Unlock document.
This document is partially blurred.
Unlock all pages and 1 million more documents.
Get Access
Sodium azide decomposes rapidly to produce nitrogen gas.
2 NaN3(s) 2 Na(s) + 3 N2(g)
What mass of sodium azide will inflate a 60.0 L airbag for a car to a pressure of 1.50
atm at 32 C? (R = 0.08206 Latm/molK)
A.2.40 g
B.67.2 g
C.156 g
D.234 g
E.351 g
For which of the following pure solids is it necessary to break covalent bonds to make a
liquid or gas: C(graphite), CO2(s), C60(s), and C(diamond)?
A.C(graphite) only
B.CO2(s) only
C.CO2(s) and C60(s)
D.C(graphite), C60(s) and C(diamond)
E.C(graphite) and C(diamond)
Which of the following statements is/are CORRECT?
1/ Solubility is defined as the concentration of solute in equilibrium with undissolved
solute in a saturated solution.
2/ If two liquids mix to an appreciable extent to form a solution, they are miscible.
3/ If two liquids mix completely in any proportion to form a solution, the resulting
solution is supersaturated.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.2 and 3
What mass of water is produced by the complete combustion of 2.68 grams of ethanol,
C2H5OH?
A.1.05 g
B.1.17 g
C.3.14 g
D.0.439 g
E.20.6 g
At its boiling point of 58.8 C, 3.66 kJ of heat is required to vaporize 19.5 g of bromine
(Br2). What is the molar enthalpy of vaporization of bromine?
A.0.447 kJ/mol
B.10.0 kJ/mol
C.30.0 kJ/mol
D.44.7 kJ/mol
E.71.4 kJ/mol
If a metal crystallizes in a body-centered cubic lattice, each metal atom has ____
"nearest neighbors."
A.3
B.4
C.6
D.8
E.12
Which of the following formulas is not correct?
A.AlPO4
B.KClO4
C.CaS
D.Na(NO3)2
E.Na2HPO4
The weight percent of concentrated HClO4(aq) is 70.5% and its density is 1.67 g/mL.
What is the molarity of concentrated HClO4?
A.4.20 M
B.7.18 M
C.11.7 M
D.14.2 M
E.39.7 M
Write a balanced net ionic equation for the reaction of calcium sulfide and aqueous
nitric acid.
A.CaS(s) + 2 H+(aq) Ca2+(aq) + S2"(aq) + H2(g)
B.CaS(s) + 2 H+(aq) Ca2+(aq) + H2S(g)
C.CaS(s) + 2 HNO3(aq) Ca(NO3)2(aq) + H2S(g)
D.CaS(s) + 2 HNO3(aq) Ca(NO3)2(s) + H2S(s)
E.S2-(aq) + 2 H+(aq) H2S(g)
What is the H3O+ concentration in 7.1 10"3 M NaOH(aq) at 25 C? (Kw = 1.01 10"14)
A.7.2 10"17 M
B.1.4 10"12 M
C.2.9 10"3 M
D.12 M
E.7.0 1011 M
Which of the following atoms contains the largest number of protons?
A.231Pa
B.238U
C.232Th
D.244Pu
E.244Am
The change in energy for the following reaction is referred to as the ____ for boron.
B(g) + e" B"(g)
A.oxidation number
B.electron affinity
C.electronegativity energy
D.first ionization energy
E.second ionization energy
An amine reacts with a(n) ____ to form an amide.
A.ether
B.alcohol
C.ester
D.aldehyde
E.carboxylic acid
Magnesium sulfide (molar mass 56.37 g/mol) has a face-centered cubic unit cell with
magnesium ions in octahedral holes. The ionic radii of magnesium ions and sulfide ions
are 79 pm and 184 pm, respectively. What is the density of MgS (in g/cm3)?
A.1.29 g/cm3
B.2.57 g/cm3
C.3.64 g/cm3
D.5.15 g/cm3
E.7.28 g/cm3
What is the charge on the copper ion in Cu3P?
A.3"
B.1"
C.0
D.1+
E.3+
What is the highest oxidation state of arsenic?
A."3
B.0
C.+3
D.+5
E.+8
If 5.00 g Br2 and 1.10 g NH3 react according to the equation below, what is the
maximum mass of ammonium bromide produced?
3 Br2( ) + 8 NH3(g) 6 NH4Br(s) + N2(g)
A.3.06 g
B.6.13 g
C.12.9 g
D.4.74 g
E.8.43 g
Which of the following statements concerning the attraction of ions to polar molecules
is/are CORRECT?
1/ The energy of attraction between an ion and a polar molecule is inversely
proportional to the square of the distance between the center of the ion and the
oppositely charged pole of the dipole.
2/ The higher the ion charge, the stronger the attraction between the ion and a polar
molecule.
3/ The greater the magnitude of the dipole, the greater the attraction between the ion
and a polar molecule.
A.1 only
B.2 only
C.3 only
D.2 and 3
E.1, 2, and 3
The SI base unit of length is the ____.
A.Newton
B.liter
C.meter
D.cm3
E.ngstrom
Which of the following properties is associated with the value of the n quantum
number?
