CHEM 13 EXAMS
1990 - 2002
PRACTICE BOOKLET
THE QUESTIONS CONTAINED IN THIS FILE ARE TAKEN FROM PAST
EXAM BOOKLETS. QUESTIONS DELETED FROM THE EXAMS HAVE
BEEN OMITED FROM THIS FILE AND IN SOME CASES THE
QUESTIONS HAVE BEEN EDITED FROM THERE ORIGINAL FORMAT
Answer grids are found at the end of this booklet
Last Revised by D. Lougheed 7/3/00
1990
1.
2.
3.
A temperature of 1000 K is the same as
(a) 1273 °C
(b) 1000 °C (c) 727 °C
(d) 538 °C
How many protons are there in one atom of sodium?
(a) 11
(b) 12
(c) 16
(d) 23
(e) 273 °C
(e) 34
23
One valence electron is removed from an atom of 10 Ne. The resulting ion has
(a) 9 protons, 14 neutrons and 9 electrons
(b) 10 protons, 13 neutrons and 9 electrons
(c) 9 protons, 14 neutrons and 10 electrons
(d) 10 protons, 13 neutrons and 11 electrons
(e) 11 protons, 12 neutrons and 11 electrons
4.
The chemical properties of element number 20 will most closily resemble those of element number
(a) 12
(b) 17
(c) 19
(d) 21
(e) 28
5.
What charge does the ion [SiO4]n have?
(a) n = +4
(b) n = +2
(c) n = 0
(d) n = -2
(e) n = -4
6.
Select the correct electrolyte description for each of the following solutions in water.
1 Methanol solution
X Weak electrolyte
2 Potassium bromide solution
Y Nonelectrolyte
3 Ammonium hydroxide solution Z Strong electrolyte
(a) 1X, 2Y, 3Z (b) 1X, 2Z, 3Y(c) 1Y, 2X, 3Z
(d) 1Y, 2Z, 3X(e) 1Z, 2X, 3Y
7.
What volume of 1.00 mol/L aqueous NaOH solution will neutralize 100 mL of 1.00 mol/L aqueous
H2SO4 solution?
(a) 50.0 mL
(b) 100 mL (c) 150 mL
(d) 200 mL (e) 400 mL
8.
Titanium (IV) sulfate has the formula
(a) TiSO4
(b) Ti4SO4
(c) Ti(SO4)2
9.
(d) Ti(SO4)4
(e) Ti2SO4
The number of atoms of phosphorus in one mole of Ca3(PO4)2 is
(a) 3.0 x 1023 (b) 6.0 x 1023
(c) 12 x 1023
(d) 18 x 1023
(e) 36 x 1023
10. The solubility of sodium chloride in water at 25°C is 36.6 g in 100 mL of solution. How many
grams of sodium ion will be found in one litre of solution?
(a) 10.0 g
(b) 23.0 g
(c) 144 g
(d) 230 g
(e) 366 g
11. The shape of the NH3 molecule is
(a) a perfect tetrahedron
(b) a planar triangle
(d) a perfect square
(e) a triangular pyramid
Last Revised by D. Lougheed 7/3/00
(c) a bent line
12. What volume of water must be added to 800 L of 0.130 mol/L solution to dilute it to 0.100 mol/L?
(a) 1840 L
(b) 1040 L
(c) 560 L
(d) 240 L
(e) 24 L
16
13. If the scale of relative atomic masses were changed to the basis 8 O = 100, what would be the
relative molecular mass of CO2? (Actual scale, C, 12; O, 16)
(a) 350
(b) 275
(c) 250
(d) 244
(e) 44
14. If the mass of the neutron were half of its actual mass, and that of the electron were twice its actual
32
mass, then the mass of one atom of 16 S would be, approximately
(a) unchanged (b) increased by 25% (c) decreased by 25% (d) doubled (e) halved
15. The radius of a proton 1.4 x 10-15 m, and the mass of the proton is 1.7 x 10-24 g. What is the
density of the proton?
(a) 1.2 x 10-12 kg/m3
(b) 3 x 10-13 kg·m3
(c) 8 x 10-13 kg/m3
(d) 1.0 x 10+14 kg/m3
(e) 1.5 x 10+17 kg/m3
16. A container holds one mole of gaseous helium at a known temperature and pressure. A second,
identical container holds gaseous neon at three times the pressure and twice the temperature (K).
Approximately how many moles of neon are in the second container?
(a) 0.67 mol
(b) 1.0 mol
(c) 1.5 mol
(d) 2.0 mol
(e) 6.0 mol
17. If G.N. Lewis's rules about electron-dot structures are observed, what is the formal number of pairs
of unshared valence electrons in the NO2+ ion?
(a) eight
(b) four
(c) two
(d) one
(e) zero
18. The salt CuSO4 · 5H2O is slowly heated until only pure CuSO4 · H2O remains. What fraction of
the mass of CuSO4·5H2O has been lost?
(a) 0.072
(b) 0.289
(c) 0.361
(d) 0 406
(e) 0.711
19. Element "J" forms the stable compounds J(NO3)3, JS and JSO4. Which one of the following could
be "J"?
(a) Sodium
(b) Iron
(c) Carbon
(d) Magnesium
(e) Copper
20. Which molecule is most polar?
(a) H2O
(b) N2
(c) CH4
21. Nitric acid is made when
(a) NO (g) is bubbled through water
(c) HNO2 is reduced
(e) NO2 (g) is added to water
Last Revised by D. Lougheed 7/3/00
(d) CO2
(e) Cl2
(b) Steam acts on an alkali metal nitrate
(d) Ice is dropped into liquid ammonia
22. The vapour pressure at equilibrium of a pure liquid depends mainly on the
(a) volume of liquid present
(b) size of the container
(c) atmospheric pressure
(d) density of the liquid
(e) temperature of the liquid
23. A solid which melts at 1083°C, is malleable and conducts an electric current, is
(a) an organic polymer
(b) a metal
(c) a salt
(d) a polar covalent compound
(e) a nonpolar covalent compound
24. What mass of ammonia, is found in 300 mL of a 0.196mol/L solution of NH3 in water?
(a) 1.0 g
(b) 0.06 g
(c) 0.20 g
(d) 3.3 g
(e) 11.1 g
25. The equilibrium vapors pressure of water in air is 3.5 kPa at 27°C What mass of water is present in
one litre of air?
(a) 10 mg
(b) 18 mg
(c) 25 mg
(d) 63 mg
(e) 190 mg
26. Ethanoic (acetic) acid is a week acid with K = 1.8 x10 -5. If 100 mL of a 0.10 mol/L solution of
ethanoic acid is mixed with 200 mL of a 0.10 mol/L solution of sodium hydroxide, what is the
approximate pH of the resulting solution?
(a) 1.5
(b) 4.7
(c) 7.0
(d) 9.3
(e)12.5
27. The main gaseous product of the reaction of zinc metal with dilute aqueous hydrochloric acid is
(a) Carbon dioxide
(b) Zinc oxide
(c) Chlorine (d) Hydrogen
(e) Oxygen
28. Pick the weakest (poorest) Lewis acid:
(a) H+
(b) SO2
(c) PCI5
(d) PF3
29. Which of the following can function as a Brønsted-Lowry base?
(1) NH3
(2) H2O
(3) CH3
(a) 1 only
(b) 3 only
(c) 1 and 2 only
(d) 2 and 3 only
(e) H2O
(e) 1, 2 and 3
30. A catalyst alters the
I - ∆H of a reaction
II - Mechanism of a reaction III - Activation energy of a reaction
(a) I only
(b) III only
(c) I and II only
(d) II and III only
(e) I, II and III
31. For this system at fixed pressure:
N2O4(g) ↔ 2NO2(g)
∆H = +58 kj/mol,
what is the effect of a small increase in temperature on the rate to the right (rate right), rate to the
left (rate left) and the equilibrium constant (Keq)?
rate right
rate left
Keq
(a)
higher
higher
higher
(b)
higher
higher
lower
(c)
higher
lower
higher
(d)
higher
lower
lower
(e)
lower
higher
lower
Last Revised by D. Lougheed 7/3/00
32. What is the order of the reaction
S2O82- + 2 I- ↔ 2 SO42- + I2
If the rate equation is
rate = (constant) (S2O82-) (I-) ?
(a) Zero
(b) One
(c) Two
(d) Three
(e) Four
33. Substance A decomposes according to the rate equation
Rate = k (A)
Forty minutes after a reaction begins, 70% of A still remains. What is the value of "k"?
(a) 12 s-1 (b) 28 s-1
(c) 40 s-1
(d) 9 x 10-3 s-1
(e) 1.5 x 10-4 s-1
34. If an acid is spilled, which material should be chosen to neutralize the acid without itself producing
hazardous effects.
(a) HCl (aq)
(b) NaCl (s) (c) Na (OH) (s)
(d) NH4Cl (aq)(e) NaHCO3 (s)
35. This equation represents the dissolution of calcium chloride in water:
water
CaCl2(s) ↔
CaCl2(aq)
∆H = -75.6 kJ
When 30 g of calcium chloride is dissolved in water in a well-insulated calorimeter, the
temperature of the solution
(a) increases as a result of the reaction
(b) decreases as a result of the reaction
(c) remains the same, but heat is given off to the surroundings
(d) remains the same, but heat is absorbed from the surroundings
(e) increases, but heat is absorbed from the surroundings
36. Select the compound that is not white:
(a) Sodium nitrate
(b) Copper(II) chloride
(d) Magnesium oxide
(e) Calcium carbonate
(c) Aluminum sulfate
37. The pH of a sample, (1), of rainwater is measured as 5.5. Another sample, (2), has a pH of 4.9.
The ratio of hydrogen-ion concentrations, sample (2) : sample (1) is
(a) 0.25
(b) 0.5
(c) 0.89
(d) 2.0
(e) 4.0
38. Select the largest atom or ion from the following:
(a) F(b) Ne
(c) Na+
(d) Mg2+
(e) Al3+
39. Given the following standard reduction potentials:
Al3+ (aq) + 3e- → Al(s)
E° = -1.67 V
2+
Fe (aq) + 2e → Fe(s)
E° = -0.44 V
2+
Mg (aq) + 2e → Mg(s) E° = -2.34 V
Pb2+ (aq) + 2e- → Pb(s)
E° = -0.13 V
2+
Zn (aq) + 2e → Zn(s)
E° = -0.76 V
what is the strongest oxidizing agent in the above series?
(a) Al3+ (aq)
(b) Fe2+ (aq) (c) Mg2+ (aq)
(d) Pb2+ (aq) (e) Zn2+ (aq)
Last Revised by D. Lougheed 7/3/00
40. What is ∆ E° for the reaction
Zn(s) + 2 H+ (aq) → H2(g) + Zn2+ (aq)
(a) +0.76 V
(b) +1.52 V (c) +0.38 V (d) -0.38 V
(e) -0.76 V
41. In this reaction:
H2S(aq) + I2(aq) → S(s) + 2 H+(aq) + 2 I-(aq)
the reducing agent is
(a) H2S(aq)
(b) I2(aq)
(c) S(s)
(d) H+(aq)
(e) I-(aq)
42. Compared to the elements of the halogen group, the elements at the left of the periodic table
(groups 1 and 2)
(a) are stronger oxidizing agents
(b) are of similar oxidizing or reducing power
(c) are stronger reducing agents
(d) are more readily reduced
(e) react readily with reducing agents
43. Which compounds are isomers?
(1) H3C-CO-CH3
(2) H3C-CH2-O-CH3
(3) H3C-CH2-CHO (4) HC=CH2-CHO
(a) (1) and (2) (b) (2) and (3)
(c) (3) and (4)
(d) (1) and (3)
(e) (2) and (4)
44. The most highly oxidized molecule of the following five is:
(a) H3C-CH2-CHO
(b) H3C-CO-CH3
(c) H3C-CH2-CH2OH
(d) H3C-CH2-COOH (e) H3C-CH2-CH3
45. Nitrogen and oxygen are the most abundant components of Earth's atmosphere For dry air near the
surface of Earth, which substance is next greatest in abundance?
(a) Carbon dioxide
(b) Sulfur dioxide
(c) An oxide of nitrogen
(d) Argon
(e) Ozone
46. Given Ksp = 1.0 x 10-8 for CaCO3, and Ksp = 5 x 10-9 for BaCO3 in water at 25°C, what is the
value of
[Ba2+] / [Ca2+]
in a solution in equilibrium with both solids at the same time?
(a) 5
(b) 2
(c) 1
(d) 0.7
(e) 0.5
47. The standard enthalpy (heat) of formation of SiCl4(/) is -640.1 kJ/mol. How much heat is evolved
when 10.0 g of Si and 100 g of Cl2 react?
(a) 228 kJ
(b) 451 kJ
(c) 909 kJ
(d) 1806 kJ (e) 6401 kJ
1991
1.
Which of the following is a fundamental unit of the Système International?
(a) Joule
(b) Pascal
(c) Newton (d) Ampere (e) Einstein
2.
Which substance has the lowest freezing point?
(a) Nitrogen
(b) Carbon dioxide (c) Propane
Last Revised by D. Lougheed 7/3/00
(d) Mercury (e) Gold
3.
4.
5.
The most polar molecule in this list is:
(a) PCl5
(b) OF2
(c) SF6
(d) F2
(e) SiF4
Select the one ionic radius that is clearly incorrect :
(a) 136 pm for F(b) 171 pm for N3(d) 193 pm for Se2(e) 213 pm for O2-
(c) 184 pm for S2-
Which pair of elements is nearest in atomic radius?
(a) Carbon and silicon
(b) Silicon and germanium
(d) Tin and lead
(e) Carbon and germanium
(c) Germanium and tin
6.
How many pairs of unshared (nonbonding) valence electrons are on the central atom of an XeF2
molecule?
(a) Zero
(b) One
(c) Two
(d) Three
(e) Four
7.
If one atom of copper has a radius of 128 pm, what is the average density in one atom of copper?
(a) 2.02 g/cm3
(b) 4.19 g/cm3
(c) 9.0 g/cm3
3
3
(d) 10.5 g/cm
(e) 12.0 g/cm
8.
Natural copper is a mixture of only two isotopes, one of which has29 protons, 34 neutrons and a
relative abundance of 69.17%. The relative atomic mass of natural copper is 63.6. How many
neutrons must there be in the second isotope?
(a) 29 neutrons
(b) 32 neutrons
(c) 35 neutrons
(d) 36 neutrons
(e) 38 neutrons
9.
Which one of the following elements has the highest first ionization energy?
(a) Lithium
(b) Boron
(c) Nitrogen
(d) Sodium (e) Phosphorus
10.
The difference between a strong acid and a weak acid is that
(a) Strong acid is always more concentrated
(b) weak acids are less soluble than strong acids
(c) weak acids have a smaller degree of dissociation than strong acids
(d) strong acids don't exist in dilute solutions
(e) weak acids are better electrical conductors than strong acids
11.
Which one of the following is an example of a covalently bonded solid that does not contain
discrete molecules?
(a) Dry Ice (carbon dioxide)
(b) Quartz (silicon dioxide)
(c) Copper
(d) Paraffin wax
(e) Sodium chloride
12.
Which molecule has the greatest bond dissociation energy?
(a) H2
(b) F2
(c) N2
(d) O2
13.
(e) Cl2
If the hydroxide ion concentration in an aqueous solution is 5.0 x 10 -5 mol/L, what is the pH?
(a) 4.3
(b) 5.0(c) 5.7
(d) 9.0
(e) 9.7
Last Revised by D. Lougheed 7/3/00
14.
If copper reacts according to this unbalanced equation, how many moles of nitric acid are required
for every mole of copper consumed?
__ Cu(s) + __ HNO3(aq) → __ Cu(NO3)2(aq) + __ NO(g) + __ H2O
(a) 2/3 mol
(b) 1 mol
(c) 4/3 mol (d) 3/2 mol (e) 8/3 mol
15.
The oxidation state, +1 is
(a) found only in the periodic group headed by lithium
(b) the most stable oxidation state of the boron group
(c) most stable for bismuth among all the p-block elements
(d) more stable at the bottom of the boron group than at the top
(e) common for all the elements from lithium to fluorine
16.
Given that the bond dissociation energy for H-H is 436 kJ/mol and that for C-H is 413 kJ/mol, and
the sublimation energy for graphite is 716 kJ/mol, what is the heat (enthalpy) of formation of
methane?
(a) - 46 kJ/mol
(b) - 64 kJ/mol
(c) - 133 kJ/mol
(d) - 1588 kJ/mol
(e) - 1652 kJ/mol
17.
To the equilibrium system shown below, a little PCl3 is added. What happens?
PCl5 ↔ PCl3 + Cl2
(a) The amounts of all substances increase
(b) The amounts of all substances decrease
(c) The amounts of PCl5 and Cl2 both increase
(d) The amount of PCl5 decreases ; Cl2 increases
(e) The amount of PCl5 increases; Cl2 decreases
18.
If a weak acid is 5.0% ionized in 0.10 mol/L aqueous solution, what will be the percentage
ionization in 0.20 mol/L solution?
(a) Exactly double (10.0%)
(b) Slightly greater than 5.0 %
(c) The same (5.0%)
(d) Slightly less than 5.0%
(e) Exactly half (2.5%)
19.
Which of the following aqueous mixtures is a buffer solution when equal volumes are mixed?
(a) 1.0 M H2SO4 mixed with 1.0 M HCl
(b) 1.0 M NH3 mixed with 1.0 M NaOH
(c) 0.5 M KOH mixed with 1.0 M HNO3
(d) 0.5 M H3C-COOH mixed with 0.5 M HCl
(e) 0.5 M HCl mixed with 1.0 M NH3
20.
Which functional group does not contain an oxygen atom?
(a) An amide (b) An amine
(c) An aldehyde
Last Revised by D. Lougheed 7/3/00
(d) An alcohol
(e) An ester
21.
Reaction of OH-(aq) with H3C-CH2Br will make
(a) H3C-CH2OH(aq) and Br(aq)
(b) H2C = CH2(g) , Br(aq) and H2O
(c) HOCH2-CH2Br(aq)
(d) H3C-CH(OH)Br(aq)
+
(e) H3C-CH2 and HOBr(aq)
22.
Atoms of which element are being oxidized in the following reaction?
2 KCl(aq) + MnO2(s) + 2 H2SO4(aq) ↔ K2SO4(aq) + MnSO4(aq) + Cl2(g) + 2
H2O
(a) Potassium (b) Chlorine (c) Manganese
(d) Oxygen (e) Sulfur
23.
At the surface of Earth (27°C) a weather balloon is filled with helium to a pressure of 100 kPa,
when it has a volume of 1000 m3. The balloon rises until the pressure is 40 kPa and its volume has
become 2000 m3. What is the temperature in the balloon?
(a) +1227°C
(b) +102°C (c) -213°C (d) -123°C (e) -33°C
24.
