21) Identify the location of reduction in an electrochemical
cell.
A) the anode
B) the cathode
C) the electrode
D) the salt bridge
E) the socket
Answer:View Answer
44) Calculate the boiling point of a solution of 500.0 g of
ethylene glycol (C2H6O2) dissolved in 500.0 g of water. Kf=
1.86C/m and Kb= 0.512C/m. Use 100C as the boiling point of water.
A) 108C
B) 92C
C) 130C
D) 70C
E) 8.3C
Answer:View Answer
5) Which of the following bond monosaccharide units together into
polysaccharides?
A) hydrogen bonds
B) glycosidic linkages
C) disulfide linkages
D) hydrogen bonds
E) ester linkages
Answer:View Answer
63) The aquation of tris(1,10-phenanthroline)iron(II) in acid
solution takes place according to the equation:
Fe(phen)32++ 3 H3O++ 3 H2O Fe(H2O)62++ 3 phenH+.
If the activation energy, Ea, is 126 kJ/mol and the rate constant
at 30C is 9.8 10-3min-1, what is the rate constant at 35C?
A) 4.4 10-3min-1
B) 2.2 10-2min-1
C) 4.5 101min-1
D) 2.3 102min-1
Answer:View Answer
48) Which of the following is not a standard state?
A) for a liquid, it is 25F
B) for a solid, it is 25C
C) for a solid, it is 1 atm
D) for a solution, it is 1 M
E) for a liquid, it is 1 atm
Answer:View Answer
88) Identify a carboxylic acid.
A) CH3CH2SCH2CH3
B) CH3CH2Br
C) CH3CH2NH2
D) CH3CH2CH2CH3
E) CH3COOH
Answer:View Answer
27) Calcium oxide reacts with water in a combination reaction to
produce calcium hydroxide:
CaO(s) + H2O(l) Ca(OH)2(s)
A 4.50-g sample of CaO is reacted with 4.34 g of H2O. How many
grams of water remain after the reaction is complete?
A) 0.00
B) 0.00892
C) 2.90
D) 1.04
E) 0.161
Answer:View Answer
8) The bond angle in NH3is
A) 107
B) 104.5
C) 120
D) 109.5
E) 95
Answer:View Answer
41) What is the mole fraction of oxygen in a gas mixture that is
37% oxygen and 63% nitrogen by volume?
A) 0.34
B) 0.37
C) 0.25
D) 0.52
Answer:View Answer
86) If a room requires 25.4 square yards of carpeting, what is
the area of the floor in units of ft2?
(3 ft = 1 yd)
A) 76.2 ft2
B) 8.47 ft2
C) 152.4 ft2
D) 229 ft2
E) 64.5 ft2
Answer:View Answer
82) How many grams of water are required to produce 5.50 L of
hydrogen gas at 25.0C and 755 mm Hg pressure according to the
chemical equation shown below?
BaH2(s) + 2 H2O(l) Ba(OH)2(aq) + 2 H2(g)
A) 2.01 g
B) 4.02 g
C) 4.07 g
D) 8.04 g
Answer:View Answer
42) Which of the following is the lowest temperature?
A) 42C
B) 57F
C) 318 K
D) All of these temperatures are all equal.
Answer:View Answer
10) ________ are used to image bones and internal organs.
A) Ultraviolet light
B) Gamma rays
C) Microwaves
D) X-rays
E) Radio waves
Answer:View Answer
13) Which of the following hold two strands of DNA in an a-helix?
A) ester linkages
B) sulfide linkages
C) peptide bonds
D) hydrogen bonds
E) glycosidic linkages
Answer:View Answer
33) Which molecule or compound below contains an ionic bond?
A) CO2
B) C2Br4
C) SiF4
D) OCl2
E) NH4NO3
Answer:View Answer
54) What is the pH of a 0.100 M NH3solution that has Kb= 1.8
10-5? The equation for the dissociation of NH3is
NH3(aq) + H2O(l) NH4+(aq) + OH-(aq).
A) 1.87
B) 2.87
C) 11.13
D) 10.13
Answer:View Answer
57) What is the mass of 3.91 1024molecules of SeO2? The molar
mass of SeO2is 110.96 g/mol.
A) 205 g
B) 294 g
C) 721 g
D) 341 g
E) 685 g
Answer:View Answer
1) Identify the radioactive green light that glows in the dark.
A) phenol red
B) radioactivity
C) phosphorescence
D) desensitivity
E) argon
Answer:View Answer
5) Identify the polar solvent.
A) acetone
B) hexane
C) diethyl ether
D) toluene
E) carbon tetrachloride
Answer:View Answer
27) How much energy is evolved during the formation of 197
g of Fe, according to the reaction below?
Fe2O3(s) + 2 Al(s) Al2O3(s) + 2 Fe(s) Hrxn = -852 kJ
A) 1.52 x 103kJ
B) 3.02 x 103kJ
C) 8.40 x 103kJ
D) 964 kJ
E) 482 kJ
Answer:View Answer
16) Determine the electron geometry (eg) and molecular geometry
(mg) of the underlined atom CH3OCH3.
A) eg=tetrahedral, mg=tetrahedral
B) eg=linear, eg=linear
C) eg=tetrahedral, mg=bent
D) eg=trigonal bipyramidal, mg=tetrahedral
E) eg=octahedral, mg=square planar
Answer:View Answer
3) When filling degenerate orbitals, electrons fill them singly
first, with parallel spins is known as
A) Pauli exclusion principle
B) Hund’s rule
C) Aufbau principle
D) Heisenberg uncertainty principle
Answer:View Answer
58) Give the numbers for mlfor an s orbital.
