Nitric acid decomposes slowly in sunlight with nitrogen dioxide and oxygen as
reduction and oxidation products, respectively. Write a balanced chemical equation for
this reaction.
A.HNO3(aq) NO2(g) + 1/2 O2(g)
B.HNO3(aq) NO2(g) + 1/2 O2(g) + H+(aq)
C.2 HNO3(aq) 2 NO2(g) + O2(g) + H2(g)
D.4 HNO3(aq) 2 NO2(g) + + N2(g) + 3 O2(g) + 2 H2O(g)
E.4 HNO3(aq) 4 NO2(g) + O2(g) + 2 H2O(g)
The pressure of O2 in a 15.0 L flask is 322 mm Hg at 44 C. What mass of O2 is in the
flask? (R = 0.08206 Latm/molK)
A.0.244 g
B.5.80 g
C.7.82 g
D.15.2 g
E.56.3 g
Place the following ions in order from smallest to largest ionic radii: Se2″, Sr2+, Y3+,
and Br“.
A.Se2″ < Sr2+ < Y3+ < Br“
B.Se2″ < Br“ < Sr2+ < Y3+
C.Br“ < Se2″ < Y3+ < Sr2+
D.Y3+ < Sr2+ < Br“ < Se2″
E.Sr2+ < Y3+ < Se2″ < Br“
Write a balanced half-reaction for the reduction of hydrogen peroxide to water in an
acidic solution.
A.2 H2O2( ) 2 H2O( ) + O2(g)
B.2 H2O2( ) + 2e“ 2 H2O( ) + O2(g)
C.H2O2( ) + 2 H+(aq) + 2 e“ 2 H2O( )
D.H2O2( ) + 4 H+(aq) + 2 e“ 2 H2O( ) + H2(g)
E.H2O2( ) + 2 H+(aq) + 4 e“ 2 H2(g) + O2(g)
Write a balanced chemical equation for the reaction of aqueous solutions of ammonium
sulfate and sodium hydroxide.
A.(NH4)2SO4(aq) + 2 NaOH(aq) 2 NH4OH(aq) + SO3(g) + Na2O(aq)
B.(NH3)2SO4(aq) + NaOH(aq) 2 NH3(g) + NaOHSO4(aq)
C.(NH3)2SO4(aq) + 2 NaOH(aq) 2 NH3(g) + Na2SO4(aq) + 2 OH–(aq)
D.(NH4)2SO4(aq) + 2 NaOH(aq) 2 NH4
+(g) + Na2SO4(aq) + 2 OH–(aq)
E.(NH4)2SO4(aq) + 2 NaOH(aq) 2 NH3(g) + 2 H2O( ) + Na2SO4(aq)
Which of the following molecules or ions is amphiprotic in water?
A.NH4
+
B.F“
C.CH3CO2H
D.HC2O4
“
E.CO3
2″
At 298.15 K, all of the following substances have a standard free energy of formation of
zero EXCEPT ____.
A.Br2(g)
B.I2(s)
C.S8(s)
D.Cl2(g)
E.Hg( )
At high temperatures limestone decomposes according to which balanced chemical
equation?
A.Ca(OH)2(s) CaO(s) + H2O(g)
B.2 CaO(s) 2 Ca(s) + O2(g)
C.CaCO3(s) CaO(s) + CO2(g)
D.Ca(OH)2(s) CaH2(s) + O2(g)
E.2 CaCO3(s) 2 Ca(s) + O2(g) + CO2(g)
The DrG for the following reaction is “100.4 kJ.
C2H4(g) + H2(g) C2H6(g)
Given DfG [C2H4(g)] = +68.4 kJ/mol, calculate DfG [C2H6(g)].
A.”168.8 kJ/mol-rxn
B.”32.0 kJ/mol-rxn
C.+1.486 kJ/mol-rxn
D.+32.0 kJ/mol-rxn
E.+168.8 kJ/mol-rxn
Diagram 9-1
The molecular orbital diagram below may be used for the following problem(s). For
oxygen and fluorine, the s2p orbital should be lower in energy than the p2p. However,
the diagram will still yield correct bond order and magnetic behavior for these
molecules.
Energy ________ s*2p
________ ________ p*2p
________ s2p
________ ________ p2p
________ s*2s
________ s2s
________ s*1s
________ s1s
Refer to Diagram 9-1. According to molecular orbital theory, which of the following
species is the most likely to exist (i.e., which will have the greatest bond order)?
