Chemistry 0110, Spring Term 2008 – Dr. Michael’s section
Study Outline for the second Exam, 3/21/08
Study Outline:
The exam covers Chapters 5-8: the quiz will consist of 10 multiple choice questions and about 5
problems and/or questions.
On these last 5 problems, you will need to show your numerical
work or, as appropriate, use sentences and/or annotated diagrams to answer the questions.
There will be more questions/points related to Chapters 7 and 8 than to Chapters 5 and 6.
Chapter 5: The Gaseous State
Know the SI units related to this chapter – pressure, temperature, volume, energy, momentum,
etc.
You need to know the Ideal Gas Law (PV=nRT) and know how to rearrange it to deduce the
empirical gas laws: Boyle’s, Charles’s, Combined Gas Law, Avagadro’s Law.
Be able to perform calculations with Gas Laws (YES, ou will be given the gas constant and its
units).
Solve stoichiometric problems involving gas volumes.
Understand gas mixtures and
partial pressures.
Be able to explain and use the Kinetic-Molecular Theory.
Calculate rms
molecular speeds.
Understand diffusion and effusion.
Know the differences between ideal and
real gasses.
Additional recommended problems:
63, 67, 69, 75, 79, 85, 87, 89.
You should move on to the
general and cumulative-skills questions when you are ready to study for the second exam.
The gas laws will not be provided.
You do not need to know each individual one, but you
do need to know the Ideal Gas Law itself (PV=nRT) and how to use it to derive other gas
laws.
Boyles Law:
PV = a constant
Boyle’s Law works when the amount and temperature of the ideal gas are fixed.
Boyles Law indicates that pressure times the volume is a constant: this leads to two other forms
of the Law:
V
const
P
=
,
which shows that pressure and volume are inversely proportional to each other
2
2
1
1
V
P
V
P
=
, i.e. that as the pressure and/or volume of the ideal gas sample is changed, the
product of pressure and volume holds constant.