101/111
1st Chemistry Hour Examination
October 12, 2007 1a
CHEMISTRY 101/111, FALL 2007 First Hour Examination
DO NOT BEGIN TO WORK ON THE EXAMINATION UNTIL THE PROCTOR TELLS YOU TO DO SO! INSTRUCTIONS: Before you begin the examination, please fill-in the identification information requested on the answer sheet. You must use a No. 2 pencil to fill in this information. In the STUDENT ENROLLMENT SHEET section of the form, fill in the I.D. NUMBER (your person number, format = 12345678--, i.e., left adjusted with two blank spaces on the right), NAME (your last name, first name, M.I.), and CODE (your recitation section code, format = ab) fields. Be sure to fill in the correct circles completely. Your examination score cannot be credited to the correct person if the computer cannot read the bubbled in information. In the SCORE SHEET section of the form, sign your name on the line for NAME. +
#2
=
For each question you are to fill in the circle on the answer sheet that corresponds to the BEST answer. Make sure the answer number used is the same as the question number! Use a No. 2 pencil; make heavy marks that fill-in the circle; erase completely any answer you wish to change. Questions with more than one answer marked will be graded as incorrect. The only answers that will be accepted are those which appear on the bubble sheet. . The examination consists of 26 questions, each of which bears 4 points. (The last question is a "bonus" question.) Check that you have a complete examination (9 pages). Please place your name on the top of every page. Do not leave any answers blank - guess if you don't know. Do not make any stray marks on the answer sheet! Use the space between the problems on the examination pages for your scratch work. Raise your hand if you have a question or need a pencil.
PLEASE READ AND THEN SIGN THE ACADEMIC HONESTY STATEMENT BELOW. I hereby certify that the answers given to this examination represent my own unaided work. Signature ___________________________________ Key A, Person Number __ __ __ __ - __ __ __ __ Printed Name ___________________________________ first last Recitation Section Code __ __
THIS FORM MUST BE TURNED IN WITH YOUR ANSWER SHEET AT THE END OF THE EXAMINATION OR THE ANSWER SHEET WILL NOT BE GRADED.
Chemistry 101/111
1st Hour Examination
October 12, 2007 2a
1.
What is the correct answer (using the rules for "significant figures") to the expression:
(18 + 95) x (0.077351)?
A. B. C. D. E. 2. 8.7 8.74 8.741 8.7406 8.74066
Which of the following pairs of symbol & element is correct? A. Ca B. Fl C. K D. Ir E. Co carbon fluorine potassium iron copper
3.
Which could not be used to physically separate the components of a mixture? A. distillation B. chromatography C. filtration D. fractional crystallization E. combustion
4.
Bromine (Br2) is a red-brown liquid. What is its density (in g/mL) if 586g of bromine occupies 188 mL A. B. C. D. E. 776 g/mL 398 g/mL 6.24 g/mL 3.12 g/mL 0.312 g/mL
Chemistry 101/111 5.
1st Hour Examination
October 12, 2007 3a
A rectangular-sided block has measurements of 5.000 in x 7.000 in x 10.000 in. What is the volume of this block in cm3 ? (1 in = 2.54 cm exactly) A. B. C. D. E. 21.36 350.0 889.0 2258. 5735.
6.
An atom has a mass of 3.90 x 10-22 g. What is its mass in atomic mass units (amu)? A. B. C. D. E. 6.5 23.5 65 117 235
7. Naturally occurring copper consists of two isotopes: Cu (mass 62.93 amu) and Cu (mass 64.93 amu). The average atomic weight determined for copper is 63.548. What is the % 63 abundance of Cu A. B. C. D. E. 69.1 77.1 30.9 40.8 61.3
63
65
8.
Which of the following is an ionic compound? A. B. C. D. E. CO AlN HCl SiCl4 NH3
Chemistry 101/111
1st Hour Examination
October 12, 2007 4a
9.
Which of the following name-formula pairs is not correct? A. B. C. D. E. Sulfuric acid Sodium carbonate Ammonia Iron(III) phosphate Sodium nitride H2SO4 NaCO3 NH3 FePO4 Na3N
10.
The charges for the most stable monatomic (one atom) ions for the following elements: S, F, Al, N, Sr (in this sequence) are as follows
A. B. C. D. E.
+2 -2 -1 -2 -2
-1 -2 -2 -1 -1
+3 +2 +1 +3 +2
-3 -2 +3 -3 -2
+2 +2 +1 +2 +2
11.
