Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

ap chem > unit 9 > Flashcards

unit 9 Flashcards

You may prefer our related Brainscape-certified flashcards:
Periodic Table flashcards Chemistry 101 flashcards AP® Chemistry flashcards Organic Chemistry 101 flashcards
1
Q

reversible reaction

A

a reaction that can proceed in both the forward and reverse directions

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

dynamic equilibrium

A

the rate of the reverse reaction equals the rate of the forward reaction

(this does not mean that [reactants] and [products] are equal to one another at equilibrium)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

Equilibrium constant (K)

A

Quantifies the relationship between [reactants] and [products] at equilibrium

K = [products]/[reactants]

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

significance of large K
(K&raquo_space; 1)

A

forward reaction is favored
-K lies far to right
-high [product] and low [reactant] at equilibrium
-forward reaction proceeds essentially to completion

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

significance of small K
(K &laquo_space;1)

A

-reverse reaction is favored
-K lies far to left
-Low [product] and high [reactant] at equilibrium
-Forward reaction does not proceed very far

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

if you reverse the equation, _ K

A

invert

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

what happens to K when you multiply the coefficients in the equation?

A

raise K by the same factor you multiplied the coefficients

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

what do you do to K when you add two or more individual chemical equations to each other to obtain an overall equation?

A

multiply K’s from all equations

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

What is dynamic equilibrium? Why is it called dynamic?

A

Rate of the forward reaction = rate of the reverse reaction

Even though [reactants] and [products] remain constant, both the forward and reverse reactions are occurring-reactants and products form at the same rate that they are depleted

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What is the significance of the equilibrium constant? What does a large equilibrium constant tell us about a reaction? A small one?

A

Indicates if the forward reaction (large K) or the reverse reaction (small K) is favored

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

concentration of gas equation

A

n/V = P/RT

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

pressure of a gas and concentration proportion

A

direct

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

Kc

A

equilibrium constant expressed in terms of concentrations of reactants and products

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

Kp

A

equilibrium constant for gaseous reactions, expressed in terms of partial pressure in atm

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

is the partial pressure of a gas in atm the same as the molar concentration of that gas?

A

no

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

Kc and Kp are only equal when

A

there is no change in the number of gas phase particles during the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

gas particle change equation

A

Kp = Kc (RT)^∆n

∆n = mol products - mol reactants

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

Explain the difference between Kc and Kp. For a given reaction, how are the two constants related?

A

Kc is the equilibrium constant with respect to concentration in molarity

Kp is the equilibrium constant for gaseous reactions in terms of partial pressures

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
19
Q

why don’t pure liquids/solids included in equilibrium expressions?

A

their concentrations do not change in the course of the reaction

they’re incorporated into values of Kc or Kp

ONLY INCLUDE GASES IN EQUILIBRIUM EXPRESSION

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
20
Q

The equilibrium [reactants] and [products] can vary depending on

A

their initial concentrations

21
Q

the equilibrium constant is always constant at

A

any temp, regardless of initial concentrations

22
Q

reaction quotient (Qc)

A

gauges the progress of a reaction relative to equilibrium, when the reaction mixture is not at equilibrium and contains reactants and products

-same as equilibrium constant, doesn’t need to be at equillibrium

23
Q

differences between Kc and Qc:

A

-Kc has only one value and specifies relative amounts of reactants and products at equilibrium
-Qc depends on the current state of the reaction and has many different values as the reaction proceeds

24
Q

what is the value of Qc when there are only reactants?

A

0

25
Q

what is the value of Qc when there are only products?

A

infinity

26
Q

what is the value of Qc when there are equal amounts of products and reactants?

A

1

27
Q

what happens when Q < K?

A

Reaction goes to the right (towards products)

28
Q

what happens when Q > K?

A

Reaction goes to the left (towards reactants)

29
Q

what happens when Q = K?

A

equilibrium

30
Q

when the equilibrium constant is small, will the reaction proceed far?

A

no

31
Q

Le Chatelier’s Principle

A

When a chemical system at equilibrium is disturbed, the system shifts in a direction that minimizes the disturbance.

A chemical system can be disturbed by changing [reactant] or [product], changing volume or pressure and changing temperature.

32
Q

volume and pressure proportion

A

inversely related

33
Q

if a system is at equilibrium, what happens when you decrease the volume?

A

the reaction shifts in the direction that has fewer moles of gas particles

34
Q

if a system is at equilibrium, what happens when you increase the volume?

A

the reaction shifts in the direction that has greater moles of gas particles

35
Q

does adding an inert gas to the mixture have an effect on the equilibrium?

A

no

36
Q

Increasing the concentration of one or more reactants (makes Q < K) causes the reaction to shift to the

A

right (toward products)

37
Q

Increasing the concentration of one or more products (makes Q > K) causes the reaction to shift to the

A

left (toward reactants)

38
Q

Decreasing the concentration of one or more reactants (makes Q > K) causes the reaction to shift to the

A

left (toward reactants)

39
Q

Decreasing the concentration of one or more products (makes Q < K) causes the reaction to shift to the

A

right (toward products)

40
Q

is a reaction has the same number of gas particles on both sides, what happens when the volume changes?

A

nothing

41
Q

what happens when you increase the temp in an exothermic reaction?

A

reaction shifts left
K decreases

42
Q

what happens when you decrease the temp in an exothermic reaction?

A

reaction shifts right
K increases

43
Q

what happens when you increase the temp in an endothermic reaction?

A

reaction shifts right
K increases

44
Q

what happens when you decrease the temp in an endothermic reaction?

A

reaction shifts left
K decreases

45
Q

do catalysts affect the position of equilibrium?

A

no

46
Q

solubility product constant (Ksp)

A

equilibrium constant for dissolution of an ionic compound

(measure of solubility)

47
Q

molar solubility

A

solubility in units of mol/L

-only one value at a given temp
-can have different values in different types of solutions

48
Q

what is lower, the solubility of an ionic compound in a solution containing a common ion or the solubility of an ionic compound in water?

A

in solution containing a common ion

49
Q

what happens when you add a soluble salt to a reaction that contains an insoluble salt?

A

it increases the solubility of the insoluble salt

ap chem (11 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2024 Bold Learning Solutions. Terms and Conditions