Nitrogen atoms in the salt ammonium nitrate have formal oxidation numbers of
(a) +1 in the cation, -1 in the anion
(b) +1 in the cation, +1 in the anion
(c) -1 in the cation, +1 in the anion
(d) 0 in the cation, +2 in the anion
(e) -3 in the cation, +5 in the anion
25.
Select the one incorrect statement:
(a) H3C-CH2OH is more highly oxidized than CO
(b) H2C=CH2 is more highly reduced than H3C-CHO
(c) H3C-CHO is more highly oxidized than H3C-CH2OH
(d) H3C-CH3 is more highly reduced than H2C=CH2
(e) CH3-CHO is more highly oxidized than H3C-CH3
26.
What is the major product of the ionic reaction between propene and hydrogen bromide?
(a) BrCH2-CH = CH2
(b) H3C-CBr = CH2
(c) H3C-CH = CHBr
(d) H3C-CH2-CH2Br
(e) H3C-CHBr-CH3
27.
What is the enthalpy (heat) change for this reaction under standard conditions?
2 SO2(g) + O2(g) ↔ 2 SO3(g)
°
∆ Hf for SO3(g) = -395 kJ/mol
°
∆ Hf for SO2(g) = -297 kJ/mol
(a) -98 kJ/(mol O2)
(b) -196 kJ/(mol O2)
(d) -1384 kJ/(mol O2) (e) + 101 kJ/(mol O2)
Last Revised by D. Lougheed 7/3/00
(c) -692 kJ/(mol O2)
28.
+
2+
The energy input for M(g) = M(g) + e- will be greatest if M is
(a) Sodium
(b) Boron
(c) Carbon (d) Nitrogen (e) Oxygen
29.
Choose the correct statement about these two reactions:
-1
F- + BF3 ↔
BF4
F- + H2O ↔ HF + OH(a) F- does not act as a Lewis acid or base in either of these reactions
(b) F- acts as a Lewis base in both of these reactions
(c) F- acts as a Lewis base only in the first reaction
(d) F- acts as a Lewis acid only in the second reaction
(e) F- acts as a Lewis acid in both of these reactions
30.
A sodium chloride solution (0.200 mol/L) is slowly added to 50.0 ml of a 0.130 mol/L aqueous
solution of silver nitrate. What volume of sodium choride solution has been added when [Ag+} =
[Cl-]?
For AgCl, Ksp = 1.8 x 10-10 at 25°C
(a) 100 mL
(b) 82.5 mL (c) 76.9 mL (d) 50.0 mL (e) 32.5 mL
31.
What is Ksp for silver iodide if the solubility in water is 9.0 x 10-9 mol/L at 25°C?
(a) 9.5 x 10-5
(b) 1.8 x 10-8
(c) 4.5 x 10-9
(d) 8.1 x 10-17
(e) 9.5 x 10-18
32.
Which is the most soluble salt in water at 25°C?
(a) AgCl
Ksp = 1.8 x 10-10
(b) Ag2CO3
(c) AgBr
Ksp = 5.0 x 10-13
(d) Ag3PO4
(e) Ag S
Ksp = 8.0 x 10-51
Ksp = 8.1 x 10-12
Ksp = 1.8 x 10-18
2
33.
If a small, neutral atom at its lowest energy has only three valence electrons, it is likely to belong
to the periodic group (column) headed by
(a) Beryllium (b) Boron
(c) Carbon (d) Nitrogen (e) Oxygen
34.
Select the one false statement:
(a) Activation energy depends on the reaction mechanism
(b) Reaction rate depends on the energy of activation
(c) A catalyst can decrease the energy of activation
(d) Activation energies are always positive
(e) Activation energy is determined by the overall reaction energy
Last Revised by D. Lougheed 7/3/00
35.
Initial rates and concentrations are measured for the following reaction:
2 NO(g) + 2 H2(g) → N2(g) + 2 H2O(g)
Initial [NO]
Initial [H2]
Initial Rate
(mol/L)
(mol/L)
(mol L-1 s-1)
0.0005
0.0005
0.000025
0.0005
0.0010
0.000050
0.0010
0.0010
0.00020
The rate equation for the reaction is
(a) Rate = k [NO]
(b) Rate = k [NO]2
(c) Rate = k [NO] [H2]
(d) Rate = k [NO]2 [H2]2
(e) Rate = k [NO]2[H2]
36.
To 150 mL of 0.20 mol/L NaOH(aq), 50 mL of 0.10 mol/L H2SO4(aq) is added. What is the
concentration of sodium ions in the solution?
(a) 0.30 mol/L
(b) 0.25 mol/L
(c) 0.20 mol/L
(d) 0.15 mol/L
(e) 0.10 mol/L
37.
A certain amount of electricity passes through a cell in which 27.9 g Fe(s) is deposited from
FeSO4(aq). How much Au(s) would be deposited if the same amount of electricity passed through
K[AuCl4](aq)?
(a) 27.9 g
(b) 32.8 g
(c) 65.7 g
(d) 98.5 g
(e) 131 g
38.
The molecule H3C-CH2-CO-OCH3 is named
(a) Ethyl ethanoate
(b) Propyl methanoate
(d) Butanoic acid
(e) Methyl propanoate
(c) Ethyl acetate
39.
Which one of the following particles would not be deflected in a magnetic field?
(a) An alpha particle
(b) A beta particle
(c) A positron
(d) A proton
(e) A neutron
40.
Which monomer would be used to make the polymer polyvinylidene chloride,
-(CCl2-CH2-CCl2-CH2)n- ?
(a) CH2=CCl2
(b) CH2=CHCl
(c) CHCl=CHCl
(d) CH2=CH2
(e) CH3-CHCl2
41.
When 100 mL of 1.00 mol/L NaOH(aq) at 25.0°C is added to 200 mL of 1.00 mol/L HCl(aq) at
25.0°C, the temperature of the mixture rises to 29.4°C. Assuming no heat loss to the surroundings,
the heat of reaction for
H+(aq) + OH-(aq) = H2O(liq)
is therefore about
(a) 56 kJ/mol
(b) 28 kJ/mol
(c) 11.2 kJ/mol
(d) 5.6 kJ/mol
(e) 2.8 kJ/mol
Last Revised by D. Lougheed 7/3/00
42.
Which pair of solutions (all are 0.10 mol/L aqueous) would result in a titration curve like this one?
14
12
10
8
pH
6
4
2
0
0
10
20
15
Volume of Base Added (mL)
(a) H2SO4 with NaOH
(b) H3C-COOH with KOH
(c) HCl with NaCl
(d) HC2H3O2 with KOH
(e) HNO3 with NH3
43.
5
25
Which indicator should be chosen for the titration of 0.10 mol/L HCl by the addition of 0.10 mol/L
NH3? for NH3, Kb = 1.8 x 10-5 at 25°C
Indicator
(a) Thymol blue
(b) Methyl red
(c) Litmus
(d) Thymol blue
(e) Alizarin yellow
pH
1-3
4-6
6-8
Colour change
red - yellow
red - yellow
red - blue
8 - 10
yellow - blue
10 - 12
yellow – lavender
44.
Four gases (1.00 mol Cl2, 2.00 mol IBr, 3.00 mol ClBr, and 4.00 mol ICl) are placed in a container
and allowed to come to equilibrium (temperature is constant; K = 4.0). What is the final amount of
Cl2?
Cl2(g) + IBr(g) ↔ ClBr(g) + ICl(g)
(a) 0.80 mol
(b) 1.20 mol (c) 1.40 mol (d) 1.60 mol (e) 1.80 mol
45.
What is the standard cell voltage for
Cd(s) + 2 Ag+(aq) ↔ Cd2+(aq) + 2 Ag(s)?
E°= + 0.799 V for Ag+(aq) + e- → Ag(s)
E°= - 0.402 V for Cd2+(aq) + 2 e- → Cd(s)
(a) + 0.397 V (b) + 0.799 V
(c) +1.000 V
(d) + 1.201 V
Last Revised by D. Lougheed 7/3/00
(e) +2.000 V
1994
1.
2.
3.
Which element is NOT part of the beryllium group?
(a) Radium
( b) Barium (c) Calcium
(d) Vanadium (e) Magnesium
Which one of the following contains a triple bond?
(a) CO2
(b) SiC
(c) Diamond
(d) C2H2
Select the compound that is an isomer of ethanol:
(a) H3CCHO
(b) H3CCH2CH2OH
(d) H3COCH3
(e) H3CCOCH3
(e) C2H4
(c) H3CCH2Br
4.
Identify the compound that shows the LEAST hydrogen bonding in the following list.
(a) H3CCH2OH
(b) H3CNH2 (c) HF
(d) SiH4
(e) NH3
5.
Analysis of the hydrocarbon CxHy reveals a hydrogen content of 11.84% by mass. What is the
simplest formula for the compound?
Relative atomic masses: H, 1.008; C, 12.01
(a) C5H8
(b) C3H4
(c) C2H5
(d) CH2
(e) CH
6.
Gaseous CO2 is bubbled into a solution of NH3 in water. Select the one correct statement:
(a) CO2 is reduced to CO by NH3
(b) A solution of an electrolyte is produced
(c) Most of the NH3 is expelled as a gas
(d) Carbonic acid and gaseous NO result
(e) Molecules of H2N−COOH are formed
7.
Which light photons have the highest energy?
(a) Red
(b) Blue
(c) Green
(d) Violet
The number of neutrons in one nucleus of 238U is
(a) 46
(b) 92
(c) 146
(d) 238
(e) 340
8.
9.
(e) Yellow
A student observes that dissolving potassium nitrate in room-temperature water causes the solution
to become cool. The student may safely conclude that
(a) The solubility of potassium nitrate will be greater in warm water than in room temperature
water
(b) No chemical change has occurred, as all chemical changes liberate energy
(c) The solubility of potassium nitrate will be less in warm water than room temperature water
(d) Potassium and nitrate ions have reacted to produce potassium nitrate molecules, and this
process requires energy
(e) A solubility - temperature prediction should not be made, because dissolving is merely a
physical process
Last Revised by D. Lougheed 7/3/00
10. Select the molecule with zero dipole moment:
(a) NH3
(b) NO2
(c) HOCl
(d) H2O
(e) BeF2
11. In solid sodium chloride, the centre of a sodium ion is separated from the centre of the nearest
chloride ion by 282 pm. How many sodium ions are there in 1.00 cm3 of sodium chloride?
(a) 1.8 x 107
(b) 5.4 x 1021
(c) 1.1 x 1022
(d) 2.2 x 1022
(e) 6.0 x 1023
12. In the relationship k = Z x 10−W/T, Z and W are constants. Use the following data to obtain a value
for W:
k
T
50
10
5
5
(a) −10
(b) −0.10
(c) 0.1
(d) 10
(e) 1010
13. H2S(g) burns in oxygen to make H2O(g) and SO2(g). Given the following enthalpies (heats) of
formation, what is the approximate enthalpy of combustion of H2S(g)?
H2(g) + S(s) → H2S(g)
∆H = −40 kJ/mol
H2(g) + Ω O2 → H2O(g)
∆H = −242 kJ/mol H2
S(s) + O2 → SO2(g)
∆H = −297 kJ/mol
(a) −579 kJ/(mol H2S)
(b) −499 kJ/(mol H2S)
(c) −95 kJ/(mol H2S)
(d) −55 kJ/(mol H2S)
(e) −15 kJ/(mol H2S)
14. At what temperature would the molar volume of an ideal gas be 100.0 L? Assume a standard
pressure of 100.0 kPa. At 100.0 kPa and 25°C the molar volume of an ideal gas is 24.790 L.
(a) 101°C
(b) 347°C
(c) 930°C
(d) 1057°C
(e) 1203°C
15. Graphite and carbon monoxide have standard enthalpies (heats) of combustion to CO2(g) of
−393 and −283 kJ/mol respectively. What is the standard enthalpy of formation of carbon
monoxide?
(a) −1069 kJ/mol
(b) −676 kJ/mol
(c) −535 kJ/mol
(d) −251 kJ/mol
(e) −110 kJ/mol
Last Revised by D. Lougheed 7/3/00
16. A proton approaches a molecule of ethanol:
H
H


aî
íb
íc
íd
H C  C O H


H
H
ëe
To which atom will the proton be most strongly attracted?
(a) Atom a
(b) Atom b
(c) Atom c
(d) Atom d
17. What is the overall order of the reaction
S2O82- + 2 I-1 → 2 SO42- + I2 (s)
if the rate equation is
rate = k[S2O82-][ I-1]
(a) Zero
(b) One
(c) Two
(e) Atom e
(d) Three
(e) Four
18. The isotope 209Pb decays by β− emission, losing 90.0% of its radioactivity in 10.80 h. What is its
half-life?
(a) 0.308 h
(b) 1.80 h
(c) 3.25 h
(d) 4.69 h
(e) 6.77 h
19. The atomic radius of a rubidium atom is 253 pm. The radius of the Rb+ ion is nearest to
(a) 10 pm
(b) 148 pm
(c) 253 pm
(d) 275 pm
(e) 300 pm
20. A catalyst alters the
(1) ∆H of a reaction
(2) activation energy of a reaction
(3) mechanism of a reaction
(a) (1), (2) and (3) are correct
(b) Only (1) and (2) are correct
(c) Only (2) and (3) are correct
(d) Only (2) is correct
(e) Only (3) is correct
21. "An acid is a proton donor." By this definition, which of the substances in the following system
exhibit acidic behaviour?
H2O + NH3 → NH4+ + OH−
(a) Both NH3 and NH4+
(b) Both H2O and NH4+
(c) NH4+ only
(d) NH3 only
(e) H2O only
Last Revised by D. Lougheed 7/3/00
The following data apply to Questions 22 to 24:
H2O(l) + 57 kJ → H+(aq) + OH−(aq)
Kw = 1.00 x 10−14 at 25°C
22. Raising the temperature of the water
(a) makes it more basic
(b) makes it more acidic
(c) does not alter the pH
(d) decreases the concentration of both H+(aq) and OH−(aq)
(e) increases the concentration of both H+(aq) and OH−(aq)
23. Select the correct relationship for pure water:
(a) pH + 1/pOH = 14
(b) pH = 1/pOH
(d) (pH) x (pOH) = Kw
(e) pH + pOH = pKw
(c) pH + pOH = Kw
24. The pH of an aqueous solution with [OH−] = 2.0 x 10−5 mol/L will be
(a) 4.70
(b) 9.30
(c) 9.70
(d) 10.50
(e) 10.70
25. Given the standard enthalpies (heats) of formation shown below, what is the heat of reaction for
HCOOH(l) → CO(g) + H2O(l)
∆Hf° −409
−110 −286 (all kJ/mol)
(a) −905 kJ/mol
(b) −805 kJ/mol
(c) −695 kJ/mol
(d) −585 kJ/mol
(e) +13 kJ/mol
26. Which of the following equilibria will be shifted to the right by an increase in temperature but to
the left by an increase in pressure?
(1)
CaCO3(s) ↔ CaO(s) + CO2(g), ∆H > 0
(2)
2 SO2(g) + O2(g) ↔ 2 SO3(g), ∆H < 0
(3)
2 HI(g) ↔ H2(g) + I2(g), ∆H > 0
(a) (1) and (3) only
(b) (1) and (2) only
(c) (2) and (3) only
(d) (1) only
(e) (2) only
27. Select the most highly oxidized molecule:
(a) H3C−CO−CH3
(b) H3C−CH2−CHO
(d) H3C−CH2−COOH
(e) H3C−CH2−CH2OH
(c) H3C−CH2−CH3
28. At a fixed, elevated temperature, the following equilibrium constants are determined:
K = 67 for
CoO(s) + H2(g) ↔ Co(s) + H2O(g)
and
K = 490 for
CoO(s) + CO(g) ↔ Co(s) + CO2(g)
What is K at the same temperature for
CO2(g) + H2(g) ↔ CO(g) + H2O(g) ?
(a) 67 x 490
(b) 1/490
(c) 67 (d) 67 − 490 (e) 67/490
Last Revised by D. Lougheed 7/3/00
29. If 1.0 mol/L aqueous NaOH is used to titrate each of the following 1.0 mol/L solutions to a
phenolphthalein endpoint, which acid will require the greatest volume of NaOH solution?
(a) 45 mL of sulfuric acid, H2SO4
(b) 60 mL of 1.0 mol/L maleic acid, HC(COOH)HC(COOH)
(c) 75 mL of hydrochloric acid, HCl
(d) 80 mL of formic acid, HCOOH
(e) 90 mL of acetic acid, H3CCOOH
30. If a 1.0 mol/L solution of a monoprotic weak acid is 10.0% ionized, its ionization constant is
(a) 0.9 x 102
(b) 0.9 x 10−2
(c) 1.1 x 10−2
(d) 1.1 x 102
(e) 0.10
31. The solubility product constant for AgBr in water at 25°C is 5.2 x 10−13. What is the aqueous
solubility of AgBr at 25°C?
(a) 5.2 x 10−13 mol/L
(b) 2.8 x 10−7 mol/L
(c) 7.2 x 10−7 mol/L
(d) 5.2 x 10−6 mol/L
(e) 5.1 x 10−5 mol/L
32. A2B is the salt of a strong acid and a strong base. At a constant temperature, a saturated solution of
A2B has a concentration of 0.020 mol/L. What is the concentration of A+ ions in the solution?
(a) 4.0 x 10−2 mol/L
(b) 2.0 x 10−2 mol/L
(c) 1.6 x 10−3 mol/L
−4
−7
(d) 4.0 x 10 mol/L
(e) 1.0 x 10 mol/L
33. What mass of SO3(g) results when 32.0 g of SO2(g) and 9.00 g O2(g) react according to
2 SO2(g) + O2(g) → 2 SO3(g) ?
Relative atomic masses: S, 32.066; O, 16.00
(a) 20.0 g
(b) 33.0 g
(c) 35.0 g
(d) 40.0 g
(e) 45.0 g
34. Compared to the elements of the halogen group, the elements at the left of the periodic table
(lithium and beryllium groups)
(a) are stronger oxidizing agents
(b) are stronger reducing agents
(c) are of similar oxidizing or reducing power
(d) are more easily reduced
(e) react readily with reducing agents
35. When the following half-reaction is balanced by inserting electrons and the correct coefficients:
__ OH− + __CrO2-1 → __ CrO42- + __ H2O
how many OH− are required for every CrO2-1?
