Unit 1: Reaction Kinetics Flashcards

0
Q

The equation for rate is…

A

Change in amount of reactant or product/ change in time

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1
Q

Reaction kinetics is the study of…

A

The rate of reaction and the factors which effect the rate

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2
Q

Colour, temperature, pressure, mass, PH, conductivity, and concentration change are all examples of way you can measure…

A

Reaction rates

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3
Q

Name 7 examples of ways to measure reaction rates

A

Colour, temperature, pressure, mass, PH, conductivity, and concentration

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4
Q

Name six factors which effect the rate of a reaction

A
Temperature
Concentration
Surface area (heterogenous mixtures only)
Pressure (gasses)
Nature of reactants
Catalysts and inhibitors
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5
Q

The lower the temperature the _____ the reaction rate

A

Slower

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6
Q

The greater the temperature the _____ the reaction rate

A

Faster

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7
Q

Chemical reactions only occur when…

A

Collisions have enough energy to cause the atoms to rearrange

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8
Q

Only particles whose kinetic energy _____ the threshold energy have enough kinetic energy to _____.

A

EXCEEDS

React

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9
Q

Molecules to the left of the threshold may collide, but these collisions will not lead to….

A

The formation of products

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10
Q

Some particles that exceed the energy threshold still do not react because…

A

Of improper collision geometry

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11
Q

At lower temperatures _____ molecules have enough _____ to collide and _____ exceed the threshold

A

Few
Kinetic energy
Few

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12
Q

At _____ temperatures the entire molecules distribution shifts _____ which cause _____ molecules to exceed the threshold

A

Higher
Right
More

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13
Q

What two things are needed for particles to collide effectively and produce products?

A

needs to succeed threshold energy and have favourable collision geometry

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14
Q

As the concentration of a reactant increases the likelyhood that reactant molecules will collide ____ which translates into an _____ in reaction rate

A

Increases

Increase

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15
Q

The equation of the ideal gas law is..

A

Pressure (KPa) x volume=
n (# of moles) x gas constant
(8.31 KPa • L/mol - K) x Temperature (°K)

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16
Q

Volume and pressure are _____ proportional

A

Inversely

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17
Q

A pressure increase is equivalent to increase in ____ of gases

A

Concentration

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18
Q

When pressure is increased so is the likelihood that reactant molecules will _____.

A

Collide

increase in concentration= increase in collision frequency= increase in reaction rate

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19
Q

Nature of reactants is a factor which effects reaction rate because…

A

Some reactants are naturally more reactive than others

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20
Q

Some reactants are naturally more reactive than others because of…

A

Their chemical properties and their bonds involved in the chemical reaction

21
Q

The number and strength of ____ effects the reaction rate

22
Q

Surface area yields an increased reaction rate only when the reaction is _____.

A

Heterogenous (reaction where the reactants are in more than one phase)

23
Q

Catalysts increase the rate of reaction. What is a catalyst?

A

Catalysts are chemicals which increase the rate of a chemical reaction without itself undergoing permanent chemical change in the process

24
Inhibitors slow the rate of reaction. What is a inhibitor?
Inhibitors are chemicals which decrease the rate of a chemical reaction without itself undergoing permanent chemical change in the process
25
Instantaneous rate is found by
Finding the slope of the line tangent to the curve
26
All reactions ____ ____ over time
Slow down
27
The best indicator of the rate of a reaction is the instantaneous rate near the _____ of the reaction
Begining
28
Energy is ____ when bonds are formed
Released
29
Collisions have a variety of ____
Energies
30
In chemical reactions bonds are...
Broken and new ones are formed
31
As temperature increases the particles... (3 things)
Move faster Collide more often Collide with more energy
32
Matter consists of
Moving particles
33
You need a _____ to have a reaction
Collision
34
Collisions provide the ____ required to break bonds
Energy
35
Most collisions ___(are/are not) successful
Are not
36
The minimum amount of energy required for reaction is called...
Activation energy (Ea)
37
Reactions cannot occur unless the molecule possesses....
Sufficient energy to get over the activation energy barrier
38
What does a reaction coordinate diagram show?
A reaction coordinate diagram shows the energy of the reactants and products as a reaction proceeds
39
The high points on a reaction coordinate diagram are the ____ _____. The species present at this point are called ____ ____
Tradition states | Activated complexes
40
The energy gap between the reactants and the activated complex is the ....
Activation energy barrier
41
If change in H is positive the reaction is _____ If the change in H is negative the reaction is _____
Endothermic Exothermic
42
The _____ _____ is the actual sequence of steps which make-up the overall reaction
Reaction mechanism
43
Most reactions occur in ____ (1/>1 ) step
>1 | Most reaction require a sequence of steps
44
And elementary process is...
a one step reaction; only two particles involved
45
The slowest step in a reaction is...
The rate determining step
46
Almost any reaction having _____ reactant particles in a balanced equation will occur in more than one step
3 (or more)
47
Catalysts is a substance which provides an overall reaction with an _____ ____ which has a _____ activation energy
Alternative mechanism | Lower
48
When a catalyst is used the activation energy is lowered so more reactants will have enough kinetic energy to form _____ _____
Activated complexes
49
Catalysts increase the reaction rate for both the _____ and _____ reaction
Forward | Reverse
50
Phase effects the rate of reaction. Order the following phases from fastest reacting to slowest Gasses/ liquids, solids, aqueous ions
Aqueous ions>gasses/liquids> solids
51
Out of the 6 factors which effect reaction rate which one does not apply to homogenous substances
Surface area