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A) Chemistry > Kinetecs > Flashcards

Kinetecs Flashcards

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0
Q

Rate law

A

Rate=k[A]^n

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1
Q

Rates of chemical change

A

Change in the concentration of a specific element over a period of time
Units of M per second
See the book for practice

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2
Q

Instantanteous Rate

A 
Limit as (t-initial)+(t-final) approaches the designated time 
In Δ[elementConcentration]/Δt
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3
Q

First order reactant

A

The rate varies directly with the concentration of reactant-A, forms a linear curve
Rate=k[A]^1

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4
Q

Second order reactant

A

The rate of the reaction changes exponentially with a change in the concentration of the A reactant
Rate=k[A]^2

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5
Q

Reaction order for multiples reactants

A

Rate=k([A]^m)([B]^n)

The order of the individual reactant remains unchanged in the reaction, only the k-value changes (depends on the how many, as well as which, reactants factor into the problem here

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6
Q

Integrated rate Law

A

The concentrations of the reactants is related to time time

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7
Q

First order integrate rate law

A

Natrual log [A] as a ratio to its original concentration for the simplest linear function

Ln([A]sub-t)/([A]sub-0)=-k*t

Write it out for practice

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8
Q

Second-order integrated rate law

A

Describes the reciprocal of the concentration of [A] in terms of ‘t’
Basically just the inverse of the zero-order law

1/([A]sub-t)=-k*t +(1/[A]sub-0)

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9
Q

Zero-order integrated rate law

A

Describes concentration as a linear function of (t)

[A]sub-t= -k*t +[A]sub-0

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10
Q

Half life of a reaction

A

T sub-1/2= 0.693/k

Or

T sub-1/2= ([A]sub-0)/2k

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11
Q

Arrhenius Equation

A

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

A=frequency factor, individual to each reaction
Ea=activation energy
R= gas constant
T= temperature in kelvin

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12
Q

Activation energy

A

Energy that much be accumulated for the reaction to take plac

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13
Q

Activated complex (transition state)

A

The high energy state all molecules go through to go from reactants to products

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14
Q

Frequency factor (A)

A

Number of time the reactants approach the activation energy level per minute

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15
Q

Exponential factor

A

e^(-Ea/RT)
Represents a number 0 through 1 represents the fraction of molecules that have enough energy to participate in the reaction

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16
Q

Arrhenius plot

A

Linear equation that represents the relationship between the temperature and the ‘k-value’

Ln k=-Ea/R*(1/T) +ln A

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17
Q

Arrhenius Equation (two point form)

A

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

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18
Q

Collision Model

A

The reaction in question calls for an energetic collision between two molecules

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19
Q

Orientation factor (p)

A

Numerical representation of the angle at which the molecules must collide with one another for the reaction to occur

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20
Q

Collision frequency (z)

A

Number of particle collisions that occur per unit of time

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21
Q

K-value from Collision model

A

k=pz(exponentialFactor)

Write it out

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22
Q

Reaction mechanism

A

Series of individual chemical equations by which an overall chemical reaction occurs

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23
Q

Elementary step

A

The simplest possible step, chemical equation) into which an entire reaction mechanism can always be broken down

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24
Q

Law of elementary steps in reaction mechanisms

A

An entire reaction mechanism can always be broken down into one simple chemical equation that describes the entire process, known as the elementary step

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25
Q

Reaction intermediate

A

A molecule formed in an elementary step of a reaction mechanism but broken down by another reaction mechanism’s elementary step

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26
Q

Molecularity

A

Number of reactant particles involved in a step

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27
Q

Unimolecular reaction

A

Only one reactant is required

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28
Q

Bimolecular

A

Two reactants are required

29
Q

Termolecular

A

Elementary steps in which three reactant particles collide,

Very rare to occur

30
Q

Rate-determining step

A

The slowest step in the reaction mechanism

31
Q

Activation energy in reaction mechanisms

A

Each require a little more energy, constant energy must be supplied

32
Q

Instantanteous Rate

A 
Limit as (t-initial)+(t-final) approaches the designated time 
In Δ[elementConcentration]/Δt
33
Q

