Brainscape's Knowledge GenomeTM

Browse over 1 million classes created by top students, professors, publishers, and experts.


See full index

Physical Chemistry > 3.1.5 Kinetics > Flashcards

3.1.5 Kinetics Flashcards

1
Q

What is rate of reaction?

A

Rate of reaction is the change in the amount of reactant or product over time

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
2
Q

What does collision theory state

A

Reaction won’t take place between two particles unless the conditions are correct

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
3
Q

What are the conditions in collision theory which allow reactions to take place (direction)?

A

Particles need to collide in the right direction (facing each other the right way)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
4
Q

What are the conditions in collision theory which allow reactions to take place (energy)?

A

Particles need to collide with at least a certain minimum amount of kinetic energy (activation energy)

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
5
Q

Define activation energy

A

The minimum amount of kinetic energy particles need to react

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
6
Q

What is activation energy needed for

A

this much energy is needed to break the bonds within reactant particles to start the reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
7
Q

How easily do reactions with low activation energies happen

A

Reactions with low activation energies often happen easily

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
8
Q

How easily do reactions with high activation energies happen

A

Reactions with high activation energies don’t happen easily

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
9
Q

Why does a Maxwell Boltzmann graph start at (0,0)

A

Because no molecules have zero energy

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
10
Q

What does the peak of the curve on a Maxwell Boltzmann graph represent

A

Peak of the curve represents the most probable energy (Emp) of any single molecule

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
11
Q

What does just right of the peak of a Maxwell Boltzmann graph show?

A

Mean average energy of all the molecules is a bit to the right of the peak

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
12
Q

What does the area under a Maxwell Boltzmann distribution curve show

A

Area under a Maxwell Boltzmann distribution curve is equal to the total number of of molecules

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
13
Q

How does temperature affect rate of reaction?

A

Increasing the temperature, increases rate of reaction

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
14
Q

What happens to the proportion of molecules with at least the activation energy when temperature is increased

A

Greater proportion of molecules will have at least the activation energy and be able to react

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
15
Q

What happens when you increase temperature in terms of energy

A

If you increase temperature, the molecules will on average have more kinetic energy and will move faster

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
16
Q

What happens to molecules due to their increase in kinetic energy after a temperature increase

A

The molecules will be moving around quicker so they will collide more often

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
17
Q

How will increasing temperature affect the shape of the Maxwell Boltzmann distribution curve?

A

Increasing temperature will push the Maxwell Boltzmann distribution curve over to the right

How well did you know this?
1
Not at all
2
3
4
5
Perfectly
18
Q

How will decreasing temperature affect the shape of the Maxwell Boltzmann distribution curve?

A

Decreasing temperature will the push the Maxwell Boltzmann distribution curve over to the left

19
Q

Does changing temperature change the area under the Maxwell Boltzmann distribution curve?

A

No as number of molecules stays the same

20
Q

Does changing temperature change the activation energy

A

Changing temperature doesn’t change the activation energy

21
Q

How does increasing temperature affect the most probable energy

A

Increasing temperature increases the most probable energy

22
Q

How does decreasing temperature affect the most probable energy

A

Decreasing temperature will decrease the most probable energy

23
Q

How does concentration affect rate of reaction

A

Increasing concentration will increase rate of reaction

24
Q

What does increasing concentration do to how close particles are together

A

If you increase the concentration of reactants in a solution, the particles will on average be closer together

25
Q

What happens as a result of particles being closer together

A

If particles are closer together, collisions are more frequent

26
Q

What happens if collisions are more frequent

A

If collisions are more frequent, there will be more chances for particles to react so rate of reaction increases

27
Q

How does changing concentration affect activation energy value

A

Changing concentration doesn’t change activation energy value

28
Q

How does changing concentration affect most probable energy value

A

Changing concentration doesn’t change most probable energy value

29
Q

How does increasing concentration affect area under the Maxwell Boltzmann distribution curve?

A

Increasing concentration increase area under Maxwell Boltzmann distribution curve
If concentration is doubled, so will the area

30
Q

How does decreasing concentration affect area under Maxwell Boltzmann distribution curve

A

Decreasing concentration decreases area under Maxwell Boltzmann distribution curve
If concentration is halved, so will the area

31
Q

How does increasing concentration affect the number of molecules with energies above activation energy

A

Increasing concentration increases molecules available to collide in a given volume. Will also be more molecules with energies above the activation energy

32
Q

How does increasing temperature affect the number of molecules that have at least the activation energy

A

At higher temperatures, more molecules have at least the activation energy

33
Q

How does changes in pressure affect rate of reaction

A

Changes in pressure affect rate of reaction the same way as changes in concentration

34
Q

What can you use catalysts to do?

A

You can use catalysts to make chemical reactions happen faster

35
Q

What does a catalyst do to rate of reaction

A

A catalyst increases the rate of a reaction

36
Q

How does a catalyst increase rate of reaction

A

Catalyst increases rate of reaction by providing an alternative reaction pathway with a lower activation energy

37
Q

Do catalysts get used up in reactions

A

Catalysts don’t get used up in the reaction

38
Q

Do catalysts take part in reactions

A

Catalysts do take part in reactions but are remade at the end of

39
Q

Why does lowering activation energy increase rate if reaction

A

More particles with enough energy to react when they collide so in a set time for particles react

40
Q

Does adding a catalyst change the shape of the Maxwell Boltzmann distribution curve?

A

Maxwell Boltzmann distribution curve is unchanged as molecules still have the same amount of energy

41
Q

Does adding a catalyst change the activation energy

A

Adding a catalyst lowers the activation energy, so shifts it to the left on a Maxwell Boltzmann distribution curve

42
Q

How do you work out rate of reaction?

A

(Amount of reactant used or product formed) / (time)

43
Q

How does increasing pressure increase rate of reaction

A

Increasing pressure pushes all of the gas particles closer together so increases the number in a given volume, this increases the frequency of collisions and so also rate of reaction

Physical Chemistry (5 decks)

Brainscape helps you reach your goals faster, through stronger study habits.
© 2025 Bold Learning Solutions. Terms and Conditions