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Chemistry 12 > Unit 1: Reaction Kinetics > Flashcards

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

A

Bonds

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
Q

Inhibitors slow the rate of reaction. What is a inhibitor?

A

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

25
Q

Instantaneous rate is found by

A

Finding the slope of the line tangent to the curve

26
Q

All reactions ____ ____ over time

A

Slow down

27
Q

The best indicator of the rate of a reaction is the instantaneous rate near the _____ of the reaction

A

Begining

28
Q

Energy is ____ when bonds are formed

A

Released

29
Q

Collisions have a variety of ____

A

Energies

30
Q

In chemical reactions bonds are…

A

Broken and new ones are formed

31
Q

As temperature increases the particles… (3 things)

A

Move faster
Collide more often
Collide with more energy

32
Q

Matter consists of

A

Moving particles

33
Q

You need a _____ to have a reaction

A

Collision

34
Q

Collisions provide the ____ required to break bonds

A

Energy

35
Q

Most collisions ___(are/are not) successful

A

Are not

36
Q

The minimum amount of energy required for reaction is called…

A

Activation energy (Ea)

37
Q

Reactions cannot occur unless the molecule possesses….

A

Sufficient energy to get over the activation energy barrier

38
Q

What does a reaction coordinate diagram show?

A

A reaction coordinate diagram shows the energy of the reactants and products as a reaction proceeds

39
Q

The high points on a reaction coordinate diagram are the ____ _____. The species present at this point are called ____ ____

A

Tradition states

Activated complexes

40
Q

The energy gap between the reactants and the activated complex is the ….

A

Activation energy barrier

41
Q

If change in H is positive the reaction is _____

If the change in H is negative the reaction is _____

A

Endothermic

Exothermic

42
Q

The _____ _____ is the actual sequence of steps which make-up the overall reaction

A

Reaction mechanism

43
Q

Most reactions occur in ____ (1/>1 ) step

A

> 1

Most reaction require a sequence of steps

44
Q

And elementary process is…

A

a one step reaction; only two particles involved

45
Q

The slowest step in a reaction is…

A

The rate determining step

46
Q

Almost any reaction having _____ reactant particles in a balanced equation will occur in more than one step

A

3 (or more)

47
Q

Catalysts is a substance which provides an overall reaction with an _____ ____ which has a _____ activation energy

A

Alternative mechanism

Lower

48
Q

When a catalyst is used the activation energy is lowered so more reactants will have enough kinetic energy to form _____ _____

A

Activated complexes

49
Q

Catalysts increase the reaction rate for both the _____ and _____ reaction

A

Forward

Reverse

50
Q

Phase effects the rate of reaction. Order the following phases from fastest reacting to slowest

Gasses/ liquids, solids, aqueous ions

A

Aqueous ions>gasses/liquids> solids

51
Q

Out of the 6 factors which effect reaction rate which one does not apply to homogenous substances

A

Surface area

Chemistry 12 (7 decks)

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