26 Gases - I
This is the first of a number of lectures on the properties of gases. The kinetic molecular theory is introduced. The idea that gases exert pressure is an important concept that sets gases apart from other forms of matter. Boyle's law (variation of volume with pressure) is introduced and demonstrated.
ppt-26     Chap.9    A-09  Gases

27 Gases II
More on Boyle's law, especially how it is not perfect due to the fact that gas molecules actually do interact with one another. Charles law (expansion of a gas with increasing temperature) is introduced and demonstrated. Along with Avogadro's law (volume is proportional to the number of moles of gas), these can be combined into a "Universal"gas law, the "Ideal Gas Law".
ppt-27     Chap.9    A-09  Gases

28 Gases III
Several examples of how to use the ideal gas law are presented. Some examples of the importance of gas denity are given. Dalton's law of partial pressures is explained, as is the idea of "mole fractions".
ppt-28     Chap.9    A-09 Gases

29 Gases IV
The effect of pressure on the position of the equilibrium in a gas phase reaction is shown to depend on the number of moles of gas on each side of the reaction. The effect of temperature on an exothermic reaction is also shown. Together, these two effects can be used to predict the optimum conditions for a particular reaction (e.g. the synthesis of ammonia). An introduction to molecular speed is given.
ppt-29     Chap.9    A-09  Gases

30 Gases V
Calculations of gas particle velocity distributions show that lighter species have larger velocities and a wider range of velocities. There is thus the chance that light species such as hydrogen can escape from the atmosphere, altering the atmospheric chemistry over time. Effusion, diffusion and Graham's Law are explained. A practical use of the different diffusion rates of species is enrichment of uranium hexafluoride. Some other interesting material related to gases is presented.
ppt-30     Chap.9    A-09 Gases

31 Gases VI - Non-Ideal Gases, The Atmosphere
The first portion of the lecture is a quick look at how the ideal gas law can be improved to take account of molecular interactions and molecular sizes. This is done using the van der Waals' equation.

The first portion of a discussion of the chemistry of the atmosphere is presented. The chemistry of the ozone layer and reasons for its apparent destruction are described.
ppt-31     Chap.9    A-09 Gases

32 Gases VII - The Atmosphere
The problem of global warming is explained from the point of view of chemistry. The scale on which we pollute the atmosphere is shown to be fantastically large. The chemistry of smog (and hence ground level ozone) is explained.
ppt-32     Chap.9    A-09 Gases

33 Gases VIII - The Atmosphere
The chemistry of photochemical smog is explained. Some chemical aspects of acid rain and its effects on us are described.

The lecture finishes with a few interesting points about gases. Specifically, thje liquefaction of gases is explained, since we will be looking at the liquid phase in the second term. The chemistry of airbags is outlined, and the physical chemistry behind the use of gases for refrigeration is explained.
ppt-33     Chap.9    A-09 Gases