Chem. 102, Spring 2014
Fundamentals of Chemistry: II
Environmental and Physical Chemistry
section A01/A04
Instructor: Prof. Rob Lipson
[email protected]
Time and Place:
M & R: 8:30 - 9:50 am
SCI B150
Prerequisites:
1. Chem. 101 and BC Chem. 12 from high school
(or Chem. 091 or equivalent)
2. Must be registered in a lab
Resources
• Instructor: Dr. Rob Lipson, Office:
Elliott 166. Office hours: make an
appointment with me by email
([email protected]).
• Course website
http://web.uvic.ca/~chem102/index.html
• **Section website:
http://web.uvic.ca/~rlipson/C102-2014/
• Drop-in Centre: Elliott second floor
lobby. Will open week of Jan 15th.
Please register your clickers for C102 if you
haven’t done so as yet.
Direct all your administrative questions about
course and Mastering Chemistry to the Course
Coordinator Prof. Sandy Briggs
[email protected]
Office Elliott 313
Be sure that you are registered in a lab section
as soon as possible.
Labs start the week of January 13th.
Direct all your administrative questions about
labs to the Senior Lab Instructor for First-Year,
Monica Reimer
[email protected]
Office Elliott 228
Chem 102
15
Learning objectives
At the end of this course you will be able to:
 Explain how the energy transfers in all forms (E, S, H, G) and rates of reactions
affect interconnected environmental processes.
 Apply the ideal gas law to calculate the properties of gases under a variety of
conditions
 Describe the kinetic-molecular theory and explain the difference between real
and ideal gases
 Describe the chemistry of the atmosphere in terms of equilibria and
energetically favored reactions.
 Interpret a phase diagram and explain the molecular basis for vapor pressure
 Identify the factors that affect the rate of a chemical reaction and use rate
law expressions to quantify rates
 Use the collision model to explain how the rate of a reaction depends on
temperature.
 Employ equilibrium constant expressions to predict the direction of a reaction,
the concentrations of species at equilibrium or the value of the equilibrium
constant
 Apply the laws of thermodynamics to determine whether the reactants or
products of a chemical reaction are favored.
 Explain how enthalpy is related to internal energy and PV work and how these
concepts characterize reaction properties
 Explain entropy in terms of heat transfer and at the molecular level.
 Relate free energy to the equilibrium constant
 Summarize the interacting processes that affect the chemistry of water in the
hydrosphere.
After one term of Chemistry I now
intend to major in:
A. Chemistry (What else?)
B. The Biological Sciences (Biology,
Biochemistry & Microbiology)
C. The Physical Sciences (Physics &
Astronomy; Earth & Ocean Sciences)
D. Mathematics & Statistics
Chapter 8
Gases
•
Pressure
•
Gas Laws
•
Ideal Gas Equation
•
Gas Mixtures and
Partial Pressures
•
Kinetic-Molecular
Theory
•
Real Gases: Deviations
from Ideal Behavior
8.1 Characteristic of Gases
Physical properties of gases similar for all compounds and atoms
Properties can understood in terms of molecular behavior.
So many of the properties of matter, especially when in the gaseous form, can be
deduced from the hypothesis that their minute parts are in rapid motion, the
velocity increasing with the temperature, that the precise nature of this motion
becomes a subject of natural curiosity. James Clark Maxwell, (1831-1879)
Gases differ importantly from liquids and solids
• expand to fill the container
• volume changes with pressure (compressible)
• form homogeneous mixtures regardless of chemical makeup
air: 78% N2, 21% O2, Ar, CO2, Ne, He, CH4
Why? gas molecules are far apart – gas is mostly empty space
density of N2:
gas 1.25 g/L (at 20 ºC and 101 kPa)
liquid = 808 g/L (at -196 ºC and 101 kPa)
solid = 1020 g/L (at -210 ºC and 101 kPa)
8.2 Pressure
F
Pressure, P, is the force, F, that acts on a given area, A. P 
A
Recall that force = mass x acceleration
pressure units = (kg  m s-2)/ (m2) = N m-2 = 1 pascal = 1 Pa
Newton
Gases exert a pressure on any surface
they contact.
Why?
gas molecules are constantly colliding
with the surface; i.e., applying a force to
the surface with each collision
The walls of the container
are the surfaces
experiencing force.
Measuring pressure
column height measures
Patm in mm of Hg
Barometer: measures
Patm = Pvacuum + Ph
average atmospheric pressure at
sea level = 760 mm Hg
Units: 1 atm = 760 mm Hg
= 760 torr = 101.325 kPa
Manometer: compares pressure of a sample
gas to atmospheric pressure
when Pgas > Patm
Pgas = Patm + Ph
0
Pressure at lowest point in one
arm must be equal to pressure
at that point in other arm.
if Pgas < Patm
Ph + Pgas = Patm