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CHEM1603 CH > Section E > Flashcards

Section E Flashcards

1
Q

What is the rate of reaction?

A

Rate at which reagents are used up and products are formed

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2
Q

What is the rate equation?

A

Rate = k[A]^m.[B]^n

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3
Q

How do you find overall order from partial order?

A

Overall order: m + n (if m or n are partial orders)

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4
Q

What does the rate constant vary with?

A

Temperature and the nature of reactants

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5
Q

Define a zero order reaction

A

Rate of the reaction does not depend on concentration

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6
Q

What is the equation for a zero order reaction?

A

[A] = [A0] - kt

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7
Q

In a zero order reaction, what decreases linearly over time?

A

Concentration of reactants

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8
Q

What is the equation for first order reactions?

A

[A] = [A0].e^-kt

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9
Q

Define T 1/2

A

Half life, time required for the concentration to drop to half of its original value

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10
Q

What is the equation to find half life from rate constant?

A

T 1/2 = ln2/k

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11
Q

what are the two processes occurring during drug metabolism?

A

Renal and metabolic elimination

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12
Q

What is the equation for drug metabolism kinetics?

A

-d[drugs]/dt = ae^-k1t + be^-k2t (k1/2 are diff. rate constants, a/b are weighting factors)

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13
Q

What form of kinetics is radioactive decay?

A

First order

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14
Q

What is the definition of radioactive activity (Bq)?

A

number of decay events per second

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15
Q

what are the units for radioactive activity?

A

Becquerels

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16
Q

What is 1 curie equivalent to?

A

3.7 x 10^10 disintegrations per second

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17
Q

What are 2 equations to find activity?

A

Activity = -dN/dt = kN

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18
Q

What is the equation for radioactive decay?

A

N = N0.e^-kt

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19
Q

What is an alternative equation for radioactive decay?

A

N = N0.e^(-ln2.t/t 1/2)

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20
Q

What is the half life of Krypton 85 gas?

A

10.8 years

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21
Q

Define a second order reaction

A

Rate of reaction proportional to square of concentration of the reagent

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22
Q

What is the equation for a second order reaction?

A

1/[A] = 1/[A0] + kt

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23
Q

What is the general procedure to measure a rate of reaction?

A

start reaction, measure property as function of time, convert measurement to concentration, analyse data

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24
Q

What spectrophotometric method is used to measure the rate of reaction for very fast reactions?

A

Flash photolysis

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25
Q

What spectrophotometric method is used to measure the rate of reaction for fast reactions?

A

Stopped flow method

26
Q

How would you determine the order of a reaction experimentally?

A

diff. [A0] but same [B], plot [A] vs T (if linear then 0 order), plot ln[A] vs T (if linear then 1st order), plot 1/[A] vs T (if linear 2nd order)

27
Q

What is the initial rates/differential method for determining order of a reaction?

A

keep [B] same, but [B]»>[A] so [B] constant, run reaction at different [A0], determine initial rate of each, plot against time, then put into equation: log(rate) = log(k obs) + alog[A]

28
Q

What are pseudo-order conditions?

A

having such a high concentration of a substrate that it’s concentration remains effectively constant throughout the reaction

29
Q

Define an elementary reaction

A

most reactions require several steps for the reaction to go to completion, reactions go via intermediates, two types e.g. photochemical reactions of alkanes

30
Q

What is a unimolecular reaction?

A

Single species undergoes a change, type of elementary reaction, e.g. bond cleavage

31
Q

What is a bimolecular reaction?

A

Two species come together, type of elementary reaction e.g bond formation

32
Q

Define an elementary step

A

Reaction at molecular level e.g. collision between 2 molecules/bond breaking or formation

33
Q

What is the equation for rate law in a unimolecular step?

A

Rate = k[A2] assuming reaction: A2 —> A + A

34
Q

What is the equation for rate law in a homonuclear and bimolecular step?

A

Rate = k[A]^2 assuming reaction: A + A —> A2

35
Q

What is the equation for rate law in a heteronuclear and bimolecular step?

A

Rate = k[A][B] assuming reaction: A + B —> AB

36
Q

What is the rate determining step?

A

If reaction is a series of steps, then slowest step governs the rate of reaction,

37
Q

What is the equation for rate constant from temperature?

A

k = Ae^-Ea/RT OR lnk = lnA - Ea/RT

38
Q

What is the Arrhenius relation?

A

Rate constant depending on temperature, equation = k = Ae^-Ea/RT OR lnk = lnA - Ea/RT

39
Q

Why do reactions depend on temperature?

A

depends on collisions, molecules require collision of threshold energy = activation energy

40
Q

What is the Boltzmann distribution?

A

A distribution of the kinetic energy of molecules within a sample, represented by the equation e^-E/RT

41
Q

What does the equation e^-E/RT represent?

A

The fraction of molecules at a temperature T which have energy greater than E

42
Q

What is the significance of the pre-exponential factor A?

A

A usually represents the total number of collisions occurring per second in a reaction (if more complex then important to factor in orientation of collision)

43
Q

Define a catalyst

A

A substance which takes part in a reaction and changes its rate but which can be recovered unchanged at the end of the reaction

44
Q

Why do catalysts work?

A

Provides the reaction with a separate mechanism with a lower activation energy

45
Q

What is a homogenous catalyst?

A

Catalyst in the same phase as the reactants

46
Q

What is a heterogenous catalyst?

A

Catalyst in different phase as reactants

47
Q

What is an example of an enzyme which shows extreme specificity?

A

Urease

48
Q

Who proposed the lock and key method in 1958?

A

Koshland

49
Q

What is the michealas-menten equation to find rate of product formed?

A

V = k2[E0][S]/(Km+[S])

50
Q

What measure is km?

A

Measure of how strongly something binds, small Km = strong binding

51
Q

What is the equation for Vmax?

A

Vmax = limiting rate = k2.[E0}

52
Q

What is the equation for rate (V)?

A

V = Vmax.[S]/(Km+[S])

53
Q

When does [S]+Km occur?

A

At very high [S]

54
Q

What is the equation for Kcat?

A

Kcat = Vmax/[E0]

55
Q

What is the definition of Kcat?

A

How many substrate molecules can be processed per second by 1mole of catalyst

56
Q

What do you plot on a line weaver burke plot?

A

1/[S] (x) against 1/V (y)(double reciprocal plot)

57
Q

What does the slope, X=0, Y=0 equal?

A

slope=Km/Vmax, X=0= -1/Km, Y=0= 1/Vmax

58
Q

What is an Eadie-Hofstee plot?

A

rearrange v equation to: V = -V/[S].Km + Vmax, plot V against V/[S], Vmax at X=0, slope= -Km

59
Q

What is a competitive inhibitor?

A

Inhibitor binds reversibly to active site, enzyme retains ability to process enzyme (Vmax same), but cannot bind S (Km changed) - gradient rotates up around 1/Vmax point

60
Q

What is a non-competitive inhibitor?

A

Inhibitor binds to a remote site, affects its activity not ability to bind substrate so Vmax changes, Km same

61
Q

What is an irreversible inhibitor?

A

Binds to active site and shuts down activity so [E] decreases

CHEM1603 CH (6 decks)

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