Name: __________________________ Date: _____________
1. Ni(CO)4 can be prepared by reacting nickle (Ni) with gasous carbon monoxide (CO).
If you have CO in a 1.50 L flask at a pressure of 418 mmHg at 25 oC along with excess
Ni powder, what is the theoretical yield of Ni(CO)4?
A)
B)
C)
D)
E)
1.44 g
5.75 g
2.88 g
1.31 g
3.83 g
2. If you place gasous unknown compound containing 25.53 % S in a 89.0 mL flask at
45 oC, and the total mass of the comound is 0.0955 g and the pressure is 83.8 mmHg.
What is the molecular formula SxFy?
A)
B)
C)
D)
E)
S2F10
SF5
S3F15
S2F2
S2F5
3. In an experiment, it is determined that 0.66 moles of CF4 effuse through a porous barrier
over a 4.8 minute period. How long will it take for 0.66 moles of CH4 to effuse
through the same barrier?
A)
B)
C)
D)
E)
2.0 min
0.66 min
0.33 min
1.5 min
1.2 min
4. Absolute zero is the point at which
A)
B)
C)
D)
E)
a straight-line graph of V versus T (K) intersects the origin.
a straight-line graph of V versus 1/P at constant T intersects the origin.
gaseous helium liquefies.
a straight-line graph of 1/V versus P at constant T intersects the origin.
a straight-line graph of V versus T (°C) intersects the origin.
Page 1
5. The pressure of 5.4 L of nitrogen gas in a flexible container is decreased to one-half its
original pressure, and its absolute temperature is increased to double the original
temperature. The volume is now
A)
B)
C)
D)
E)
22 L
2.7 L
5.4 L
11 L
1.4 L
6. Hydrogen and oxygen gas are mixed in a 7.75 L flask at 65 oC, and contains 0.482 g of
hydrogen and 4.98 g of oxygen. What is the partial pressure of oxygen in the flask?
A)
B)
C)
D)
E)
0.557 atm
0.043 atm
1.11 atm
33.5 atm
67.0 atm
7. You add 0.255 g of a molecular compound to 11.2 g of benzene. The boiling point of
the benzene rises from 80.10 oC to 80.26 oC. What is the molar mass of the compound?
Kb = 2.53 oC/m
A)
B)
C)
D)
E)
360. g/mol
63.0 g/mol
111 g/mol
700. g/mol
130. g/mol
8. Concentrated aqueous ammonia (NH3) has a molarity of 14.8 mol/L and a density of
0.90 g/cm3. What is the molality of the solution?
A)
B)
C)
D)
E)
23 m
6.5 m
13 m
15 m
19 m
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9. A solution is made by adding 50.0 mL of ethanol (C2H5OH, d = 0.789 g/mL) to 50.0 mL
of water (d = 0.998 g/mL). What is the total vapor pressure over the solution at 20.0
o
C? Given: Vapour pressure for the pure ethanol is 43.6 mmHg and water is 17.5
mmHg at 20.0 oC.
A)
B)
C)
D)
E)
23.7 mmHg
35.6 mmHg
27.7 mmHg
38.5 mmHg
19.3 mmHg
10. The solubility of nitrogen gas at 25°C and a nitrogen pressure of 522 mmHg is 4.7×10– 4
mol/L. What is the value of the Henry's Law constant in mol L–1 atm–1?
A)
B)
C)
D)
E)
6.8 × 10–4
1.5 × 103
3.2 × 10–4
9.0 × 10–7
4.7 × 10–4
11. From the following list of aqueous solutions and water, select the one with the highest
boiling point.
A)
B)
C)
D)
E)
0.75 m CuCl2
0.75 m NaCl
1.0 m KNO3
2.0 m C12H22O11 (sucrose)
pure water
12. A 0.100 m MgSO4 solution has a freezing point of –0.23°C. What is the van't Hoff
factor for this solution? Kf = 1.86°C/m
A)
B)
C)
D)
E)
1.2
1.5
2.0
1.8
1.4
Page 3
13. You are given a small bar of metal M. The density of the metal is 10.5 g/cm3. The
edge of the face-centered cubic unit is 4.09 x 10-8 cm. Identify the M.
A)
B)
C)
D)
E)
Ag
Au
Co
Pt
Cu
14. The distance between layers in a MX crystal is 182 pm. X rays are diffrated from these
layers at an angle of 22.20°. Assuming that n =1, calculate the wavelength of the X
rays in nanometers.
A)
B)
C)
D)
E)
0.138 nm
138 nm
14.2 nm
142 nm
0.142 nm
15. In hydrogen iodide, __________________ are the most important intermolecular forces.
A)
B)
C)
D)
E)
dipole–dipole forces
covalent bonds
polar covalent bonds
hydrogen bonding
London dispersion forces
16. The energy needed to increase the surface area of a liquid is
A)
B)
C)
D)
E)
surface tension.
viscosity.
capillary action.
cohesion.
specific elasticity.
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17. How much energy (heat) is required to convert 52.0 g of ice at –10.0°C to steam at
100°C?
specific heat of ice:
2.09 J/g·°C
Hfus = 6.02 kJ/mol
specific heat of water: 4.18 J/g·°C
Hvap = 40.7 kJ/mol
specific heat of steam: 1.84 J/g·°C
A)
B)
C)
D)
E)
157.6 kJ
2570 kJ
1086 kJ
2296 kJ
40.20 kJ
18. Krypton has a higher melting point than argon because of its
A)
B)
C)
D)
E)
stronger dispersion forces.
permanent dipole moment.
greater ionization energy.
ionic bonds.
ion-dipole interactions among Krypton atoms.
