CEE 370

Fall 2010

 

Study Guide for Mid-term Exam

 

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

1

Know significant figures

General features of John Snowís story

8 Sept

 

         Environmental Legislation & Regulation

2

Slides 2,4,5,11-14,18

10 Sept

 

II. Environmental Chemistry

         Basics: Bonding & definitions

Chapter 2

3

Slides 4,7-9,11, pH

13 Sept

 

         Units of concentration

         Reactions & stoichiometry

         Equilibrium

4

Measures of concentration, Ideal gas law, stoichiometry, ThOD calculations

15 Sept

#1

         Kinetics

         Water, soil & air chemistry

5

Slides 2-8,10-12,14, Debye Huckel Eq.

17 Sept

#2

         Thermodynamics

         Acids & Bases

6

Slides 3,7,9-10,15-18,28,35,42-43,46,55

20 Sept

#3

         Organic Nomenclature

7

Chemical names in slides 2-3, but donít memorize the constants, slides 15,16,22,24-26,28-34

22 Sept

 

III. Environmental Biology

       Microbiology Basics

Chapter 3

8

Slides 4-7, 9-10, donít memorize exact structures

24 Sept

 

         Bacterial and microbial growth

9

Slides 5-9, but donít memorize structures, 13-14, 21

27 Sept

 

         Microbiology & Biochemical pathways

10

Slides 2-4,9,11,16,18,22,28,30-31,40,42,47

29 Sept

 

         Molecular Biology

11

Slides 3,5,8 (minus fine detail),9-12,13-22 (minus diagrams), 23-28

1 Oct

 

IV. Material & Energy Balance

         Basic principles

Chapter 4

12

Slides 3-6,8-12

4 Oct

#4

         PFR, CMFRs

13

Slides 3-4,8-10,15,19-21

6 Oct

       Reactors & reactor analysis

14

Slides 3-9, 14 except for 2nd order reactor equations

8 Oct

       Reactors & reactor analysis (cont.)

15

Slides 11-12, know the 5 great lakes

12 Oct

 

V. Ecosystems

       Major biogeochemical cycles

Chapter 5

16

Slides 4-5 donít memorize numbers, 6-7,11,17,22-23,25,34,36-46

13 Oct

 

         Growth & Population models

17

Slides 2-4,9,11,17-19,21

15 Oct

#5

VI. Risk

         Perception ,Assessment Mgmt

Chapter 6

18

Slides 4,6,9,18-19,21, know general story behind Milwaukee & Woburn

18 Oct

 

VII. Water Resources

         Definitions

         Hydrologic Cycle

Chapter 7

19

Slides 3-4, 5-6 are repeats, 12-13,15

20 Oct

 

         Streams & rivers

         Advection & Dispersion

20

Rainfall concepts, gaging & flow measuring, slides 19-27, 31-32, 34

22 Oct

 

         Groundwater

21

Slides 3-6

25 Oct

 

         Groundwater; Review for Exam

22

Slides 2-8, 11-13

27 Oct

 

 


 

Instructions provided with Exam

 

Closed Book, one sheet of notes allowed

 

 

 

Special information provided with Exam

 

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 ļF, ν = 1.217 x 10-5 ft2/s††

 

Selected Chemical Constants

Element

Symbol

Atomic #

Atomic Wt.

Valence

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, 25įC, 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] Iíve 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 donít list example problems, because the specifics of these arenít too important.They are useful, however, in learning to apply the important concepts.This is my best general assessment, but it isnít perfect.There may be a few questions on topics not listed among the most important slides.