R = 8.314×10-3 kJ/mol·K         R = 0.08206 L·atm/mol·K
ΔHsoln= -ΔHlattice + ΔHhydr      q = mcΔT         Sgas = kH×Pgas
ΔTb = ikb m      ΔTf = ikf m      Π = iMRT         ΔP = iXsoluteP°solv
Psolv = XsolvP°solv            Psolute = XsoluteP°solute   Ptot = Psolv + Psolute



1.
The boiling point of a liquid depends on
A.
the external pressure
B.
the external temperature
C.
the amount of the liquid
D.
its heat capacity
E.
the value of the gas constant, R


2.
The boiling point of the molecular compound A is 56.6°C. How much energy is needed to heat 16.4 g of A from 20.1°C to 97.7°C?
Specific heat capacity of A(l)
3.69 J/(g⋅K)
Specific heat capacity of A(g)
2.06 J/(g⋅K)
Heat of vaporization of A
36.6 kJ/mol
Molar mass of A
30.7 g/mol
 
A.
26.4 kJ
B.
21.9 kJ
C.
23.1 kJ
D.
18.7 kJ
E.
31.4 kJ


3.
A compound has vapor pressure of 48.0 torr at 47.7°C and 449.0 torr at 122.0°C. Calculate its heat of vaporization.
A.
33.5 kJ/mol
B.
29.3 kJ/mol
C.
25.9 kJ/mol
D.
31.7 kJ/mol
E.
22.4 kJ/mol


4.
Examine the following phase diagram and identify the phase change occurring as one goes from point E to point F.
A.
melting caused by decreasing the pressure
B.
vaporization caused by decreasing the pressure
C.
condensation caused by decreasing the pressure
D.
sublimation caused by decreasing the pressure
E.
deposition caused by decreasing the pressure


5.
Which of the following substances will have hydrogen bonds between the molecules?
A.
HCl
B.
(CH3)2O
C.
CH3CH2F
D.
CH3SH
E.
CH3NH2


6.
Which of the following should have the highest boiling point?
A.
CH3I
B.
CH3Br
C.
CH3Cl
D.
CH3F
E.
CH3CH3


7.
The resistance of liquids to flow is called
A.
surface tension.
B.
viscosity.
C.
capillary action.
D.
cohesion.
E.
specific elasticity.


8.
A metal with a body-centered lattice will have ________________ atom(s) per unit cell.
A.
4
B.
9
C.
2
D.
8
E.
1


9.
What is the coordination number for a metal that crystalizes in the simple cubic lattice?
A.
2
B.
4
C.
8
D.
6
E.
12


10.
The electrical conductivity of metal conductors
A.
increases with increasing temperature
B.
is relatively small
C.
is very small to non-existent
D.
is independent of temperature
E.
decreases with increasing temperature


11.
Which of the following pairs of ions is arranged so that the ion with the smaller (i.e. less negative) heat of hydration is listed first?
A.
Sr2+, Ca2+
B.
Al3+, Mg2+
C.
Ca2+, K+
D.
S2–, Se2–
E.
None of the above pairs are arranged in this way.


12.
The Henry's Law constant for carbon monoxide in water at 25°C is 9.71×10-4 mol/L·atm. How many moles of CO will dissolve in 1.00 L of water at this temperature if the partial pressure of CO is 246.3 torr?
A.
0.00300 mol
B.
0.000315 mol
C.
0.239 mol
D.
0.000395 mol
E.
0.000266 mol


13.
Which of the following statements is correct?
A.
The molarity of a supersaturated solution is lower than the molar solubility of the solute.
B.
Only solids can have saturated solutions.
C.
Unsaturated solutions can dissolve more solute.
D.
All of these statements are correct.
E.
None of these statements are correct.


14.
What is the molality of a solution prepared by dissolving 15.3 g of hexane, C6H14, in 74.6 g of benzene, C6H6?
A.
2.24 m
B.
2.85 m
C.
1.85 m
D.
2.38 m
E.
3.25 m


15.
Procaine hydrochloride (M = 272.8 g/mol) is used as a local anesthetic. Calculate the molarity of a 2.66 m solution of procaine hydrochloride in water which has a density of 1.061 g/mL.
A.
1.73 M
B.
1.93 M
C.
2.13 M
D.
1.20 M
E.
1.64 M


16.
Which of the following statements is correct?
A.
Raoult's Law relates the vapor pressure of the solvent above the solution to its mole fraction in the solution.
B.
Raoult's Law relates the vapor pressure of the solvent above the solution to the molarity of the solution.
C.
Raoult's Law applies exactly to all solutions.
D.
Raoult's Law applies only to non-ideal solutions.
E.
Raoult's Law relates the vapor pressure of the solute above the solution to the degree of its dissociation in the solution.


17.
From the following list of aqueous solutions and water, select the one with the highest boiling point. (Note: Use the ideal values of the van't Hoff factor.)
A.
0.87 M NaCl
B.
0.46 M Na2SO4
C.
0.78 M CaBr2
D.
0.31 M AlBr3
E.
pure water


18.
Which of the following statements is correct with regard to the following two solutions? (Note: Use the ideal values of the van't Hoff factor.)
      (I) 0.67 m RbBr              and          (II) 0.41 m BaBr2
A.
The two solutions have the same vapor pressure
B.
Solution (I) has lower vapor pressure.
C.
Solution (I) has higher vapor pressure
D.
Solution (I) has lower vapor pressure and lower osmotic pressure
E.
Solution (II) has higher osmotic pressure


19.
Determine the boiling point of a solution which contains 0.32 mol of glucose in 85 g of water. (For water Kf = 1.86°C/m and Kb = 0.512°C/m)
A.
98.1°C
B.
107.0°C
C.
93.0°C
D.
101.9°C
E.
100.0°C


20.
An aqueous solution contains 3.32 g of the unknown compound X. The volume of the solution is 774.0 mL and its osmotic pressure is 3.13 atm at 25.0°C. Assuming that X is a nonvolatile nonelectrolyte, what is the molar mass of this compound?
A.
31.8 g/mol
B.
45.3 g/mol
C.
29.0 g/mol
D.
25.8 g/mol
E.
33.5 g/mol


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