A6 Kinetics II Flashcards

1
Q

Define Rate of Reaction

A

Change in quantaties of reactants or products over time

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2
Q

What does it mean if the reaction is 0th order with respect to a reactant

A

Changing the concentration will have no effect on rate

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3
Q

What does it mean if the reaction is 1st order with respect to a reactant

A

Concentration is proportional to rate

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4
Q

What does it mean if the reaction is 2nd order with respect to a reactant

A

Concentration is proportional to rate (^2)

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5
Q

When given a table to determine the reaction order with respect to a reactant, what must always be included in the explaination of each reactant

A
  • From experiment X to Y
  • How the concentration of each reactant changes
  • How the rate changes
  • The reaction will be 0th/1st/2nd order with respect to the reactant
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6
Q

What will always be included in the rate equation

A

Rate = k [reagents that are 1st or 2nd order]

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7
Q

How are 0th order reactants included in rate equations

A

They are not

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8
Q

How are 1st order reactants included in rate equations

A

To the power of 1 (by itself)

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9
Q

How are 2nd order reactants included in rate equations

A

Squared

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10
Q

Define Overall Order

A

Overall effect of the concentrations of all reactants on the rate of reaction

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11
Q

How to determine the overall order of a reaction

A

The sum of the orders of the reactants

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12
Q

How can the rate constant, K , be determined from a rate equation

A

Re-arrange so that K = rate / [reactants]

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13
Q

What will the unit for rate always be

A

dm -3 mol s-1

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14
Q

What will the unit for K always contain

A

s-1

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15
Q

How should answers in kinetics always be written

A

dm then mol then s

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16
Q

What does the red line represent on this concentration-time graph

A

A reactant that is first order

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17
Q

What does the blue line represent on this concentration-time graph

A

A reactant that is 0tt order

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18
Q

Describe the line on a concentration-time graph, that is 1st order

A

Line where consecutive half-lives are constant

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19
Q

Describe the line on a concentration-time graph, that is 0th order

A

Straight line, with a constant negative gradient

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20
Q

Define half-lives

A

Time taken for the concentration of a reactant to half

21
Q

On a concentration-time graph, what does it mean if a reactant has constant consecutive half-lives

A

The reaction is 1st order with respect to the reactant

22
Q

When can the value of K be determined from a concentration-time

A

When the reaction is first order with respect to the reactant

23
Q

What is the formula for K when calculating with a 1st order concentration-time graph

24
Q

What is an alternative to using the following formula to determine K on a 1st order concentration time graph

A

Drawing a tangent to the line at t=0s, and determining the gradient

25
What does the blue line represent on this rate-concentration graph
A 0th order reactant
26
What does the red line represent on this rate-concentration graph
A 1st order reactant
27
What does the green line represent on this rate-concentration graph
A 2nd order reactant
28
Describe a 1st order reactant on a rate-concentration graph
Line that goes through the origin, with a constant positive gradient
29
Describe a 0th order reactant on a rate-concentration graph
A horizontal line, with a gradient of 0
30
Describe a 2nd order reactant on a rate-concentration graph
A curve that has a gradient that gets more positive, as concentration increases
31
When investigating initial rate, what should be ensured when the reaction is 0th order to a reactant
A large excess of it is used, to ensure that the concentration is constant throughout
32
What must be ensured when investigating initial rate with reactants that are 0th order
A large excess of it is used, to ensure that the concentration is constant throughout
33
Why is a large excess of a 0th order reactant used when determining initial rate experimentally
To ensure that the concentration is constant throughout
34
When is colorimetry used experimentally in initial rates reactions
When one of the reactants is coloured (E.g iodine solution is orange)
35
What is the trend with abosrbancy (measured with a colorimeter) when a reactant is coloured
Absorbancy decreases as concentration decreases
36
Define rate-determining step
The slowest step of the reaction
37
Of all the reactants in an equation, what reactants will the rate equation include
Only those from the rate-determining step
38
How to tell that a mechanism is consistent with the rate equation
When all the mechanism steps (before and including the rate determining step) together give the reactants and products in the same stochiometric ratio as in the rate equation
39
When all the mechanism steps (before and including the rate determining step) together give the reactants and products in the same stochiometric ratio as in the rate equation
The mechanism is consistent with the rate equation
40
Why would a two-step mechanism be unlikely to occur in one step
* Stochiometry in the rate equation doesn't match stochiometry in overall equation * Successful collisions are unliekl with more than two particles
41
For Arrhenius graph, how is the Ea determined
42
Draw a Maxwell-Boltzmann graph, and show and explain how an increased temperature would affect this
* Increasing temperature means that there is a greater area under the curve above the activation energy * A greater number of molecules have energy greater than the activation energy
43
Equation for determining activation energy from an Arrhenius graph
44
Units for gradient on Arrhenius graph
K
45
What does the y-intercept of an arrhenius graph represent
ln A
46
How to determine A from an Arrhenius graph
e (to the power of intercept number)
47
Equation for ln K of Arrhenius graph
48
How to determine ln K from an Arrhenius graph
49
Units for horizontal line of Arrhenius graph
K (-1)