A.H2
2+
B.F2
2″
C.N2
2″
D.Be2
E.O2
2+
The standard free energy change for a chemical reaction is +13.3 kJ/mol. What is the
equilibrium constant for the reaction at 125 C? (R = 8.314 J/Kmol)
A.2.8 10“6
B.2.0 10“5
C.4.7 10“3
D.1.8 10“2
E.2.1 102
Express 0.00720 in exponential notation.
A.7.20 103
B.7.2 10“3
C.7.20 10“3
D.7.2 103
E.7.2000 10“3
What is the hybridization of the central atom in a molecule with a square-pyramid
molecular geometry?
A.sp
B.sp2
C.sp3
D.sp3d
E.sp3d2
As pure molecular solids, which of the following exhibit only induced dipole/induced
dipole forces: CO2, CH2Cl2, and SO2?
A.CO2 only
B.CH2Cl2 only
C.SO2 only
D.CO2 and CH2Cl2
E.CO2 and SO2
What nucleus decays by successive b, b, a emissions to produce uranium-236?
A.
B.
C.
D.
E.
Which one of the following functional groups is a base?
A.aldehyde
B.alcohol
C.carboxylic acid
D.ether
E.amine
What is the mass percent of chlorine in magnesium chloride?
A.25.53%
B.37.24%
C.40.67%
D.59.33%
E.74.47%
What is the oxidation number of iodine in potassium iodate, KIO3?
A.”1
B.0
C.+3
D.+5
E.+7
What is the OH“ concentration in 0.48 M CH3CO2
“(aq)? (Kb of CH3CO2
“ = 5.6 10“10)
A.2.7 10“10 M
B.6.2 10“10 M
C.1.1 10“5 M
D.1.6 10“5 M
E.2.4 10“5 M
What is the boiling point of a solution containing 0.852 g naphthalene(C10H8, molar
mass = 128.2 g/mol) dissolved in 14.0 g benzene? The boiling point of pure benzene is
80.10 C and the boiling point elevation constant, Kbp, is 2.53 C/m.
A.78.70 C
B.80.25 C
C.81.30 C
D.82.50 C
E.85.43 C
Nitrosyl bromide decomposes according to the chemical equation below.
2 NOBr(g) 2 NO(g) + Br2(g)
When 0.260 atm of NOBr is sealed in a flask and allowed to reach equilibrium, 22% of
the NOBr decomposes. What is the equilibrium constant, Kp, for the reaction?
A.2.3 10“3
B.4.5 10“3
C.3.5 10“2
D.4.8 10“2
E.8.0 10“2
In general, as temperature increases, the rate of a chemical reaction
A.decreases due to fewer collisions with proper molecular orientation.
B.increases for exothermic reactions, but decreases for endothermic reactions.
C.increases due to a greater number of effective collisions.
D.remains unchanged.
E.decreases due to an increase in the activation energy.
The lattice energy of NaBr is “752 kJ/mol. This energy corresponds to which reaction
below?
A.Na(s) + 1/2 Br2(g) NaBr(s)
B.Na(g) + Br(g) NaBr(s)
C.Na(g) + Br(g) NaBr(s)
D.Na+(g) + Br“(g) NaBr(s)
E.Na+(aq) + Br“(aq) NaBr(s)
What is the product of the addition of HCl to ethylene?
A.chloroethane
B.chloroethylene
C.1,2-dichloroethane
D.1,1-dichloroethane
E.1,1,2,2-tetrachloroethylene
Which of the following statements concerning intermolecular forces is/are CORRECT?
1/ Dipole-dipole attractions occur in all molecules that contain polar bonds, regardless
of whether the molecule has a dipole.
2/ Induced dipole/induced dipole forces exist in all molecular solids.
3/ Hydrogen bonding only occurs in all molecules containing OH bonds.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Which of the following statements is INCORRECT?
A.The solubility of a gas in water decreases with increasing temperature.
B.The solubility of a gas in water is proportional to the partial pressure of the gas above
the water.
C.The dissolution of a gas in water is usually an exothermic process.
D.The relationship between the solubility of a gas and its partial pressure is known as
Henry’s law.
E.The solubility of a gas in water is inversely proportional to the molar mass of the gas.
Which of the following molecules or ions will have a Lewis structure most like that of
phosphorus trichloride, PCl3?
A.ClO3
“
B.SO3
C.CO3
2″
D.BF3
E.Cl2CO
Which of the following chemical equations refers to the second ionization of Al?
A.Al(s) + 2e“ Al2″(s)
B.Al+(g) Al2+(g) + e“
C.Al(g) Al2+(g) + 2e“
D.Al(s) Al+(s) + e“
E.Al2+(g) + e“ Al+(g)
What is the half-life of a first-order reaction if it takes 4.4 10“2 seconds for the
concentration to decrease from 0.50 M to 0.20 M?
