Which of the following types of radiation will pass through a piece of paper, but will be
stopped by 0.5 cm of lead?
A.a
B.b
C.
D.g
E.All of the above will pass through 0.5 cm of lead.
What volume of oxygen will react with 21 mL of ethanol, assuming the gases are
present at the same temperature and pressure?
2 CH3CH2OH(g) + 6 O2(g) 4 CO2(g) + 6 H2O(g)
A.7.0 mL
B.14 mL
C.21 mL
D.42 mL
E.63 mL
Which of the following statements is/are CORRECT?
1/ Water soluble ionic compounds, such as NaCl, are strong electrolytes.
2/ Some molecular compounds, such as HCl, are strong electrolytes.
3/ Some molecular compounds, such as acetic acid, are weak electrolytes.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Which of the following statements concerning molecular orbital (MO) bond theory
is/are CORRECT?
1/ MO theory can describe molecular bonding in excited states.
2/ MO theory accurately describes bonding in O2 and NO, VB theory does not.
3/ MO theory predicts that electrons are localized between pairs of atoms.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Which of the following statements is/are CORRECT?
1/ The most stable allotrope of sulfur is orthorhombic sulfur, which consists of
8-member rings of sulfur atoms.
2/ Diatomic sulfur, S2, is the most common allotrope of sulfur. Typical air samples
contain between 0.5 and 2.0% S2(g).
3/ Plastic sulfur is an allotrope of the element that consists of long chains of sulfur
atoms.
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
What concentration of silver nitrate (in ppm) is present in 7.1 10“7 M AgNO3(aq)? For
very dilute aqueous solutions, you can assume the solution’s density is 1.0 g/mL. The
molar mass of AgNO3 is 169.9 g/mol.
A.0.0071 ppm
B.0.12 ppm
C.0.71 ppm
D.1.7 ppm
E.8.3 ppm
What is the mass of 0.71 mol Na?
A.1.2 10“24 g
B.12 g
C.16 g
D.0.031 g
E.32 g
What is the molar mass of a nonpolar molecular compound if 3.37 grams dissolved in
45.3 grams benzene begins to freeze at “0.04 C? The freezing point of pure benzene is
5.50 C and the freezing point depression constant, Kfp, is “5.12 C/m.
A.35.1 g/mol
B.68.8 g/mol
C.80.5 g/mol
D.116 g/mol
E.359 g/mol
For a proton (mass = 1.673 10“27 kg) moving with a velocity of 2.83 104 m/s, what is
the de Broglie wavelength (in pm)?
A.0.356 pm
B.3.56 pm
C.14.0 pm
D.7.15 pm
E.28.5 pm
What is the correct Lewis structure for SF4?
A.
B.
C.
D.
E.
Ores are often found mixed with impurities such as sand and clay. In metallurgy, these
impurities are called ____.
A.gangue
B.alloys
C.slags
D.roasts
E.precipitates
How many electrons can be described by the following quantum numbers: n = 2, = 1,
= “1, ms = “1/2?
A.0
B.1
C.2
D.3
E.4
Which action(s) will decrease the equilibrium concentration of an inert gas (such as N2)
in water?
1/ decreasing the temperature of the water
2/ increasing the volume of water
3/ decreasing the pressure of the gas above the liquid
A.1 only
B.2 only
C.3 only
D.1 and 3
E.1, 2, and 3
What volume of O2, measured at 225 C and 0.970 atm, will be produced by the
decomposition of 3.16 g KClO3? (R = 0.08206 Latm/molK)
2 KClO3(s) 2 KCl(s) + 3 O2(g)
A.1.09 L
B.1.24 L
C.1.63 L
D.3.26 L
E.52.1 L
A volume of 25.0 mL of 0.100 M C6H5CO2H(aq) is titrated with 0.100 M NaOH(aq).
What is the pH after the addition of 12.5 mL of NaOH? (Ka of benzoic acid = 6.3 10“5)
A.2.60
B.4.20
C.5.40
D.7.00
E.8.60
What is the pH of the buffer that results when 32 g sodium acetate (NaCH3CO2) is
mixed with 500.0 mL of 1.0 M acetic acid (CH3CO2H) and diluted with water to 1.0 L?
(Ka of CH3CO2H = 1.8 10“5)
A.2.52
B.4.23
C.4.44
D.4.64
E.4.74
A 3p orbital has ?
A.0 planar nodes and 1 spherical node.
B.1 planar node and 0 spherical nodes.
C.1 planar node and 1 spherical node.
D.1 planar node and 2 spherical nodes.
E.2 planar nodes and 1 spherical node.
Aluminum reacts with hydrochloric acid to produce aluminum chloride and hydrogen
gas.
2 Al(s) + 6 HCl(aq) 2 AlCl3(aq) + 3 H2(g)
What mass of H2(g) is produced from the reaction of 0.75 g Al(s) with excess
hydrochloric acid?
A.0.056 g
B.0.084 g
C.0.17 g
D.1.1 g
E.2.3 g
Two nonpolar solvents, such as hexane and carbon tetrachloride, may be miscible even
though the enthalpy of mixing of these liquids might be small. A reason that mixing
occurs is that mixtures have greater disorder than pure solvents. The tendency toward
disorder is a thermodynamic function called ____.