(a) One (b) Two
(c) Three
(d) Four
36. Select the strongest oxidizing agent from among the following elements:
(a) Nitrogen
(b) Silicon
(c) Sodium
(d) Iodine
(e) Chlorine
37. In this reaction:
H2S(aq) + I2(aq) → S(s) + 2 H+(aq) + 2 I−(aq)
the reducing agent is
(a) H2S(aq)
(b) I2(aq)
(c) S(s)
(d) H+(aq)
(e) I−(aq)
Last Revised by D. Lougheed 7/3/00
(e) Five
38. What mass of N2(g) is required to fill a bicycle tire of volume 331 mL at 455 kPa and 25°C?
Relative atomic mass of N, 14.01
Ideal gas constant, R, 8.314 J mol−1 K−1
(a) 0.556 g
(b) 1.70 g
(c) 20.3 g
(d) 28.0 g
(e) 1.70 kg
The following data apply to Questions 39 and 40
Standard reduction potentials:
Al3+(aq) + 3 e− → Al(s)
E° = −1.67 V
Fe2+(aq) + 2 e− → Fe(s)
E° = −0.44 V
2+
−
Mg (aq) + 2 e → Mg(s) E° = −2.34 V
Pb2+(aq) + 2 e− → Pb(s)
E° = −0.13 V
2+
−
Zn (aq) + 2 e → Zn(s)
E° = −0.76 V
39. Select the metal that is the strongest reducing agent:
(a) Aluminum (b) Iron
(c) Magnesium
(d) Lead
(e) Zinc
40. What is E° for the reaction
2 Al(s) + 3 Zn2+(aq) → 2 Al3+(aq) + 3 Zn(s) ?
(a) +5.62 V
(b) +2.43 V (c) +0.91 V (d) +0.00 V (e) −0.91 V
1995
1.
Select the structural isomer of
(H3C)2CH−CH2−CH2−CH3
(a) H3C−CH2−CH2−CH3
(b) H3C−CH−CH3

H3C−CH2
(c) H3C

H3C−CH−CH2−CH3
(d) (H3C)2−CH−CH(CH3)2
(e) H3C−CH2−CH=CH−CH2−CH3
2.
What is the official (IUPAC) name for this compound?
HOCH2
CH3


H3C−CH−CH−CH−CH2−CH3

CH2−CH3
(a) 2-methyl-3,5-diethyl-2-pentanol
(c) 3,5-dimethyl-4-ethyl-6-hexanol
(e) 3-decanol
Last Revised by D. Lougheed 7/3/00
(b) 2-methyl-3-isobutyl-1-pentanol
(d) 2,4-dimethyl-3-ethyl-1-hexanol
3.
Select the substitution reaction:
(a) C2H5Cl + Cl2 → C2H4Cl2 + HCl
(b) 2 C6H6 + 15 O2 → 12 CO2 + 6 H2O
(c) C3H6 + HCl → C3H7Cl
(d) H3CCOOH + H2O → H3O+ + H3CCOO−
(e) C3H7Cl + OH− → C3H6 + H2O + Cl−
4.
Which molecule is an ester and also an amide?
O

(a) H2N−CH2−C−H
O

(b) H2N−CH2−C−OCH3
O

(c) H2N−CH2−C−OH
O

(d) H2N−CH2−C−NH2
O
O


(e) H3C−C−OCH2C−NH2
5.
Normal boiling points increase in the order
(a) CH4 < C2H5OH < C4H10
(b) CH4 < C4H10 < C2H5OH
(c) C4H10 < C2H5OH < CH4
(d) C2H5OH < C4H10 < CH4
(e) C2H5OH < CH4 < C4H10
6.
Which molecule has a triple bond?
(a) C H
(b) NO −
(c) SO 2−
2
7.
4
3
3
(d) HCN
(e) NH3
In cellular respiration, glucose, C6H12O6, is converted into water and carbon dioxide. Such a
reaction is
(a) exothermic, and oxygen is the oxidant
(b) exothermic, and oxygen is the reductant
(c) exothermic, and oxygen is neither reductant nor oxidant
(d) endothermic, and oxygen is the reductant
(e) endothermic, and oxygen is the oxidant
Last Revised by D. Lougheed 7/3/00
8.
Which statement about water is incorrect?
(a) Water is a good solvent for KNO3
(b) Water has a greater density than liquid hydrocarbons at the same temperature
(c) The solvent behaviour of water is strongly associated with the polar character of its V-shaped
molecules
(d) Pure water conducts electricity better than aqueous KNO3
(e) Water expands as it is warmed above 4°C, and also expands as it freezes
9.
Select the incorrect generalization about the relative properties of typical metals and typical ionic
solids.
(a) Metals are deformable; ionic solids are brittle
(b) Metals have high thermal conductivity; ionic solids are poor thermal conductors
(c) Metals have high melting points; ionic solids have low melting points
(d) Metals have higher density; ionic solids have lower density
(e) Metals have high electrical conductivity; ionic solids are poor conductors
10. What is the approximate energy released in the reaction
CH4(g) + Br2(g) → CH3Br + Hbr,
given these average bond energies in kJ/mol?
H−H 436
C−Br 288
Br−Br 194
C−H 413
H−Br 366
C−C 348
(a) 47 kJ/mol
(b) 141 kJ/mol
(d) 435 kJ/mol
(e) 685 kJ/mol
(c) 297 kJ/mol
11. In which one of the following (all are in their lowest-energy configuration) are all the electrons
paired?
(a) An element with electronic configuration 1s2 2s2 2p4
(b) Atomic oxygen
(c) A neutral atom with 15 protons
(d) Fe3+
(e) N3−
12. Which one of the following is planar?
(a) BeF42−
(b) BF3
(c) CF4
Last Revised by D. Lougheed 7/3/00
(d) NF3
(e) PF3
13. Energies for reactants, products, and three possible activation complexes are shown on the graph
below.
D
C
B
PE
(kJ/mol)
A
E
Reaction Coordinate
Which reaction is expected to be most rapid?
(a) from A through B to E
(b) from A through C to E
(c) from A through D to E
(d) from E through B to A
(e) from E through D to A
14. How long will it take for 1.0% of the radio-active carbon-14 in your body to decay? The half-life
of carbon-14 is 5730 years.
(a) 57 years
(b) 83 years (c) 102 years
(d) 123 years
(e) 141 years
15. A few atoms of an element of atomic number 111 and mass number 272 were made last December
by bombarding a target of 20983Bi atoms (mass number 209) with a beam of 28Ni ions. One
neutron was released for each atom of element 111 made. What was the mass number of the nickel
ions?
(a) 63
(b) 64
(c) 111
(d) 121
(e) 160
16. Select the incorrect chemical equation:
_
_
(a) Na + e → Na+ + energy
(b) Mg + energy → Mg2+ + 2e
_
(c) H2 + energy → 2 H+ + 2e
_
(d) F + e- → F + energy
_
(e) Ne+ + e → Ne + energy
17. The rate of the chemical reaction between substances A and B follows the equation
rate = k[A]2[B]
where “k” is a constant. If the initial concentration of A is halved, what should be done to the
initial concentration of B to make the reaction go, initially, at 75% of its former rate? The initial
concentration of B should be
(a) kept constant
(b) doubled (c) tripled
(d) halved
(e) multiplied by 4/3
Last Revised by D. Lougheed 7/3/00
18. Which system, initially at equilibrium reacts toward the left upon an increase in external pressure,
but toward the right upon an increase in temperature?
(a) 2 NO2(g) + 54 kJ ↔ 2 NO(g) + O2(g)
(b) H2(g) + I2(g) ↔ 2 HI(g) + heat
(c) PCl3(g) + Cl2(g) ↔ Pcl5(g),
∆H = +16.6 kJ/mol
(d) CaO(s) + CO2(g) ↔ CaCO3(s) + heat
(e) N2(g) + 3 H2(g) ↔ 2 NH3(g) + 100 kJ
19. Select the reaction in which the entropy of the chemical system decreases. In each case temperature
is held constant.
(a) H2O(l) → H2O(g)
(b) H2(g, 200 kPa) → H2(g, 100 kPa)
(c) PCl5(g) → PCl3(g) + Cl2(g)
(d) Na(s) → Na(l)
+
(e) Ag (aq) + Cl (aq) → AgCl(s)
20. BaSO4 is used in the radiographic investigation of the gastrointestinal tract because it has a low
solubility and is opaque to X-rays. Still, some patients are allergic to barium ions. You have
added solid BaSO4 to water to make a saturated solution, but wish to lower [Ba2+] substantially
prior to ingestion by the patient. Which procedure would you recommend, given that
Heat + BaSO4(s) → Ba2+(aq) + SO42−(aq)?
(a) Heat the mixture
(b) Add sulfuric acid until [H+] = 2 mol/L
(c) Add more solid barium sulfate
(d) Remove some of the saturated solution
(e) Add enough sodium sulfate to produce [Na+] = 0.05 mol/L
21. Identify the one false statement among the following:
(a) A system at chemical equilibrium has a constant mass
(b) A system in chemical equilibrium acts so as to oppose slight disturbances
(c) Reactant and product concentrations vary with time in a system at chemical equilibrium
(d) Forward and reverse reactions proceed at the same rate in a system at chemical equilibrium
(e) A system at chemical equilibrium must have a constant temperature
22. A mixture of exactly 1.00 mol of each of the four gases shown below is allowed to come to
equilibrium at a fixed temperature. What is the final amount of ClBr(g) if K = 4.0?
IBr(g) + Cl2(g) = ClBr(g) + ICl(g)
(a) 0.33 mol
(b) 0.40 mol (c) 0.67 mol (d) 1.33 mol (e) 1.60 mol
23. a solution of pH = 4.35, what is [H+]?
(a) 6.7 x 10−3 mol/L
(b) 3.5 x 10−4 mol/L
(d) 3.5 x 10−5 mol/L
Last Revised by D. Lougheed 7/3/00
(e) 4.5 x 10−5 mol/L
(c) 4.5 x 10−4 mol/L
24. At a high, constant temperature, these equilibrium constants are determined:
K = 67 for
CoO(s) + H2(g) = Co(s) + H2O(g)
K = 490 for
CoO(s) + CO(g) = Co(s) + CO2(g).
What is K at the same temperature for
CO2(g) + H2(g) = CO(g) + H2O(g)?
(a) 1/490 (b) 67 - 490
(c) 67/490
(d) 67
(e) 490 x 67
25. For this system at chemical equilibrium, identify the false claim.
2 SO3(g) = 2 SO2(g) + O2(g)
(a) SO2 is produced at the same rate as it is consumed
(b) The number of moles of SO3 is the same as the number of moles of SO2
(c) SO3 is continually decomposing
(d) The mass of SO3 remains constant
(e) Changing the temperature changes the amount of oxygen in the system
26. What is [H+] in a 0.15 mol/L solution of ethanoic (acetic) acid in water at 25°C if Ka = 1.8 x 10−5?
(a) 1.1 x 10−2 mol/L
(b) 1.6 x 10−3 mol/L
(c) 1.2 x 10−4 mol/L
(d) 1.8 x 10−5 mol/L
(e) 2.7 x 10−6 mol/L
27. Which one of these ions will make an aqueous solution basic?
(a) Na+ (b) Br− (c) H3C−COO−
(d) HSO4−
(e) H+
28. What is the concentration of silver ions in a saturated silver bromide solution? The solubilityproduct constant for silver bromide at 25°C is 3.3 x 10−13.
(a) 4.3 x 10−5 mol/L
(d) 2.8 x 10−7 mol/L
(b) 7.0 x 10−5 mol/L
(e) 3.3 x 10−13 mol/L
(c) 5.7 x 10−7 mol/L
29. Ka1 for the loss of the first proton from sulfuric acid is very large, but Ka2 for the loss of the second
proton is about 0.01. In a 0.10 mol/L aqueous solution of sulfuric acid the correct order of
increasing concentration will be
(a) [SO 2−] < [HSO −] < [H SO ]
(b) [H SO ] < [HSO −] < [SO 2−]
4
4
2
(c) [HSO4−] < [SO42−] < [H+]
(e) [SO 2−] < [HSO −] < [H+]
4
4
2
(d) [SO4
4
2−
4
] < [H ] < [HSO4−]
4
+
4
30. Neutralization is reached if 41.32 mL of 0.1077 mol/L aqueous HCl solution is mixed with 50.00
mL of aqueous sodium hydroxide solution. What was the concentration of the sodium hydroxide
solution before the mixing?
(a) 0.0890 mol/L
(b) 0.131 mol/L
(c) 0.222 mol/L
(d) 7.66 mol/L
(e) 11.2 mol/L
Last Revised by D. Lougheed 7/3/00
31. H2O and H+ have been omitted from this skeleton oxidation-reduction equation. When the
equation has been balanced, what is the ratio of the number of H2O to the number of Cr3+?
Cr O 2− + I → Cr3+ + IO −
2
(a) 1.20
(b) 1.70
7
(c) 2.00
2
3
(d) 2.83
(e) 3.40
32. These two reactions are combined into a working galvanic cell:
Ag+(aq) + e− → Ag(s)
E° = +0.80 V
Sn2+(aq) + 2e− → Sn(s)
What is the standard cell potential?
(a) 1.74 V
(b) 1.08 V
(c) 0.94 V
(d) 0.66 V
E° = −0.14 V
(e) 0.52 V
33. The ion containing bromine in its highest oxidation state is
(a) Br+ (b) BrO−
(c) BrO −
(d) BrO −
(e) BrO −
2
3
4
34. Select the reaction that is not an oxidation-reduction reaction:
(a) CH4(g) + Br2(g) → CH3Br(g) + HBr(g)
(b) 2 Na(s) + 2 H2O(l) → 2 NaOH(aq) + H2(g)
(c) 2 H2(g) + O2(g) → 2 H2O(l)
(d) 3 HNO2(aq) → HNO3(aq) + 2 NO(g) + H2O(l)
(e) CO2(g) + Ca(OH)2(s) → CaCO3(s) + H2O(l
35. During the discharge of a lead storage battery, both electrodes build up a layer of
(a) PbO2
(b) PbO
(c) Pb3O4
(d) PbSO4
(e) Pb metal
36. To what temperature should 1.00 L of an ideal gas at 25°C be heated to change its volume to
4.00 L?
(a) 100°C
(b) 200°C
(c) 801°C
(d) 920°C
(e) 1193°C
1996
1.
Which one of the following compounds has the highest boiling point under standard pressure?
(a) CH4 (b) C2H6
(c) C2H4
(d) C3H8
(e) C4H10
2.
The compound H3CCOCH3 belongs to the family of
(a) alcohols
(b) aldehydes
(c) carboxylic acids
3.
(d) ethers
(e) ketones
If 1.00 mol of an ideal gas occupies 1.00 m3 at 1.00 kPa, what must be the Kelvin temperature?
The ideal gas constant is 8.314 J·mol-1·K-1.
(a) 0.120 K
(b) 120 K
(c) 273 K
(d) 8 314 K (e) 120 000 K
Last Revised by D. Lougheed 7/3/00
4.
What is the IUPAC name for this compound?
H
H
H
C
H
H
C
H
H H
C
H H
C
C
C
C
H
H
H
H
(a) 2-methyl-4-propylhexane
(c) 2-methyl-4-ethylhexane
(e) 2-methyl-4-ethylheptane
5.
H
H
H
H
C
C
C
H
H
H
H
(b) 3-isobutylhexane
(d) 3-methyl-5-ethylheptane
Select the compound that is most highly oxidized.
(a) CH3COOH (b) CH3CH2NH2
(c) CH3CH3
(d) CH3CH2OH
(e) CH3CHO
6.
Helium is the second most abundant element in the universe, but it is rare on Earth. This is because
(a) Helium is more dense than air
(b) Helium nuclei have fused to form heavier elements on Earth
(c) Helium remains trapped underground
(d) Radioactive decay occurs slowly on Earth
(e) Helium readily escapes Earth’s gravitational pull
7.
Which substance should be the most soluble in the nonpolar solvent pentane, C5H12?
(a) AgBr
(b) LiBr
(c) CsBr
(d) MgBr2
(e) Br2
8.
What is the correct electronic configuration for a sulphur atom in its lowest energy state?
(a) 1s22s22p43s23p43d2
(b) 1s22s22p63s23p6
(c) 1s22s22p63p6
(d) 1s22s22p63s33p4
(e) 1s22s22p63s23p2
9.
Which molecule has the strongest bond?
(a) N2
(b) F2
(c) Na2
(d) Au2
(e) I2
10. Which ion will bind water molecules most strongly?
(a) Mg2+
(b) Na+
(c) Cs+
(d) Ba2+
(e) Br-1
11. Select the molecule or ion that is square planar.
(a) CF4
(b) BF4-1
(c) PF4-1
(e) XeF4
(d) SF4
12. The formation of atoms of element 106 (isotope of mass number 263) is accompanied by the
releases of at least one neutron. This is achieved by bombarding element 98 (mass number 249
with another element, E. Element E must be
(a) nitrogen
(b) oxygen
(c) aluminum (d) silicon
(e) iron
Last Revised by D. Lougheed 7/3/00
13. A soluble salt affects the freezing and boiling points of water in which of the following ways?
(i)
it raises the freezing point
(ii)
it lowers the freezing point
(iii)
it lowers the boiling point
(iv)
it raises the boiling point
(a) I, II and III only
(b) I and III only
(c) II and IV only
(d) IV only
(e) I and IV only
14. Which factor does not, in general, affect the rate of reaction between two substances in the same
solution?
(a) The energy released in the reaction
(b) The temperature of the solution
(c) The collision frequency of the particles
(d) The orientation of the particles
(e) The activation energy
15. The activation energy of a chemical reaction
(a) depends on whether or not reactant collisions generate products
(b) varies with concentrations of the reactants
(c) is directly proportional to the Kelvin temperature
(d) is the energy difference between products and reactants
(e) is the energy required to form the activated complex
16. Which process has the largest energy output per mole of product?
(a) 21H + 21H → 23H e
(b) H2O(g) → H2O(l)
+ 01n
(c) H2 (g) → H(g) + H(g)
(d) 2 H2 (g) + O2 (g) → 2 H2O(g)
+
-1
(e) Na (g) + e → Na(s)
17. Breaking the chemical bond in H2 requires 436 kJ/mol; for Br2, 194 kJ/mol. What is the minimum
energy required to break the H-Br bond? The following reaction is known to be exothermic
H2 (g) + Br2 (g) → 2 HBr(g)
(a) -630 kJ/mol HBr
(b) -315 kJ/mol HBr
(c) -121 kJ/mol HBr
(d) -102 kJ/mol HBr
(e) -25 kJ/mol HBr
18. The experimental rate constant for a particular chemical reaction depends upon four of the
following factors. Which one does not affect the size of the experimental rate constant for that
reaction?
(a) the nature of the solvent
(b) the nature of the reactants
(c) temperature
(d) the observed rate of the reaction
(e) the concentrations of the reactants
19. In which reaction will the standard molar heat combustion of methane be liberated?
(a) CH4 (g) + 2 O2 (g) → CO2 (g) + H2O(l)
(b) CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(l)
(c) CH4 (g) + 2 O2 (g) → CO2 (g) + 2 H2O(g)
(d) CH4 (g) + 2 O2 (g) → CO2 (l) + 2 H2O(g)
(e) CH4 (g) + 2 O2 (g) → CO2 (l) + 2 H2O(l)
Last Revised by D. Lougheed 7/3/00
20. CS2 (2.0 mol) and Cl2 (4.0 mol) are mixed and this equilibrium is established:
CS2 (g) + 3 Cl2 (g) ⇔ S2Cl2 (g) + CCl4 (g)
At equilibrium, 0.30 mol of CCl4 is found. How much Cl2 is left?
