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AP Chemistry > Chapter 13 > Flashcards

Chapter 13 Flashcards

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1
Q

static equilibrium does not occur in?

A

chemical systems

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2
Q

chemical equilibrium

A

usually studied in a closed system with controlled variables.

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3
Q

Equilibrium

A

the state where the concentrations of reactants and products remain constant over a period of time

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4
Q

all reactions that are carried out in a closed system will?

A

reach equilibrium at some point.

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5
Q

If little product is formed the equilibrium is?

A

far to the left or reactant favored

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6
Q

If little reactant remains the equilibrium is?

A

far to the right or product favored

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7
Q

In static equilibrium, reactions?

A

do not take place

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8
Q

In dynamic equilibrium, reactions?

A

continue to take place

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9
Q

In static equilibrium, products?

A

will remain products

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10
Q

In dynamic equilibrium, products?

A

continue to be converted to reactants

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11
Q

In dynamic equilibrium, when products continue to be converted to reactants what is that called?

A

reverse reaction

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12
Q

In static equilibrium all unused reactant molecules will?

A

remain unreacted

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13
Q

In dynamic equilibrium reactant molecules continue?

A

being converted into products

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14
Q

Causes of equilibrium?

A

beginning of reaction, middle of reaction, at equilibrium

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15
Q

Equilibrium at beginning reaction

A

only reactant molecules exist, so only reactant molecules may collide

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16
Q

Equilibrium in the middle of reaction

A

as product concentration increases, collisions may take place that lead to the reverse reaction.

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17
Q

equilibrium at equilibrium

A

rates of forward and reverse reaction are identical

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18
Q

k is a constant called?

A

the equilibrium constant

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19
Q

k varies depending on?

A

temperature and value of the coefficients of the balanced equation

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20
Q

equilibrium position

A

a set of specific conditions that define when the system has reached the equilibrium point

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21
Q

In the equilibrium position k can only have ?

A

one value at a specific temperature

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22
Q

k can only have ___ value but_____?

A

one, the system can have an infinite number of equilibrium positions

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23
Q

Why can a system have an infinite number of equilibrium positions?

A

the specific equilibrium position is dependent on the initial concentrations of the species in the reaction.

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24
Q

When the balanced equation for a reaction is multiplied by some factor, the equilibrium position for?

A

the new reaction is the original expression raised to the nth power

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25
Q

For a particular reaction at a given temperature, the value of k is?

A

constant regardless of the amount of gases that are mixed together.

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26
Q

the position of heterogeneous equilibrium does not?

A

depend on the amounts of pure solids or liquids present because their concentrations remain constant

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27
Q

In a heterogeneous equilibrium, if pure solids or gases are present we?

A

omit them from our law of mass action equation

28
Q

In a heterogeneous equilibrium, only gases and aqueous solution are?

A

included in mass action laws when working with heterogeneous reactions

29
Q

reactions with large equilibrium constants

A

k > 1

30
Q

when k > 1 the reaction is likely to?

A

be completed and equilibrium position is far to right.

31
Q

large equilibrium constants generally have?

A

large and negative Δ E

32
Q

reactions with small equilibrium constants

A

k < 1

33
Q

when k < 1 the reaction is likely to?

A

not take place, consist of mainly reactants, and equilibrium position is far to left.

34
Q

time required to reach equilibrium is related to?

A

the reaction rate and activation energy

35
Q

time required to reach equilibrium is not related to?

A

the magnitude of k

36
Q

to find Q, we use?

A

the initial concentrations and not the equilibrium concentrations.

37
Q

If Q = K the system is at?

A

equilibrium and no shift occurs

37
Q

If we apply the law of mass action to our initial concentrations, than we can?

A

determine what direction the reaction must move in order to achieve equilibrium

38
Q

If Q > K the system will?

A

shift to the left, consuming products and forming reactants to reach equilibrium

39
Q

If Q < K the system will?

A

shift to the right, consuming reactants and forming products to reach equilibrium.

40
Q

Le Chatlier Principle

A

States that any equilibrium reaction will do what is necessary to return to equilibrium if we change a condition.

41
Q

Equilibrium systems want to remain?

A

constant

42
Q

For Le Chatlier Principle, systems must be?

A

closed so that the adjustment occurs

43
Q

If we increase the concentration of any compound of an equilibrium system, the system will shift?

A

away from the change in opposite direction

44
Q

The opposite shift that takes place during an increase in concentration will?

A

consume anything that is on the same side as what we increased

45
Q

The opposite shift that takes place during an decrease in concentration will?

A

consume anything that is on the same side as what we decreased

46
Q

Ways to change pressure

A

-add or remove a gaseous reactant or product
-add an inert gas
-change the volume of the container

47
Q

inert gases _____ the pressure but have no effect on ______ or ________.

A

increase, concentrations, partial pressures

48
Q

If pressure is increased on a system, the equilibrium will shift?

A

to the side with less moles of gas

49
Q

If pressure is decreased on a system, the equilibrium will shift?

A

to the side with more moles of gas to maintain energy

50
Q

When volume is reduced the shift is?

A

high # of moles to low # of moles

51
Q

When volume is increased the shift is?

A

low # of moles to high # of moles

52
Q

in endothermic systems heat is a?

A

reactant

53
Q

in endothermic reactions if we increase temp/heat/energy the shift is?

A

to the right

54
Q

in endothermic reactions if we decrease temp/heat/energy the shift is?

A

to the left

55
Q

endothermic reactions have __ Delta h

A

positive

56
Q

in exothermic systems heat is a?

A

product

57
Q

in exothermic reactions if we increase temp/heat/energy the shift is?

A

to the left

58
Q

in endothermic reactions if we decrease temp/heat/energy the shift is?

A

to the right

59
Q

exothermic reactions have __ Delta h

A

negative

60
Q

add a reactant shift to?

A

products

61
Q

add a product shift to?

A

reactants

62
Q

increase temperature

A

shift away from heat

63
Q

decrease temperature

A

shift towards heart

64
Q

increase pressure

A

shift to side with fewer moles of gas

65
Q

decrease pressure

A

shift to side with more moles of gas

66
Q

the only stress that changes Keq is?

A

temperature

AP Chemistry (16 decks)

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