1) Alkali metals tend to be more reactive than alkaline earth metals because ________.
A) alkali metals have lower densities
B) alkali metals have lower melting points
C) alkali metals have greater electron affinities
D) alkali metals have lower ionization energies
E) Alkali metals are not more reactive than alkaline earth metals.
2) Which one of the following molecular formulas is also an empirical formula?
A) C6H6O2
B) C2H6SO
C) H2O2
D) H2P4O6
E) C6H6
3) Which of the following is insoluble in water at 25 °C?
A) Mg3(PO4)2
B) Na2S
C) (NH4)2CO3
D) Ca(OH)2
E) Ba(C2H3O2)2
4) A sample of gas (24.2 g) initially at 4.00 atm was compressed from 8.00 L to 2.00 L
at constant temperature. After the compression, the gas pressure was ________ atm.
A) 4.00
B) 2.00
C) 1.00
D) 8.00
E) 16.0
5) The standard Gibbs free energy of formation of ________ is zero.
(a) H2O (l)
(b) Fe (s)
(c) I2 (s)
A) (a) only
B) (b) only
C) (c) only
D) (b) and (c)
E) (a), (b), and (c)
6) If the rate law for the reaction
2A + 3B –> products
is first order in A and second order in B, then the rate law is rate = ________.
A) k[A][B]
B) k[A]2[B]3
C) k[A][B]2
D) k[A]2[B]
E) k[A]2[B]2
7) All of the halogens ________.
A) exist under ambient conditions as diatomic gases
B) tend to form positive ions of several different charges
C) tend to form negative ions of several different charges
D) exhibit metallic character
E) form salts with alkali metals with the formula MX
8) How many significant figures should be retained in the result of the following
calculation?
12.00000 X 0.9893 + 13.00335 X 0.0107
A) 2
B) 3
C) 4
D) 5
E) 6
9) The energy released by combustion of 1 g of a substance is called the ________ of
the substance.
A) specific heat
B) fuel value
C) nutritional calorie content
D) heat capacity
E) enthalpy
10) The freezing point of ethanol (C2H5OH) is -114.6 oC. The molal freezing point
depression constant for ethanol is 2.00 oC/m. What is the freezing point (oC) of a
solution prepared by dissolving 50.0 g of glycerin (C3H8O3, a nonelectrolyte) in 200.0
g of ethanol?
A) -115.0
B) -5.43
C) -132.3
D) -120.0
E) -114.6
11) A 22.5-g sample of ammonium carbonate contains ________ mol of ammonium
ions.
A) 0.467
B) 0.288
C) 0.234
D) 2.14
E) 3.47
12) Which one of the following is a weak acid?
A) HNO3
B) HCl
C) HI
D) HF
E) HClO4
13) Calculate the percentage by mass of oxygen in Pb(NO3)2.
A) 9.7
B) 14.5
C) 19.3
D) 29.0
E) 33.4
14) An ion has 26 protons, 29 neutrons, and 23 electrons. The symbol for the ion is
________.
A) 55Fe3+
B) 55Fe3-
C) 52Cu3+
D) 52Cu3-
E) 55V3-
15) Which one of the following is used as a radiotracer to study blood?
A) iron-59
B) technetium-99
C) sodium-23
D) iodine-131
E) phosphorus-32
16) When the following equation is balanced, the coefficient of C3H8O3 is ________.
C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g)
A) 1
B) 2
C) 3
D) 7
E) 5