A) 0
B) -1, 0, 1
C) 0, 1
D) 1
Answer:View Answer
43) Choose the best Lewis structure for XeI2.
A) 
B) 
C) 
D) 
E) 
Answer:View Answer
23) How many of the following elements have 1 unpaired electron
in the ground state?
B Al O F
A) 1
B) 2
C) 3
D) 4
Answer:View Answer
29) Write the balanced chemical equation for the addition of HBr
to CH2=CHCH2CH3.
A) CH2=CHCH2CH3+ HBr CH3BrCH2CH2CH3
B) CH2=CHCH2CH3+ 2 HBr 2 CH2BrCH3
C) CH2=CHCH2CH3+ 2 HBr CH3Br + CH2BrCH2CH3
D) CH2=CHCH2CH3+ 4 HBr 4 CH3Br
E) CH2=CHCH2CH3+ HBr CH3CHBrCH2CH3
Answer:View Answer
35) It is possible to determine the ionization energy for
hydrogen using the Bohr equation. Calculate the ionization energy
for an atom of hydrogen, making the assumption that ionization is
the transition from n = 1 to n = .
A) -2.18 10-18J
B) +2.18 10-18J
C) +4.59 10-18J
D) -4.59 10-18J
E) +4.36 x 10-18J
Answer:View Answer
16) Determine the oxidation state of bromine in BrO.
A) 0
B) +1
C) -3
D) -1
E) +2
Answer:View Answer
22) Which of the following compounds can exhibit fac-mer
isomerism?
A) [Cu(CO)5Cl]+
B) [Co(H2O)3(CO)3]3+
C) [Fe(CO)5NO2]2+
D) [Fe(NH3)2(H2O)4]2+
E) [Cr(H2O)4Br2]+
Answer:View Answer
42) A 100.0 mL sample of 0.10 M Ca(OH)2is titrated with 0.10 M
HBr. Determine the pH of the solution after the addition of 400.0
mL HBr.
A) 1.00
B) 1.40
C) 1.22
D) 1.30
E) 2.11
Answer:View Answer
27) What decimal power does the abbreviation f represent?
A) 1 106
B) 1 103
C) 1 10-1
D) 1 10-15
E) 1 10-12
Answer:View Answer
1) Which of the following statements is TRUE?
A) There is a “heat tax” for every energy transaction.
B) A spontaneous reaction is always a fast reaction.
C) The entropy of a system always decreases for a spontaneous
process.
D) Perpetual motion machines are a possibility in the near
future.
E) None of the above are true.
Answer:View Answer
35) Calculate Srxnfor the following reaction. The S for each
species is shown below the reaction.
4 NH3(g) + 5 O2(g) 4 NO(g) + 6 H2O(g)
S(J/molK) 192.8 205.2 210.8 188.8
A) +287.4 J/K
B) -401.2 J/K
C) +160.0 J/K
D) -336.6 J/K
E) +178.8 J/K
Answer:View Answer
16) What is n for the following equation in relating Kcto Kp?
CH4(g) + H2O(g) CO(g) + 3 H2(g)
A) -3
B) -1
C) -2
D) 2
E) 0
Answer:View Answer
30) Identify the number of bonding pairs and lone pairs of
electrons in water.
A) 1 bonding pair and 1 lone pair
B) 1 bonding pair and 2 lone pairs
C) 2 bonding pairs and 2 lone pairs
D) 2 bonding pairs and 1 lone pair
E) 3 bonding pairs and 2 lone pairs
Answer:View Answer
138) Determine the oxidation state of nitrogen in KNO3.
A) +5
B) +3
C) 0
D) +2
E) +4
Answer:View Answer
15) What pressure will 14.0 g of CO exert in a 3.5 L container at
75C?
A) 4.1 atm
B) 5.0 atm
C) 6.4 atm
D) 1.1 atm
E) 2.3 atm
Answer:View Answer
10) Place the following in order of decreasing molar entropy at
298 K.
HF N2H4 Ar
A) Ar > N2H4 > HF
B) Ar > HF > N2H4
C) N2H4 > Ar > HF
D) N2H4 > HF > Ar
E) HF > N2H4 > Ar
Answer:View Answer
51) What is the reaction at the anode in a breathalyzer?
A) Ethanol is oxidized to acetic acid.
B) Acetic acid is reduced to ethanol.
C) Oxygen is reduced.
D) Hydrogen is oxidized.
E) Ethanol is oxidized to acetaldehyde.
Answer:View Answer
11) Balance the following equation.
_____ C10H12 + _____ O2 _____ H2O + _____ CO2
Answer:View Answer
4) What is the difference between ferromagnetism and
paramagnetism?
Answer:View Answer
6) Define dipole moment.
Answer:View Answer
59) How many grams of NaOH (MW = 40.0) are there in 250.0 mL of a
0.275 M NaOH solution?
Answer:View Answer
3) Explain how the order of a reaction can be determined.
Answer:View Answer
6) Define chain reaction in terms of the fission of uranium
nucleus.
Answer:View Answer
7) Describe the difference between complete ionic and net ionic
equations.
Answer:View Answer
3) What is the autoionization of water?
Answer:View Answer
5) Are anions typically larger or smaller than their
corresponding atom? Why?
Answer:View Answer
2) Why can’t we say that a spontaneous reaction is a fast
reaction?
Answer:View Answer