Kinetics Flashcards

1
Q

Energy barrier to reaction pathway

A

Activation energy

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2
Q

Transition state

A

Local energy maxima, unstable

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3
Q

Intermediate

A

Local energy minima, stable and can be isolated

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4
Q

Rate

A

-d[reactant]/dt or d[product]/dt

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5
Q

Rate at time t

A

Found with tangent of either graph of [product] against t or -[reactant] against t

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6
Q

General rate of

aA + bB → cC + dD

A

-1/ad[A]/dt
-1/b
d[B]/dt
1/cd[C]/dt
1/d
d[D]/dt

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7
Q

Differential rate equation

A

k[A]^m[B]^n

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8
Q

Pseudo-rate equation

A

When B is in large excess compared to A, [B] is roughly constant

Rate=k’[A]^m, where k’=k[B]^n

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9
Q

Method of initial rates

A

Initial rate=k’[A]0^m

Taking logs gives linear equation

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10
Q

Zeroth order integrated rate law

A

[A]=[A]0-kt

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11
Q

First order integrated rate law

A

[A]=[A0]e^(-kt)

ln[A]=ln[A]0

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12
Q

Second order (rate=k[A]^2) integrated rate law

A

1/[A]=1/([A]0)+kt

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13
Q

Second order (rate=k[A][B]) integrated rate law

A

ln(([B]/[B]0)/([A]/[A]0))

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14
Q

First order half life

A

ln(2)/k

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15
Q

Second order half life

A

1/([A]0k)

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16
Q

Arrhenius equation

A

k=Ae^-(Ea/RT)

17
Q

Activation energy

A

Minimum energy reacting molecules must have to overcome an energy barrier to reaction

18
Q

Catalyst

A

Provides an alternate pathway of lower activation energy, dramatically decreases value of k

19
Q

Rate at eqm

A

0

20
Q

Rate determining step

A

Slowest step with highest activation energy

21
Q

Kinetic control

A

Ratio of product concentrations depends on the rate coefficients and hence the different activation energies

Irreversible conditions

22
Q

Thermodynamic control

A

Depends on the eqm constants and hence the standard free energies

Reversible conditions

23
Q

Competitive enzyme inhibition

A

Substrate and inhibitor can not bind at the same time