(a) 0.30 mol
(b) 0.90 mol
(c) 1.8 mol
(d) 3.1 mol
(e) 3.4 mol
21. Kc = 4.0 for the equilibrium
2 NH3 (g) + Cl2 (g) ⇔ N2H4 (g) + 2 HCl(g)
If 2.0 mol of ammonia and 4.0 mol of chlorine are in equilibrium with 6.0 mol N2H4 in a one Litre
container, what is the equilibrium concentration of HCl?
(a) 1.2 mol/L
(b) 3.3 mol/L (c) 5.3 mol/L (d) 10.7 mol/L(e) 12.0. mol/L
22. If Kp = 6.0 x 10-8 for the equilibrium
N2 (g) ) ⇔ 2 N(g),
what is Kp at the same temperature for
N(g) ) ⇔ 1/2 N2 (g)?
-8
(a) 6.0 x 10
(b) 2.4 x 10-4 (c) 4.1 x 103 (d) 8.3 x 106
(e) 1.7 x 107
23. How would you increase the number of moles of O2 at equilibrium in the system
N2 (g) + 2 O2 (g) ) ⇔ N2O4 (g),
∆H > 0?
(a) add a catalyst
(b) increase the temperature
(c) increase the pressure in the system (d) decrease the volume of the system
(e) add N2O4 (g) to the system
24. Equal volumes of aqueous solutions of 0.10 M Pb(NO3)2 and 0.10 M NaBr are mixed and come to
equilibrium at 25°C. For
Pb2+(aq) + 2 Br-1(aq) ) ⇔ PbBr2 (s)
the equilibrium constant, Kc, is larger than 105. What is [Pb2+(aq)] at equilibrium?
(a) 0.10 M
(b) 0.050 M (c) 0.025 M (d) 0.0040 M (e) 0.0010 M
25. The Ksp of CaF2 is 4.0 x 10-11 at 25°C. What is the molar solubility of CaF2?
(a) 6.3 x 10-6 M
(b) 3.1 x 10-6 M
(c) 2.2 x 10-4 M
(d) 3.4 x 10-4 M
(e) 4.3 x 10-4 M
26. Which solution should be added to Fe(NO3)2 (aq) to cause a precipitate to form?
(a) Mg(NO3)2 (aq) (b) NH4NO3 (aq)
(c) HCl(aq)
(d) H2SO4 (aq) (e) HsS(aq)
27. A saturated solution of BaF2 in water at 25°C has [F-1] = 1.4 x 10-2 M. What is Ksp for BaF2?
(a) 3.4 x 10-7
(b) 1.4 x 10-6 (c) 2.7 x 10-6 (d) 1.1 x 10-5 (e) 7.0 x 10-3
28. What hydrogen ion concentration corresponds to a pH of 2.40?
(a) 2.5 x 10-12M
(b) 2.5 x 10-2 M
(c) 4.0 x 10-2 M
(d) 2.5 x 10-3 M
(e) 4.0 x 10-3 M
29. What [H+] is expected in an aqueous monoprotic weak acid solution (0.10 M) if Ka = 1.0 x 10-5?
(a) 0.10 M
(b) 0.010 M (c) 0.0010 M (d) 1.0 x 10-5 M
(e) a.0 x 10-10 M
Last Revised by D. Lougheed 7/3/00
30. If a 0.10 M solution of a monoprotic weak acid also contains 0.20 M of its sodium salt, and the
solution has a [H+] of 1.0 x 10-4 M, what is Ka for the weak acid?
(a) 4.0 x 10-8
(b) 5.0 x 10-5 (c) 1.0 x 10-4 (d) 2.0 x 10-4 (e) 1.4 x 10-2
31. The HCO3-1 ion is a weak acid with Ka of 6 x 10-11 in water at 25°C. The pH of a 0.20 M Na2CO3
solution should be nearest to
(a) 7
(b) 10 (c) 12 (d) 13 (e) 14
32. NH3 (aq), 0.10 M) is titrated by the addition of HCl(aq, 0.10 M). At the equivalence point
(a) [H+] = [OH-1]
(b) [H+] = [NH3]
(c) [NH3 = [Cl-1]
(d) [H+] = [NH4+1]
(e) [NH3] = [OH-1]
33. When this skeleton equation is balanced with the smallest whole-number coefficients, what is the
coefficient of H+1?
IO3-1(aq) + NO(g) + H2O((l) → I2 (s) + NO3-1(aq) + H+1(aq)
(a) 2
(b) 3 (c) 4 (d) 10 (e) 40
34. Substance X is oxidized by substance Y in a spontaneous chemical reaction under standard state
conditions. How must the standard reduction potentials (SRPs) be related, in general?
(a) the SRP of the oxidized product of X must be lower (more negative) than the SRP of Y
(b) the SRP of the oxidized product of X must equal the SRP of Y
(c) both Y and the oxidized product of X must have an SRP greater than that of the standard
hydrogen electrode
(d) the sum of the SRPs of Y and the oxidized product of X must be positive
(e) the SRP of the oxidized product of X must be positive and the SRP of Y must be negative
35. According to the usual rules of oxidation numbers, which compound of manganese contains Mn in
the +3 oxidation state?
(a) K3[Mn(CO)4]
(b) KMnO4 (c) BaMnO4
(d) Mn2O3
(e) MnO
36. Using these standard reduction potentials:
O2 (g) + 4 H+1(aq) + 4 e-1 → 2 H2O(ll) E° = +1.23 volts
Cu2(aq) + 2 e-1 → Cu(s)
E° = +0.34 volts
decide which applied voltage listed below is nearest to the minimum voltage needed to deposit
Cu(s) under standard conditions.
(a) 0.0 V (b) 0.5 V
(c) 1.0 V
(d) 1.5 V
(e) 2.0 V
37. What is E° for
AgCl(s) → Ag+1(aq) + Cl-1(aq),
given
Ag+1(aq) + e-1 → Ag(s)
E° = +0.80 V
and
(a) +1.02 V
AgCl(s) + e-1 → Ag(s) + Cl-1(aq),
(b) +0.58 V (c) 0.00 V
(d) -0.58 V
Last Revised by D. Lougheed 7/3/00
E° = +0.22 V
(e) -1.02 V
38. What is E° for
Cr+3(aq) + 3 e-1 → Cr(s),
given
Cr(s) + 3 Ag+1(aq) → 3 Ag(s) +
Cr+3(aq)
E° = +1.54 V
(d) 0.96 V
E° = +0.80 V
(e) 2.34 V
and
(a) -0.86 V
Ag+1(aq)) + e-1 → Ag(s)),
(b) -0.74 V
(c) 0.06 V
39. Passing a certain quantity of electricity through H2SO4 (aq) generates 2.0 mol of gaseous hydrogen.
How many moles of gaseous hydrogen will be generated if the same quantity of electricity is
passed through HCl(aq)?
(a) 2.0 mol
(b) 1.5 mol
(c) 1.0 mol
(d) 0.50 mol (e) 0.00 mol
1997
1.
Which molecule is an ester and also an amine?
(a)
(b)
(c)
(d)
(e)
2.
The reaction between glycine and alanine, may be classified as
(a) saponification
3.
(b) condensation
(c) esterification.
(d) addition
(e) hydrolysis
Which of the structural formulas shown above is a monomer - polymer pair?
(1) H3C-CH3
(2) H2C=CH2
(3)
(4) H(CH2CH2)nH
(5) H3C-(CH2)4-CH3
(a) (1) and (2) (b) (1) and (3)
Last Revised by D. Lougheed 7/3/00
(c) (1) and (5)
(d) (2) and (3)
(e) (2) and (4)
4.
Cold purple potassium permanganate solution in aqueous base (MnO4-/H2O/OH- ) is used to test for
unsaturation in hydrocarbons. Which unsaturated hydrocarbon will discharge the colour of
permanganate ion?
(a)
5.
(b)
(c) H2C=CH2 (d) H3C-CH2-CH3
Select the compound that is an isomer of propanol:
(a) H3CCH2CHO
(b) H3CCH2COCH3
(d) H3CCH2CH2Br
(e) H3CCH2OCH3
(e) H3C-CH2-CH2-C=O
|
OH
(c) H3CCH2CH2CH2OH
6.
A weather balloon contains 12 L of hydrogen at 740 mm Hg pressure. At what pressure in mm Hg
will the volume become 20 L (temperature is constant)?
(a) 370
(b) 444
(c) 760
(d) 1230
(e) 1480
7.
If the mass of the neutron were half of its actual mass, and that of the electron were twice its actual
mass, then the mass of one atom of 126°C would be, approximately,
(a) decreased by 25%
(b) increased by 25%
(c) halved
(d) doubled
(e) unchanged
8.
The correct order of increasing radius is
(a) Mg2+ < Al3+ < Na+
(b) Mg2+ < Na+ < Al3+ (c) Al3+ < Mg2+ < Na+
+
2+
3+
(d) Na < Mg < Al
(e) Na+ < Al3+ < Mg2+
9.
At 100°C and standard pressure, which substance is a liquid?
(a) aluminum (b) sodium chloride (c) ethanol
(d) propane
(e) mercury
10. Which atoms in the Lewis structure shown below have one or more unshared pairs of electrons?
(a) Atoms (4) and (5) only
(c) Atoms (1), (4) and (5) only
(e) none of the above
Last Revised by D. Lougheed 7/3/00
(b) Atoms (1), (2) and (3) only
(d) Atoms (2), (4) and (5) only
11. Which chemical reaction is consistent with the following graph?
(a) 2X → Y + 2Z
(d) X + 2Y → Z
(b) X → Y + Z
(e) X → 2Y + Z
(c) X + Y → Z
12. Relative energies of reactants, intermediates and products in a chemical reaction are shown in the
graph below. What is the rate determining step in the reaction of A → E ?
(a) A → B
13.
(b) B → C
(c) C → D
(d) D → E
(e) A → E
For the graph in question 12, the enthalpy change for the reaction A → E is given by
(a) E1 - E5
(b) E1 - E3
(c) E4 - E3
(d) E5 - E3
(e) E3 - E1
14. Which one of the following statements is true?
(a) A catalyst decreases the enthalpy change of the reaction.
(b) A catalyst decreases the entropy change of the reaction.
(c) A catalyst increases the concentration of the products.
(d) A catalyst increases the rate of formation of the products.
(e) A catalyst increases the concentration of the reactants.
15. In its lowest energy state, which one of the following atoms or ions has an unpaired p-electron?
(a) K+ (b) Mg
(c) Al
(d) C
(e) F16. For the reaction
2H2O2 → 2H2O + O2
the following plot confirms that the rate is first-order with respect to H2O2:
What is the ordinate (Y) of the plot?
(a) [H2O2]
(b) 1/[H2O2]
(c) [H2O2]2
(d) log[H2O2]
(e) 1/log[H2O2]
Last Revised by D. Lougheed 7/3/00
17. What is "x" when the following equation is balanced with "1" as the coefficient of (NH2)2CO?
1(NH2)2CO + x H2O → yNH4+ + zCO32(a) 1/2
(b) 1
(c) 3/2
(d) 2
(e) 5/4
18. Which of the following occur(s) when K2O is added to water?
(1) the water freezes
(2) a gas is released
(3) a black precipitate is formed
(4) heat is liberated
(a) (2) and (3) only
(b) (4) only
(c) (2) and (4) only
(d) (1) and (3) only
(e) (1), (2) and (3)only
19. Given
C(s) + O2(g) → CO2(g) + 393 kJ/(mol O2)
2C(s) + O2(g) → 2CO(g) + 218 kJ/(mol O2)
How much energy is produced in the complete combustion of 56 g CO(g)?
(a) 350 kJ
(b) 568 kJ
(c) 830 kJ
(d) 1002 kJ (e) 1222 kJ
20. Which reaction, initially at equilibrium, shifts to the left upon an increase in external pressure, but
to the right upon an increase in temperature?
(a) heat + N2 + O2 → 2NO
(b) H2(g) + I2(g) → 2HI(g) + heat
(c) PCl3(g) + Cl2(g) → PCl5(g) ,∆H = +16.6 kJ/mol
(d) 2CO2(g) + heat → 2CO(g) + O2(g)
(e) N2(g) + 3H2(g) → 2NH3(g) + 100 kJ
21. A container holds one mole of gaseous argon at a known temperature and pressure. A second,
identical container holds gaseous krypton at twice the pressure and three times the absolute
temperature. Approximately how many moles of krypton are in the second container?
(a) 0.67 mol
(b) 1.0 mol
(c) 1.5 mol
(d) 2.0 mol
(e) 3.0 mol
22. Which compound is a peroxide?
(a) CO2
(b) O2
(c) NO2
(d) BrO2
(e) BaO2
23. Consider the interrelated equilibria:
Cu2+(aq) + 4NH3(aq) → Cu(NH3)42+(aq)
NH3(aq) + H2O → NH4+ (aq) + OH- (aq)
3OH- (aq) + Fe3+(aq) → Fe(OH)3(s)
Addition of more Fe3+ will
(a) increase the amount of Cu2+
(b) increase the amount of Cu(NH3)42+
2+
(c) decrease the amount of Cu
(d) decrease the amount of NH4+
(e) increase the amount of OH-
Last Revised by D. Lougheed 7/3/00
24. Consider the following reversible reaction. All substances are gases and are in an insulated closed
chamber with a constant volume and are at equilibrium.
2H2O + 2Cl2 → 4HCl + O2 ∆H = +113 kJ
What will be the effect of increasing the temperature?
(a) More Cl2 will be produced.
(b) More HCl will be produced.
(c) The volume of each of the gases will increase.
(d) More water will be formed.
(e) There will be no change.
25. Which statement is true, by definition, for a system that has reached a state of chemical
equilibrium?
(a) The substance having the smaller volume has a tendency to form at the expense of the other
substances.
(b) No further reaction occurs in either direction.
(c) The concentrations of reactants and products are necessarily equal.
(d) The opposing reactions have equal rates.
(e) The total mass of the products is equal to the total mass of the reactants.
26. What is the pH of a 0.30 M sodium acetate, NaC2H3O2, solution?
(a) 2.6
(b) 4.7
(c) 7.0
(d) 9.1
(e) 11.4
27. The oxidation number for chlorine is the highest in:
(a) HCl
(b) HclO
(c) HClO2
(d) HClO3
(e) HClO4
28. Typical "hard" water contains about 2.0 x 10-3 mol of Ca2+ per litre. Calculate the maximum
concentration of fluoride ion which could be present in hard water.
(a) 2.0 x 10-3 M
(b) 4.0 x 10-3 M
(c) 1.4 x 10-4 M
(d) 2.0 x 10-8 M
(e) 4.0 x 10-11 M
29. Silver chloride is precipitated by adding HCl to a solution of a silver salt until the concentration of
chloride ions (Cl-) is 0.20 M. Neglecting the effects of interionic attraction, what is the
concentration of silver ions remaining in solution?
(a) 1.25 x 10-5 M(b) 2.79 x 10-5 M
(c) 7.80 x 10-10 M
(d) 1.56 x 10-10 M
(e) 0.20 M
30. Which of the following chemists was nearly denied a doctoral degree because he claimed that salts
dissolved in water to produce charged ions?
(a) SavanteArrhenius
(b) Gilbert N. Lewis
(c) T.M. Lowry
(d) J.N. Bronsted
(e) Michael Faraday
31. Why can zinc be used as an expendable metal to prevent iron from rusting in water?
(a) Zinc loses electrons more easily than iron.
(b) Zinc gains electrons more easily than iron.
(c) Zinc is reduced more easily than iron(II).
(d) Zinc loses protons more easily than iron.
(e) Zinc loses protons more easily than iron.
Last Revised by D. Lougheed 7/3/00
32. Which provides the best experimental evidence for the fact that acetic acid is a weaker acid than
hydrobromic acid?
(a) Zinc reacts more rapidly with 0.1 M HBr than with 0.1 M acetic acid.
(b) Acetic acid tends to donate protons to a basic solvent more strongly than HBr.
(c) In the HBr bond the electrons are shifted more towards the bromine than they are towards the
oxygen in the H-O bond of acetic acid.
(d) Inorganic acids are stronger than organic acids.
(e) Less NaOH is required to neutralize one mole of acetic acid than to neutralize one mole of HBr.
33. Which equation represents the anode half-reaction for the electrolysis of aqueous HCl?
(a) Cl2(g) → 2Cl-(aq) + 2e(b) 2Cl-(aq) → Cl2(g) + 2e(c) 2HCl(aq) → Cl2(g) + H2(g)
(d) O2(g) + 4H+(aq) + 4e- → 2H2O(l)
(e) H2O + Cl- → ClO- + 2H+ + e34.
If a piece of zinc metal is placed in a 1 M Cu(NO3)2 solution,
Standard Reduction Potentials (E°)
Zn2+ 2e- → Zn
-0.76 V
Cu2+ 2e- → Cu
+0.34 V
A zinc dissolves completely.
B reaction occurs, and when equilibrium is reached [Zn2+] >> [Cu2+].
C reaction occurs, and when equilibrium is reached [Zn2+] << [Cu2+].
D reaction occurs until equilibrium is reached, at which time [Zn2+] = [Cu2+].
E zinc dissolves initially and then plates out on the walls of the container.
35.
Copper is more active chemically than gold. What is the best theoretical explanation for this?
(a) The copper atom may lose as many as two electrons, whereas the gold atom may lose as many
as three electrons.
(b) Gold can be alloyed with copper.
(c) The copper ion has less tendency to lose electrons than the gold ion.
(d) Gold oxide requires less heat per mole for decomposition than copper oxide.
(e) Copper loses electrons more readily than gold.
36. Who of the following Nobel laureates most recently won the Nobel prize in the field of Chemistry?
(a) Lester Pearson
(b) Gerhard Herzberg
(c) John Charles Polanyi
(d) Frederick Banting
(e) Michael Smith
37.
Balance the following equation using the smallest whole number coefficients.
? MnO4- + ? H2O2 + ? H3O+ → ? Mn2+ + ? O2 + ? H2O
The coefficient for H2O2 in the balanced equation is
(a) 1
(b) 2 (c) 5 (d) 7 (e) 8
Last Revised by D. Lougheed 7/3/00
38. Using the standard reduction potentials given in question 40, calculate ∆E° for the reaction,
Fe(s) + 2 H+ (aq) → H2(g) + Fe2+ (aq)
(a) -0.22 V
(b) -0.44 V
(c) +0.22 V (d) +0.44 V (e) +0.88 V
39. Equal volumes of two aqueous solutions (each 1.0 mol/L) of substances, W and X, are mixed. The
reaction rapidly reaches equilibrium, and the concentration of Y is measured as 0.40 mol/L. What
is the equilibrium concentration of W, assuming the fol lowing equilibrium is established?
