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Gen Chem 2 > Exam 2 > Flashcards

Exam 2 Flashcards

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1
Q

what need to collide to react

A

reactants

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2
Q

what to collisions need to have to initiate a reaction

A

activation energy

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3
Q

molecules must collide in an orientation that can lead to an rearrangement of the atoms

A

steric factor

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4
Q

effective collisions lead to the formation of an ______ ________ which is also known as the _______ _______

A

activated complex
transition state

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5
Q

Arrhenius equation

A

k=Axe^-Ea/ RT

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6
Q

what plot of the Arrhenius equation gives a straight line

A

ln(k) verus 1/T
slope -Ea/R
intercept= ln(A)

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7
Q

Arrhenius equation used to find activation energy

A

Ea= (-R*lnk2/k1)/ (1/T2 - 1/T1)

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8
Q

Arrhenius equation used to find rate constant

A

ln k2/k1 = -Ea/R (1/T2 - 1/T2)

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9
Q

what is a sequence of molecular events, or reaction steps, that defines the pathway from reactants to products

A

reaction mechanism

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10
Q

what can be describes as a sequence of elementary reactions or elementary steps

A

overall reaction

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11
Q

the overall reaction describes the reaction stoichiometry but does not tell us how the reaction ________

A

proceeds

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12
Q

an _______ ________ is a single step based on one collision (describes behavior of molecule)

A

elementary reaction

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13
Q

what appears is the mechanism but not in the overall balanced equation

A

intermediate

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14
Q

what always sum up to overall reactions and can involve intermediates

A

elementary reactions

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15
Q

reactions are often classified by their ________

A

molarity

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16
Q

the experimentally observed rate law for an ______ _______ must depend on the ________ _________

A

overall reaction
reaction mechanism

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17
Q

the slowest step with determine the rate: called

A

rate determining step

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18
Q

the energy of reactants and products stays the same the ______ _______ changes

A

transition state

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19
Q

what affects the reaction rate but is not consumed

A

catalyst

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20
Q

the ______ is the same before and after the reaction

A

catalyst

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21
Q

can the catalyst be a part of the rate law

A

yes

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22
Q

what type of catalyst can be in the same phase as the reaction / reactants

A

Homogeneous

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23
Q

what type of catalyst is in a different phase than the reaction/ reactants

A

heterogeneous

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24
Q

are enzymes a separate class of catalysts

A

yes

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25
Q

a mixture where [reactants] and [products] are in an equilibrium state is called an

A

equilibrium mixture

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26
Q

chemical equilibrium is a

A

dynamic equilibrium

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27
Q

in a dynamin equilibrium there is no _______ __________ which means forward and reverse rates are ________

A

net conversion
equal

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28
Q

a reaction that occurs in both directions is called a

A

reversible reaction

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29
Q

strictly: all reactions are _______
But: we call reactions that proceed nearly to completion __________

A

reversible
irreversible

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30
Q

Kc or equilibrium constant equation

A

Kf/Kr

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31
Q

Kc is __________

A

dimensionelss

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32
Q

Kc will always be the ________ at a particular temperature

A

same

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33
Q

Qc reaction quotient equation

A

Qc=[c]^c t [D]^d t / [A]^a t [B]^b t

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34
Q

Kc reaction quotient equation

A

[C]^c eq [ D]^d eq / [A] ^a eq [B]^b eq

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35
Q

at equilibrium Kc= Qc known as the

A

law of mass action

36
Q

law of mass action holds for ______ reaction

A

any

37
Q

if Qc<Kc net reaction

A

left to right

38
Q

if Qc>Kc net reaction

A

right to left

39
Q

Qc = Kc at equilibrium

A

no net reaction

40
Q

Kc«1 denominator much larger than the numerator ______ dominate

A

reactants

41
Q

Kc»1 numerator much larger than denominator ________ dominate

A

products

42
Q

solutions and pure gas phase reactions are considered

A

homogenous equilibria

43
Q

reactions for which reactants and products belong to more tan one phase are examples of

A

heterogenous equilibria

44
Q

the concentration of a solid is directly related to its density it will ______ ________ with the amount of solid you have

A

not change

45
Q

are concentrations of pure solids and pure liquids included when writing the equilibrium constant expression

A

NO

46
Q

Kc’ equation

A

[A]^a [B]^b/ [C]^c[D]^d = 1/Kc

47
Q

equilibrium constant Kp equation

A

Kp= Kc(RT)^ delta n

48
Q

the concentration of an _____ reactant or product is relieved by reaction in the direction that ________ the added substance

A

added
consumes

49
Q

the concentration stress of a ________ reactant or product is relieved by reaction In the direction that _________ the removed substance

A

removed
replenishes

50
Q

applying a stress to an equilibrium mixture will produce a net reaction in the direction that relieves the stress

A

la chateliers principle

51
Q

decreasing the volume in an equation will favor the side with

A

less molecules

52
Q

endothermic processes are favored when temp ______

A

increases

53
Q

exothermic processes are favored when temp __________

A

decreases

54
Q

a catalysts ________ the rate at which equilibrium is reached. it ____ ______ affect the ________ of the equilibrium mixture

A

accelerates
does not
composition

55
Q

what transfers a proton to another substance

A

bronsted lowry acid

56
Q

what accepts a proton

A

bronsted Lowry bases

57
Q

chemical species that only differ by 1 H+ are called

A

conjugate acid-base pairs

58
Q

what is the ion product of water equation

A

Kw= [H3O+][OH-]= 1.0 x 10 ^-14

59
Q

shorthand of pH

A

pH= - log[H3O+] and [H3O+] = 10^pH

60
Q

pH<7

A

acid

61
Q

pH>7

A

base

62
Q

pH=7

A

neutral

63
Q

pOH=

A

-log[OH-]

64
Q

pOH equation

A

14= -log[H3O+] - log [OH-] = pH+pOH

65
Q

strong acids dissociate

A

100%

66
Q

strong acids have very ______ conjugate bases

A

weak

67
Q

HCl

A

hydrochloric acid

68
Q

HBr

A

hydrobromic acid

69
Q

HI

A

hydroiodic acid

70
Q

HNO3

A

nitric acid

71
Q

H2SO4

A

sulfuric acid

72
Q

HClO4

A

perchloric acid

73
Q

HClO3

A

chloric acid

74
Q

strong bases react

A

100%

75
Q

strong bases have very ______ conjugate acids

A

weak

76
Q

LiOH, NaOH, KOH, RbOH, CsOH

A

alkali metal hydroxides

77
Q

Mg(OH)2, Ca(OH)2, Si(OH)2, Ba(OH)2

A

alkaline earth metal hydroxides

78
Q

weak acids dissociate _______

A

<100%

79
Q

acid ionization constant equation Ka

A

Ka= [H3O+][A-]. or [H+][A-]
——————— —————–
[HA] [HA]

80
Q

percent dissociation equation

A

%diss= [HA] diss/ [HA] initial X 100%

81
Q

base dissociation constant equation Kb

A

Kb= [BH+][OH-]/ [B]

82
Q

ion product of water equation

A

Kw=KaXKb

83
Q

acid strength: for elements in the same group ________ dominates

A

bond strength

84
Q

acid strength increases going from _____ to _______ of the periodic table

A

top to bottom

85
Q

for elements in the same row increasing ______ and ______ dominate

A

electronegativity and polarity

86
Q

acid strength increases going from _____ to _____ in the periodic table

A

left to right

Gen Chem 2 (3 decks)

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