Maxwell Boltzmann Distribution and rate curves Flashcards

1
Q

What do Maxwell Boltzmann distribution curves show?

A

how energy is distributed amongst gas particles

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

Why does the curve go through the origin?

A

as no particle has zero energy

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

What is the total area under the curve?

A

the total number of molecules

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

What goes on the x and y axis?

A

number of particles- y axis
kinetic energy- x axis

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

What is N.m.p?

A

number of particles with the most probable energy

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

What is E.m.p and where is it on the graph?

A

most probable energy, marked on x axis at the highest point of the curve

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

What is E.mean, where is it in relation to E.m,p?

A

the mean energy of the particles, and is just after the E.m.p

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

What is the shaded area of the graph right at the very end?

A

the Ea (activation energy)

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

What happens to the shaded area of particles with Ea when a catalyst is used?

A

the line moves back the graph, showing more particles have Ea

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

How does the shape of the curve change when there is a lower temperature?

A

the curve peaks higher and earlier, but comes down more steeply and to a lower point

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

Why does the shape of the curve change when there is a lower temperature?

A

at lower temperature there are fewer higher energy particles and more lower energy particles, so fewer particles have activation energy above the activation energy, so fewer successful collisions hence the slower the rate. lower temp= lower E.m.p

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

How does the shape of the curve change when there is a higher temperature?

A

the curve peaks lower and later, but comes down less steeply and to a higher point

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

Why does the shape of the curve change when there is a higher temperature?

A

at higher temperature there are more higher energy particles and fewer lower energy particles, and at higher temperature there are more particles with energy above the activation energy so more successful collisions hence the faster rate. higher temp= higher E.m.p

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

How do you calculate rate? (mol dm-3 s-1)

A

change in conc / change in time

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

Why is rate fastest at the start of a reaction?

A

more particles per unit volume, so most frequent successful collisions per second at the start

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

What happens as time progresses?

A

rate decreases as reactant particles get used up, so fewer successful collisions per second

17
Q

What do the curves look like with a powder vs a granule?

A

both reach same conc/vol, but powder has a steeper initial rate than granules

18
Q

What do the curves look like for granules, where one has a higher temp?

A

both reach same conc/vol, but one with higher temp has a steeper initial rate