1) Which of the following is soluble in water at 25 °C?
A) AgNO3
B) Hg2Cl2
C) PbCl2
D) Ag2S
E) AgCl
2) The value of ΔH° for the reaction below is +128.1 kJ:
CH3OH (l) → CO (g) + 2H2 (g)
How many kJ of heat are consumed when 15.5 g of CH3OH (l) decomposes as shown
in the equation?
A) 0.48 kJ
B) 62.0 kJ
C) 1.3 x 102 kJ
D) 32 kJ
E) 8.3 kJ
3) A sample of H2 gas (12.28 g) occupies 100.0 L at 400.0 K and 2.00 atm. A sample
weighing 9.49 g occupies ________ L at 353 K and 2.00 atm.
A) 109
B) 68.2
C) 54.7
D) 147
E) 77.3
4) A second-order reaction has a half-life of 18 s when the initial concentration of
reactant is 0.71 M. The rate constant for this reaction is ________ M-1s-1.
A) 7.8 x 10-2
B) 3.8 x 10-2
C) 2.0 x 10-2
D) 1.3
E) 18
5) Which of the following liquids has the greatest density?
A) 13 cm3 with a mass of 23 g
B) 3.5 cm3 with a mass of 10 g
C) 0.022 cm3 with a mass of 0.10 g
D) 54 cm3 with a mass of 45 g
E) 210 cm3 with a mass of 12 g
6) The Ksp for Zn(OH)2 is 5.0 x 10-17. Determine the molar solubility of Zn(OH)2 in a
buffer solution with a pH of 11.5.
A) 5.0 x 106
B) 1.2 x 10-12
C) 1.6 x 10-14
D) 5.0 x 10-12
E) 5.0 x 10-17
7) The solubility of nitrogen gas at 25 oC and 1 atm is 6.8 x 10-4 mol/L. If the partial
pressure of nitrogen gas in air is 0.76 atm, what is the concentration (molarity) of
dissolved nitrogen?
A) 6.8 x 10-4 M
B) 5.2 x 10-4 M
C) 4.9 x 10-4 M
D) 3.8 x 10-4 M
E) 1.1 x 10-5 M
8) A Brnsted-Lowry acid is defined as a substance that ________.
A) increases Ka when placed in H2O
B) decreases [H+] when placed in H2O
C) increases [OH–] when placed in H2O
D) acts as a proton acceptor
E) acts as a proton donor
9) The molecular geometry of the right-most carbon in the molecule below is
________.
A) trigonal planar
B) trigonal bipyramidal
C) tetrahedral
D) octahedral
E) T-shaped
10) For the species in the reaction below, ΔH°f is zero for ________.
2Co (s) + H2 (g) + 8PF3 (g) → 2HCo(PF3)4 (l)
A) Co (s)
B) H2 (g)
C) PF3 (g)
D) HCo(PF3)4 (l)
E) both Co(s) and H2 (g)
11) The Kp for the reaction below is 1.49 x 108 at 100.0 oC:
CO (g) + Cl2 (g) COCl2 (g)
In an equilibrium mixture of the three gases, PCO = PCl2 = 1.00 x 10-4 atm. The partial
pressure of the product, phosgene (COCl2), is ________ atm.
A) 1.49
B) 1.49 x 1016
C) 6.71 x 10-17
D) 1.49 x 104
E) 1.49 x 1012
12) Z– is a weak base. An aqueous solution of NaZ is prepared by dissolving 0.350 mol
of NaZ in sufficient water to yield 1.0 L of solution. The pH of the solution was 8.93 at
25.0 oC. The Kb of Z– is ________.
A) 1.2 x 10-5
B) 6.9 x 10-9
C) 2.1 x 10-10
D) 9.9 x 10-2
E) 2.8 x 10-12
13) When the following equation is balanced, the coefficients are ________.
Al(NO3)3 + Na2S → Al2S3 + NaNO3
A) 2, 3, 1, 6
B) 2, 1, 3, 2
C) 1, 1, 1, 1
D) 4, 6, 3, 2
E) 2, 3, 2, 3
14) Thermodynamic Quantities for Selected Substances at 298.15 K (25 oC)
The value of H o for the decomposition of gaseous sulfur trioxide to its component
elements,
2SO3 (g) –> 2S (s, rhombic) + 3O2 (g)
is ________ kJ/mol.
A) +790.4
B) -790.4
C) +395.2
D) -395.2
E) +105.1
15) Consider the following electron configurations to answer the questions that follow:
(i)1s2 2s2 2p6 3s1
(ii)1s2 2s2 2p6 3s2
(iii)1s2 2s2 2p6 3s2 3p1
(iv)1s2 2s2 2p6 3s2 3p4
(v)1s2 2s2 2p6 3s2 3p5
The electron configuration of the atom with the most negative electron affinity is
________.
A) (i)
B) (ii)
C) (iii)
D) (iv)
E) (v)
16) Exactly 3.5 moles if N2O4 is placed in an empty 2.0-L container and allowed to
reach equilibrium described by the equation
N2O4 (g) 2NO2 (g)
If at equilibrium the N2O4 is 25% dissociated, what is the value of the equilibrium
constant for the reaction?
17) The primary chemical pollutants that create acid rain are ________ dioxide and
________ oxides.
18) Describe the process of reverse osmosis that is used to desalinate seawater.
19) Metal oxides and hydroxides that are relatively insoluble in neutral water, but are
soluble in both strongly acidic and strongly basic solutions are said to be ________.
20) When an isotope undergoes electron capture, what happens to the captured
electron?
21) What is the concentration (M) of sodium ions in 4.57 L of a 2.98 M Na3PO4
solution?
22) Write the correctly balanced equation for the reaction between elemental fluorine
and sodium iodide.