W(aq) + X(aq) Y(aq) + Z(aq)
(a) 0.10 mol/L (b) 0.20 mol/L
(c) 0.60 mol/L
(d) 0.80 mol/L
(e) 1.40 mol/
40. Given the following standard reduction potentials,
Al3+ (aq) + 3 e- → Al(s)
E° = -1.67 V
2+
Fe (aq) + 2 e → Fe(s)
E° = -0.44 V
2+
Mg (aq)+ 2 e → Mg(s)
E° = -2.34 V
Pb2+ (aq) + 2 e- → Pb(s)
E° = -0.13 V
2+
Zn (aq) + 2 e → Zn(s)
E° = -0.76 V
what is the weakest oxidizing agent in the above series?
(a) Al3+ (aq)
(b) Fe2+ (aq)
(c) Mg2+ (aq)
(d) Pb2+ (aq)
(e) Zn2+ (aq)
1998
1.
What is the correct order of increasing bond angle between bonded H, C and C atoms?
(a) alkenes < alkynes < alkanes (b) alkanes < alkynes < alkenes
(c) alkanes < alkenes < alkynes
(d) alkynes < alkanes < alkenes
(e) alkynes < alkenes < alkanes
2.
Which functional group does not contain an oxygen atom?
(a) an amide
(b) an amine (c) an aldehyde
(d) an alcohol (e) an ester
3.
2-methylpropane differs from butane in that the former
(a) has a higher molecular weight.
(b) has a different percentage composition.
(c) is not a saturated hydrocarbon.
(d) has a different empirical formula.
(e) has a different structural formula.
4.
Which compound will react most rapidly with bromine?
(a) CH4
(b) C6H6
(c) C2H4
(d) C2H6
5.
(e) C2H4Cl2
Which compound would not be expected to react with metallic sodium?
(a) CH3-O-CH3
(b) CH3CH2OH
(d)
(e) C2H5NH2
Last Revised by D. Lougheed 7/3/00
(c)
6.
The reaction of an alcohol with a carboxylic acid in organic chemistry resembles the reaction of an
inorganic hydroxide with an acid only in
(a) the speed of the reaction.
(b) the completeness of the reaction.
(c) the production of an ionic salt as one end product.
(d) the production of water as one end product.
(e) the production of an ester as one end product.
7.
Which of the following represents the ground state electron configuration of the Mn3+ ion?
(Atomic number of Mn is 25)
(a) 1s2 2s22p6 3s23p63d4
(b) 1s2 2s22p6 3s23p63d5 4s2
(c) 1s2 2s22p6 3s23p63d2 4s2
(d) 1s2 2s22p6 3s23p63d6 4s2
2
2
6
2
6
3
1
(e) 1s 2s 2p 3s 3p 3d 4s
8.
The critical temperature of a substance is
(a) the temperature at which the vapour pressure of the liquid is equal to the external pressure.
(b) the temperature at which the vapour pressure of the liquid is equal to 760 mm Hg.
(c) the temperature at which the solid, liquid, and vapour phases are all in equilibrium.
(d) the temperature at which liquid and vapour phases are in equilibrium at 1 atmosphere.
(e) the lowest temperature above which a substance cannot be liquefied at any applied pressure.
9.
How many of the molecules and ions below have a total of eight valence electrons?
H3O+ CH4 NO3- NH4+
CO32- H2O N3OCNO3
CO2 PCl5 SF6
(a) 2
(b) 4
(c) 6
(d) 7
(e) 8
10. Of the following elements, which has the highest melting point at standard pressure?
(a) aluminum (b) silicon
(c) phosphorus(d) sulfur
(e) chlorine
11. Which one of the following species has a molecular dipole moment of zero?
(a) CO2
(b) H2O
(c) CH2Cl2
(d) CCl4
(e) NH3
12. In which of the following series are the diatomic molecules arranged in order of increasing bond
length?
(a) F2, Cl2, ICl , BrCl , I2
(b) F2, Cl2, BrCl , ICl , I2
(c) F2, BrCl , Cl2, I2, ICl
(d) F2, Cl2, BrCl , I2, ICl
(e) F2, ICl , BrCl , Cl2, I2
13. When a sample of oxygen gas in a closed container of constant volume is heated until its absolute
temperature is doubled, which of the following is also doubled?
(a) the density of the gas
(b) the pressure of the gas
(c) the average velocity of the gas molecules
(d) the number of molecules per cm3
(e) the potential energy of the molecules
Last Revised by D. Lougheed 7/3/00
14. The oxidation of iodide ions by arsenic acid in acidic aqueous solution occurs according to the
stoichiometry shown below.
H3AsO4 + 3 I- + 2 H3O+ → H3AsO3 + I3- + 3H2O
The experimental rate law of the reaction is:
Rate = k [H3AsO4] [I-] [H3O+]
What is the order of the reaction with respect to I- ?
(a) 1
(b) 2 (c) 3 (d) 5 (e) 6
15.
From the energy profile diagram shown below, choose the one correct statement:
(a) Letter A represents the enthalpy change of the reaction for XY and C is the activation energy
for XY.
(b) Letter B represents the heat of reaction for XY and A is the activation energy for XY.
(c) Letter A represents the heat of reaction for XY and C is the activation energy for YX.
(d) Letter B represents the heat of reaction for XY and C is the activation energy for YX.
(e) Letter C represents the heat of reaction for YX and B is the activation energy for YX.
16.
In 30 days, 32P loses one-half of its radioactivity. What percentage of the original radioactivity
would remain at the end of 15 days?
(a) 100%
(b) 87%
(c) 75%
(d) 71%
(e) 50%
17. Complete and balance the equation for the combustion of ZnS in excess oxygen,
? ZnS + ? O2 → ? ZnO + ?
Use the smallest whole number coefficients (no fractions). The number of moles and the formula
of the product containing S are
(a) 2S
(b) S8
(c) SO2
(d) 2SO2
(e) SO3
Last Revised by D. Lougheed 7/3/00
18. What is the ratio of the volume of hydrogen liberated by the reaction of 0.2431 g magnesium with
an excess of 2.0 M hydrochloric acid and the volume of hydrogen liberated by the reaction of the
same weight of magnesium with an excess of 1.5 M sulphuric acid? (The molar mass of Mg is
24.31 g/mol)
(a) 1:4
(b) 1:2
(c) 1:1
(d) 2:3
(e) 4:3
19. Which one of the following statements is false ?
(a) A system at chemical equilibrium has a constant mass.
(b) Reactant and product concentrations vary with time in a system at chemical equilibrium.
(c) Forward and reverse reactions proceed at the same rate in a system at chemical equilibrium.
(d) A system at chemical equilibrium opposes slight disturbances.
(e) A system at chemical equilibrium must have a constant temperature.
20. Given the following heats of reaction under standard conditions,
C(s) + O2(g) → CO2(g)
∆H° = -394 kJ /(mol C)
H2(g) + (O2(g) → H2O(l)
∆H° = -286 kJ /(mol H2)
CH4(g) + 2 O2(g) → CO2(g) + 2H2O(l)
∆H° = -890 kJ /(mol CH4)
what heat of reaction is expected for the reaction,
C(s) + 2H2 (g) → CH4 (g) ?
(a) +1068 kJ/mol°C
(b) +782 kJ/mol°C
(c) -76 kJ/mol°C
(d) -1570 kJ/mol°C
(e) -1856 kJ/mol°C
21. Two flexible containers for gases are at the same temperature and pressure. One holds 0.50 grams
of hydrogen and the other holds 8.0 grams of oxygen. Which one of the following statements
regarding these gas samples is false? (The relative atomic mass of oxygen is 16.0 and that of
hydrogen is 1.0)
(a) The volume of the hydrogen container is the same as the volume of the oxygen container.
(b) The number of molecules in the hydrogen container is the same as the number of molecules in
the oxygen container.
(c) The density of the hydrogen sample is less than that of the oxygen sample.
(d) The average kinetic energy of the hydrogen molecules is the same as the average kinetic energy
of the oxygen molecules.
(e) The average speed of the hydrogen molecules is the same as the average speed of the oxygen
molecules.
22. For this system at fixed pressure,
2SO3(g) _ 2SO2(g) + O2(g) _H° = + 43 kJ/( mol SO3)
what is the effect of a small increase in temperature on the rate to the right (rateright), rate to the
left (rateleft), and the equilibrium constant (Keq)?
rate right
rate left
Keq
(a)
lower
higher
lower
(b)
higher
lower
unchanged
(c)
higher
higher
unchanged
(d)
higher
higher
higher
(e)
higher
higher
lower
Last Revised by D. Lougheed 7/3/00
23. -B- If a salt is dissolved in water under conditions that the solution becomes supersaturated, then
the solution
(a) must contain some undissolved solute.
(b) is not truly at equilibrium.
(c) must be hot.
(d) has an ion product less than the solubility product constant of the salt.
(e) must be above room temperature.
24. -E-If the following equation is balanced using the smallest whole number coefficients,
?MnO4- + ?H+ _ ?Mn2+ + ?H2O + ?NO3what number appears before the HNO2 molecule?
(a) 1
(b) 2 (c) 3 (d) 4 (e) 5
25.
How many moles of H3O+ are there in 1.8 L of pure water at 25°C? (Kw = 1.0 x 10-14 at 25°C)
(a) 95 mol
(b) 32 mol
(c) 1.0 x 10-7 mol
(d) 1.8 x 10-7 mol
(e) 1.0 x 10-14 mol
26. Choose the correct statement about these two reactions:
Cl- + H2O → HCl + OHCl- + PCl3 → PCl4(a) Cl- does not act as a Lewis acid or base in either of these reactions.
(b) Cl- acts as a Lewis base in both of these reactions.
(c) Cl- acts as a Lewis base only in the second reaction.
(d) Cl- acts as a Lewis acid only in the first reaction.
(e) Cl- acts as a Lewis acid in both of these reactions.
27. Which compound is the strongest acid in aqueous solution?
(a) HOCN
(b) HOCl
(c) HOClO
(d) HOClO2
(e) HOClO3
28. A chemist accidentally mixes white NaBr powder with white CsBr powder. When 1.00 g of the
mixture is analyzed, it is found to contain 0.492 g Br. What is the percentage, by mass, of NaBr in
the mixture?
Relative Atomic Mass
Cs
132.91
Na
22.99
Br
79.90
(a) 82.3% NaBr
(b) 51.8% NaBr
(c) 43.9% NaBr
(d) 29.1% NaBr
(e) 18.4% NaBr
29. Silver chloride is precipitated by adding HCl to a solution of a silver salt until the concentration of
chloride ions (Cl-) is 0.20 M. What is the concentration of silver ions in the remaining solution?
Solubility Product Constant, Ksp AgCl = 1.56 x 10-10
(a) 1.3 x 10-5 M
(b) 2.8 x 10-5 M
(c) 7.8 x 10-10 M
(d) 1.6 x 10-10 M
(e) 0.20 M
Last Revised by D. Lougheed 7/3/00
30. Aluminum cookware does not react appreciably with hot water because
(a) the reaction is exothermic.
(b) hydrolysis of aluminum salts occurs.
(c) the aluminum has an oxide coating.
(d) aluminum is not active enough to displace hydrogen.
(e) the radius to charge ratio of aluminum atoms is small.
31.
When the same amount of sodium acetate is added to a 0.1 M solution of each substance listed
below, the acetate ions will attract protons from the acid that is present. From which substance will
the acetate ions attract the largest number of protons?
Acid
Conjugate
Base
Ka (Ionization Constant of Acid)
2HSO4
SO4
1.2 x 10-2
HNO2
NO24.0 x 10-4
HC2H3O2
C2H3O
1.8 x 10-5
HCN
CN7.2 x 10-10
2HS
S
1.2 x 10-13
(a) NaHSO4
(b) HNO2
(c) HC2H3O2 (d) HCN
(e) NaHS
32. Given,
Pb2+(aq) + 2 e- → Pb(s),
E° = -0.13 V
2+
Ni (aq) + 2 e → Ni(s),
E° = -0.25 V
2+
Fe (aq) + 2 e → Fe(s),
E° = -0.44 V
which of the following reactions is(are) spontaneous under standard conditions?
(1) Fe(s) + Ni2+(aq) → Fe2+(aq) + Ni(s)
(2) Ni(s) + Pb2+(aq) → Ni2+(aq) + Pb(s)
(3) Pb(s) + Fe2+(aq) → Pb2+(aq) + Fe(s)
(a) (1), (2) and (3)
(b) (1) and (2) only
(c) (1) and (3) only
(d) (2) and (3) only
(e) (3) only
33. To protect a buried pipe line made of iron from corrosion, a bar of magnesium is buried close to the
pipe and connected to the iron. What is the best explanation for this protective action?
(a) Mg forms a protective coating over the iron.
(b) Mg gains electrons more readily than Fe, keeping the Fe from oxidizing.
(c) Fe loses electrons less readily than Mg, making Mg the anode.
(d) Mg is more active than iron and forces the iron to act as an anode.
(e) An electrolytic cell is set up, with H2 gas being evolved at the surface of Mg.
Last Revised by D. Lougheed 7/3/00
34. Sulfur may act as either an oxidizing agent or as a reducing agent. What is the best theoretical
explanation for this statement?
(a) Sulfur forms sulfur dioxide as well as calcium sulfide.
(b) Sulfur is a nonmetal.
(c) Sulfur forms both organic and inorganic compounds.
(d) With six electrons in its outer shell the sulfur atom can either gain electrons from other
elements or share its electrons with other elements.
(e) Sulfur is soluble in carbon disulfide as well as in alcohol.
35.
Which of the following is the strongest oxidizing agent?
(a) F2
(b) Cl2
(c) Br2
(d) I2
(e) Cl-
36. Two electrolytic cells, one containing a silver nitrate solution and the other containing a copper(II)
sulfate solution, were connected so that the same current passed through both cells. A current was
passed through both solutions until 53.95 g of silver had been deposited. What mass, in grams, of
copper was deposited?
Atomic Molar Masses
Ag 107.9 g/mol
Cu 63.5 g/mol
(a) 15.9
(b) 27
(c) 31.8
(d) 54
(e) 63.5
37. Given the following standard reduction potentials,
Mg2+ + 2e- → Mg
-2.37 V
3+
Al + 3e → Al
-1.66 V
2+
Zn + 2e → Zn
-0.76 V
Fe2+ + 2e- → Fe
-0.44 V
2+
Cu + 2e → Cu
+0.34 V
+
Ag + e → Ag
+0.80 V
What combination of metals together with their 1 M salt solutions would give a voltaic cell with
the highest possible voltage?
(a) Mg and Al
(b) Zn and Cu
(c) Mg and Ag
(d) Mg and Fe
(e) Al and Ag
38. Which substance is the source of the gas that fills an automobile's air bag?
(a) compressed N2(g)
(b) NaHCO3(s)
(c) compressed CO2(g)
(d) Na2SO4(s)
(e) NaN3(s)
39. The electrolysis of a 0.1 M solution of potassium hydroxide in water produces
(a) hydrogen at the anode and oxygen at the cathode.
(b) hydrogen at the cathode and oxygen at the anode.
(c) oxygen at the cathode and potassium at the anode.
(d) potassium at the cathode and oxygen at the anode.
(e) potassium at the anode and hydrogen at the cathode.
Last Revised by D. Lougheed 7/3/00
1999
1.
What is the structural formula of 2-chloro-3-pentanol?
H
(a)
H
(c)
H3C
H
Cl
Cl
H
H
C
C
C
C
C
OH
OH
OH
OH
OH
H
Cl
H
C
C
C
H
H
H
OH
H
C
C
OH
C
CH3
H
Cl
H
H
(b)
HO
H
(d)
H
Cl
H
H
H
C
C
C
C
C
OH
H
H
OH
OH
H
Cl
H
C
C
C
CH3
H
H
H
CH3
H
(e)
2.
Which one of the following statements is true of a solution of a strong electrolyte in water?
(a) Its freezing point is above 0°C.
(b) Its boiling point is below 100°C.
(c) Its vapour pressure is lower than that of pure water.
(d) It contains a high proportion of undissociated salt.
(e) It conducts electricity less well than pure water.
3.
The compound
H3C
C
O
H3C
is an example of
(a) an ether.
(b) an alcohol. (c) an acid.
(d) an aldehyde.
(e) a ketone.
4.
A compound of carbon and hydrogen is burned completely in air to yield 0.045 9 water and 0.22 g
of carbon dioxide. Which one of the following is consistent with such data?
(a) C2H2 (b) C2H4
(c) C2H6
(d) C6H12
(e) C6H14
5.
When an organic acid and an alcohol react, the products are water and
(a) an aldehyde. (b) an ester. (c) an ether. (d) a carbohydrate. (e) a ketone.
6.
A gas consists of 85.6% carbon and 14.38% hydrogen (both by weight). What is the empirical
formula of the gas?
(a) CH
(b) CH2
(c) CH3
(d) CH4
(e) C3H4
Last Revised by D. Lougheed 7/3/00
7.
Which of the following substances has the highest melting point?
(a) n-butane (C4H10)
(b) n heptane (C7H16)
(c) n-hexane (C6H14
(d) n-pentane (C5H12)
(e) n-propane (C3H8)
8.
Which atom or ion could have this electron configuration:
1s2 2s2 2p6 3s2 3p6 3d8 ?
+
(a) Fe
(b) Co
(c) Ni2+
(d) Cu+ (e) Zn2+
9.
Which straight chain hydrocarbon is unsaturated?
(a) C5Hl0 (b) C7H16
(c) C6H14
(d) C2H6
(e) C3H8
10. In which of the following series are the diatomic molecules arranged in the order of increasing
bond length?
(a) F2, C12, ICI, BrCI, I2
(b) F2, Cl2, BrCI, ICI, I2
(c) F2, BrCI, Cl2, I2,ICI
(d) F2, Cl2, BrCI, I2, ICI
(e) F2, ICI, BrCI, C12, I2
11. What is the correct formula for the nitrite ion?
(a) NO+
(b) N3(c) NO2(d) NO-
(e) NO3-
12. An element M forms an ion M3+. The atom M and the ion M3+ have the same
(a) radius.
(b) number of electrons.
(c) ionization energy.
(d) nuclear charge.
(e) chemical properties.
13. Which of the following molecules has bond angles of 120 degrees?
(a) H20
(b) NF3
(c) CH4
(d) BeF2
(e) BF3
14. If doubling the pressure doubles the number of collisions in a sample of gas, one expects that
doubling the pressure causes the number of productive collisions leading to a chemical reaction to
b
(a) unchanged.
(b) halved.
(c) doubled. (d) more than halved.
(e) more than
doubled.
15. Given these two standard reaction enthalpies:
S(s) + O2(g) ⇔ SO2(g)
∆H = -295 kJ
and
S(s) + 3/2 O2(g) ⇔ SO3(g)
∆H = -395 kJ,
what is the reaction heat for
2 SO2(g) + O2(g) ⇔ 2 SO3(g)
under the same conditions?