A.entropy
B.enthalpy
C.saturation
D.adhesion
E.cohesion
The atomic number of fluorine is ____.
A.7A
B.9
C.10
D.19
E.0
Iron oxide reacts with aluminum in an exothermic reaction.
Fe2O3(s) + 2 Al(s) 2 Fe(s) + Al2O3(s)
The reaction of 5.00 g Fe2O3 with excess Al(s) evolves 26.6 kJ of energy in the form of
heat. Calculate the enthalpy change per mole of Fe2O3 reacted.
A.”5.32 kJ/mol
B.”1.33 102 kJ/mol
C.”2.12 104 kJ/mol
D.”2.12 102 kJ/mol
E.”8.50 102 kJ/mol
Ideally, colligative properties depend only on the
A.relative numbers of solute and solvent particles in a solution.
B.molar masses of the solute particles in a solution.
C.density of a solution.
D.hydrated radii of the molecules or ions dissolved in a solution.
E.partial pressure of the gases above the surface of a solution.
Which of the following compounds might be used to reduce a carboxylic acid to an
aldehyde?
A.H+
B.Cl2
C.K2Cr2O7
D.KMnO4
E.NaBH4
Given the following acid dissociation constants,
Ka (H3PO4) = 7.5 10“3
Ka (NH4
+) = 5.6 10“10
determine the equilibrium constant for the reaction below at 25 C.
H3PO4(aq) + NH3(aq) NH4
+(aq) + H2PO4
–(aq)
A.4.2 10“12
B.7.5 10“8
C.4.2 102
D.1.3 107
E.2.4 1011
The rate constant for the decay of copper-62 is 9.8 minutes-1. What is the half-life of
this isotope?
A.0.071 m.
B.1.6 m.
C.14 m.
D.0.10 m.
E.9.8 m.
What 2+ ion has the following ground state electron configuration?
A.Cd2+
B.Sr2+
C.Zn2+
D.Sn2+
E.None
What mass of Na2SO4 must be dissolved in 100.0 grams of water to lower the freezing
point by 2.50 C? The freezing point depression constant, Kfp, of water is “1.86 C/m.
Assume the van’t Hoff factor for Na2SO4 is 2.85.
A.3.77 g
B.6.36 g
C.6.70 g
D.11.3 g
E.19.1 g
The thermochemical equation for the combustion of methanol is shown below.
CH3OH( ) + 3/2 O2(g) CO2(g) + 2 H2O(g) DrH = “638.7 kJ/mol-rxn
What is the enthalpy change for the combustion of 8.59 g CH3OH?
A.”171 kJ
B.”19.9 kJ
C.”2.38 103 kJ
D.”5.49 103 kJ
E.”1.76 106 kJ
The freezing point depression constant for water is “1.86 C/m. At what temperature will
a solution containing 7.75 g KCl and 45.0 g H2O begin to freeze? Assume that no
ion-pairing occurs between K+ and Cl“.
A.”8.59 C
B.”4.30 C
C.”2.15 C
D.”1.59 C
E.”0.51 C
How many protons, neutrons, and electrons are in a nitrogen-15 atom?
A.15 protons, 15 neutrons, 15 electrons
B.15 protons, 7 neutrons, 15 electrons
C.8 protons, 7 neutrons, 7 electrons
D.7 protons, 8 neutrons, 7 electrons
E.8 protons, 7 neutrons, 8 electrons
The following processes occur spontaneously at 25 C. Which of these processes is/are
endothermic?
1/ NH4NO3 dissolving in water (which is accompanied by a cooling of the water).
2/ the expansion of a real gas into a vacuum (which is accompanied by a cooling of the
gas).
3/ liquid water in an ice cube tray freezing into ice after being placed in a freezer.
A.1 only
B.2 only
C.3 only
D.1 and 2
E.1, 2, and 3
Iron(II) sulfide has a primitive cubic unit cell with sulfide ions at the lattice points. The
ionic radii of iron(II) ions and sulfide ions are 88 pm and 184 pm, respectively. What is
the density of FeS (in g/cm3)?
A.2.56 g/cm3
B.4.71 g/cm3
C.5.25 g/cm3
D.6.66 g/cm3
E.8.97 g/cm3
A mixture of ethanol and benzoic acid is heated in the presence of acid. What is the
primary product of the reaction?
A.
B.
C.
D.
E.
At 25 C, what is the osmotic pressure of a homogeneous solution consisting of 21.0 g
urea (CON2H4) diluted with water to 2.50 L? (R = 0.08206 Latm/molK)
A.0.205 atm
B.3.42 atm
C.8.55 atm
D.12.3 atm
E.147 atm
Calculate the equilibrium constant for the following reaction at 25 C,
2 IO3
“(aq) + 5 Hg( ) + 12 H+(aq) I2(s) + 5 Hg2+(aq) + 6 H2O( )
given the following thermodynamic information.
IO3
“(aq) + 6 H+(aq) + 5 e“ I2(s) + 3 H2O( ) E = +1.20 V
Hg2+(aq) + 2 e“ Hg( ) E = +0.86 V
A.3 10“58
B.6 105
C.3 1011
D.6 1028
E.3 1057