|
CEE 370 |
Fall 2010 |
Approximate Relative importance: Homeworks>Slides>Book
Mid-term exam covers lectures #1-22; topics below:
|
Topics |
Book |
Lecture# with advice on important slides/concepts[1] |
Date |
Home-work |
I. Introduction·
Environmental
Engineering Overview ·
Sources of
Information |
Chapter 1 |
Know significant figures General features of John
Snow’s story |
8 Sept |
|
|
·
Environmental
Legislation & Regulation |
Slides 2,4,5,11-14,18 |
10 Sept |
|
|
II. Environmental Chemistry·
Basics: Bonding
& definitions |
Chapter 2 |
Slides 4,7-9,11, pH |
13 Sept |
|
|
·
Units of
concentration ·
Reactions &
stoichiometry ·
Equilibrium |
Measures of concentration, Ideal gas law, stoichiometry, ThOD calculations |
15 Sept |
||
|
·
Kinetics ·
Water, soil
& air chemistry |
Slides 2-8,10-12,14, Debye Huckel Eq. |
17 Sept |
||
|
·
Thermodynamics ·
Acids &
Bases |
Slides 3,7,9-10,15-18,28,35,42-43,46,55 |
20 Sept |
||
|
·
Organic
Nomenclature |
Chemical names in slides 2-3, but don’t memorize the constants, slides 15,16,22,24-26,28-34 |
22 Sept |
|
|
III. Environmental Biology·
Microbiology
Basics |
Chapter 3 |
Slides 4-7, 9-10, don’t memorize exact structures |
24 Sept |
|
|
·
Bacterial and
microbial growth |
Slides 5-9, but don’t memorize structures, 13-14, 21 |
27 Sept |
|
|
|
·
Microbiology
& Biochemical pathways |
Slides 2-4,9,11,16,18,22,28,30-31,40,42,47 |
29 Sept |
|
|
|
·
Molecular
Biology |
Slides 3,5,8 (minus fine detail),9-12,13-22 (minus diagrams), 23-28 |
1 Oct |
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IV. Material & Energy Balance·
Basic
principles |
Chapter 4 |
Slides 3-6,8-12 |
4 Oct |
|
|
·
PFR, CMFRs |
Slides 3-4,8-10,15,19-21 |
6 Oct |
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|
·
Reactors &
reactor analysis |
Slides 3-9, 14 except for 2nd order reactor equations |
8 Oct |
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|
·
Reactors &
reactor analysis (cont.) |
Slides 11-12, know the 5 great lakes |
12 Oct |
|
|
V. Ecosystems·
Major
biogeochemical cycles |
Chapter 5 |
Slides 4-5 don’t memorize numbers, 6-7,11,17,22-23,25,34,36-46 |
13 Oct |
|
|
·
Growth & Population models |
Slides 2-4,9,11,17-19,21 |
15 Oct |
||
VI. Risk·
Perception
,Assessment Mgmt |
Chapter 6 |
Slides 4,6,9,18-19,21, know general story behind Milwaukee & Woburn |
18 Oct |
|
VII. Water Resources·
Definitions ·
Hydrologic
Cycle |
Chapter 7 |
Slides 3-4, 5-6 are repeats, 12-13,15 |
20 Oct |
|
|
·
Streams &
rivers ·
Advection &
Dispersion |
Rainfall concepts, gaging & flow measuring, slides 19-27, 31-32, 34 |
22 Oct |
|
|
|
·
Groundwater |
Slides 3-6 |
25 Oct |
|
|
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·
Groundwater;
