1) The molecular weight is always a whole-number multiple of the empirical formula
weight.
2) The DNA double helix is held together by hydrogen bonds and London dispersion
forces.
3) In the reaction
BF3 + F––> BF4
–
BF3 acts as a Brnsted-Lowry acid.
4) The solubility of a slightly soluble salt is decreased by the presence of a second
solute that provides a common ion to the system.
5) All oxides are ionic compounds.
6) Units of the rate constant of a reaction are independent of the overall reaction order.
7) The boiling points of normal hydrocarbons are higher than those of branched
hydrocarbons of similar molecular weight because the London-dispersion forces
between normal hydrocarbons are greater than those between branched hydrocarbons.
8) Molecules containing only single bonds do not exhibit liquid-crystal behavior
because free rotation can occur around single bonds making these molecules flexible.
9) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC)
The value of H o for the decomposition of calcium chloride into its constituent
elements,
CaCl2 (s) –> Ca (s) + Cl2 (g)
is ________ kJ/mol.
A) 0.00
B) -397.9
C) +397.9
D) -795.8
E) +795.8
10) The reaction below is first order in [H2O2]:
2H2O2 (l) –> 2H2O (l) + O2 (g)
A solution originally at 0.600 M H2O2 is found to be 0.075 M after 54 min. The
half-life for this reaction is ________ min.
A) 6.8
B) 18
C) 14
D) 28
E) 54
11) Which of the following liquids will have the highest freezing point?
A) pure H2O
B) aqueous glucose (0.60 m)
C) aqueous sucrose (0.60 m)
D) aqueous FeI3 (0.24 m)
E) aqueous KF (0.50 m)
12) How many milliliters of 0.120 M NaOH are required to titrate 50.0 mL of 0.0998 M
hypochlorous acid to the equivalence point? The Ka of hypochlorous acid is 3.0 x 10-8.
A) 7.60
B) 50.0
C) 41.6
D) 60.1
E) 7.35
13) The average rate of disappearance of A between 20 s and 40 s is ________ mol/s.
A) 8.5 x 10-4
B) 1.7 x 10-3
C) 590
D) 7.1 x 10-3
E) 1.4 x 10-3
14) The most abundant fossil fuel is ________.
A) natural gas
B) petroleum
C) coal
D) uranium
E) hydrogen
15) SO2 (5.00 g) and CO2 (5.00 g) are placed in a 750.0 mL container at 50.0 °C. The
partial pressure of SO2 in the container was ________ atm.
A) 2.76
B) 4.02
C) 6.78
D) 0.192
E) 1.60
16) The following reaction would produce a(n) ________.
A) aldehyde
B) carboxylic acid
C) ester
D) ether
E) amide
17) The unit of force in the English measurement system is . The SI unit of force
is the Newton, which is ________ in base SI units.
A)
B)
C)
D)
E)
18) Which electron configuration represents a violation of the Pauli exclusion
principle?
A)
B)
C)
D)
E)
19) The pressure exerted by a column of liquid is equal to the product of the height of
the column times the gravitational constant times the density of the liquid, P = ghd.
How high a column of water (d = 1.0 g/mL) would be supported by a pressure that
supports a 713 mm column of mercury (d = 13.6 g/mL)?
A) 14 mm
B) 52 mm
C) 713 mm
D) 1.2 x 104 mm
E) 9.7 x 103 mm
20) A temperature of 290. K is the same as ________ °F.
A) 63
B) 81
C) 260
D) 711
E) 351
21) What is the mass number of a neutron?
A) 2
B) 1
C) 3
D) 4
E) 0
22) Which atom has the largest number of neutrons?
A) phosphorus-30
B) chlorine-37
C) potassium-39
D) argon-40
E) calcium-40
23) A triatomic molecule cannot be linear if the hybridization of the central atoms is
________.
A) sp
B) sp2
C) sp3
D) sp2 or sp3
E) sp2d or sp3d2
24) The isomerization of methylisonitrile to acetonitrile
CH3NC (g) –> CH3CN (g)
is first order in CH3NC. The half-life of the reaction is 2.70 x 104 s at 463 K. The rate
constant when the initial [CH3NC] is 0.030 M is ________ s-1.
A) 3.90 x 104
B) 1.23 x 10-3
C) 2.57 x 10-5
D) 8.10 x 102
E) 1.25 x 107
25) A sample of CH4O with a mass of 32.0 g contains ________ molecules of CH4O.
A) 5.32 x 10-23
B) 1.00
C) 1.88 x 1022
D) 6.02 x 1023
E) 32.0
26) The three radioactive series that occur in nature end with what element?
A) Bi
B) U
C) Po
D) Pb
E) Hg
27) The enthalpy change for converting 10.0 g of ice at -50.0 oC to water at 50.0 oC is
________ kJ. The specific heats of ice, water, and steam are 2.09 J/g-K, 4.18 J/g-K, and
1.84 J/g-K, respectively. For H2O, ΔHfus = 6.01 kJ/mol, and ΔHvap = 40.67 kJ/mol.
A) 12.28
B) 4.38
C) 3138
D) 6.47
E) 9.15
28) The correct name for CaH2 is ________.
A) hydrocalcium
B) calcium dihydride
C) calcium hydroxide
D) calcium dihydroxide
E) calcium hydride
29) Given the equation:
C2H6 (g) + O2 (g) → CO2 (g) + H2O (g) (not balanced)
Determine the number of liters of O2 consumed at STP when 60.0 grams of C2H6 is
burned.
30) Briefly explain why carbon and silicon can form oxides with such different physical
properties, gaseous CO2and solid SiO2.
31) The correct answer (reported to the proper number of significant figures) to the
following is ________.
(1501-1496) X (9.18 X 3.68) = ________
32) Calculate G o(in kJ/mol) for the following reaction at 1 atm and 25 oC:
C2H6 (g) + O2 (g) –> CO2 (g) + H2O (l) (unbalanced)
Gf
o C2H6 (g) = -32.89 kJ/mol; Gf
oCO2 (g) = -394.4 kJ/mol; Gf
o H2O (l) = -237.13
kJ/mol
33) The sensation of vision results from a nerve impulse that is triggered by the
separation of retinal from ________.