1) Kp = 0.0198 at 721 K for the reaction
2HI (g) H2 (g) + I2 (g)
In a particular experiment, the partial pressures of H2 and I2 at equilibrium are 0.678
and 0.788 atm, respectively. The partial pressure of HI is ________ atm.
A) 7.87
B) 27.0
C) 5.19
D) 0.103
E) 0.0106
2) The kinetic energy of a 26.9-g object moving at a speed of 81.9 m/s is ________ J.
A) 145
B) 0.950
C) 90.2
D) 90200
E) 1450
3) Carbon-11 decays by positron emission:
C –> B + e
The decay occurs with a release of 2.87 x 1011 J per mole of carbon-11. When 5.00 g of
carbon-11 undergoes this radioactive decay, ________ g of mass is converted to energy.
A) 1.45 x 10-3
B) 4.35 x 105
C) 1.45 x 10-6
D) 6.90 x 102
E) 1.59 x 10-2
4) When calcium reacts with sulfur the compound formed is ________.
A) Ca2S2
B) Ca3S2
C) CaS
D) CaS2
E) Ca2S3
5) In which of the following aqueous solutions would you expect AgBr to have the
lowest solubility?
A) 0.040 M SrBr2
B) pure water
C) 0.040 M NaBr
D) 0.040 M KBr
E) 0.010 M AgNO3
6) S is positive for the reaction ________.
A) CaO (s) + CO2 (g) –> CaCO3 (s)
B) N2 (g) + 3H2 (g) –> 2NH3 (g)
C) 2SO3 (g) –> 2SO2 (g) + O2 (g)
D) Ag+ (aq) + Cl– (aq) –> AgCl (s)
E) H2O (l) –> H2O (s)
7) What is the missing product from this reaction?
Ca –> Sc + ____
A) e
B) ³
C) e
D) He
E) Ca
8) The value of Keq for the equilibrium
H2 (g) + I2 (g) 2HI (g)
is 794 at 25 oC. What is the value of Keq for the equilibrium below?
H2 (g) + I2 (g) HI (g)
A) 397
B) 0.035
C) 28
D) 1588
E) 0.0013
9) A sample of oxygen gas was found to effuse at a rate equal to two times that of an
unknown gas. The molecular weight of the unknown gas is ________ g/mol.
A) 64
B) 128
C) 8
D) 16
E) 8.0
10) The hybrid orbitals used for bonding by Xe in the unstable XeF2 molecule are
________ orbitals.
A) sp2
B) sp3
C) sp3d
D) sp3d2
E) sp
11) The equilibrium constant for the gas phase reaction
2NH3 (g) N2 (g) + 3H2 (g)
is Keq = 230 at 300 oC. At equilibrium, ________.
A) products predominate
B) reactants predominate
C) roughly equal amounts of products and reactants are present
D) only products are present
E) only reactants are present
12) The number with the most significant zeros is ________.
A) 0.00002510
B) 0.02500001
C) 250000001
D) 2.501 X 10-7
E) 2.5100000
13) In what type of radioactive decay does the atomic number of the product decrease
by one?
A) positron emission
B) corrosion
C) alpha
D) beta
E) gamma
14) At elevated temperatures, methylisonitrile (CH3NC) isomerizes to acetonitrile
(CH3CN):
CH3NC (g) –> CH3CN (g)
The dependence of the rate constant on temperature is studied and the graph below is
prepared from the results.
The energy of activation of this reaction is ________ kJ/mol.
A) 160
B) 1.6 x 105
C) 4.4 x 10-7
D) 4.4 x 10-4
E) 1.9 x 104
15) Which of the following would have to lose three electrons in order to achieve a
noble gas electron configuration?
A) Si, P
B) Al
C) P
D) Cl
E) Mg, Al, P
16) Which of the following is an illustration of the law of constant composition?
A) Water boils at 100 °C at 1 atm pressure.
B) Water is 11% hydrogen and 89% oxygen by mass.
C) Water can be separated into other substances by a chemical process.
D) Water and salt have different boiling points.
E) Water is a compound.
17) The order of the reaction in A is ________.
A) 1
B) 2
C) 3
D) 4
E) 0
18) Name the compound, [Os(en)3]2 [NiCl2Br2]3.
19) What is meant by the prefix tetrakis-, and when is it used?
20) The salinity, density, and temperature of seawater varies with ________.
21) Lactose is a disaccharide of glucose and ________.
22) Show how a molecule of C2F2Cl2 can destroy two molecules of ozone, O3.
23) Hydrogenation of an alkene requires high temperatures and a catalyst such as
nickel. Why is this?
24) Water (H2O) and the alcohol methanol (CH3OH) are infinitely soluble in each other.
The primary intermolecular force responsible for this is ________.
25) What is the concentration (M) of CH3OH in a solution prepared by dissolving 10.2
g of CH3OH in sufficient water to give exactly 230 mL of solution?
26) What are the three steps in the Ostwald process of nitric acid synthesis?