1) The principal component of smog is sulfur dioxide.
2) The concentration of reactants or products at any time during the reaction can be
calculated from the integrated rate law.
3) Emulsifying agents typically have a hydrophobic end and a hydrophilic end.
4) The quantity of energy gained by a system equals the quantity of energy gained by its
surroundings.
5) The correct name for Na3N is sodium azide.
6) Municipal water treatment consists of five steps ending with chlorination.
7) The heme unit of myoglobin is bound to the protein via a nitrogen-containing ligand.
8) One joule equals 1 kg-m2/s2.
9) When dealing with gases, the volume fraction and the mole fraction are the same.
10) The quantitative amount of charge separation in a diatomic molecule contributes to
the dipole moment of that molecule.
11) After swimming in the ocean for several hours, swimmers noticed that their fingers
appeared to be very wrinkled. This is an indication that seawater is supertonic relative
to the fluid in cells.
12) XeF4 is a polar molecule.
13) The reduction of metal oxides uses carbon monoxide.
14) Green and orange are complementary colors.
15) Automobile air bags use the decomposition of sodium azide as their source of gas
for rapid inflation:
2NaN3 (s) → 2Na (s) + 3N2 (g).
What mass (g) of NaN3 is required to provide 40.0 L of N2 at 25.0 °C and 763 torr?
A) 1.64
B) 1.09
C) 160
D) 71.1
E) 107
16) Combustion of a 0.9827-g sample of a compound containing only carbon,
hydrogen, and oxygen produced 1.900 g of CO2 and 1.070 g of H2O. What is the
empirical formula of the compound?
A) C2H5O
B) C4H10O2
C) C4H11O2
D) C4H10O
E) C2H5O2
17) The ionization energy of NO is 890 kJ/mol:
NO + hv –> NO+ + e–
The maximum wavelength of light capable of causing the ionization of NO is ________
nm.
A) 2967
B) 1.35 10-4
C) 1.35 10-7
D) 134.5
E) 1.35 105
18) A reversible process is one that ________.
A) can be reversed with no net change in either system or surroundings
B) happens spontaneously
C) is spontaneous in both directions
D) must be carried out at low temperature
E) must be carried out at high temperature
19) Consider the following reaction:
3A –> 2B
The average rate of appearance of B is given by [B]/t. Comparing the rate of
appearance of B and the rate of disappearance of A, we get [B]/t = ________ x (-[A]/t).
A) -2/3
B) +2/3
C) -3/2
D) +1
E) +3/2
20) Which one of the following should have the lowest boiling point?
A) CH4
B) PCl3
C) C2H5COOH
D) LiCl
E) Cl2S
21) The oxidation number of iron in Fe2O3 is ________.
A) -2
B) +1
C) +3
D) +2
E) -3
22) Horizontal rows of the periodic table are known as ________.
A) periods
B) groups
C) metalloids
D) metals
E) nonmetals
23) The bond angles marked a, b, and c in the molecule below are about ________,
________, and ________, respectively.
A) 90°, 90°, 90°
B) 120°, 120°, 90°
C) 120°, 120°, 109.5°
D) 109.5°, 120°, 109.5°
E) 109.5°, 90°, 120°
24) Formulas that show how atoms are attached in a molecule are called ________.
A) molecular formulas
B) ionic formulas
C) empirical formulas
D) diatomic formulas
E) structural formulas
25) In ionic bond formation, the lattice energy of ions ________ as the magnitude of the
ion charges _______ and the radii ________.
A) increases, decrease, increase
B) increases, increase, increase
C) decreases, increase, increase
D) increases, increase, decrease
E) increases, decrease, decrease
26) The Haber process is used to make ________ from ________.
A) HNO3, N2
B) O2, KClO3
C) NH3, N2
D) NO2, O2
E) NO, N2
27) The number 1.00430 has ________ significant figures.
A) 2
B) 3
C) 5
D) 6
E) 4
28) What is the concentration (in M) of hydro xide ions in a solution at 25.0 oC with pH
= 4.282?
A) 4.28
B) 9.72
C) 1.92 x 10-10
D) 5.22 x 10-5
E) none of the above
29) In the nuclear transmutation represented by O(p, ) N, the emitted particle is
________.
A) a beta particle.
B) an alpha particle.
C) a proton.
D) a positron.
E) a neutron.
30) Cesium-131 has a half-life of 9.7 days. What percent of a cesium-131 sample
remains after 60 days?
A) 100
B) 0
C) 1.4
D) 98.6
E) more information is needed to solve the problem
31) All of the orbitals in a given subshell have the same value as the ________ quantum
number.
A) principal
B) angular momentum
C) magnetic
D) A and B
E) B and C
32) In what two ways can an object appear blue?
33) The formation of aspirin by reacting salicylic acid with acetic acid is a(n) ________
reaction.
34) An added electron to the element bromine goes into which orbital?
35) How many grams of H3PO4 are in 415 mL of a 4.00 M solution of H3PO4?
36) The van der Waals equation corrects the ideal gas law for the finite volume and
________ of gas molecules.
37) What is the name of the compound below?
38) Calculate the concentration (M) of arsenic acid (H3AsO4) in a solution if 25.00 mL
of that solution required 35.21 mL of 0.1894 M KOH for neutralization.
39) What is the oxidation number of the central metal in [Mo(H2O)5NO3]Cl2
40) In a reaction, if the bonds in the reactants are stronger than the bonds in the product,
the reaction is ________.