Chapter 13

Question 1

static equilibrium does not occur in?

Answer 1

chemical systems

Question 2

chemical equilibrium

Answer 2

usually studied in a closed system with controlled variables.

Question 3

Equilibrium

Answer 3

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

Question 4

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

Answer 4

reach equilibrium at some point.

Question 5

If little product is formed the equilibrium is?

Answer 5

far to the left or reactant favored

Question 6

If little reactant remains the equilibrium is?

Answer 6

far to the right or product favored

Question 7

In static equilibrium, reactions?

Answer 7

do not take place

Question 8

In dynamic equilibrium, reactions?

Answer 8

continue to take place

Question 9

In static equilibrium, products?

Answer 9

will remain products

Question 10

In dynamic equilibrium, products?

Answer 10

continue to be converted to reactants

Question 11

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

Answer 11

reverse reaction

Question 12

In static equilibrium all unused reactant molecules will?

Answer 12

remain unreacted

Question 13

In dynamic equilibrium reactant molecules continue?

Answer 13

being converted into products

Question 14

Causes of equilibrium?

Answer 14

beginning of reaction, middle of reaction, at equilibrium

Question 15

Equilibrium at beginning reaction

Answer 15

only reactant molecules exist, so only reactant molecules may collide

Question 16

Equilibrium in the middle of reaction

Answer 16

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

Question 17

equilibrium at equilibrium

Answer 17

rates of forward and reverse reaction are identical

Question 18

k is a constant called?

Answer 18

the equilibrium constant

Question 19

k varies depending on?

Answer 19

temperature and value of the coefficients of the balanced equation

Question 20

equilibrium position

Answer 20

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

Question 21

In the equilibrium position k can only have ?

Answer 21

one value at a specific temperature

Question 22

k can only have ___ value but_____?

Answer 22

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

Question 23

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

Answer 23

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

Question 24

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

Answer 24

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

Question 25

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

Answer 25

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

Question 26

the position of heterogeneous equilibrium does not?

Answer 26

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

Question 27

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

Answer 27

omit them from our law of mass action equation

Question 28

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

Answer 28

included in mass action laws when working with heterogeneous reactions

Question 29

reactions with large equilibrium constants

Answer 29

k > 1

Question 30

when k > 1 the reaction is likely to?

Answer 30

be completed and equilibrium position is far to right.

Question 31

large equilibrium constants generally have?

Answer 31

large and negative Δ E

Question 32

reactions with small equilibrium constants

Answer 32

k < 1

Question 33

when k < 1 the reaction is likely to?

Answer 33

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

Question 34

time required to reach equilibrium is related to?

Answer 34

the reaction rate and activation energy

Question 35

time required to reach equilibrium is not related to?

Answer 35

the magnitude of k

Question 36

to find Q, we use?

Answer 36

the initial concentrations and not the equilibrium concentrations.

Question 37

If Q = K the system is at?

Answer 37

equilibrium and no shift occurs

Question 37

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

Answer 37

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

Question 38

If Q > K the system will?

Answer 38

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

Question 39

If Q < K the system will?

Answer 39

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

Question 40

Le Chatlier Principle

Answer 40

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

Question 41

Equilibrium systems want to remain?

Answer 41

constant

Question 42

For Le Chatlier Principle, systems must be?

Answer 42

closed so that the adjustment occurs

Question 43

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

Answer 43

away from the change in opposite direction

Question 44

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

Answer 44

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

Question 45

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

Answer 45

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

Question 46

Ways to change pressure

Answer 46

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

Question 47

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

Answer 47

increase, concentrations, partial pressures

Question 48

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

Answer 48

to the side with less moles of gas

Question 49

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

Answer 49

to the side with more moles of gas to maintain energy

Question 50

When volume is reduced the shift is?

Answer 50

high # of moles to low # of moles

Question 51

When volume is increased the shift is?

Answer 51

low # of moles to high # of moles

Question 52

in endothermic systems heat is a?

Answer 52

reactant

Question 53

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

Answer 53

to the right

Question 54

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

Answer 54

to the left

Question 55

endothermic reactions have __ Delta h

Answer 55

positive

Question 56

in exothermic systems heat is a?

Answer 56

product

Question 57

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

Answer 57

to the left

Question 58

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

Answer 58

to the right

Question 59

exothermic reactions have __ Delta h

Answer 59

negative

Question 60

add a reactant shift to?

Answer 60

products

Question 61

add a product shift to?

Answer 61

reactants

Question 62

increase temperature

Answer 62

shift away from heat

Question 63

decrease temperature

Answer 63

shift towards heart

Question 64

increase pressure

Answer 64

shift to side with fewer moles of gas

Question 65

decrease pressure

Answer 65

shift to side with more moles of gas

Question 66

the only stress that changes Keq is?

Answer 66

temperature