(a) -200 kJ
(b) -295 kJ
(c) -690 kJ
(d) -790 kJ
(e) -1380 kJ
16. Which one of the following chemical reactions is not possible?
(a) Ca + energy → Ca2+ + 2e(b) K + e- → K+ + energy
(c) H2 + energy → 2H+ + 2e(d) Cl + e- → Cl- + energy
(e) Ar++ e- → Ar + energy
17. The bubbles that can be seen in boiling water are mainly
(a) air. (b) hydrogen.
(c) oxygen. (d) water vapour.
Last Revised by D. Lougheed 7/3/00
(e) hydrogen and oxygen.
18. Relative energies of reactants, intermediates and products in a chemical reaction are shown in the
graph below. What is the rate determining step in the reaction of A → E?
(a) Α → Β
(b) B → C
(c) C → D
(d) D → E
(e) A → E
19. The half-life of a radioactive isotope is 10 days. What percentage of the isotope will have
decomposed after 60 days?
(a) 60.0%
(b) 94.0%
(c) 96.9%
(d) 98.4%
(e) 100.0%
20. Generally an increase of ten degrees Celsius doubles the rate of reaction between gases. What is
the explanation for this increase in reaction rate?
(a) The pressure is doubled.
(b) The concentration of the reactants is doubled.
(c) The average kinetic energy of the molecules is doubled.
(d) The number of intermolecular collisions per unit of time is doubled.
(e) The number of collisions with an energy above a minimum activation energy I doubled.
21. Equal weights of zinc metal and iodine are mixed together and the iodine is completely converted
into ZnI2. What fraction of the weight of zinc remains unreacted?
(a) 0.74 (b) 0.48
(c) 0.37
(d) 0.24
(e) 0.00
22. Select the gas in which the average speed of the molecules is the highest (all are at 25°C and 1
atm).
(a) xenon(b) methane (c) oxygen (d) sulfur dioxide
(e) isobutane
23. For a system at chemical equilibrium, the system
(a) is insensitive to external influences such as changes of pressure and temperature.
(b) responds to an external influence in a way which reinforces it.
(c) has a very high energy, consequently all equilibria are very rapidly established
(d) has constant mass, temperature, pressure and concentrations of reactants and products.
(e) is chemically unreactive; atoms in reactant molecules are never exchanged for similar atoms in
product molecules.
Last Revised by D. Lougheed 7/3/00
24. Given that two reactions in the same solution,
H2S(aq) = H+ (aq) + HS-(aq)
(K1)
and
HS-(aq) = H+ (aq) + S2-(aq)
(K2)
have equilibrium constants K1 and K2, respectively, with K1>>K2, choose the one correct
relationship:
[HS-1 ]2
[H+ ]2 [S-2 ]
(a) K1 - K2 =
(b) K1 +K2 =
[H2S]
[H2 S][S-2 ]
(c)
K 2 / K1 =
(e) K1 / K2 =
[H2 S][S-2 ]
[HS-1 ]
[H2 S][S-2 ]
(d) K1K2 =
[H+ ]2 [S-2 ]
[H2S]
[HS-1 ]2
25. Which one of the following is the strongest acid in water at 25°C? (All are at the same
concentration.)
(a) HCOOH
Ka = 2.0 x 10-4
(b) HOCl
Ka = 3.0x10-8
-2
(c) HOClO
Ka = 1.0 x 10
(d) HOClO2
Ka = 102
(e) HOClO3
Ka = 1011
26. An equilibrium mixture at constant temperature and pressure,
SO3(g) + NO(g) ⇔ SO2(g) + NO2(g)
was analyzed and found to contain 0.100 mole of SO2, 0.200 mole of NO2, 0.300 mole of NO and
0.500 mole of SO3 in a 10-litre container. What is the equilibrium constant for this reaction?
(a) 7.5
(b) 1.1
(c) 0.30
(d) 0.13
(e) 0.018
27. A 46 1itre vessel contained a mixture of two unreactive gases, A and B, at 27°C and a total
pressure of 12 atm. When a certain amount of gas A was removed, the pressure dropped to 87.5%
of its original value. How many moles of A were removed? (R = 0.08205 L atm K-1 mol-1)
(a) 5.00 (b) 10.0
(c) 35.0
(d) 70.0
(e) 111.0
28. For the stellar nuclear reaction,
16
16
4
8 O + 8 O → X + 2He,
the conservation laws require that the product, X, must be
24
28
31
(a) 12
(b) 12
Mg
(c) 14
Si
(d) 15
P
6 C
(e)
32
16 S
29. Which one of the following will occur if a 0.10 mol/L solution of a weak base is diluted to 0.010
mol/L at constant temperature?
(a) The hydroxide ion concentration will decrease to 0.010 molar.
(b) The pH will increase.
(c) The dissociation constant of the weak base will increase.
(d) The solution will become more basic.
(e) The percentage ionization will increase.
Last Revised by D. Lougheed 7/3/00
30. Which one of the following will react appreciably with water at room temperature and pressure to
produce hydrogen?
(a) H2S (b) CH4
(c) CaH2
(d) NH3
(e) HCI
31. One gram of sodium chloride is dissolved in enough water to make 415 cm3 of solution. The
molarity of NaCI in the solution is
(a) 0.0071
(b) 0.0171 (c) 0.0412
(d) 0.140
(e) 1.00
32. Which process illustrates chemical precipitation?
(a) The formation of a solid as sodium chloride and silver nitrate solutions are mixed.
(b) The reaction between 1.00 mol/L solutions of sodium hydroxide and hydrochloric acid.
(c) The slight break-up of acetic acid molecules in water to form hydrated protons and acetate ions.
(d) The conversion of sodium atoms to sodium ions.
(e) The conversion of sulfur molecules, S8, to sulfur atoms, S.
33. Which one of the following statements is true of aqueous solutions?
(a) The pH is directly proportional to the concentration of hydrogen ions.
(b) The pH is inversely proportional to the concentration of hydrogen ions.
(c) The pH is directly proportional to the self- ionization constant for water.
(d) The concentration of hydrogen ions is directly proportional to the concentration of hydroxide
ions.
(e) The concentration of hydrogen ions is inversely proportional to the concentration of hydroxide
ions.
34. What are the products of the electrolysis of water?
(a) H+ and OH(b) H2 and O2
(c) O2 and OH+
35. In the equation
2 H2SO4 + 6 H2S → S8 + 8 H2O
(a) sulfur is oxidized and there is no reduction.
(b) sulfur is both reduced and oxidized.
(c) sulfur is reduced and hydrogen is oxidized.
(d) sulfur is oxidized and hydrogen is reduced.
(e) sulfur is reduced and there is no oxidation.
36. What is the oxidation number of chromium in Na2Cr2O7 ?
(a) –6
(b) –2
(c) +3
(d) +6
(e) +12
37. In an electrochemical cell in which the reaction is
Zn(s) + Cu2+(aq) → Zn2+(aq) + Cu(s),
the voltage is related to concentration by
[Zn 2+ ]
= 1.10 - 0.029 log
[Cu 2+ ]
The cell was set up with 1.0 mol/L Cu2+(aq) and excess Zn(s) in a volume of 1.00 L and allowed to
run down to equilibrium. What is the concentration of Cu2+(aq) at equlibrium?
(a) 72 mol/L
(b) 38 mol/L (c) 0.50 mol/L (d) 0.026 mol/L
(e) less than 10-5 mol/L
Last Revised by D. Lougheed 7/3/00
38. Which process represents a general method for the preparation of a metal from its compounds?
(a) neutralization
(b) reduction (c) oxidation
(d) fusion
(e) sublimation
39. Given the unbalanced equation,
? ClO3- + ? NO2- → ? Cl- + NO3How many moles of NO2- will react with 1 mol of Cl03- ?
(a) 1
(b) 2
(c) 3
(d) 4
(e) 6
40. Use the following information to answer this question.
Fe2+ + 2e- → Fe
E° = -0.40V
2+
Ni + 2e → Ni
E° = -0.25V
3+
Fe + 3e → Fe
E° = -0.04V
Fe3+ + e- → Fe2+
E° = +0.77 V
Br2 + 2e → 2 Br
E° = +1.09V
Which one of the following reactions is not spontaneous under standard conditions?
(a) Fe2+ + Ni → Fe + Ni2+
(b) 2 Fe3+ + 3 Ni → 2 Fe + Ni2+
3+
2+
2+
(c) 2 Fe + Ni → 2 Fe + 3 Ni
(d) 2 Fe3+ + Fe → 3 Fe2+
(e) 2 Fe + 3 Br2 → 2 Fe3+ + 6 Br2000
1.
How many isomeric alcohols have the molecular formula C4H10O?
(a) 6
(b) 5
(c) 4
(d) 3
(e) 2
2.
The reaction
O
O
||
||
CH3OH + CH3C-OH → CH3C-O-CH3 + H2O
is an example of
(a) neutralization.
(b) hydrolysis.
(d) esterification.
(e) combination.
3.
The molecule
O
||
CH3 -CH2 - O - CH-CH2 - C – OH
|
NH2
is an
(a) alcohol, amide, and ketone
(c) ether, carboxylic acid, and amine
(e) amine, ketone, and alcohol
4.
(c) dehydration.
(b) alcohol, amine, an
(d) ether, carboxylic acid, and amide
Which one of the following compounds is not very soluble in water?
(a) ethanoic acid
(b) ethanol
(c) ethanal
(d) chloroethane
(e) ethanamine
Last Revised by D. Lougheed 7/3/00
5.
Which of the following compounds is expected to have the highest boiling point?
O
O
||
||
(a) CH3CCH3
(b) H–C–H
(c) H–C≡C–CH3
(d) CH3CH2CH2–OH
(e) HO–CH2CH2–OH
6.
What is the IUPAC name for the following compound?
CH2CH3
|
CH3 - CH - CH - CH - CH3
|
|
Br
CH2CH3
(a) 2-bromo-3,4-diethylpentane
(b) 2,3-diethyl-4-bromopentane
(c) 1-methyl-2,3-diethyl-3-bromobutane
(d) 2-bromo-3-ethyl-4-methylhexane
(e) 3-ethyl-4-methylhexyl bromide
7.
Which compound is most likely to polymerize to form very large molecules (macromolecules)?
(a) CH2=CHCl
HO OH OH
| |
|
(b) H2C–CH–CH2
(c) HO–CH2CH2–OH
(d) CH3CI
(e) C17H35COOH
8.
Which one of the following statements concerning benzene, C6H6, is not correct?
(a) The carbon atoms form a flat hexagon with bond angles of approximately 1200.
(b) Two equivalent Lewis structures (i.e. electron-dot structures) can be drawn for benzene.
(c) The double bonds in the benzene molecule oscillate rapidly back and forth between adjacent
pairs of carbon atoms.
(d) Benzene is an aromatic compound.
(e) The carbon atom in benzene is sp2 hybridized,
9.
The species 178O 2- has
(a) 8 protons
(b) 8 electrons
(c) 8 neutrons
(d) 6 electrons
(e) 6 protons
10. Atoms of element X form a binary compound with scandiurn having the formula Sc2X3. The
element X could be
(a) oxygen
(b) nitrogen
(c) hydrogen
(d) fluorine
(e) carbon
11. According to the building-up principle (Aufbau procedure), the ground-state electron configuration
of Zr2+ is
(a) 1s2 2s2 2p6 3s2 3p6 4s2 4p6 5s2 5p6 6s2 6p2
(b) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d2
(c) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s2
(d) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4f 2
(e) 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 5s1 4d1
Last Revised by D. Lougheed 7/3/00
12. In which one of these salts are the ions isoelectronic (i.e. the ions have the same number of
electrons)?
(a) MgC12
(b) Mg3P2
(c) NaCl
(d) MgO
(e) MgS
13. In the Lewis structure for CIF3, the number of lone pairs of electrons around Cl, the central atom, is
(a) 0
(b) 1
(c) 2
(d) 3
(e) 4
14. Which one of the following pure compounds contains both ionic and covalent bonds?
(a) SiO2(s)
(b) NH4Cl(s)
(c) CH3Cl(g)
(d) graphite(s)
(e) H2S(g)
15. Which one of the following molecules is not planar?
(a) H2CCH2
(b) H2NNH2
(c) HNNH
(d) H2CO
(e) BF3
16. In liquid water, the strongest bonds between water molecules are
(a) ionic bonds
(b) covalent bonds
(c) Van der Waals bonds
(d) hydrogen bonds
(e) metallic bonds
17. Given the following information, what is the standard enthalpy of formation for butane, C4H10(g)?
C4H10(g) + 13 /2 O2(g) → 4 CO2(g) + 5 H2O(g)
∆H° = -2658.3 kJ
°
∆H f = -393.5 kJ/mol for CO2(g)
= -241.8 kJ/mol for H2O(g)
= -285.9 kJ/mol for H2O(l)
(a) +2023 kJ/mol
(b) - 345 kJ/mol
(c) - 124.7 kJ/mol
(d) - 634.0 kJ/mol
°
(e) The answer cannot be determined because ∆H f for O2(g) is not given.
18. At a certain temperature and pressure, the enthalpy of combustion of solid iron to form Fe2O3(s) is
-822 kJ per mole of Fe2O3. The enthalpy of combustion of solid carbon to form CO2(g) is -394 kJ
per mole of CO2. What is the enthalpy change at the same temperature and pressure for the
reaction,
2 Fe2O3(s) + 3 C(s) → 4 Fe(s) + 3 CO2(g) ?
(a) -428 kJ
(b) -462 kJ
(c) -2106 kJ
(d) +1250 kJ
(e) +462 kJ
19. The rate law for the reaction
X(aq) → products
is Rate = k[X]. If it takes 55.5 minutes for [X] to decrease from 1.00 M to 0.700 M, how long will
it take for [X] to decrease from 1.00 M to 0.500 M?
(a) 92.5 min
(b) 32.0 min
(c) 108 min
(d) 66.6 min
(e) 77.7 min
Last Revised by D. Lougheed 7/3/00
20. Consider the following reaction profile,
Which of the following statements is/are correct?
I
The activation energy for the forward reaction is 25 kJ/mol.
II
The activation energy for the reverse reaction is 15 kJ/mol.
III
Increasing the temperature will increase the forward and reverse reaction rates by the
same factor.
IV
The forward reaction is exothermic.
(a) II and III
(b) I and III
(c) III and IV
(d) I and IV
(e) II
only
21. Which one of the following statements concerning catalysts is true?
(a) A catalyst increases the rate of the forward reaction only.
(b) Adding a catalyst to an equilibrium mixture increases the concentration of products.
(c) A catalyst lowers the enthalpy change for the reaction it catalyzes.
(d) A catalyst increases the activation energy of a reaction.
(e) There is no net consumption of a catalyst, though it may be temporarily changed.
22. Tripling the Kelvin temperature of an ideal gas and doubling its pressure would change the volume
of a 1.0-L sample to
(a) 6.0 L
(b) 1.5 L
(c) 0.67 L
(d) 0.44 L
(e) 0.11 L
23. The density of a gas, assumed ideal, is 1.25 g/L at 273 K and 101.3 kPa. What is the molar mass of
this gas?
(a) 44.0 g·mol-1
(b) 28.0 g·mol-1
(c) 16.0 g·mol-1
-1
-1
(d) 32.0 g·mol
(e) 42.1 g·mol
24. For the gas phase reaction
2 SO2(g) + O2(g) ↔ 2 SO3(g) + heat,
which one of the following operations will increase the amount of SO3 in the equilibrium mixture?
(a) raising the temperature
(b) adding a catalyst
(c) decreasing the volume of the reaction vessel
(d) increasing the reaction time
(e) removing some oxygen
25. A 2.00-L container of gas A at 101 kPa and a 4.00-L container of gas B at 152 kPa are connected
by a tube of negligible volume. The valve between the flasks is opened and the gases mix at
constant temperature. What is the final pressure, assuming A and B do not react?
(a) 42 kPa
(b) 118 kPa
(c) 127 kPa
(d) 135 kPa
(e) 253 kPa
Last Revised by D. Lougheed 7/3/00
26. The phase diagram for a certain pure substance is shown below.
The triple point is at 517 kPa and -57°C, What transition does this substance go through when the
temperature is raised from -150°C to –50°C under a constant pressure of 400 kPa?
(a) vaporization
(b) sublimation
(c) condensation
(d) fusion
(e) atomization
27. The acid used in lead storage batteries is sulfuric acid, H2SO4 (molar mass, 98.08 mol·L-1). A
concentrated aqueous solution of H2SO4 is 38.0% H2SO4 (by mass) and has a density of 1.29 g/mL
What is the molar concentration of the solution?
(a) 3.0 mol·L-1
(b) 5.0 mol·L-1
(c) 6.0 mol·L-1
-1
-1
(d) 12 mol·L
(e) 29 mol·L
28. What is the final pH of a solution obtained by mixing 20.00 mL of 0.0200 M HCI and 10.00 mL of
0.0500 M NaOH at 25°C?
(a) 1.88
(b) 1.70
(c) 2.48
(d) 11.52
(e) 13.00
29. The pH of a saturated solution of Ca(OH)2 is 12.40 at 25°C. What is Ksp for Ca(OH)2(s) ?
(a) 7.9 x 10–6
(b) 1.6 x 10-5 (c) 6.3 x 10-5 (d) 3.2 x 10-4 (e) 6.3 x 10-38
30. A basic aqueous solution contains the following ions. Which ion makes the solution basic?
(a) A13+
(b) NO31
(c) Br-1
(d) NH4+
(e) F-1
31. What is the hydrogen ion concentration of rain water at 25°C if the pH is 5.50?
(a) 5.0 x 10-5 mol·L-1
(b) 3.2 x 10-6 mol·L-1
(c) 1.0 x 10-7 mol·L-1
(d) 2.5 x 10-8 mol·L-1
(e) 3.2 x 10-9 mol·L-1
32. What volume of 0.060 M Co2(SO4)3 Will contain .020 mole of sulfate ions?
(a) 3.0 L
(b) 0.037 L (c) 0.33 L
(d) 9.0 L
(e) 0.11 L
33. Exactly 3.0 mol NO and 2.0 mol O2 were placed in a 1.00 L flask. These gases react as follows:
2 NO + O2 ↔ 2 NO2
At equilibrium, the mixture contained 2.0 mol NO2. What is the Kc for the reaction above?
(a) 0.50
(b) 1.00
(c) 2.0
(d) 2.5
(e) 4.0
34. A steady current of 25.0 amperes is passed through an aqueous solution Of CuS04 for 32.2
minutes. What is the maximum mass of copper that can be deposited?
(a) 15.9 g
(b) 7.95 g
(c) 31.8 g
(d) 63.6 g
(e) 7.88 x 10-3 g
Last Revised by D. Lougheed 7/3/00
35. If the following equation is balanced and written with the smallest whole number coefficients, what
is the coefficient of HNO2 ?
