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CHEM 401 > CH14: CHEM. KINE. > Flashcards

CH14: CHEM. KINE. Flashcards

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1
Q

Zero-Order Rxns - Integrated Rate Law

A

[A] = -kt + [A]

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2
Q

Chemical Kinetics

A

study of factors affecting the rxn rate

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3
Q

Ectotherms

A

animals whose blood temperature matches the environmental temperature

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4
Q

what is rxn rate/rate of rxn?

A

(∆ concentration)/(∆ time)

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5
Q

simple rate/avg. rate

A

∙ -[∆A/∆t] or +[∆A/∆t]

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6
Q

for rct, the simple rate/average rate is..

A

(-) cuz it’s being used to create product over time

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7
Q

for products, the simple rate/average rate is..

A

positive (+) cuz it’s increasing by using reactants over time

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8
Q

rxn rate

A

(-1/a)[∆A/∆t] or +(1/a)[∆A/∆t]

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9
Q

[elem. or cmp.]

A

the M (molarity) of the elem. or cmp.

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10
Q

instantaneous rate in terms of chemistry

A

change in concentration at one particular time

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11
Q

relationship btwn the rxn rate and concentration of rcts

A

directly proportional

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12
Q

3 ways to monitor rxn mixtures

A

polarimetry, spectrometry, and pressure measurement/total pressure

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13
Q

polaritmetry

A

measuring the change in the degree of rotation of plane-polarized light caused by 1 components over time

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14
Q

spectrophotometry

A

measuring the amount of light of a particular λ absorbed by 1 component over time

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15
Q

total pressure

A

equal to the partial pressures of the rxn

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16
Q

aliquots - definition and method

A

samples (from the rxn mixture) drawn off at specific times and analyzed quantitatively

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17
Q

gas chromatography

A

separation method using gas flow through a glass or metal column that separates cmps. based on both volatility (material that can easily evaporate) and interaction w/ (l) stationary phase

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18
Q

methods to determine concentration in mixtures

A

spectrophotometry and gas chromatography

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19
Q

rate law

A

a mathematical description of how rate of rxn/rxn rate relate to concentration of rcts

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20
Q

provide the general rate law for A → products

A

Rate = k∙[A]ⁿ

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21
Q

k in rate law

A

rate constant and needs to be calculated

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22
Q

ⁿ in rate law

A

order w/ respect to the rct

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23
Q

overall order

A

total of all exponents added up

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24
Q

what is the rxn order with respect to NO from the equation: Rate = k[NO]²[O₂]?

A

2nd order

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25
Q

what is the overall order of the equation: Rate = k[NO]²[O₂]?

A

3rd order

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26
Q

order of rxn - mathematically

A

method of initial rates (rate₁/rate₂)

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27
Q

Integrated Rate Law

A

mathematical description tha relates time of rxn to the concentration of A (rct)

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28
Q

Zero-Order Rxns - Rate Law

A

Rate = k∙[A]⁰ or Rate = k

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29
Q

First-Order Rxns - Rate Law

A

Rate = k∙[A]¹ or Rate= k∙[A]

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30
Q

Second-Order Rxns - Rate Law

A

Rate = k∙[A]²

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31
Q

Second-Order Rxns - Integrated Rate Law

A

(1/[A]) = kt + (1/[A]₀)

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32
Q

First-Order Rxns - Integrated Rate Law

A

ln[A] = -kt + ln[A]₀

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33
Q

Zero-Order Rxns - Half-life

A

t(₁/₂) = ([A]₀/(2k))

34
Q

First-Order Rxns - Half-life

A

t(₁/₂) = (ln(2)/(k))

35
Q

Second-Order Rxns - Half-life

A

t(₁/₂) = (1/(k[A]₀))

36
Q

Zero-Order Rxns - Units of k

A

(M/s)