Reaction order for multiples reactants

A

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

34
Q

First order integrate rate law

A

Ln([A]sub-t)/([A]sub-0)=-k*t

Write it out for practice

35
Q

Second-order integrated rate law

A

1/([A]sub-t)=-k*t +(1/[A]sub-0)

36
Q

Zero-order integrated rate law

A

[A]sub-t= -k*t +[A]sub-0

37
Q

Half life of a reaction

A

T sub-1/2= 0.693/k

Or

T sub-1/2= ([A]sub-0)/2k

38
Q

Arrhenius Equation

A 
k= Ae^ ((-Ea)/RT)
Or ln(k)=ln(A)-(Ea/RT)

A=frequency factor, individual to each reaction
Ea=activation energy (in kJ/mol)
R= gas constant
T= temperature in kelvin

39
Q

Activation energy

A

Energy that much be accumulated for the reaction to take plac

40
Q

Activated complex (transition state)

A

The high energy state all molecules go through to go from reactants to products

41
Q

Frequency factor (A)

A

Number of time the reactants approach the activation energy level per minute

42
Q

Exponential factor

A

e^(-Ea/RT)
Represents a number 0 through 1 represents the fraction of molecules that have enough energy to participate in the reaction

43
Q

Arrhenius plot

A

Linear equation that represents the relationship between the temperature and the ‘k-value’

Ln k=-Ea/R*(1/T) +ln A

44
Q

Arrhenius Equation (two point form)

A

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

45
Q

Collision Model

A

The reaction in question calls for an energetic collision between two molecules

46
Q

Orientation factor (p)

A

Numerical representation of the angle at which the molecules must collide with one another for the reaction to occur

47
Q

Collision frequency (z)

A

Number of particle collisions that occur per unit of time

48
Q

K-value from Collision model

A

k=pz(exponentialFactor)

Write it out

49
Q

Reaction mechanism

A

Series of individual chemical equations by which an overall chemical reaction occurs

50
Q

Elementary step

A

The simplest possible step, chemical equation) into which an entire reaction mechanism can always be broken down

51
Q

Law of elementary steps in reaction mechanisms

A

An entire reaction mechanism can always be broken down into one simple chemical equation that describes the entire process, known as the elementary step

52
Q

Reaction intermediate

A

A molecule formed in an elementary step of a reaction mechanism but broken down by another reaction mechanism’s elementary step

53
Q

Molecularity

A

Number of reactant particles involved in a step

54
Q

Unimolecular reaction

A

Only one reactant is required

55
Q

Bimolecular

A

Two reactants are required

56
Q

Reaction Order

A

Power ‘n’ to which the concentration is raised in the rate formula, determines the effect the concentration of that product has on the rate.
The ‘n’ in
Rate=k*[A]^n

57
Q

Zero order reactant

A

Rate=k*[A]^0

The rate is independent of the concentration of that particular reactant

58
Q

Reaction order for a catalyst

A

Always zero

59
Q

Overall rates of reaction

A

Same as the rate of a reactant with a single coefficient

60
Q

Individual reactant rate

A

Same as the overall reaction rate multiplied by its coefficient

61
Q

Reaction rate when coefficient is multiplied

A

The rate is multiplied by that same value

62
Q

Approximating reactant order

A

Graph- value=zeroOrder, linear=firstOrder, exponential=secondOrder

Algebra- [A]^x=OverallRate/k, x-is reactant order

63
Q

Approximating k-value

A

k=Rate/[A]^x

64
Q

When graphing concentration vs time

A

Use arhennious equations

A

65
Q

Catalyst mechanism of action

A

Lowers the activation energy required for the reaction to take place

66
Q

Activating energy from the k-value

A

Ea=[Ln(k)-Ln(A)]*(RT)

67
Q

Reaction enthalpy ΔH

A

The net energy change when the reactants are transformed into products

68
Q

Termolecular

A

Elementary steps in which three reactant particles collide,

Very rare to occur

69
Q

Rate-determining step

A

The slowest step in the reaction mechanism

70
Q

Activation energy in reaction mechanisms

A

Each require a little more energy, constant energy must be supplied

A) Chemistry (9 decks)

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