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Chemistry > 40S Unit 3: Chemical Equilibrium I > Flashcards

40S Unit 3: Chemical Equilibrium I Flashcards

1
Q

what are the 2 types of equilibrium

A

dynamic and static

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2
Q

what is a static equilibrium

A

a motionless equilibrium involving the balance of stationary objects

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3
Q

what is a dynamic equilibrium

A

an equilibrium that involves the balance of opposing motions in which the rate of the forward reaction is equal to the rate of the reverse reaction

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4
Q

what are the 3 types of dynamic equilibriums

A

solubility, phase and chemical

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5
Q

what is a closed system

A

a system that may exchange energy but not matter with its surroundings

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6
Q

what do dynamic equilibriums always have

A

they always involve 2 opposing reaction rates that are equal in size yet opposite in flow

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7
Q

do the amounts of species on each side of a reaction have to be equal in dynamic equilibriums?

A

no, they do not need to be equal in concentration or amount

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8
Q

what is a solubility equilibrium and give an example

A

they involve solutions where the rate of dissolving and the rate of precipitation are equal.
e.g.:
NaCl(s) in equilibrium with Na+(aq) + Cl-(aq)

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9
Q

what is a phase equilibrium and give an example

A

equilibrium between opposing phase change rates where the chemical reactant and product are the same but the phase changes and can occur between any phases
e.g.:
H2O(l) in equilibrium with H2O(g)

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10
Q

what is a chemical equilibrium and give an example

A

equilibrium between the forward rate of reaction and the reverse rate of reaction
e.g.:
2H2(g) + O2(g) in equilibrium with 2H2O(g)

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11
Q

when does equilibrium occur on a graph

A

whenever the concentration of reactants and products plateau

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12
Q

what is percent reaction and what is the formula

A

an indication of how completely the reactants have formed products

% reaction = (actual yield / theoretical max yield) x 100%

the theoretical max yield is the yield provided by the stoichiometry

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13
Q

if a reaction is 99% complete, what is it called

A

a quantitative reaction (considered to be a one way reaction)

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14
Q

what are the 4 ways we can express equilibrium

A
  1. graphs/pictures
  2. words
  3. numbers
  4. ICE chart
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15
Q

what does ICE stand for

A

I - initial concentration
C - change in concentration
E - equilibrium concentration

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16
Q

what is the formula for moles (n), concentration (C) and volume (V)

A

n = C x V

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17
Q

if a reaction is a quantitative reaction, what is its % reaction

A

99%

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18
Q

if a reaction is product favoured, what is its % reaction

A

50% < x < 99%

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19
Q

if a reaction is neither favored, what is its % reaction

A

50%

20
Q

if a reaction is reactant favoured, what is it’s % reaction

A

1% < x < 50%

21
Q

if there is no reaction, what is it’s % reaction

A

1% or less

22
Q

if there is ________________________________________ we have an equilibrium

A

more than 1% reverse reaction

23
Q

if one reactant changes _________, all other reactants must change negatively but all products change ________

A

negatively, positively

24
Q

state if this is product favoured, reactant favoured or neither

reactants changes negatively and products change positively

A

product favoured

25
Q

state if this is product favoured, reactant favoured or neither

no changes

A

neither favoured

26
Q

state if this is product favoured, reactant favoured or neither

reactants change positively and products change negatively

A

mostly reactant favoured

27
Q

who determined the formula for the equilibrium constant

A

Guldberg and Waage in the 1800s
they realized that no matter how a reaction starts and ends, something stays the same

28
Q

given the reaction
aA + bB in equilibrium with cC + dD
what is the equilibrium constant equation

A

k = [D]^d • [C]^c / [A]^a • [B]^b

k is measured in M

only using equilibrium concentrations not initial

29
Q

what is the difference between the rate law and the equilibrium constant

A

the rate law doesnt use coefficients as the exponents, it uses the reaction rate, but the equilibrium constant uses the coefficients

30
Q

how do you differentiate between the equilibrium constant for the regular reaction and the reverse reaction

A

regular —> k = products / reactants
reverse —> k’ = reactants/ products

31
Q

when is the equilibrium constant true

A

when the temperature and pressure are constant as k stays constant regardless of initial concentration

32
Q

what is a limitation of k

A

changing anything other than concentration as it will result in a different k

33
Q

when does concentration change, when i add more solid, liquid or gas

A

when i add more gas and/or aqueous solutions

34
Q

when does concentration change, when i add more solid, liquid or gas

A

when i add more gas and/or aqueous solutions

35
Q

what appears on ICE charts, solids, liquids, gases or aqueous solutions

A

gases and aqueous only

36
Q

determine which is product favoured, which is neither and which is reactant favored

k < 1, k > 1, k = 1

A

k < 1 is reactant favoured
k > 1 is product favored
k = 1 is neither favored

37
Q

what is Le Chatelier’s principle

A

when a chemical system in equilibrium is disturbed by a change in a property, the system responds to oppose that change

38
Q

as the system changes to oppose the disturbance, ________ species in the equilibrium changes

A

every

39
Q

what are 3 ways to disturb a system

A
  • change concentration
  • change temperature
  • change pressure
40
Q

if a reaction is exothermic, what side is heat added to the reaction

A

the products side because heat is released

41
Q

in an exothermic reaction, is H negative or positive

A

negative

42
Q

where is heat added in an endothermic reaction

A

to the reactants side

43
Q

in an endothermic reaction, is H negative or positive

A

positive

44
Q

the amount of concentration changes depending on the __________________

A

stoichiometry

45
Q

what type of equilibriums do pressure disturbances affect

A

equilibrium systems containing at least one species that is a gas

46
Q

if we increase the pressure on an equilibrium, how will the system respond

A

the system will respond to decrease the pressure by flowing to the side with less moles of gas

47
Q

if we decrease the pressure on an equilibrium, how will the system respond

A

the system will respond to increase the pressure by flowing to the side with more moles of gas

Chemistry (8 decks)

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