A.the number of electrons in an orbital
B.the size of an orbital
C.the orientation in space of an orbital
D.the energy of an orbital
E.the shape of an orbital
Calculate the standard entropy change for the following reaction,
2 SO2(g) + O2(g) 2 SO3(g)
given S[SO2(g)] = 248.2 J/Kmol-rxn, S[O2(g)] = 205.1 J/Kmol-rxn, and S[SO3(g)] =
256.8 J/Kmol-rxn.
A."196.5 J/K
B."94.0 J/K
C."187.9 J/K
D.+187.9 J/K
E.+196.5 J/K
The only acid that decomposes silicon dioxide is ____.
A.CF3CO2H
B.H2SO4
C.HBr
D.HF
E.HClO4
All of the following metals may be found in nature as free elements EXCEPT ____.
A.Ir
B.Au
C.Pt
D.Ti
E.Rh
Identify the element with the ground state electron configuration [Xe]4f145d66s2.
A.Ir
B.Ta
C.Os
D.Ru
E.Au
What role do the cadmium control rods play in a fission reactor?
A.The rods control the rate of fission by absorbing neutrons.
B.The cadmium combines with spent uranium fuel to produce a non-radioactive
product.
C.The rods focus the neutrons toward the center of the reactor.
D.The cadmium acts as a catalyst, enabling fission to occur at lower temperatures.
E.The rods move forward and backward, driving the pistons that turn the turbines.
If 12 ounces of a liquid has a mass of 317 g, what is the density of the liquid in grams
per cubic centimeter? (29.6 cm3 = 1.00 oz.)
A.0.0013 g/cm3
B.0.89 g/cm3
C.1.1 g/cm3
D.0.0013 g/cm3
E.130 g/cm3
Which of the following atoms is diamagnetic in the ground electronic state?
A.Ge
B.S
C.I
D.Mn
E.Sr
Which of the following are standard conditions for an electrochemical cell?
1/ Solutes in aqueous solution has a concentration of 1 M.
2/ Gaseous reactants or products have a pressure of 1 bar.
3/ Solids are present in quantities of 1 mole.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Quartz is the pure crystalline form of
A.silica, SiO2.
B.sodium silicate, NaSiO4.
C.calcium orthosilicate, Ca2SiO4.
D.silicon tetrachloride, SiCl4.
E.silicon carbide, SiC.
Use VSEPR theory to predict the molecular geometry around either carbon atom in
acetylene, C2H2.
A.linear
B.bent
C.trigonal-planar
D.tetrahedral
E.octahedral
Which of the following statements concerning induced dipole/induced dipole forces
is/are CORRECT?
1/ In general, induced dipole/induced dipole interactions decrease as the size of a
molecule increases.
2/ Induced dipole/induced dipole forces are the attractive forces in molecular solids
consisting of nonpolar molecules.
3/ Induced dipole/induced dipole forces exist in both polar and nonpolar molecular
solids.
A.1 only
B.2 only
C.3 only
D.2 and 3
E.1, 2, and 3
What volume is occupied by 35.0 g of C2H2 at 471 mm Hg and 21 C? (R = 0.08206
Latm/molK)
A. 29.0 L
B.52.3 L
C.3.74 L
D.20.1 L
E.0.0689 L
What is the mass of 8.04 10"3 mol O2?
A.2.51 10"4 g
B.5.03 10"4 g
C.0.129 g
D.3.89 g
E.0.257 g
The heat of vaporization of benzene, C6H6, is 30.7 kJ/mol at its boiling point of 80.1 C.
How much energy in the form of heat is required to vaporize 102 g benzene at its
boiling point?
A.0.302 kJ
B.23.6 kJ
C.24.2 kJ
D.40.1 kJ
E.3.14 103 kJ
Which type of experiment demonstrates that light has the properties of a particle?
A.nuclear fission
B.electron diffraction
C.light emission from atomic gases
D.mass spectroscopy
E.photoelectric effect
Molecules with nonsuperimposable mirror images are termed chiral. Pairs of
nonsuperimposable, mirror image molecules are called ________.
The following equation is known as ________ law: .
The standard enthalpy of formation of ammonia is "46.1 kJ/mol.
1/2 N2(g) + 3/2 H2(g) NH3(g)
Commercially, the reaction is carried out at high temperatures. Using your knowledge
of kinetics and equilibrium, explain an advantage and a disadvantage of synthesizing
ammonia at high temperatures.
The element ________ has the following electron configuration: [Rn]5f127s2.
When 1.0 mole of acetic acid is diluted with water to a volume of 1.0 L at 25 C, 0.42%
of the acetic acid ionizes to form acetate ion and hydronium ion.
CH3CO2H(aq) + H2O( ) CH3CO2
"(aq) + H3O+(aq)
What percentage of the acid ionizes when 0.75 mole of acetic acid is diluted with water
to 1.0 L at 25 C?
Which of the following volumes are equivalent to 75 mL?
1. 0.75 cm3
2. 7.5 ´ 10"2
3. 0.0075 L
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
In molecular orbital theory, the bond order is defined as 1/2 (the number of electrons in
________ orbitals minus the number of electrons in antibonding orbitals).
If one of the factors determining the equilibrium of a system is changed, the system
adjusts to counteract that change. This is known as ________ principle.
Give two examples of the allotropes of elemental oxygen.
Write a net ionic equation for the neutralization reaction of hydrochloric acid and
potassium hydroxide. Identify the spectator ion(s).