Review for Exam |
Slides 2-8, 11-13 |
27 Oct |
|
Closed Book, one sheet of notes allowed
Conversions
7.48 gallon = 1.0 ft3 1 gal = 3.7854x10-3
m3
1 MGD = 694 gal/min =
1.547 ft3/s = 43.8 L/s
1 ft3/s = 449
gal/min
g = 32 ft/s2
W= = 62.4 lb/ft3 = 9.8 N/L
1 hp = 550 ft-lbs/s = 0.75 kW
1 mile = 5280 feet 1 ft = 0.3048 m
1 watt = 1 N-m/s
1 psi pressure = 2.3 vertical feet of water (head)
At 60 ºF, ν = 1.217 x 10-5 ft2/s
Selected Chemical Constants
|
Element |
Symbol |
Atomic # |
Atomic Wt. |
|
Electronegativity |
|
|
Aluminum |
Al |
13 |
26.98 |
3 |
1.47 |
|
|
Boron |
B |
5 |
10.81 |
3 |
2.01 |
|
|
Calcium |
Ca |
20 |
40.08 |
2 |
1.04 |
|
|
Carbon |
C |
6 |
12.01 |
2,4 |
2.50 |
|
|
Chlorine |
Cl |
17 |
35.453 |
1,3,5,7 |
2.83 |
|
|
Chromium |
Cr |
24 |
52.00 |
many |
1.56 |
|
|
Helium |
He |
2 |
4.00 |
0 |
|
|
|
Holmiuum |
Ho |
67 |
164.93 |
3 |
1.10 |
|
|
Hydrogen |
H |
1 |
1.01 |
1 |
2.20 |
|
|
Magnesium |
Mg |
12 |
24.31 |
2 |
1.23 |
|
|
Manganese |
Mn |
25 |
54.94 |
2,3,4,6,7 |
1.60 |
|
|
Nitrogen |
N |
7 |
14.01 |
many |
3.07 |
|
|
Oxygen |
O |
8 |
16.00 |
2 |
3.50 |
|
|
Potassium |
K |
19 |
39.10 |
1 |
0.91 |
|
|
Sodium |
Na |
11 |
22.99 |
1 |
1.01 |
|
|
Sulfur |
S |
16 |
32.06 |
2,4,6 |
2.44 |
|
Selected Acidity Constants (Aqueous Solution, 25°C, I = 0)
|
NAME |
FORMULA |
pKa |
|
|
Hydrochloric acid |
HCl = H+ + Cl- |
-3 |
|
|
Sulfuric acid |
H2SO4= H+ + HSO4- |
-3 |
|
|
Nitric acid |
HNO3 = H+ + NO3- |
-0 |
|
|
Bisulfate ion |
HSO4- =
H+ +
SO4-2 |
2 |
|
|
Phosphoric acid |
H3PO4 = H+ + H2PO4- |
2.15 |
|
|
Hydrofluoric acid |
HF = H+ + F- |
3.2 |
|
|
Nitrous acid |
HNO2 = H+ + NO2- |
4.5 |
|
|
Acetic acid |
CH3COOH = H+ + CH3COO- |
4.75 |
|
|
Propionic acid |
C2H5COOH = H+ + C2H5COO- |
4.87 |
|
|
Carbonic acid |
H2CO3 = H+ + HCO3- |
6.35 |
|
|
Hydrogen sulfide |
H2S = H+ + HS- |
7.02 |
|
|
Dihydrogen phosphate |
H2PO4- =
H+ + HPO4-2 |
7.2 |
|
|
Hypochlorous acid |
HOCl = H+ + OCl- |
7.5 |
|
|
Ammonium ion |
NH4+ =
H+ + NH3 |
9.24 |
|
|
Hydrocyanic acid |
HCN = H+ + CN- |
9.3 |
|
|
Phenol |
C6H5OH = H+ + C6H5O- |
9.9 |
|
|
Bicarbonate ion |
HCO3- =
H+ + CO3-2 |
10.33 |
|
|
Monohydrogen phosphate |
HPO4-2
= H+ + PO4-3 |
12.3 |
|
|
Bisulfide ion |
HS- = H+
+ S-2 |
13.9 |
|
[1] I’ve listed slides by number within each lecture as they are currently (Oct 20) posted on the CEE 370 website (http://www.ecs.umass.edu/cee/reckhow/courses/370/sched.htm). I generally don’t list example problems, because the specifics of these aren’t too important. They are useful, however, in learning to apply the important concepts. This is my best general assessment, but it isn’t perfect. There may be a few questions on topics not listed among the most important slides.