Chem 1010 - General Chemistry 1 » Summer 2021 » Final Exam
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Question #1
Calculate the atomic mass of element "X", if it has 2 naturally occurring isotopes with the following masses and natural abundances: X-45 - 44.8776 amu - 32.88% X-47 - 46.9443 amu - 67.12%
A.
46.26 amu
B.
45.91 amu
C.
44.99 amu
D.
46.34 amu
E.
46.84 amu
Question #2
Arrange the elements given in order from largest to smallest atomic radii.
A.
Ar>K>Na>Ne>P
B.
Ar>P>Na>Ne>K
C.
K, Ne, Ar, Na, P
D.
K>Ar>P>Na>Ne
E.
Ne>Ar>P>Na>K
F.
K>Na>P>Ar>Ne
Question #3
In the reaction given below, how many grams of C14H9Cl5 will be produced by the reaction of 25.0g of each of the starting materials? C2HOCl3 + 2 C6H5Cl→ C14H9Cl5 + H2O
A.
39.4 g
B.
157 g
C.
121 g
D.
78.7 g
E.
354 g
Question #4
Which of the following is a mathematical representation of Charles' law?
A.
PV = constant
B.
P/T = constant
C.
n x T = constant
D.
V/T = constant
E.
V x T = constant
Question #5
Calculate the pH of 0.051 M solution of sodium acetate (CH3COONa) The Ka lactic acid id 1.4 x 10 - 4
A.
1.29
B.
8.28
C.
12.71
D.
11.43
E.
2.57
Question #6
Which group includes only exothermic processes?
A.
melting, condensation, deposition
B.
melting, evaporation, sublimation
C.
freezing, vaporizartion, deposition
D.
freezing, condensation, deposition
E.
melting, condensation, sublimation
Question #7
You want to prepare 208 grams of 14.8% Cr(NO3)2. How many grams of Chronium (II) Nitrate and how many mL of water is needed. Imagine that density of water is 1 g/ml.
A.
14.8 g Cr(NO3)2 and 85.2 g H2O
B.
14.8 g Cr(NO3)2 and 85.2 g H2O
C.
14.8 g Cr(NO3)2 and 208 g H2O
D.
30.8 g Cr(NO3)2 and 177 g H2O
Question #8
What is the enthalpy change for the combustion of 1.44 g C4H10 in excess oxygen? C4H10 (g) + 13 O2 (g) …..... 8CO2(g) + 10 H2O(g) Ho = -3788 kj
A.
-93.9 kj
B.
-46.9 kj
C.
-22.6 kj
D.
-2.63 x 103 kj
E.
-1.32 x 103 kj
Question #9
Determine the iodine ion concentration (in molarity) in a solution containing 12.6 g Cal2 dissolved in 2750 mL of solution.
A.
0.0312 M
B.
4.58 M
C.
9.16 M
D.
0.0156 M
E.
0.0993 M
Question #10
How many different values of ml are possible in the 5d sublevel?
A.
3
B.
5
C.
2
D.
7
E.
1
Question #11
What answer should be reported, with the correct number of significant figures, for the following calculation? (249.362 + 41) / 63.498
A.
4.573
B.
4.57
C.
4.5277
D.
4.6
E.
4.5728
Question #12
An aqueous solution is 13.0% by mass potassium bromide, KBr, and has a density of 1.10 g/mL. The molality (m) of potassium bromide in the solution is:
A.
1.26 m
B.
2.52 m
C.
.99 m
D.
13.92 m
Question #13
Which molecule is nonpolar?
A.
SF4
B.
SO2
C.
CH2CI2
D.
SO3
E.
H2S
Question #14
What is the conjugate base of H2PO4?
A.
H3PO4
B.
HPO42-
C.
OH
D.
PO43-
E.
H3O+
Question #15
In which of the following sets do all species have the same number of protons?
A.
F-, Ne, Mg2+
B.
K+, Rb+,Cs+
C.
Br, Br-, Br+
D.
Ge, Se2-, Br -
Question #16
Gas is sold for $1.399 per liter in Toronto, Canada. Your car needs 12.00 gallons. How much will your credit be charged in Canadian dollars?
A.
$4.44
B.
$67.15
C.
$16.79
D.
$63.54
Question #17
Inidcate whether each of the following is a physical change (P) or a chemical change (C) : the tendency of copper to turn green when exposed to air
A.
C
B.
P
Question #18
Inidcate whether each of the following is a physical change (P) or a chemical change (C) : the tendency of automobile paint to dull over time
A.