MnO4-1 + H+ + HNO2 → Mn2+ + H2O + NO3-1
(a) one
(b) two
(c) three
(d) four
(e) five
36. A galvanic cell is composed of a zinc metal electrode in a 1.0 M Zn(NO3)2 solution and a nickel
metal electrode in a 1.0 M Ni(NO3)2 solution. A salt bridge connects the two half-cells and a wire
connects the two electrodes. The temperature is 25°C.
E° = -0.24 V for
Ni2+ + 2e-1 → Ni(s)
E° = -0.76 V for
Zn2+ + 2e-1 → Zn(s)
Which one of the following statements is correct?
(a) Electrons flow from the nickel electrode through the wire to the zinc electrode.
(b) Positive ions in the salt bridge migrate towards the nickel half-cell.
(c) No reaction occurs.
(d) The standard cell potential is 1.00 V.
(e) The zinc electrode is the cathode.
37. In the reaction
XeF2 + BrO3-1 + H2O → Xe + 2 HF + BrO4-1
(a) xenon is oxidized, oxygen is reduced.
(b) xenon is reduced, bromine is oxidized.
(c) fluorine is reduced, bromine is oxidized.
(d) xenon is reduced, fluorine is oxidized,
(e) bromine is reduced, xenon is oxidized.
38. Two wires are connected to a battery and a light bulb in series. When the free ends of the wires are
dipped into a beaker of water, the bulb remains unlit. A substance was then dissolved in the water
but the bulb remains unlit. Which substance was added?
(a) HNO3
(b) H2SO4
(c) KCI
(d) C2H5OH
(e) NaOH
39. W, X, Y, and Z represent different neutral second row atoms. Lewis symbols (i.e. electron dot
structures) for these four atoms are shown below.
W
X
Y
Which atoms will combine in a four-to-one ratio?
(a) W and X
(b) W and Y
(c) W and Z
Z
(d) X and Y
(e) X and Z
40. A solution containing both Ba2+ and Ca2+ ions will be treated with Na2CrO4 in an attempt to
separate the ions by precipitation. If the initial concentrations of Ba2+ and Ca2+ are 0.050 M and
0.20 M, respectively, how much Na2CrO4 should be added to 1.0 L of the solution to maximize the
separation of Ba2+ and Ca2+?
Ksp = 1.2 x 10-10 for BaCrO4
Ksp = 7.1 x 10-4 for CaCrO4
(a) 0.050 mol (b) 0.20 mol (c) 1.4 x 10-4 mol
(d) 2.4 x 10-9 mol
(e) 3.6 x 10-3 mol
Last Revised by D. Lougheed 7/3/00
CHEM 13 NEWS EXAM 2001
UNIVERSITY OF WATERLOO
DEPARTMENT OF CHEMISTRY
9 MAY 2001
TIME: 75 MINUTES
This exam is being written by several thousand students. Please be sure that you follow the instructions below.
We'll send you a report on your performance. Top performers are eligible for a prize.
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RESPONSE sheet.
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Also fill in the corresponding circles below your printed
name.
3. Select, and enter on the STUDENT RESPONSE
sheet, one of the following CODE numbers:
Code 1
5. Now answer the exam questions. Indicate your choice
on the STUDENT RESPONSE sheet by marking one
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•Mark only one answer for each question.
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•There is a penalty (1/4 off) for each incorrect
Code 4
Any other Ontario student
answer, but no penalty if you do not answer.
Code 5
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student
Questions are not in order of difficulty.
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•Questions are all of the same value.
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filling the oval.
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student
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or Prince Edward Island high school student
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high school student
Be careful that any erasures are complete—make the
sheet white again.
Code 11 High school student outside Canada
Code 12 Teacher
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Cs
Ba
La*
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Fr
Ra
Ac**
* Lanthanides
** Actinides
1
Which compound is an organic acid ?
4
What is the correct IUPAC name for the
compound shown below?
O
A
H3C
C
CH3
CH3
B
H3C
O
C
H3C
CH2
H3C
C
5
2
3
H3C
B
1,1-dimethylpropane
C
2,2-dimethylpropane
D
1,1,1-trimethylethane
E
2-methylisobutane
H3C
H3C
C
CH3
H3C
What is the oxidation state of the phosphorus
atom in H3PO4 ?
OH
O
E
tert-methylmethane
OH
O
D
A
C
H
A
−2
B
+1
C
0
D
+5
E
+6
Which compounds are isomers ?
(1) H3C–CO–CH3
(2) H3C–CH2–O–CH3
(3) H3C–CH2–CHO
(4) H2C=CH–CHO
A
(1) and (2)
B
(2) and (3)
C
(3) and (4)
D
(1) and (3)
E
(2) and (4)
6
Which hydrocarbon belongs to the series of
The following is an acceptable Lewis structure for
the phosphate anion, PO43 .
••
•
•
•O •
••
•
•O
••
What is the formal charge on phosphorus ?
A
−3
B
−2
A
acetylene
C
−1
B
ethane
D
0
C
benzene
E
+1
D
xylene
E
propene
2 / CHEM 13 NEWS EXAM © 2001 UNIVERSITY OF WATERLOO
••
O
••
•
•
•O •
••
compounds that starts with ethene, the smallest
of the series?
P
3−
7
How many orbitals are there in the n = 4 shell of
10
an atom ?
Which ion has the smallest radius?
A
Ca2+
B
K+
A
1
B
4
C
Cl
C
5
D
S2
D
14
E
P3
E
16
11
-
Which one of the following atoms commonly
forms an ion having the same ground-state
electron configuration as Na+ ?
8
Which one of the following electron configurations
is inconsistent with Hund’s rule ?
1s
2s
2p
A
A
Li
B
Be
C
O
D
S
E
Cl
B
12
most polar ?
C
D
E
9
Which one of the following covalent bonds is the
A
H−O
B
H−N
C
H−Cl
D
H−S
E
H−F
What is the ground-state electron configuration of
an isolated Fe atom ?
13
In which one of the following molecules does the
central atom have no lone pairs ? (The central
A
[Ar] 3d 8
B
[Ar] 4s 2 3d 6
C
atom is underlined.)
2
8
2
6
[Ar] 4s 3d
D
[Ar] 5s 4d
E
[Ar] 4d
8
A
PF3
B
SO3
C
NH3
D
ClF3
E
XeO3
© 2001 UNIVERSITY OF WATERLOO CHEM 13 NEWS EXAM / 3
14
What is the molecular geometry of SOCl2?
18
An aqueous solution of ethanol, C2H5OH, is
(S is the central atom and all the other atoms are
95.6% ethanol by mass and it has a density of
bonded to it.)
0.804 g/mL. What is the molar concentration of
ethanol in this solution ?
15
A
linear
B
trigonal planar
C
trigonal pyramidal
D
V-shaped
E
trigonal bipyramidal
Which of the following substances has the highest
19
A
42.7 M
B
21.7 M
C
17.5 M
D
16.7 M
E
1.97 M
Atomic weights:
H, 1.01
O, 16.00
C, 12.01
Exactly 2.07 g of a pure compound is obtained
when 1.50 g of solid iron reacts with excess
vapour pressure at 300 K?
oxygen. What is the empirical formula of this
16
A
H2O
B
H2S
C
NH3
A
FeO
D
H2Se
B
Fe2O3
E
CH4
C
Fe3O4
D
Fe2O
E
Fe4O5
compound ?
Atomic weights:
O, 16.00
Fe, 55.85
o
If 3.0 L of oxygen gas at 177 C is cooled at
constant pressure until the volume becomes
1.50 L, what is the final temperature?
20
The chemical equation for the neutralization of
H2SO4 by KOH is
17
A
−48 C
B
o
86 C
C
o
o
H2SO4(aq) + 2KOH(aq)
0oC = 273 K
R = 8.3145 kPa L K 1 mol 1
40 C
→ K2SO4(aq) + 2H2O(l) .
If it takes 34.5 mL of 0.1234 M KOH to neutralize
o
D
3.4 C
20.0 mL of aqueous H2SO4 solution, what is the
E
−184 C
concentration of the H2SO4 solution ?
o
How many carbon atoms are there in
130 mg of solid carbon ?
A
5.0 × 1022
B
6.5 × 1021
C
6.0 × 1023
D
7.8 × 10
E
5.6 × 10
22
Atomic weight
of C, 12.01
Avogadro’s number,
6.022×1023 mol 1
22
4 / CHEM 13 NEWS EXAM © 2001 UNIVERSITY OF WATERLOO
A
0.0617 M
B
0.106 M
C
0.123 M
D
0.213 M
E
0.426 M
21
23
What is the pH of a 0.0020 M formic acid,
Given that
-4
HCOOH, solution? (Ka = 1.7×10 )
22
A
2.70
B
3.30
C
3.60
D
3.90
E
4.20
-
2N2(g) + O2(g) ‡ 2N2O(g)
Kp = 5.04×10 37
N2(g) + O2(g) ‡ 2NO(g)
Kp = 4.23 × 10 31
-
what is Kp for the reaction,
2N2O(g) + O2(g) ‡ 4NO(g) ?
-
A
3.55 × 10 25
B
2.13 × 10 67
C
1.19 × 10 6
D
8.39 × 10+5
E
cannot be determined.
-
The titration curve for an acid-base titration is
shown below. Which pH indicator is appropriate
for detecting the increase in pH that occurs near
24
Consider the reversible, gas-phase reaction
N2H4 + 2HCl ‡ 2NH3 + Cl2.
the equivalence point?
The reaction is exothermic in the forward
pH
direction. Which of the following actions increases
the equilibrium concentration of N2H4 ?
11
9
7
4.5
3
Volume of titrant
A
B
25
decreasing the external pressure
B
increasing the external pressure
C
adding a catalyst
D
increasing the temperature
E
none of these actions increases [N2H4]
When the concentrations of reactants are
Alizarin yellow: yellow at pH 10, violet at
increased at constant temperature, the rate of the
pH 12
reaction also increases. This is best explained by
Bromophenol blue: yellow at pH 3, blue at
A
pH 4.5
C
A
have enough energy to react.
Bromocresol green: yellow at pH 3.5, blue at
B
pH 5
an increase in the fraction of molecules that
an increase in the frequency of the molecular
collisions.
D
Methyl red: red at pH 4.5, yellow at pH 6
E
Thymol blue: yellow at pH 8, blue at pH 9.5
C
an increase in the rate constant.
D
an increase in the kinetic energy of the
molecules.
E
an increase in the average potential energy of
the molecules.
© 2001 UNIVERSITY OF WATERLOO CHEM 13 NEWS EXAM / 5
26
In a chemical reaction at constant temperature,
29
The solubility of silver oxalate, Ag2(C2O4), in
-
-
the addition of a catalyst
water is 1.1 × 10 4 mol L 1 at 298 K. What is Ksp
A
value for silver oxalate?
increases the value of the equilibrium
constant.
B
C
A
1.5×10 16
than a given kinetic energy.
B
5.3×10 12
C
1.3×10 12
D
2.4×10 8
E
1.2×10 8
decreases the energy released in the
chemical reaction.
D
provides an alternative reaction mechanism
with a lower activation energy.
E
-
increases the fraction of molecules with more
-
-
-
-
increases the rate at which the molecules
collide with one another.
27
The enthalpy change for the reaction,
30
A 10-g sample of ethyl acetate was boiled with
100 g of water. By this treatment two new
A+B → C+D
substances were formed. They were
is ∆H = -244 kJ. If the activation energy for the
forward reaction is 52 kJ, what is the activation
energy for the reverse reaction, C + D → A + B ?
28
A
methanal and acetone.
B
methanol and ethane.
A
-52 kJ
C
diethyl ether and ethanoic acid.
B
-192 kJ
D
ethanol and ethanoic acid.
C
296 kJ
E
ethanol and methanal
D
192 kJ
E
-296 kJ
The decomposition of CH3CHO to CH4 and other
31
products obeys the rate law,
-d[CH3CHO] / dt = k [CH3CHO]
Sodium hydroxide, NaOH, is gradually added to a
-
3.5×10 4 M CoSO4 solution. At what pH will cobalt
hydroxide begin to precipitate?
-
with k = 0.035 min 1. How long does it take for
[CH3CHO] to decrease from 0.4 M to 0.3 M?
A
less than 1 minute
B
4 minutes
C
8 minutes
D
16 minutes
E
greater than 16 minutes
6 / CHEM 13 NEWS EXAM © 2001 UNIVERSITY OF WATERLOO
A
1.85
B
4.47
C
6.07
D
7.93
E
9.53
-
Ksp = 2.5 × 10 16 for Co(OH)2
-14
Kw = 1.0 × 10
32
Copper wire is dipped into 1.0 M solutions of each
35
The oxygen-hydrogen fuel cell is based on the
of the following salts. In which case will a reaction
spontaneous reaction that occurs when the
have the greatest tendency to occur?
following half-reactions are combined:
-
33
-
2H+(aq) + 2e → H2(g)
AgNO3(aq)
Ag + e → Ag
B
KNO3(aq)
Cu2+ + 2e → Cu
+0.34 V
C
Fe(NO3)2(aq)
Ni2+ + 2e → Ni
-
-0.24 V
-0.13 V
-0.41 V
-2.9 V
A
D
Ni(NO3)2(aq)
E
Pb(NO3)2(aq)
+
-
2+
Pb
-
+ 2e → Pb
-
Fe2+ + e → Fe
-
K+ + e → K
+0.80 V
-
O2(g) + 4H+(aq) + 4e → 2H2O(l)
Eo = +1.2 V
Which of the following statements regarding the
oxygen-hydrogen fuel cell is true?
Which of the following is the strongest reducing
A
The hydrogen electrode is the anode.
B
The cell potential depends on pH.
C
Oxidation occurs at the oxygen electrode.
D
Electrons flow from the oxygen electrode to
agent in its standard state?
the hydrogen electrode.
E
None of the statements above is true.
+
A
H
B
K
C
F
D
Al3+
E
O2
-
36
The enthalpy change for the reaction,
C8H18(l) +
34
Eo = 0 V
25
2
O2(g) → 8CO2(g) + 9H2O(g),
o
Aluminum, Al(s), is produced commercially by the
is ∆H = -5407 kJ. What is the standard enthalpy
electrolysis of Al3+. What mass of Al is obtained in
of formation, ∆H f , for C8H18(l)?
o
a twenty-four hour period if a steady current of
o
∆H f
100,000 amperes is used?
A
33.5 kg
B
536 kg
C
805 kg
1 ampere
= 1 coulomb per second
D
1206 kg
Faraday’s constant:
F = 96 485 coulombs per mole
E
2412 kg
Atomic weight of Al, 26.98
A
+77 kJ/mol
CO2(g)
-394 kJ/mol
B
+4771 kJ/mol
H2O(g)
-242 kJ/mol
C
-319 kJ/mol
H2O(l)
-286 kJ/mol
D
+5407 kJ/mol
E
The answer cannot be determined because
o
∆H f for O2(g) is not given.
© 2001 UNIVERSITY OF WATERLOO CHEM 13 NEWS EXAM / 7
37
A weak monoprotic acid (HA) has an acid
40
ionization constant Ka = 1.8 x 10-5 at 298 K. If
The chemical equation for the decomposition of
nitroglycerin (C3H5N3O9) is
4C3H5N3O9 (l)
100 mL of a 0.10 mol/L solution of HA is mixed
→ 6N2(g) + 12CO2(g) + 10H2O(l) + O2(g).
with 200 mL of a 0.10 mol/L solution of sodium
hydroxide, what is the approximate pH of the
What volume of gas is produced by the complete
resulting solution at 298 K ?
decomposition of 0.200 kg C3H5N3O9, assuming
the gas is collected at 298 K and 101 kPa?
38
A
1.5
B
4.7
A
22 L
C
7.0
B
102 L
D
9.3
C
119 L
E
12.5
D
172 L
E
215 L
-
Kw = 1.0×10 14 at 298 K
H, 1.01
N, 14.01
C, 12.01
O, 16.00
-
-
R = 8.314 kPa L K 1 mol 1
The solubility of sodium chloride in water at 25oC
is 31.1 g in 100 mL of solution. How many grams
WANT TO WIN A CHEM 13 NEWS T-SHIRT?
of sodium ion will be found in one litre of solution?
Then attempt question #41. There is no penalty if you
answer it incorrectly. Students who answer the question
A
10.0 g
B
23.0 g
C
122 g
D
230 g
E
311 g
Atomic weights:
Na, 23.0
Cl, 35.5
correctly will be entered into a draw for one of our limited
edition CHEM 13 NEWS T-shirts.
41
In the year 2000, a University of Waterloo
professor was awarded the McNeil Medal from
the Royal Society of Canada in recognition of his
outstanding ability to promote and communicate
39
What material should you choose to clean up a
science to students and the public.* Some of you
small spill of aqueous sulfuric acid?
may know this professor as the Editor-in-Chief of
CHEM 13 NEWS. Who is he?
A
Hydrochloric acid solution
B
Acetic acid solution
C
Sodium hydroxide solution
D
Sodium chloride solution
E
Sodium hydrogen carbonate solution
A
Prof. David Suzuki
B
Prof. John Polanyi
C
Prof. Reginald Friesen
D
Prof. Lewis Brubacher
E
Prof. Michael Smith
* The organizers of this exam (Dr. Carey Bissonnette,
Prof. Guy Guillemette and Ms. Kathy Jackson) offer
heartfelt congratulations!
8 / CHEM 13 NEWS EXAM © 2001 UNIVERSITY OF WATERLOO
CHEM 13 NEWS EXAM 2002
UNIVERSITY OF WATERLOO
DEPARTMENT OF CHEMISTRY
8 MAY 2002
TIME: 75 MINUTES
This exam is being written by several thousand students. Please be sure that you follow the instructions below.
We'll send you a report on your performance. Top performers are eligible for a prize.
1. Print your name here:
2. Print your school name and city on your STUDENT
RESPONSE sheet.
3. Select, and enter on the STUDENT RESPONSE
sheet, one of the following CODE numbers:
Code 1
Ontario, now studying OAC Chemistry in a
nonsemestered school
Code 2
Ontario, now studying OAC Chemistry in a
semestered school
Code 3
Ontario, OAC Chemistry already completed
Code 4
Any other Ontario student
Code 5
Manitoba or Saskatchewan high school
student
Code 6
Québec high school student
4. Print your name (last name, first name and optional
middle initial) on the STUDENT RESPONSE sheet.
Also fill in the corresponding circles below your printed
name.
5. Now answer the exam questions. Indicate your choice
on the STUDENT RESPONSE sheet by marking one
letter beside the question number.
• Mark only one answer for each question.
• Questions are all of the same value.
• There is a penalty (1/4 off) for each incorrect
answer, but no penalty if you do not answer.
Questions are not in order of difficulty.