The species
56
Fe3+ contains the following fundamental particles
A. 56 protons, 56 neutrons, 29 electrons B. 26 protons, 30 neutrons, 29 electrons C. 30 protons, 26 neutrons, 29 electrons D. 26 protons, 30 neutrons, 23 electrons E. 30 protons, 26 neutrons, 23 electrons
12.
What is the correct name for HClO2? A. Perchloric acid B. Chloric acid C. Chlorous acid D. Hypochlorous acid E. Hydrochloric acid
Chemistry 101/111
1st Hour Examination
October 12, 2007 5a
13.
What is the mass percent of oxygen in the poisonous gas phosgene (COCl2)? A. 12.1% B. 16.2% C. 24.2% D. 32.4% E. 71.7%
14.
A compound contains 27.72% sulfur and 72.28% bismuth. What is its empirical formula?
A. Bi2S3 B. Bi2S5 C. Bi3S2 D. Bi3S5 E. Bi5S2
15. How many moles of hydrogen atoms are in 1.0 g of glucose ( C6H12O6) ? A. 0.067 B. 0.0056 C. 0.083 D. 0.13 E. 0.013
16.
How many sulfur atoms are present in 25.6 g Al2(S2O3)3 ?
A. x 1.94 10 22 B. 3.88 x 10 22 C. 7.90 x 10 22 D. 2.37 x 10 23 E. 5.74 x 10 23
Chemistry 101/111 17.
1st Hour Examination
October 12, 2007 6a
When the equation for the combustion of pentane (shown below) is balanced (using the lowest possible integers for coefficients), what is the coefficient (X ) for moles of O2 ?
C5H12 (g) + X O2 (g)
A. 5 B. 6 C. 7 D. 8 E. 9
Y CO 2 (g) + Z H2O (g)
18. How many of the following nine compounds are strong electrolytes in aqueous solution? (Assume equal molarity for each solution.) HCl (aq), HF (aq), HNO3 (aq), NaOH (aq), (NH4)3PO4 (aq), NH3 (aq), H3PO4 (aq), CaBr2 (aq), glucose (aq) A. 4 B. 5 C. 6 D. 7 E. 19. 8 The net ionic equation for the neutralization of sulfuric acid with sodium hydroxide is: A. SO4 2- (aq) + 2Na + (aq) Na2SO4 (aq) B. SO4 2- (aq) + 2Na + (aq) Na2SO4 (s) C. H2SO4 (aq) + 2OH - (aq) 2H2O (l) + SO4 2- (aq) D. H+ (aq) + NaOH (aq) H2O (l) + Na + (aq) E. H+ (aq) + OH - (aq) H2O (l) 20. A. B. C. D. E. The oxidation state of oxygen in OF2 is ...? +2 -2 +1 -1 Some other value
Chemistry 101/111 21.
1st Hour Examination 2Fe (s) + 3CO2 (g)
October 12, 2007 7a
In the reaction: Fe2O3 (s) + 3CO (g) A. O in CO2 B. Fe in Fe2O3 C. O in Fe2O3 D. C in CO2
Which element in which species (if any) is being reduced?
E. No species is reduced; this is not an oxidation-reduction reaction 22. Which compound below contains the atom with the highest oxidation number? A. CaSO4 B. Al(NO3)3 C. Mg(NO2)2 D. UF6 E. NH4ClO4 23. How many mL of a 0.25M solution of H2SO4 are required to neutralize 10.0 mL of 1.00M NaOH? A. 10 mL B. 20 mL C. 40 mL D. 60 mL E. 80 mL 24. Pure titanium metal is produced commercially from titanium tetrachloride (TiCl4), which is produced via the reaction:
TiO2 (s) + 2C (s) +2Cl2 (g) TiCl4 (l) + 2CO (g)
How much TiCl4 can be made from 2.0 mol TiO2 (s), 5.0 mol C (s) and 3.0 mol Cl2 (g) A. 1.0 mol B. 1.5 mol C. 2.0 mol D. 2.5 mol E. 5.0 mol
Chemistry 101/111
1st Hour Examination
October 12, 2007 8a
25. 1.00 g of hydrogen chloride gas is dissolved in water and the solution made up to 100.0 mL. What is the molarity of HCl (aq) in solution? A. 0.0100 M B. 0.0274 M C. 0.0548 M D. 0.274 M E. 0.548 M
BONUS QUESTION 26. Three vials of an unknown salt solution are treated with sodium carbonate, sodium hydroxide, and sodium phosphate. Precipitates form in the vials treated with sodium carbonate and sodium phosphate, but no precipitate is formed in the vial treated with sodium hydroxide. Which of the following could be the identity of the salt?
