CEE 370 |
Fall 2006 |
October 16, 2006
Closed Book, one sheet of notes allowed
Please answer any 4 of the following 9 questions. Each is worth 25 points. Show all work. Be neat, and box-in your answer.
The balanced stoichiometric equation is:
The ThOD is then:
The balanced stoichiometric equation is:
The ThOD is then:
The balanced stoichiometric equation is:
The ThOD is then:
Chemical Substance |
Conc. (mg/L) |
GFW |
Conc.
(mM) |
Conc.
(meq/L) |
Na+ |
12.5 |
22.9898 |
0.5437 |
0.5437 |
K+ |
1.1 |
39.0983 |
0.0281 |
0.0281 |
Ca+2 |
39.3 |
40.0800 |
0.9805 |
1.9611 |
Mg+2 |
3.5 |
24.3050 |
0.1440 |
0.2880 |
NO3- |
8.8 |
62.0049 |
0.1419 |
0.1419 |
SO4-2 |
12.4 |
96.0576 |
0.1291 |
0.2582 |
Cl- |
33.9 |
35.4530 |
0.9562 |
0.9562 |
HCO3- |
112.3 |
61.0171 |
1.8405 |
1.8405 |
TDS = 224 or 112 mg/L
Ionic Strength = 4.3 mM
Location |
Q (cfs) |
Chloride (mg/L) |
1 (main inflow) |
15 |
2 |
2 (side inflow) |
3 |
6 |
3 (side outflow) |
??? |
??? |
4 (main outflow) |
17 |
??? |
Mass Balance on Water across the entire system
Mass Balance on chloride for the system:
Recognize that we’re dealing with a conservative substance. This means that the chloride doesn’t decay. For this reason, the concentration will be constant downstream of the last input. Thus, c3 = c4.
Time (min) |
Concentration (µM) |
k (min-1) |
|
ti-1 to ti |
t0 to ti |
||
0 |
100 |
|
|
50 |
22 |
0.03028 |
|
100 |
5 |
0.02996 |
0.02963 |
Average: |
0.03012 |
|
or
So:
And we can do this several ways, as there are three sets of paired C-t data. While there is some varability among these it is rather small, and the rate constant can be said to be about
k = 0.030 min-1 = 5x10-4 sec-1
1. |
T |
The
Arrhenius equation allows one to adjust rate constants from one temperature
to another |
2. |
F |
A triprotic
acid has three times the strength as a monoprotic acid |
3. |
T |
A conjugate
base is what forms when an acid losses a proton |
4. |
T |
When an
organic compound name ends in “ol”, it usually means the compound is an
alcohol |
5. |
T |
Catalysts
accelerate chemical reactions by lowering the activation energy |
6. |
F |
When Gibbs
Free Energy increases, the reaction will tend to go forward |
7. |
T |
Alkynes all
have triple bonds |
8. |
T |
Henry’s law
describes the relationship between partial pressure and dissolved
concentration |
9. |
F |
BTEX is a
new type of dog food |
10. |
T |
Changes in
ionic strength can cause shifts in chemical equilibria |
11 |
F |
An element
of high electronegativity will share its bonding electrons equally with an
element of low electronegativity |
12 |
F |
Biochemical
oxygen demand (BOD) differs from theoretical oxygen demand (ThOD) in that BOD
only refers to oxygen demand from pharmaceuticals |
Since I give you a half-life, its reasonable to assume this is a first order process, so
And for 1st order reactions:
Which gives us:
≈125 days
HCO3- = CO3-2 + H+
The equilibrium expression for this reaction is:
So:
And therefore:
Thus:
And recognizing that at such a high pH, virtually all of the carbonate are in the form of bicarbonate and carbonate (i.e., there is essetially no carbonic acid):
Or HCO3-/total carbonate ≈ 6.3%
This is a redox (reduction-oxidation) reaction, so the electron transfer must be balanced. This requires that we first separate out the two half reactions,
First the oxidation half reaction we have carbon becoming oxidized:
Next, dichromate must be the substance that is reduced (i.e., it does the oxidizing of the butyric acid). We’re also told that an end product is Cr+3. So the reduction half reaction is:
Then combine to balance the overall equation:
3 x ()
10 x ()
Or
Next calculate the mass requirements
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 |
|