1 Chapter 12 Review How many grams of 0oC ice can be converted ...

Chapter 12 Review
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How many grams of 0 o C ice can be converted into 0 o C liquid water by the
addition of 100. kJ of heat energy? (ΔH° fus = 6.02 kJ/mol)
A) 299 g
B) 2.46 g
C) 18.6 g
D) 44.2 g
E) 23.9 g
The vapor pressure of ethanol is 100 mmHg at 34.9 o C. Its molar heat of
vaporization is 39.3 kJ/mol. What is the vapor pressure of ethanol in mmHg at
57.5 o C?
A) 623 mmHg
B) 286 mmHg
C) 173 mmHg
D) 118 mmHg
E) none of the above
Supercooling is
A) the lowering of the boiling point of a liquid by adding a solute.
B) the lowering of the melting point of a liquid by adding a solute.
C) the lowering of the temperature of a liquid by adding a solute.
D) when a substance is in the liquid state despite being below its freezing
point.
E) when a liquid is cooled at an accelerated rate.
Which of the following should have the highest boiling point?
A) CH 4
B) CH 3 OH
C) NH 3
D) CH 3 Br
E) Ne
Which of the following exhibits the most hydrogen bonding?
A) LiH
B) CH 4
C) NH 3
D) H 2 S
E) CH 2 F 2
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Formaldehyde (OCH 2 ) can hydrogen bond with water. What is the maximum
number of hydrogen bonds in which a single formaldehyde molecule can
participate?
A) 2
B) 3
C) 4
D) 5
E) 6
Which of the following carbon compounds has the highest melting point?
A) CF 4
B) CCl 4
C) CBr 4
D) CI 4
E) CH 4
Which of the following liquids would have the highest viscosity at a particular
temperature?
A) CH 2 Br 2
B) C 2 H 5 OH
C) CH 3 Cl
D) HOCH 2 CH 2 OH
E) CH 3 OCH 3
Water has such a high specific heat because
A) it has such a low molecular weight.
B) it is rather dense.
C) the O-H single bond has a high bond energy.
D) it has many relatively strong hydrogen bonds.
E) it dissolves both ionic and covalent compounds.
In a structure with a cubic unit cell, how many unit cells "share" each corner
atom of the cube?
A) 10
B) 8
C) 6
D) 4
E) 2
Calculate the volume effectively occupied by a single CsCl ion pair in the
crystal given that the density of crystalline CsCl is 3.988 g/cm 3 .
A) 0.251 cm 3
B) 7.01 × 10 -23 cm 3
C) 3.93 × 10 -26 cm 3
D) 42.2 cm 3
E) none of the above
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Vanadium crystallizes in a body-centered cubic lattice. What is the number of
nearest neighbors (atoms that make contact) around each atom in this lattice?
A) 2
B) 4
C) 6
D) 8
E) It depends on whether the atom is a corner atom or a central atom.
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In SiO 2
A) the valence band is the same as the conduction band.
B) the two bands are filled with electrons.
C) the valence band and the conduction band are separated by a large
energy gap.
D) the strong Si-O bond prevents the flow of electrons.
E) double bonds between Si and O are responsible for making it a
semiconductor.
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Which of the following has the greatest electrical conductivity?
A) Cu
B) Fe
C) Pure Ge
D) Ge doped with In
E) Al 2 O 3
Acetic acid has a heat of fusion of 10.8 kJ/mol and a heat of vaporization of
24.3 kJ/mol. Estimate the value for the heat of sublimation.
A) 35.1 kJ/mol
B) 13.5 kJ/mol
C) -13.5 kJ/mol
D) -35.1 kJ/mol
E) none of the above
Use the Clausius-Clapeyron equation to estimate the boiling point of water at
24.0 torr pressure.
(ΔH vap = 42.30 kJ/mol)
A) 33.2 °C
B) 110 °C
C) 25 °C
D) 80 °C
E) 52.9 °C
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The triple point is
A) an end to the liquid-gas line in a phase diagram.
B) the relationship between the boiling point, melting point and vapor
pressure of a substance.
C) the point on a phase diagram where solid, liquid, and gas are in
equilibrium.
D) the three pieces of data needed to solve the Clausius-Clapeyron
equation.
E) the (P,V,T) coordinate of a point on a phase diagram.
The main forces responsible for the structure of DNA are
A) ionic bonds and covalent bonds.
B) covalent bonds and ionic bonds.
C) hydrogen bonds and dipole-dipole interactions.
D) covalent bonds and hydrogen bonds.
E) covalent bonds and dipole-dipole interactions.
Which of the following is not likely to exhibit hydrogen bonding?
A) CH 3 CH 2 OH
B) CH 3 NH 2
C) H 2 O
D) NH 2 OH
E) (CH 3 ) 3 N
Methylamine (CH 3 NH 2 ) can hydrogen bond with water. What is the maximum
number of hydrogen bonds in which a single methylamine molecule can
participate?
A) 2
B) 3
C) 4
D) 5
E) 6
In which of the following molecules are dispersion forces likely to be the most
important in determining the melting and boiling points?
A) H 2 S
B) CO
C) HCl
D) ICl
E) Br 2
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Which of the following liquids would have the highest viscosity at a given
temperature?
A) C 2 H 5 OC 2 H 5
B) CH 3 CH 2 Cl
C) CH 3 CH 2 COOH
D) CH 3 COOCH 3
E) C 2 H 5 OH
Place the following in order from the least to most soluble in water:
1. HOCH 2 CH 2 CH 2 OH
2. CH 3 CH 2 CH 2 CH 3
3. HOCH 2 C(OH)HC(OH)HCH 2 OH
A) 1