A. ammonium nitrate B. calcium acetate C. potassium bromide D. magnesium chloride E. NONE of the other choices listed could be the salt.
Chemistry 101/111 1
IA
1
1st Hour Examination
October 12, 2007 9a 18
VIIIA
2
PERIODIC TABLE OF THE ELEMENTS
H 2 13
5
14
6
15
VA
7
16
8
17
9
He
10
1.008 IIA 3 4
IIIA IVA
VIA VIIA 4.003
Li
11
Be
12
B
13
C
14
N
15
O
16
F
17
Ne
18
6.941 9.012
10.81 12.01 14.01 16.00 19.00 20.18
Na
19
Mg
20
3
21
4
IVB
22
5
VB
23
6
24
7
25
8
26
9
27
10
28
11
IB
29
12
30
Al
31
Si
32
P
33
S
34
Cl
35
Ar
36
22.99 24.31 IIIB
VIB VIIB
VIIIB
IIB 26.98 28.09 30.97 32.07 35.45 39.95
K
37
Ca
38
Sc
39
Ti
40
V
41
Cr
42
Mn
43
Fe
44
Co
45
Ni
46
Cu
47
Zn
48
Ga
49
Ge
50
As
51
Se
52
Br
53
Kr
54
39.10 40.08
44.96 47.88 50.94 52.00 54.94 55.85 58.93 58.69 63.55 65.39 69.72 72.61 74.92 78.96 79.90 83.80
Rb
55
Sr
56 57
Y
58-
Zr
72
Nb
73
Mo
74
Tc
75
Ru
76
Rh
77
Pd
78
Ag
79
Cd
80
In
81
Sn
82
Sb
83
Te
84
I
85
Xe
86
85.47 87.62
88.91 91.22 92.91 95.94 (98) 101.1 102.9 106.4 107.9 112.4 114.8 118.7 121.8 127.6 126.9 131.3
La + 71 Hf Ta W Re Os Ir Pt Au Hg Tl Pb Bi Po At Rn 132.9 137.3 138.9 * 178.5 180.9 183.9 186.2 190.2 192.2 195.1 197.0 200.6 204.4 207.2 209.0 (209) (210) (222)
90- 104 105 106 107 108 109 110 111 112 Fr Ra Ac + 103 Rf Db Sg Bh Hs Mt Uun Uuu Uub (261) (262) (263) (262) (265) (266) (269) (272) (277) (223) (226) (227) 87 88 89
Cs
Ba
*
58
59
60
61
62
63
64
65
66
67
68
69
70
71
Ce
Pr
Nd Pm Sm
Eu
Gd
Tb
Dy
Ho
Er
Tm
Yb
Lu
140.1 140.9 144.2 (145) 150.4 152.0 157.3 158.9 162.5 164.9 167.3 168.9 173.0 175.0 90 91 92 93 94 95 96 97 98 99 100 101 102 103
Th
Pa
U
Np
Pu
Am Cm Bk
Cf
Es
Fm Md
No
Lr
232.0 231.0 238.0 (237) (244) (243) (247) (247) (251) (252) (257) (258) (259) (262)
Constant Atomic mass unit Avogadro's number Gas constant Faraday constant Planck's constant Boltzmann constant Speed of light Nernst equation term Ion product constant of water
Symbol amu NA R F h k c 2.303 RT/F Kw
Value 1.661 6.022 10
27
Conversion Factors kg 1 inch (in) = 2.54 centimeters (cm) 1 mile (mi) = 1.6093 kilometers (km) 1 angstrom () = 10 meter (m) 1 = 100 picometers (pm) 1 pound (lb) = 0.45359 kilogram (kg) 1 quart (qt) = 0.94633 liter (L) 1 calorie (cal) = 4.184 joules (J) 1 atmosphere = 101.325 kilopascals (atm) (kPa) 1 atmosphere = 760 torr (mmHg) kelvin (K) = C + 273.15
10
1023 mol1
8.314 J/Kmol 0.08206 Latm/Kmol 96485 C/mol 6.626 1.381 2.998 10 10
34
Js J/K
23 8
10 m/s
0.05916 V @ 25 C 1.0 10
14
M @ 25 C
2