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The Science Of Medicines (PHAR 1021) year 1 > Chemical kinetics > Flashcards

Chemical kinetics Flashcards

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1
Q

what is kinetics?

A

‘the study of rates of reactions’

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2
Q

why is kinetics important in pharmaceutical sciences?

A

allows predictions of rates of degrading of drugs
important in other pharmaceutical processes

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3
Q

how does kinetics help predict rates of degrading of drugs?

A

can predict the stability of drugs causing accelerating stability of drugs expiry dates given

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4
Q

how are kinetics important in other pharmaceutical processes?

A

studying drug release rates and rates of processes that occur in the body

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5
Q

what is pharmacokinetics?

A

‘behaviour of drugs in the body’

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6
Q

how are reaction rates measures?

A

concentrations of chemicals measured at certain times throughout the reaction

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7
Q

what are the methods used for slow reactions?

A

samples removed at different times of the reaction and assayed for cocentration

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8
Q

what methods used for fast reactions?

A

using stopped-flow and spectroscopic methods

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9
Q

what is the rate of reaction?

A

‘the rate of change of concentration of any species’

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10
Q

what is the rate of formulation of product?

A

P= d[P]/dt

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11
Q

what is the rate of destruction of reactant (A)?

A

A=d[A]/dt

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12
Q

relationship between P and A?

A

one P molecule is formed for every A that reacts

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13
Q

what is the equation linking P to A?

A

d[P]/dt = -d[A]/dt

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14
Q

why is d[A]/dt negative?

A

concentration is decreasing over time

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15
Q

what is the equation when one mole of A reacts with two of B?

A

d[B]/dt = 2d[A]/dt

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16
Q

rate laws?

A

‘the rate of the forward reaction is defined as minus the rate of change of one of the reactants.’

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17
Q

what is the law of mass action?

A

‘Reaction rate is found to be proportional to the concentration of the reactant raised to the power of the number of molecules involved in the reaction’

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18
Q

what happens to reactions as temperature increases?

A

faster because more molecules have energy greater or equal to the activation energy

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19
Q

what do molecules have to do to react together?

A

collide
have enough energy to overcome the activation energy

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20
Q

what does the boltzmann equation give?

A

‘the fraction of molecules with energy higher than the Ea’

21
Q

what is the boltzmann equation?

A

F= e^ (-Ea/RT)

22
Q

what is the Arrhenius equation is standard form?

A

ln k = ln A - E /RT

23
Q

what is the Keq called?

A

equilibrium constant
will be large if forward reaction is rapid so [P] will be large

24
Q

what equation show at equilibrium the two rates of A converting to P and P converting to A are the equal?

A

kf/kr =[P]/[A] = Keq

25
Q

what is the rate of zero reaction?

A

rate of disappearance of compound is constant and independent of its concentration
differential law:
-d[A]/dt = k

26
Q

what is the equation of zero order?

A

[A] = -kt+ [A]o
y=mx+c

27
Q

what does Zero order reaction look like on graph?

A

slide 3
lecture 12 chemical kinetics part 2

28
Q

what is the differential law for first order reactions?

A

-d[A]/dt = k[A]

29
Q

what is the rate of first order reaction?

A

‘rate of decay is proportional to the amount of material remaining at that time’

30
Q

what is the integrated form of the rate law of first order?

A

[A]t= [A]o e^(-kt)

31
Q

what does the graph of first order look like?

A

slide 6
lecture 12 chemical kinetics part 2

32
Q

what are the units of K in first order reaction?

A

s^-1

33
Q

how is first order reaction equation written in the form of y=mx +c

A

ln [A]t = ln [A]o -kt

34
Q

relationship between K and concentration in first order reaction?

A

‘rate constant is independent of concentration’

35
Q

what is the equation of lifetime?

A

= 1/k

35
Q

what is the equation of half-life?

A

(ln 2)/k

36
Q

what happens to the half-life in second order reactions?

A

not constant

37
Q

what are the two possible types of reactions that are second order?

A

either two of the same products colliding
-d[A]/dt = k[A]^2
or two different molecules reacting
-d[A]/dt = k[A][B]

37
Q

when Keq constant?

A

‘under a set of conditions’

38
Q

what is the half-life in first order?

A

constant

39
Q

what are parallel reactions?

A

‘when a reactant decays in one of two products’

40
Q

what is the differential rate equation of parallel equations?

A

-d[A]/dt = k [A] + k [A]

41
Q

what is the integrated rate equation of parallel equation?

A

[A]t = [A]o e ^(-(k + k ) t)

42
Q

what are the rate laws of consecutive reactions/

A

-d[A]/dt = k1 [A]
-d[B]/dt = k2 [B] - k1 [A]
d[C]/dt = k2 [B]

43
Q

what happens in consecutive reations?

A

A is turned into B which is then turned into C

44
Q

what are the different profiles of concentration against time for A, B, C and why for consecutive reactions?

A

slide 4
SOM lecture 12 chemical kinetics part 5

45
Q

what are the two concepts for consecutive reactions?

A

steady-state approximation
rate-limiting step

46
Q

what is the steady-state approximation?

A

after reaction has run for some time, concentration of B is 0
d[B]/dt=0

47
Q

what is the rate-limiting step?

A

when one step is slower than the rest

The Science Of Medicines (PHAR 1021) year 1 (20 decks)

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