A.2.5 10“2 s
B.3.3 10“2 s
C.1.6 s
D.21 s
E.27 s
At 25 C, 0.138 mg AgBr dissolves in 10.0 L of water. What is the equilibrium constant
for the reaction below?
AgBr(s) Ag+(aq) + Br“(aq)
A.5.40 10“13
B.5.40 10“11
C.1.90 10“8
D.7.35 10“7
E.1.90 10“6
Which of the following is a correct Lewis structure for sulfur dioxide, SO2?
A.
B.
C.
D.
E.
The formula of acetic acid, CH3CO2H, is an example of a(n)
A.condensed formula.
B.empirical formula.
C.structural formula.
D.ionic compound formula.
E.mass spectrum.
Which of the following statements is/are CORRECT?
1/ A paramagnetic substance is attracted to a magnetic field.
2/ An atom with no unpaired electrons is ferromagnetic.
3/ Atoms with one or more unpaired electrons are paramagnetic.
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
What is the formula for dicyanobis(ethylenediamine)zirconium(IV) nitrate?
A.Zr[(CN)2(NO3)2(en)2]
B.[Zr(CN)2(NO3)2(en)2]
C.(NO3)2[Zr(CN)2(en)2]
D.[Zr(CN)2(en)2](NO3)2
E.[Zr(NO3)2(en)2](CN)2
A nail is coated with a 0.053 cm thick layer of zinc. The surface area of the nail is 8.59
cm2. The density of zinc is 7.13 g/cm3. How many zinc atoms are used in the coating?
A.5.9 x 1020 atoms
B.3.0 x 1022 atoms
C.3.8 x 1022 atoms
D.2.0 x 1024 atoms
E.1.3 x 1026 atoms
A surfactant used for cleaning is called a(n) ________.
Given the initial rate data for the reaction A + B C, determine the rate expression for the
reaction.
[A], M [B], M D[C]/Dt (initial) M/s
0418 0.488 2.73 10“4
A.
B.
C.
D.
E.
Two electronic balances are tested using a standard weight. The true mass of the
standard is 5.0000 g. The results of 5 individual measurements on each balance are
recorded below.
Balance A
Balance B
5.2895 g 5.0001
g
5.1077 g 4.9998
g
4.6407 g 4.9999
g
4.8947 g 5.0002
g
5.0672 g 4.9999
g
average mass = 5.0000 g 5.0000
g
Which statement best describes the results?
A. A: poor precision, good accuracy. B: good precision, good accuracy.
B. A: good precision, good accuracy. B: poor precision, good accuracy.
C. A: good precision, good accuracy. B: good precision, poor accuracy.
D. A: poor precision, good accuracy. B: good precision, poor accuracy.
E. A: good precision, poor accuracy. B: poor precision, good accuracy.
If a stress is applied to an equilibrium system, the system will respond in such a way as
to relieve that stress. This is a statement of ________ principle.
One method of recovering metals from their ores involves aqueous solutions; a second
method involves heat. The method involving heat is called ________.
Why do salts containing basic anions have a greater solubility in water than predicted
from calculations using Ksp values?
If an aqueous sodium hydroxide solution is left in contact with air, the concentration of
hydroxide ion gradually decreases. The process can be hastened if a person exhales over
a sodium hydroxide solution. Write a balanced chemical equation that describes the
process by which the hydroxide ion concentration decreases.
OH“(aq) + CO2(aq) HCO3
“(aq)
A solution in which there is more dissolved solute than in a saturated solution is known
as a(n) ________ solution.
A ________, designated by the Greek symbol y, describes the wave behavior of an
electron in an atom.
One might expect PCl3 to have a trigonal planar molecular geometry since its central
atom is surrounded by three outer atoms. However, PCl3 has a trigonal pyramidal
geometry. Explain.
________ changes only occur in the direction that leads toward chemical equilibrium.
For any process, the change in entropy of the universe equals the sum of the entropy
changes for the system and for the ________.
________ acid is produced in a larger quantity than any other chemical in the United
States. This chemical is used in the production of fertilizers, pigments, alcohol, paper
and detergents.
The net ionic equation for the reaction of barium chloride and sodium sulfate is shown
below.
Ba2+(aq) + SO4
2″(aq) BaSO4(s)
Chloride and sodium ions are referred to as ________ ions because they are not
involved in the reaction.
Above its critical temperature and pressure, a substance becomes a(n) ________ fluid.
In PCl5, the Cl-P-Cl bond angle between an axial and an equatorial chlorine atom is
________ degrees.