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1) The entropy of the universe is ________.
A) constant
B) continually decreasing
C) continually increasing
D) zero
E) the same as the energy, E
2) The energy of a photon of light is ________ proportional to its frequency and
________ proportional to its wavelength.
A) directly, directly
B) inversely, inversely
C) inversely, directly
D) directly, inversely
E) indirectly, not
3) The following reaction is second order in [A] and the rate constant is 0.025 M-1s-1:
A --> B
The concentration of A was 0.65 M at 33 s. The initial concentration of A was ________
M.
A) 2.4
B) 0.27
C) 0.24
D) 1.4
E) 1.2 x 10-2
4) A 0.100 m solution of which one of the following solutes will have the highest vapor
pressure?
A) KClO4
B) Ca(ClO4)2
C) Al(ClO4)3
D) sucrose
E) NaCl
5) The number with the most significant zeros is ________.
A) 0.08
B) 0.00090
C) 90.300
D) 0.008001
E) 591
6) Which of the following is (are) the lowest temperature?
A) The freezing point of water
B) 5 °C
C) 30 °F
D) 280 K
E) A and D
7) Using the table of average bond energies below, the H for the reaction is ________
kJ.
A) +160
B) -160
C) -217
D) -63
E) +63
8) Of the choices below, which would be the best for the lining of a tank intended for
use in storage of hydrochloric acid?
A) copper
B) zinc
C) nickel
D) iron
E) tin
9) The total number of π bonds in the molecule is ________.
A) 3
B) 4
C) 6
D) 9
E) 12
10) An electron domain consists of ________.
a) a nonbonding pair of electrons
b) a single bond
c) a multiple bond
A) a only
B) b only
C) c only
D) a, b, and c
E) b and c
11) Which of the following molecules or ions will exhibit delocalized bonding?
A) NH4
+ and N3
-
B) NO2
- only
C) NO2
-, NH4
+, and N3
-
D) N3
- only
E) NO2
- and N3
-
12) The average rate of disappearance of I- between 400.0 s and 800.0 s is ________
M/s.
A) 2.8 x 10-5
B) 1.4 x 10-5
C) 5.8 x 10-5
D) 3.6 x 104
E) 2.6 x 10-4
13) Consider the following species when answering the following questions:
(i) PCl3(ii) CCl4(iii) TeCl4(iv) XeF4(v) SF6
Which of the molecules has a see-saw shape?
A) (i)
B) (ii)
C) (iii)
D) (iv)
E) (v)
14) A single individual typically uses the greatest quantity of water for ________.
A) flushing toilets
B) cooking
C) cleaning (bathing, laundering, and house cleaning)
D) watering lawns
E) drinking water
15) Which of the following expressions is the correct equilibrium-constant expression
for the reaction below?
2SO2 (g) + O2 (g) 2SO3 (g)
A) [SO3] / [SO2][O2]
B) [SO2] / [SO3]
C) [SO3]2 / [SO2]2[O2]
D) [SO3]2 / [SO2]2[O2]2
E) [SO3] / [SO2][O2]2
16) The density of ammonia gas in a 4.32 L container at 837 torr and 45.0 °C is
________ g/L.
A) 3.86
B) 0.719
C) 0.432
D) 0.194
E) 4.22 x 10-2
17) If the value for the equilibrium constant is much greater than 1, then the equilibrium
mixture contains mostly ________.
18) How can the presence of biodegradable waste in a lake result in the death of fish in
the lake?
19) What is the predominant isotope of uranium?
20) Large protein molecules that act as catalysts are called ________.
21) A compound was found to contain 90.6% lead (Pb) and 9.4% oxygen. The empirical
formula for this compound is ________.
22) What are the elements called that are located between the metals and nonmetals?
23) The use of radioisotopes in tracing metabolism is possible because ________.
24) Calculate the pH of a buffer solution that contains 0.820 grams of sodium acetate
and 0.010 moles of acetic acid in 100 ml of water. The Ka of acetic acid is 1.77 x 10-5.
25) Using the noble gas shorthand notation, write the electron configuration for Fe3+.
26) List seven nonmetals that exist as diatomic molecules in their elemental forms.
