Download presentation

Presentation is loading. Please wait.

Published byDarin Fennel Modified over 2 years ago

1
Is this your room/ Then you already know about entropy

2
Using a simple approach, Define entropy as a measure of disorder. A system (such as a room) is in a state of high entropy when its degree of disorder is high. As the order within a system increases, its entropy decreases.

3
For better or for worse, nature 'likes' chaos, disorder, high entropy... In fact, much of our life consists in fighting this disorder! A system (such as a room) is in a state of high entropy when its degree of disorder is high.

4
This can be explained in terms of probabilities. Disordered states are simply more likely to exist (or emerge) than ordered states. The spontaneous direction of change is from a less probable to a more probable state, as illustrated above. 2 20 ways to arrange?

5
In general Gases have higher entropies than liquids. Liquids have higher entropies than solids.

6
Also … Entropy is greater for larger atoms. Entropy is greater for molecules with more atoms.

7
Examples Ar has higher entropy than Ne as Ar molecules are larger. C 8 H 18(l) has higher entropy than C 5 H 12(l) as complex molecules have higher entropy than simple ones. Br 2(g) has higher entropy than Br 2(l) as gases have higher entropies than liquids since gases have more ways of being arranged

8
Entropy (CI 4.3) Liquids mix because there are more ways of being mixed than unmixed. i.e. disorder increases. Note that: not all liquids mix; e.g. water does not mix with oil, because the forces of attraction between water molecules are stronger than the forces of attraction between oil molecules they do not mix They are immiscible

9
On to CI 4.4 AS – entropy is a measure of the number of ways particles can be arranged. A2 – entropy is a measure of the number of ways quanta (packages of energy) can be arranged.

10
What happens to electrons? 1 2 3 4 Electrons absorb quanta of energy Electrons are excited Electrons move to higher energy level E = h v

11
Molecules are made of more than one atom but they still have electrons. Electronic transitions Vis + UV

12
Molecules move !

13
There are vibrational energy levels as well as electronic energy level.. I.R.

14
There are rotational energy levels as well as electronic energy level.. microwave

15
Electronic transitions Vis + UV Rotational transitions Vibrational transitions Microwave I.R.

16
EV R T

17
EV R T

18
On to CI 4.4 AS – entropy is a measure of the number of ways particles can be arranged. A2 – entropy is a measure of the number of ways quanta (packages of energy) can be arranged.

19
4 quanta – 2 molecules Molecule 1Molecule 2 04 13 22 31 40 5 ways

20
6 quanta – 2 molecules? More quanta Molecule 1Molecule 2 5 7 more ways

21
4 quanta – 2 molecules Molecule 1Molecule 2 04 13 22 31 40 5 ways

22
4 quanta – 3 molecules Molecule 1Molecule 2Molecule 3 More molecules 5 15 More ways

23
On to CI 4.4 AS – entropy is a measure of the number of ways particles can be arranged. A2 – entropy is a measure of the number of ways quanta (packages of energy) can be arranged. Entropy greater if more quanta (heat it) Entropy greater if more molecules

24
Bigger atoms/molecules have more entropy?

25
EV R T EV R T EV R T

Similar presentations

OK

* Studying energy flow in chemical changes allows us to predict what is possible and what is not. * 1 st Law of Thermodynamics PE tends only to decrease.

* Studying energy flow in chemical changes allows us to predict what is possible and what is not. * 1 st Law of Thermodynamics PE tends only to decrease.

© 2017 SlidePlayer.com Inc.

All rights reserved.

Ads by Google

Ppt on ideal gas law examples Ppt on cloud computing download Ppt on 60 years of indian parliament news Ppt on personality development for mba students Seminar ppt on blackberry technology Download ppt on conservation of fossil fuels Ppt on centring definition Ppt on conservation of environment images Ppt on holographic technology in education Ppt on congruence of triangles class 8