1) Which of the following liquids will have the lowest 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)
2) At 333 K, which of the pairs of gases below would have the most nearly identical
rates of effusion?
A) N2O and NO2
B) CO and N2
C) N2 and O2
D) CO and CO2
E) NO2 and N2O4
3) What is the wavelength of light (nm) that has a frequency 4.62 X 1014 s-1?
A) 932 nm
B) 649 nm
C) 1.39 X 1023 nm
D) 1.54 X 10-3 nm
E) 1.07 X 106 nm
4) The ground-state electron configuration of ________ is [Ar]4s13d5.
A) V
B) Mn
C) Fe
D) Cr
E) K
5) The nuclear disintegration series of ________ is the source of radon-222 in soil.
A) 235U
B) 238U
C) 236Pb
D) 235Th
E) 14C
6) With thermodynamics, one cannot determine ________.
A) the speed of a reaction
B) the direction of a spontaneous reaction
C) the extent of a reaction
D) the value of the equilibrium constant
E) the temperature at which a reaction will be spontaneous
7) Which of the subshells below do not exist due to the constraints upon the angular
momentum quantum number?
A) 4f
B) 4d
C) 4p
D) 4s
E) none of the above
8) The molarity (M) of an aqueous solution containing 22.5 g of glucose (C6H12O6) in
35.5 mL of solution is ________.
A) 3.52
B) 0.634
C) 0.197
D) 0.125
E) 1.85
9) The acid-dissociation constants of phosphoric acid (H3PO4) are Ka1 = 7.5 x 10-3, Ka2
= 6.2 x 10-8, and Ka3 = 4.2 x 10-13 at 25.0 oC. What is the pH of a 2.5 M aqueous
solution of phosphoric acid?
A) 1.82
B) 0.40
C) 2.51
D) 0.86
E) 0.13
10) The mechanism for formation of the product X is:
A + B –> C + D (slow)
B + D –> X (fast)
The intermediate reactant in the reaction is ________.
A) A
B) B
C) C
D) D
E) X
11) Of the noble gases, ________ is present in highest concentration in dry air at sea
level.
A) Ne
B) He
C) Xe
D) Kr
E) Ar
12) There are ________ σ bonds and ________ π bonds in
.
A) 14, 2
B) 10, 3
C) 12, 2
D) 13, 2
E) 16, 3
13) The molecular weight of a gas that has a density of 6.70 g/L at STP is ________
g/mol.
A) 4.96 x 102
B) 1.50 x 102
C) 7.30 x 101
D) 3.35
E) 2.98 x 10-1
14) This element reacts with hydrogen to produce a gas with the formula HX. When
dissolved in water, HX forms an acidic solution. X is ________.
A) chlorine
B) calcium
C) oxygen
D) germanium
E) arsenic
15) The conjugate base of HSO4
– is ________.
A) OH–
B) H2SO4
C) SO4
2-
D) HSO4
+
E) H3SO4
+
16) Which of the following equations correctly represents the combustion of hydrazine?
A) N2H4 (l) + O2 (g) –> NH3 (g) + HNO2 (g)
B) N2H4 (l) + 2O2 (g) –> 2NO2 (g) + 2H2 (g)
C) N2H4 (l) + O2 (g) –> 2H2NO (g)
D) N2H4 (l) + O2 (g) –> N2 (g) + 2 H2O (g)
E) N2H4 (l) + O2 (g) –> N2 (g) + 2H2 (g) + O2 (g)
17) What is the physical state in which matter has no specific shape but does have a
specific volume?
A) gas
B) solid
C) liquid
D) salts
E) ice
18) A mixture of two gases was allowed to effuse from a container. One of the gases
escaped from the container 1.43 times as fast as the other one. The two gases could
have been ________.
A) CO and SF6
B) O2 and Cl2
C) CO and CO2
D) Cl2 and SF6
E) O2 and SF6
19) The half-life of carbon-11 is 20.3 minutes. How much of a 100.0 mg sample
remains after 1.6 hours?
A) 3.77 mg
B) 0.0377 mg
C) 94.7 mg
D) 1.75 x 10-89
mg
E) 99.9 mg