Y2 Kinetics (P) Flashcards

1
Q

4 requirements in Collision Theory

A
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2
Q

2 Methods to increase rate

A
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3
Q

5 factors to affect rate

A
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4
Q

How do you measure rate?

A
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5
Q

Rate law

A
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6
Q

Zero order
How does changing the concentration affect the rate?

A
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7
Q

First order
How does changing the concentration affect the rate?

A
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8
Q

Second order
How does changing the concentration affect the rate?

A
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9
Q

How do you work out an order of reaction?

A
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10
Q

Substances that appear in the rate equation but not in the balanced equation

A

Catalysts

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11
Q

Rate constant units always end in

A

s^-1

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12
Q

The rate constant (k)

A
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13
Q

Units for rate constant

A
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14
Q

K value changes with

A

Temperature

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15
Q

Initial rates table

A
  • Using two experiments with only one change in reactants concentration. Order of a single reactant can be calculated by observing the change in rate
  • May have to ‘create’ and experiment on a new row to be able to work out the orders
    E.g double one reactant (with all others constant) that is first order, rate will double
  • To find k sub in values (from the first row of the table is easiest) into the overall rate equation
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16
Q

Which is the rate determining step?

17
Q

RDS intermediates, no of times species reactant appears, balanced equation

18
Q

Unimolecular and bimolecular reaction

19
Q

Intermediate can also be called

A

Transition state compound

20
Q

Causes of unimolecular or bimolecular reactions

21
Q

Measuring Reactions rate methods

22
Q

What does the Arrhenius Equation show

A

The relationship between rate constant, temperature and activation energy

23
Q

The Arrhenius Log graph

24
Q

The rate determining step (RDS)

25
Quenching
26
What does the Arrhenius exponential represent?
27
The Arrhenius Equation
28
Reactions constant/time method for determining rate equation
29
Graphing Arrhenius into y=mx+c
30
Oder of reaction
31
Rate constant definition
32
Suggesting a mechanism questions