1) The correct name for SO is ________.
A) sulfur oxide
B) sulfur monoxide
C) sulfoxide
D) sulfate
E) sulfite
2) Which isotope has 45 neutrons?
A) Kr
B) Br
C) Se
D) Cl
E) Rh
3) Which equation correctly represents what happens when N dissolves in water?
A) NO2 (g) + H2O (l) –> 2H+ (aq) + NO3
– (aq)
B) 3NO2 (g) + H2O (l) –> 2H+ (aq) + 2NO3
– (aq) + NO (g)
C) NO2 (g) + H2O (l) –> H2O2 (aq) + NO (g)
D) 2NO2 (g) + H2O (l) –> 2H+ (aq) + NO4
2- (aq) + NO (g)
E) 2NO2 (g) + 2H2O (l) –> 2HNO2 (aq) + O2 (g) + H2 (g)
4) The volume of fluorine gas required to react with 2.67 g of calcium bromide to form
calcium fluoride and bromine at 41.0 °C and 4.31 atm is ________ mL.
A) 10.4
B) 210
C) 420
D) 79.9
E) 104
5) The internal energy of a system ________.
A) is the sum of the kinetic energy of all of its components
B) is the sum of the rotational, vibrational, and translational energies of all of its
components
C) refers only to the energies of the nuclei of the atoms of the component molecules
D) is the sum of the potential and kinetic energies of the components
E) none of the above
6) Using the VSEPR model, the molecular geometry of the central atom in SO3 is
________.
A) linear
B) trigonal planar
C) tetrahedral
D) bent
E) trigonal pyramidal
7) The H for the solution process when solid sodium hydroxide dissolves in water is
44.4 kJ/mol. When a 12.6-g sample of NaOH dissolves in 250.0 g of water in a
coffee-cup calorimeter, the temperature increases from 23.0 °C to ________°C. Assume
that the solution has the same specific heat as liquid water, i.e., 4.18 J/g-K.
A) 35.2
B) 24.0
C) 36.4
D) 35.7
E) 40.2
8) Pressure has an appreciable effect on the solubility of ________ in liquids.
A) gases
B) solids
C) liquids
D) salts
E) solids and liquids
9) Which statement is true about liquids but not true about solids?
A) They flow and are highly ordered.
B) They are highly ordered and not compressible.
C) They flow and are compressible.
D) They assume both the volume and the shape of their containers.
E) They flow and are not compressible.
10) The mass % of C in methane (CH4) is ________.
A) 25.13
B) 133.6
C) 74.87
D) 92.26
E) 7.743
11) The volume of a sample of gas (2.49 g) was 752 mL at 1.98 atm and 62 °C. The gas
is ________.
A) SO2
B) SO3
C) NH3
D) NO2
E) Ne
12) The hybridizations of nitrogen in NF3 and NH3 are ________ and ________,
respectively.
A) sp2, sp2
B) sp, sp3
C) sp3, sp
D) sp3, sp3
E) sp2, sp3
13) In the nitrite ion (NO2
–), ________.
A) both bonds are single bonds
B) both bonds are double bonds
C) one bond is a double bond and the other is a single bond
D) both bonds are the same
E) there are 20 valence electrons
14) The acid-dissociation constants of sulfurous acid (H2SO3) are Ka1 = 1.7 x 10-2 and
Ka2 = 6.4 x 10-8 at 25.0 oC. Calculate the pH of a 0.163 M aqueous solution of
sulfurous acid.
A) 4.53
B) 1.28
C) 1.86
D) 6.21
E) 1.93