Adv. Chem Unit 7 - Entropy/Equilibrium

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reversible reactions

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81 Terms

1

reversible reactions

reactions that can take place in both directions

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equilibrium

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 <==> B Once equilibrium is established \[A\] = \[B\]

False

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T/F - A <==> B Once Eq is established k forward = k reverse

True

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T/F - A <==> B Once Eq is established the values of \[A\] & \[B\] are no longer changing

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<Ksp

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

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Phases used in Kc

aq and gas

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Phases used in Kp

gas

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