q \= [C]ᶜ[D]ᵈ / [A]ᵃ[B]ᵇ
Q Formula
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(initial concentrations)
reaction quotient
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favors the forward direction
if Q \> Keq, the reaction
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favors the reverse direction
if Q < Keq, the reaction
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has no direction affinity
if Q \= Keq, the reaction
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le chartelier's principle
states that if a system at equilibrium is disturbed by a change in temperature, pressure, or a component concentration, the system will shift its equilibrium position so as to counteract the effect of the disturbance
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the solubility product (Ksp)
the degree to which dissolution occurs
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Ksp \= [A⁺]ᵃ[B⁻]ᵇ
the solubility product
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low solubility
a small Ksp value indicates
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high solubility
a large Ksp value indicates
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molar solubility
molarity of a solute in a saturated solution (S)
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common ion
an ion that is common to two or more ionic compounds
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common ion effect
If one of the ions in a solution equilibrium is already dissolved in the solution, the equilibrium will shift to the left and the solubility of the salt will decrease
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exothermic reaction
ΔH < 0
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endothermic reaction
ΔH \> 0
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left
if you raise the temperature of a exothermic reaction, the reaction will shift to the
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right
if you lower the temperature of a exothermic reaction, the reaction will shift to the
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right
if you raise the temperature of a endothermic reaction, the reaction will shift to the
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left
if you lower the temperature of a endothermic reaction, the reaction will shift to the
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Equilibrium constant expression - Aqueous
Kc \= [products]/[reactants]
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Equilibrium constant expression - Pressure Only (g)
Kp \= [products]/[reactants]
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T/F - A
False
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T/F - A
True
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T/F - A
True
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1 atm \=
760 torr, 760 mmHg
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Solids and liquids are
not in the Equilibrium constant
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Forward reaction means:
Reactants to Products
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Reverse reaction means:
Products to Reactants
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Kc or Kp equation
Kc (or Kp) \= [products]/[reactants]
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Qc or Qp equation
Qc (or Qp) \= [products]/[reactants]
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Kc (or Kp) meaning
K gives the value of the reaction at Equilibrium
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Qc (or Qp) meaning
Q gives the value of the reaction at any given time
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Q compared to K
Q is compared to K to determine if the forward or reverse reaction are favored based on it being greater than, less than or equal to K
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Q \= K
Reaction is at equilibrium, neither the forward nor reverse reaction is favored
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Q \> K
Forward reaction (reactants to products) is favored / shifts to the left
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Q < K
Reverse reaction is favored (products to reactants) / shifts to the right
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Small K means
Because K = \[products\]/\[reactants\]
reactant number is bigger, because reactants are on the bottom and thus make a small number
Reactants are favored.
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Bigger K means
Because K = \[products\]/\[reactants\]
product number is bigger, because product are on the top and thus make a larger number
Products are favored
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Kp and Kc Units
No Units!
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Le Chatelier's Principle
If a stress is imposed on a system at equilibrium the position of the equilibrium will shift in a direction that reduces that stress
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LCP - Adding a product
shifts left (toward reactants)
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LCP - Adding a reactant
shifts right (toward products)
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LCP - Removing product
shifts right (toward products)
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LCP - Removing reactant
shifts left (toward reactants)
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LCP - Increasing volume
Shifts toward the side with more moles. This is similar to a decrease in pressure.
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LCP - Decrease volume
Shifts toward the side with fewer moles. This is similar to an increase in pressure.
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LCP - In an endothermic reaction, increasing temperature means...
Endo heat comes indoors, and is thus a reactant
so adding reactant, shifts right, the value of K increases because the concentration of the products increase and the concentration of the reactants decrease.
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LCP - In an endothermic reaction, decreasing temperature means...
Endo heat comes indoors, and is thus a reactant
so removing reactant, shifts left, value of K decreases because the concentration of the products decrease and the concentration of the reactants increase.
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LCP - In an exothermic reaction, increasing temperature means...
Exo heat exits and is thus a product so adding product, shifts left, value of K decreases because concentration of the products decrease and the concentration of reactants increase.
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LCP - In a exothermic reaction, decreasing temperature means...
Exo heat exits and is thus a product so removing product, shifts right, value of K increases because the concentration of the products increase and the concentration of the reactants decrease.
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LCP - Adding a catalyst...
Does NOT change the concentration
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LCP - Adding an inert gas
Does NOT change the concentration
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ΔH + then
Endothermic heat is a reactant
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ΔH - then
Exothermic heat is a product
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What happens to Kc in the reverse reaction?
The products become the reactants going backwards and the reactants are now products....
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Kc \= [reactants]/[products]
Kc equation
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Catalyst as it relates to Equilibrium
has no effect on the position of equilibrium but lowers activation energy, increasing the rate of forward and reverse reactions(gets to equilibrium faster)
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What happens to the value of K when flipping reactants and products?
becomes 1/K
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K of reverse reaction
1/K original
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Doubling K to equal an equation
original K squared
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Halving K to equal an equation
original K to 1/2 power (sqrt of K)
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Ksp
solubility product constant
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Ksp\=[A+]^m[B-]^n
Ksp equation
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molar solubility
the solubility of a compound in units of moles per liter
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Q
precipitate forms
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Q\>Ksp
no precipitate forms
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Two Factors Affect Solubility
pH and Common Ion Effect
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Heterogeneous Equilibrium
equilibrium involving reactants and/or products in more than one phase
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Homogeneous Equilibrium
a state of equilibrium that occurs when all the reactants and products of a reaction are in the same physical state
Studied by 3 people
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Flashcard (20)