Code 7
Code 8
Québec CEGEP student
Alberta or British Columbia high school
student
Code 9 New Brunswick, Newfoundland, Nova Scotia,
or Prince Edward Island high school student
Code 10 Northwest Territories, Nunavut, or Yukon
high school student
6. Take care that you make firm, black pencil marks, just
filling the oval.
Be careful that any erasures are complete—make the
sheet white again.
Code 11 High school student outside Canada
Code 12 Teacher
H
He
Li
Be
B
C
N
O
F
Ne
Na
Mg
Al
Si
P
S
Cl
Ar
K
Ca
Sc
Ti
V
Cr
Mn
Fe
Co
Ni
Cu
Zn
Ga
Ge
As
Se
Br
Kr
Rb
Sr
Y
Zr
Nb
Mo
Tc
Ru
Rh
Pd
Ag
Cd
In
Sn
Sb
Te
I
Xe
Cs
Ba
La*
Hf
Ta
W
Re
Os
Ir
Pt
Au
Hg
Tl
Pb
Bi
Po
At
Rn
Fr
Ra
Ac**
* Lanthanides
** Actinides
1
Which functional groups are present in the
5
molecule below?
compound shown below?
O
O
H C
What is the correct IUPAC name for the
CH3CH2
CH2 O CH2 C OCH2CH3
CH2CH2CH3
C CH2 CH CH3
O
2
A
aldehyde and ketone
B
ester and aldehyde
C
carboxylic acid, ether and aldehyde
D
ester, ketone and ether
E
aldehyde, ether and ester
Which one of the following is not an isomer of
6
A
3-methyl-1-ethyl-1-n-propyl-1-pentanol
B
4-ethyl-4-nonanol
C
4-ethyl-6-methyl-4-octanol
D
5-methyl-3-n-propyl-3-heptanol
E
5-ethyl-3-n-propyl-3-hexanol
Which elements are always present in amino
acids?
C5H11Br ?
A
C, H, and O
A
1-bromo-2,2-dimethylpropane
B
C, N, and O
B
1-bromo-3-methylbutane
C
C, N, and H
C
2-bromo-3-methylbutane
D
C, H, N and O
D
1-bromo-2-ethylbutane
E
C, H, O, N and S
E
2-bromopentane
7
3
CH2CH3
H
Natural oils, such as corn oil or sunflower oil, are
converted into solid, edible fats by a process
The longest carbon-oxygen bond is found in
called
A
ethanal (CH3CHO )
A
hydrogenation
B
carbon monoxide (CO)
B
freezing
C
ethanol (CH3CH2OH)
C
saponification
D
carbon dioxide (CO2)
D
reduction
E
propanone (CH3COCH3)
E
hydrolysis
8
4
Oxidation of 1-propanol in aqueous solution yields
A
propanal
B
ethanol and water
C
diethyl ether and water
D
propanoic acid
E
propanone
2 / CHEM 13 NEWS EXAM © 2002 UNIVERSITY OF WATERLOO
What would have to be done to the species NH2
to convert it to an ion with a -1 charge?
A
nothing; it already has a charge of -1
B
add one electron
C
remove two electrons
D
remove one proton
E
add two electrons and add one proton
9
How many electrons are there in the 3d orbitals of
13
2+
The phase diagram for a certain pure substance
is shown below. The triple point is at 43 atm and
an isolated Ni ion in its lowest energy state?
590oC. What is the only possible phase transition
10
A
10
B
9
C
8
D
7
E
6
that can occur if the pressure is decreased from
50 atm at a constant temperature of 500oC?
Which one of the following is diamagnetic in its
A
vapourization
B
condensation
C
sublimation
D
fusion
E
crystallization
lowest energy state?
11
A
K
B
N3
C
Fe
D
Cr
E
C
Gas
Temperature
-
14
2+
Which pair of elements is most likely to form an
ionic compound?
3+
What is the ground-state electron configuration of
an isolated technetium (Tc) atom ?
12
Liquid
Solid
A
[Kr] 5s 2 5d 5
B
[Kr] 4s 2 4d 5
C
[Kr] 5s 2 5p 5
D
[Kr] 5s 4d
E
[Kr] 5d 7
2
15
A
hydrogen and fluorine
B
carbon and fluorine
C
beryllium and hydrogen
D
boron and fluorine
E
calcium and oxygen
-
What is the molecular geometry of ICl4 ?
(I is the central atom and all of the Cl atoms are
5
bonded to it.)
A
tetrahedral
B
square pyramidal
In general, electron affinity
C
see-saw shaped
A
decreases from left to right across a period.
D
square planar
B
increases from top to bottom within a group.
E
T-shaped
C
increases from bottom to top within a group.
D
shows little variation within a period.
E
is largest for the noble gases.
© 2002 UNIVERSITY OF WATERLOO CHEM 13 NEWS EXAM / 3
16
19
A student proposed the following resonance
-
density of 15.0 g L 1 at a pressure of 253 kPa and
structures for the HClO4 molecule.
O
O
Cl
O
Cl
127oC?
O
O
OH
OH
O
Cl
OH
-
43 g mol 1
-
O
O
B
73 g mol 1
(i)
(ii)
(iii)
C
87 g mol 1
D
132 g mol 1
E
197 g mol 1
these structures is correct?
-
-
A
Structure (i) is the most important.
B
Structure (ii) is the most important.
C
Structure (iii) is the most important.
grams per litre. What volume of a saturated
D
All three structures are equally important.
solution of PbS contains about one Pb2+ ion?
E
Structures (i) and (ii) are not possible
because they do not obey the octet rule.
20
Which of the following solids has the highest
vapour pressure at 100 K?
-
R = 8.314 kPa L K 1 mol 1
0oC = 273 K
-
A
O
Which one of the following statements concerning
17
What is the molar mass of a gas that has a
-
The solubility of PbS in water is about 7.2×10 26
A
10 L
B
100 L
C
25 L
D
6L
E
6000 L
Atomic weights
S, 32.07 Pb, 207.2
Avogadro’s number,
6.022×1023 mol 1
A
graphite
B
PH3(s)
C
NH3(s)
D
copper
mass of 2.00 g, is dissolved in water. Silver
E
potassium chloride
nitrate solution, AgNO3(aq), is added, and all of
21
A mixture of BaCl2 and Ba(NO3)2 , with a total
-
the dissolved Cl is precipitated as AgCl. The
mass of the precipitate is 0.688 g. What is the
18
Suppose that 3.0 L of He(g) at 3.0 atm, 4.0 L of
percentage (by mass) of BaCl2 original sample?
Ne(g) at 4.0 atm and 5.0 L of Ar(g) at 5.0 atm are
introduced into a 20.0-L tank. What is the final
A
50.0%
pressure, assuming the temperature remains
B
25.0%
constant?
C
100%
D
34.4%
E
66.6%
o
0 C = 273 K
R = 0.08206 atm L K-1 mol-1
A
12 atm
B
0.60 atm
C
0.15 atm
D
2.5 atm
E
4.0 atm
4 / CHEM 13 NEWS EXAM © 2002 UNIVERSITY OF WATERLOO
Atomic weights:
Cl,
35.45
Ag,
107.9
Ba,
137.7
22
A compound that contains only carbon, hydrogen,
25
and nitrogen is analyzed and found to be 75.9%
-
What is the pH of a 0.010 mol L 1 HOCl(aq )
-
solution ? (Ka = 2.8×10 8 for HOCl )
carbon by mass and 17.7% nitrogen by mass.
What is the empirical formula of the compound?
A
C3H4N
B
C4H4N
C
C5H5N
D
C6H6N2
E
C10H7N2
Atomic weights:
H
1.01
C
12.01
N
14.01
26
A
2.00
B
3.78
C
4.78
D
7.55
E
9.55
What is the pH at the equivalence point when
-
23
-3
25 mL of a 0.100 mol L 1 solution of ascorbic acid
-1
How many millilitres of 1.55×10 mol L
-
(a monoprotic acid) is titrated with 0.050 mol L 1
HNO3(aq) are required to neutralize 100.0 mL of
-
NaOH(aq)?
-
1.90×10 4 mol L 1 Mg(OH)2(aq) ?
24
A
24.5 mL
A
11.45
B
12.2 mL
B
2.55
C
6.13 mL
C
5.75
D
49.0 mL
D
8.55
E
18.6 mL
E
8.31
-
Ka = 8.0×10 5 for ascorbic acid
Kw = 1.0×10 14
Which one of the following compounds produces
the most acidic solution when it is dissolved in
water?
27
What is the pH of a saturated aqueous solution of
Mg(OH)2 at 25oC?
A
Cl2CH−CH2−COOH
B
CH3−CCl2−COOH
A
10.22
C
CH3-CCl2−CHO
B
10.52
C
10.74
D
ClCH2−CHCl-COOH
D
8.63
E
CH3−CCl2−CH2OH
E
8.33
-11
Ksp = 1.8×10 for Mg(OH)2
-14
Kw = 1.0×10
© 2002 UNIVERSITY OF WATERLOO CHEM 13 NEWS EXAM / 5
28
What
is
the
correct
equilibrium
constant
31
expression for the reaction
The reaction profile for a two-step reaction is
shown below.
CaSO3(s) ‡ CaO(s) + SO2(g)?
[CaO] [SO2 ]
A
Kc =
B
K c = [CaO] [SO 2 ]
C
K c = [SO 2 ]
D
Kc =
b
Potential
Energy
[CaSO3 ]
c
a
E
29
Kc =
[SO2 ]
Which quantity is the most important for
determining the rate of the forward reaction?
[CaSO3 ]
[CaO] [SO2 ]
What is ∆H o for the reaction
2CH3OH(l) + 3O2(g) → 2CO2(g) + 4H2O(l)?
-1454 kJ
B
-441 kJ
C
-2410 kJ
D
-1932 kJ
E
-680 kJ
A
a
B
b
C
c
D
d
E
e
-
∆H fo (in kJ mol 1)
CH3OH(l)
CO2(g)
H2O(l)
-239
-394
-286
32
The decomposition of cyclopropane to propane
obeys a first-order rate law. The rate constant has
-
the value k = 0.056 min 1 at 450oC. How long
does it take for the concentration of cyclopropane
to decrease from 0.40 mol L-1 to 0.10 mol L-1 at
this temperature?
30
e
Reaction Coordinate
1
A
d
The reaction
A
less than 1 minute
B
25 minutes
reaches equilibrium in a closed reaction vessel.
C
134 minutes
Which one of the following actions causes the
D
5.4 minutes
equilibrium to shift to the right ?
E
71 minutes
C(s) + O2(g) ‡ CO2(g) + heat
A
increasing the volume of the reaction vessel
B
adding a catalyst
C
adding a small amount of carbon
D
lowering the temperature
E
increasing the reaction time
6 / CHEM 13 NEWS EXAM © 2002 UNIVERSITY OF WATERLOO
33
What is the enthalpy change for the reaction,
36
C(graphite) + 2H2(g) → CH4(g)?
In which one of the following series does the
oxidation state of chlorine increase from left to
right?
-
H-H bond energy: 436 kJ mol 1
34
-
A
1565 kJ
C-H bond energy: 413 kJ mol 1
A
Cl2
HClO4
HClO
HCl
B
-64 kJ
B
HClO4
Cl
Cl2
HClO
C
-780 kJ
Enthalpy of sublimation
of graphite: 716 kJ mol 1
C
HClO4
HClO
Cl2
HCl
D
652 kJ
D
HCl
Cl2
HClO
HClO4
E
-500 kJ
E
Cl2
HClO
HCl
HClO4
What is the maximum concentration of iron(II) that
can remain in an aqueous solution at 25oC if the
37
agent in its standard state?
pH of the solution is kept constant at pH 8.0?
-
Ksp = 7.9 × 10 16 for Fe(OH)2
Kw = 1.0 × 10 14
-4
Which of the following is the strongest oxidizing
A
Na+
B
K
-1
C
F
-
D
F2
E
Na
A
2.8×10 mol L
B
7.9×10-4 mol L 1
C
2.8×10-8 mol L 1
D
7.9×10-10 mol L 1
E
2.8×10-14 mol L 1
-
K+(aq) + e- → K(s)
Na+(aq) + e- → Na(s)
-
F2 + 2e- → 2F (aq)
-2.9 V
-2.7 V
2.9 V
-
-
38
What is the minimum current required to deposit
0.500 g of chromium metal from an aqueous
solution of chromium (III) nitrate in a period of one
hour?
35
What is [Ag+ ] in solution when 0.50 L of
0.10 mol L-1 AgNO3(aq) and 0.50 L of
-1
0.20 mol L NaCl(aq) are mixed?
-
A
0.05 mol L 1
B
0 mol L 1
C
1.3×10−5 mol L 1
D
9.0×10−10 mol L 1
E
3.6×10−9 mol L 1
-10
Ksp = 1.8×10
-
for AgCl
A
40.2 A
B
0.0112 A
C
0.257 A
D
0.773 A
E
2.32 A
1 A = 1 coulomb per second
Faraday’s constant:
F = 96 485 coulombs per mole
Atomic weight of Cr, 52.0
-
-
-
© 2002 UNIVERSITY OF WATERLOO CHEM 13 NEWS EXAM / 7
39
Consider the following voltaic cell.
platinum wire
salt bridge
Fe(s)
1.0 mol L- Fe(NO3)2(aq)
1
Pb(s)
1.0 mol L- Pb(NO3)2(aq)
Pb2+(aq) + 2e- → Pb(s)
Fe2+(aq) + 2e- → Fe(s)
1
Eo = -0.13 V
Eo = -0.41 V
Which one of the following statements is true?
40
A
The mass of the iron electrode decreases.
B
Positive ions in the salt bridge migrate toward
the Fe(NO3)2 solution.
C
The iron electrode is the cathode.
D
The iron electrode develops a coating of lead.
E
The cell potential is 0.57 V.
Nitrate ion, NO-3 , oxidizes copper metal in
aqueous acidic solution. The unbalanced
chemical equation for the reaction is
NO-3 (aq)
+
→
Cu(s) + H+
NO(g) + Cu2+(aq) + H2O(l).
When this chemical equation is balanced using
the smallest whole number coefficients, the
coefficient of NO-3 is
A
1
B
2
C
3
D
4
E
6
8 / CHEM 13 NEWS EXAM © 2002 UNIVERSITY OF WATERLOO
ANSWER GRIDS BY YEAR
1990
1-C
11-E
21-E
31-C
41-A
2-A
12-D
22-E
32-C
42-C
3-B
13-B
23-B
33-E
43-D
4-A
14-C
24-A
34-E
44-D
5-E
15-E
25-C
35-A
45-A
6-D
16-C
26-E
36-B
46-E
7-D
17-E
27-D
37-E
47-A
8-C
18-B
28-C
38-A
9-C
19-B
29-C
39-D
10-C
20-A
30-D
40-A
2-A
12-C
22-B
32-B
42-A
3-B
13-E
23-E
33-B
43-B
4-E
14-E
24-E
34-E
44-B
5-B
15-D
25-A
35-E
45-D
6-D
16-B
26-E
36-D
7-E
17-E
27-B
37-C
8-D
18-D
28-A
38-E
9-C
19-E
29-B
39-E
10-C
20-B
30-E
40-A
2-D
12-D
22-E
32-A
3-D
13-B
23-E
33-D
4-D
14-C
24-B
34-B
5-A
15-E
25-E
35-D
6-B
16-C
26-D
36-E
7-D
17-C
27-D
37-A
8-C
18-C
28-E
38-B
9-A
19-B
29-B
39-C
10-E
20-C
30-C
40-C
1991
1-D
11-B
21-A
31-D
41-A
1994
1-D
11-D
21-B
31-C
Last Revised by D. Lougheed 7/3/00
1995
1-D
11-E
21-C
31-B
2-D
12-B
22-D
32-C
3-A
13-A
23-E
33-E
4-E
14-B
24-C
34-E
5-B
15-B
25-B
35-D
6-D
16-A
26-B
36-D
7-A
17-C
27-C
8-D
18-A
28-C
9-C
19-E
29-E
10-A
20-E
30-A
2-E
12-B
22-C
32-B
3-B
13-C
23-E
33-C
4-E
14-A
24-C
34-A
5-A
15-E
25-C
35-D
6-E
16-A
26-E
36-C
7-E
17-B
27-B
37-D
8-D
18-E
28-E
38-B
9-A
19-B
29-C
39-A
10-A
20-D
30-D
2-B
12-B
22-E
32-A
3-E
13-B
23-A
33-B
4-BorC
14-D
24-B
34-B
5-E
15-C
25-D
35-E
6-B
16-D
26-D
36-E
7-A
17-D
27-E
37-C
8-C
18-B
28-C
38-D
9-E
19-B
29-C
39-A
10-C
20-D
30-A
40-C
2-B
12-B
22-D
32-B
3-E
13-B
23-B
33-C
4-C
14-A
24-E
34-D
5-A
15-C
25-D
35-A
6-D
16-D
26-B
36-A
7-A
17-D
27-E
37-C
8-E
18-C
28-D
38-E
9-B
19-B
29-C
39-B
10-B
20-C
30-C
2-C
12-D
22-B
32-A
3-E
13-E
23-D
33-E
4-A
14-C
24-D
34-B
5-B
15-A
25-E
35-B
6-B
16-B
26-D
36-D
7-B
17-D
27-B
37-E
8-C
18-B
28-C
38-B
9-A
19-D
29-E
39-C
10-B
20-E
30-C
40-A
2-D
12-D
22-B
32-E
3-C
13-C
23-B
33-E
4-D
14-B
24-C
34-A
5-E
15-B
25-D
35-E
6-D
16-D
26-B
36-B
7-A
17-C
27-B
37-B
8-C
18-E
28-D
38-D
9-A
19-C
29-A
39-E
10-A
20-E
30-E
40-A
1996
1-E
11-E
21-B
31-C
1997
1-A
11-E
21-A
31-A
1998
1-C
11-A
21-E
31-A
1999
1-E
11-C
21-A
31-C
2000
1-C
11-B
21-E
31-B
Last Revised by D. Lougheed 7/3/00
2001 CHEM 13 NEWS EXAM ANSWERS
1. D
2. D
3. E
4. C
5. D
6. D
7. E
8. B
9. B
10. A
11. C
12. E
13. B
14. C
15. E
16. A
17. B
18. D
19. C
20. B
21. B
22. E
23. A
24. B & D
25. B
26. D
27. C
28. C
29. B
30. D
31. D
32. A
33. B
34. C
35. A
36. A
37. E
38. C
39. E
40. B
2002 CHEM 13 NEWS EXAM ANSWERS
1. E
2. D
3. C
4. D
5. C
6. D
7. A
8. A
9. C
10. B
11. D
12. C
13. C
14. E
15. D
16. A
17. B
18. D
19. E
20. E
21. B
22. C
23. A
24. B
25. C
26. E
27. B
28. C
29. A
30. D
31. A
32. B
33. B
34. B
35. E
36. D
37. D
38. D
39. A
40. B