C
B.
P
Question #19
Inidcate whether each of the following is a physical change (P) or a chemical change (C) : the tendency of gasoline to evaporate quickly when spilled
A.
P
B.
C
C.
Question #20
Inidcate whether each of the following is a physical change (P) or a chemical change (C) : the evaporation of fingernail-polish remover (acetone) from the skin
A.
P
B.
C
Question #21
Calculate the hydronium (H3O+) ion concentration an aqueous solution with a pH of 9.85 at 25 C.
A.
8.7 x 10-10 M
B.
6.5 x 10-5 M
C.
1.4 x 10-10 M
D.
7.1 x 10-5 M
E.
4.2 x 10-10 M
Question #22
Which of the following is not a conjugate acid-base pair?
A.
H2SO3 and HSO4 -
B.
HCOOH and HCOO-
C.
CH3COOH and CH3COO-
D.
HPO42- and PO43-
E.
CH3NH3 + and CH3NH2
Question #23
Classify each type of matter as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous: mercury in a thermometer
A.
Mixture
B.
Element
Question #24
Classify each type of matter as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous: exhaled air
A.
Homogeneous mixture
B.
Heterogeneous mixture
Question #25
Classify each type of matter as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous: chicken noodle soup
A.
Heterogeneous mixture
B.
Homogeneous mixture
Question #26
Classify each type of matter as a pure substance or a mixture. If it is a pure substance, classify it as an element or a compound. If it is a mixture, classify it as homogeneous or heterogeneous: sugar
A.
Pure Substance
B.
Compound
Question #27
Which of the following has the largest ionic radius?
A.
Na+
B.
F-
C.
Cl-
D.
P3-
E.
K+
Question #28
Using VSEPR Theory, predict the molecular geometry of XeF4.
A.
triangular bipyramidal
B.
square planar
C.
square pyramidal
D.
see-saw
E.
tetrahedral
Question #29
Which of the following is a mathematical representation of Avogadro's Law
A.
n/V = constant
B.
P/V = constant
C.
n = constant
D.
1/T = constant
E.
V= constant x n
Question #30
Use VSEPR Theory to predict th X-A-X angles for the following compounds CO2, GeF4, BCl3
A.
CO2, GeF4, BCI3
B.
109.5o, 90o, 90o
C.
180o, 109.5o, 120o
D.
109.5o,109.5o,109.5o,
E.
180o, 90o, 120o
Question #31
Classify each substance as an atomic element, molecular element, molecular compound, or ionic compound: chlorine
A.
Molecular element
B.
Atomic element
Question #32
Classify each substance as an atomic element, molecular element, molecular compound, or ionic compound: Au
A.
Atomic element
B.
Ionic compound
Question #33
Classify each substance as an atomic element, molecular element, molecular compound, or ionic compound: CrCl3
A.
Ionic compound
B.
Molecular compound
Question #34
Classify each substance as an atomic element, molecular element, molecular compound, or ionic compound: NO
A.
Molecular element
B.
Molecular compound
Question #35
Classify each substance as an atomic element, molecular element, molecular compound, or ionic compound: Na2O
A.
Molecular compound
B.
Ionic compound
Question #36
If a 2.0-liter sample of gas experiences a decrease in pressure form 1.74 atm to 0.555 atm at 25oC, what is the resulting volume (inL) at 25oC?
A.
0.48 L
B.
20 L
C.
1.9 L
D.
0.64 L
E.
6.3 L
Question #37
Determine the hybridization each of the highlighted (bold) atoms, CO32-, OF2, NO2+
A.
sp2 sp3 sp
B.
sp2 sp3 sp2
C.
sp3 sp3 sp2
D.
sp2 sp2 sp
E.
sp3 sp2 sp2
Question #38
Which molecule is polar?
A.
GeF4
B.
N2
C.
CO2
D.
H2Se
E.
BF3
Question #39
Which one of the following does not have the electron configuration [Ne] 3s23p6?
A.
K+
B.
Ar
C.
Br-
D.
Ca2+
E.
Cl-
Question #40
The carbon-carbon x bond in ethylene, CH2CH2, results from the overlap of which of the following?
A.
sp3 hybrid orbitals
B.
s atomic orbitals
C.
p atomic orbitals
D.
sp hybrid orbitals
E.
sp2 hybrid orbitals
Question #41
Which substance is the reducing agent in this redox equation? HF + Cl2 → F2 + HCl
A.
none of these
B.
Cl2
C.
HF
D.
F
E.
HCl
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