37
Q

First-Order Rxns - Units of k

A

(1/s) or s-¹

38
Q

Second-Order Rxns - Units of k

A

(1/M∙s) or M⁻¹∙s⁻¹

39
Q

order of rxns - graphically

A

∙R² =1 or the best fit line

40
Q

Activation Energy

A

E needed to convert rcts to transition state (activated complex)

41
Q

Half-life, t(₁/₂)

A

time in which the concentration of rct is halved and is dependent on order of rxn

42
Q

Activated Complex

A

chemical species (kind of atom, molecule, ion, or particles) w/ partial bonds (partially broken and partially formed)

43
Q

Frequency

A

of molecules that begin to transition in a given period of time

44
Q

Arrhenius Equation - Definition

A

showing the relationship between k, rate constant, to temp.

45
Q

Arrhenius Equation - Equation

A

k = Ae^(-Ea/(RT)) = pze^(-Ea/(RT))

46
Q

Arrhenius Equation - Requirement

A

T in K (Kelvin)

47
Q

relationship between activation E and rxn rate

A

inversely proportional

48
Q

relationship between temp. and exponential factor in Arrhenius Equation

A

directly proportional

49
Q

Arrhenius Equation (in y=mx+b)

A

lnk = (-Ea/(R))∙(1/(T)) + lnA

50
Q

Two-Point Arrhenius Equation

A

ln(k₁/(k₂)) = (Ea/(R))((1/(T₁))-(1/(T₂))

51
Q

Collision Theory

A

states that atoms, ions, and molecules must collide in order to react, depending on two factors: p and the z

52
Q

z

A

collision factor

53
Q

relationship btwn frequency of effective collisions and rxn rate

A

directly proportional

54
Q

Effective Collisions

A

collisions that lead to rxn

55
Q

p in Arrhenius Equation

A

orientation factor

56
Q

p < 1

A

e- transfer

57
Q

p ≈ 1

A

atoms colliding

58
Q

p >1

A

complex rct molecules

59
Q

Reaction Mechanism

A

series of individual chemical steps that create the overall chemical rxn

60
Q

Elementary Steps

A

steps that cannot simplify and molecules interact directly

61
Q

Rct Intermediates

A

products in a early step and then rcts in a later step

62
Q

Molecularity

A

of rcts particles in an elementary step

of rct particles in an elem. step

63
Q

Unimolecular

A

1 particle

64
Q

Bimolecular

A

2 particles

65
Q

Termolecular

A

3 particles

66
Q

Rate-determining Step

A

∙ slowest step in the mechanism

67
Q

Rate Law of Overall Rct

A

expo. match coefficients

68
Q

Mechanism - Validation

A

sum of elementary steps = overall rcts and the slow rate law matches the obs. rate law

69
Q

Proposed Rate Law

A

slowest rate law

70
Q

Catalysts

A

substances that affect the rxn rate, but is not consumed by the rxn

71
Q

Catalysts in the Equation

A

consumed earlier and then made later

72
Q

heterogeneous catalysts

A

catalysts is the diff. phase as the rct particles

73
Q

homogeneous catalysts

A

catalysts is in same phase from the rct particles

74
Q

definition of rate

A

change in quantity in a given time period

75
Q

definition of avg. rate

A

change in concentrations in any particular time period

76
Q

relationship btwn half-life and concentration of rct

A

inversely proportional

77
Q

gas constant for energy-related problems

A

8.314 J/(molxk)

78
Q

gas constant for pressure-related problems

A

0.08206 (Lxatm)/(molxk)

79
Q

when the initial step of a mechanism is fast, you will need to…

A

substitute the rate law of the fast step into the rate law of the slow step

80
Q

When multiple variables of diff. expo. are being multiply, you would…

A

add the expo. of the variables tgt

81
Q

to substitute the rate law of the fast step into the rate law of the slow step, you will need to…

A

write out the inverse equ. of the rate law of the fast step

CHEM 401 (2 decks)

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