19. The cost of the gold is $ 1350 per 31.103 g. It has been estimated that 8 x 104 tons of
gold (Au) have been extracted. What is the total worth of this quantity? (1 ton =
2000 lb; 1 lb = 16 oz; 1 oz = 28.35 g)
A)
B)
C)
D)
E)
$ 3 x 1012
$ 1 x 1011
$ 9 x 1013
$ 7 x 1013
$ 8 x 1011
20. Convert 244.2°F into degrees Celsius.
A)
B)
C)
D)
E)
117.9°C
382.0°C
167.7°C
153.4°C
103.7°C
Page 5
21. What is the correct formula for aluminium hydrogen phosphate?
A)
B)
C)
D)
E)
Al2(HPO4)3
Al(HPO4)3
Al3(HPO4)2
Al(H2PO4)3
Al(HPO3)3
22. The correct name of the compound HBrO2 is
A)
B)
C)
D)
E)
bromous acid
hypobromous acid
hydrogen bromite
bromic acid
hydrogen bromine dioxide
23. A sample of xenon fluoride compound contains molecules of the type XeFn, where n is
some whole number. Given that 9.03 x 1020 molecules of XeFn, weigh 0.368 g,
determine the value for n in the formula.
A)
B)
C)
D)
E)
6
5
4
3
2
24. The empirical formula of styrene is CH; the molar mass of styrene is 104.14 g/mol.
What number of H atoms are present in a 2.00 g of styrene?
A)
B)
C)
D)
E)
9.25 x 1022
1.16 x 1022
6.13 x 1022
5.78 x 1021
1.85 x 1021
Page 6
25. Balance the following equation using the smallest set of whole numbers, then add
together the coefficients. Don't forget to count coefficients of one. The sum of the total
coefficients is
__ SF4 + __ H2O
A)
B)
C)
D)
E)
__ H2SO3 +
__ HF
9
11
13
7
6
26. What volume of 0.0350 M barium hydroxide is required to completely neutralize 26.00
mL of 0.0600 M phosphoric acid?
A)
B)
C)
D)
E)
66.9 mL
15.0 mL
29.7 mL
53.5 mL
43.3 mL
27. Which choice gives the correct oxidation numbers for all three elements in Rb2SO3 in
the order that the elements are shown in the formula?
A) +1, +4, 2
B)
2, +6, 2
C) 1, +4, 3
D) +2, +4, 2
E) +1, +6, 6
28. Use the following data to calculate the standard enthalpy of formation of hexane,
C6H14(l):
2C6H14(l) + 19O2(g) → 12CO2(g) + 14 H2O(l)
ΔH° = -8326 kJ
Given ΔH° kJ/mol: CO2(g) = -393.5; H2O(l) = -285.8
A)
B)
C)
D)
E)
-199 kJ/mol
-398 kJ/mol
398 kJ/mol
-355 kJ/mol
199 kJ/mol
Page 7
29. A baloon is being inflated to its full extent by heating the air inside it. In the final stages
of the process, the volume of the ballon changes from 4.00 x 106 L to 4.50 x 106 L by
the addition of 1.3 x 108 J of energy as heat. Assuming that the balloon expands
against a constant pressure of 1 atm, calculate ΔU for the process. [ 1L·atm = 101.3 J]
A)
B)
C)
D)
E)
8 x 107 J
5 x 105 J
2 x 108 J
1 x 108 J
3 x 106 J
30. Which of the following statements is/are correct?
i. The importance of the equation E = mc2 is that energy has mass.
ii. Electromagnetic radiation can be thought of as a stream of particles called photons.
iii. Electromagnetic radiation exhibits wave properties.
iv. Energy can only occur in discrete units called quanta.
A)
B)
C)
D)
E)
All of them
i, ii and iv only
i, iii and iv only
i, ii and iii only
ii, iii and iv only
31. What is the frequency of electromagnetic radiation with wavelength 532 nm?
A)
B)
C)
D)
E)
5.64 × 1014 s–1
4.18 × 1018 s–1
6.48 × 1012 s–1
3.75 × 1015 s–1
6.23 × 1014 s–1
32. The complete electron configuration of tin (Sn) is
A)
B)
C)
D)
E)
1s22s22p63s23p64s23d104p65s24d105p2
1s22s22p63s23p64s24p65s24d105d105p2
1s22s22p63s23p64s23d104d104p2
1s22s22p63s23p64s23d104p65s24d105d105p2
1s22s22p63s23p64s23d104p65s25d105p2
Page 8
33. Which of the following processes represents the ionization energy of bromine?
A)
B)
C)
D)
E)
Br(g)
Br2(g)
Br(s)
Br(l)
Br(s)
Br+(g) + e–
Br2+(g) + e–
Br+(s) + e–
Br+(g) + e–
Br+(g) + e–
34. Which of the following groups contains no ionic compound(s)?
A)
B)
C)
D)
E)
CH2O, CO2, NH3
HCN, NO2, Ca(NO3)2
PCl5, LiBr, Zn(OH)2
NaCl, CCl4, SF4
NaH, CaBr2, NaNH2
35. Which one of the following statements is not correct for the SF4 molecule?
A)
B)
C)
D)
E)
The molecule has sp3 hybridization.
It has a see-saw structure.
It has a total 13 lone pairs.
The molecule contains a net dipole moment
The S-F bonds are polar
36. What are the approximate O S O bond angles in SO32–?
A)
B)
C)
D)
E)
109.5
90 and 180
180
120
90
Page 9
37. Which of the following species will have expanded octet? (Note: The first atom is the
central atom)
i. TeBr4 ii. ICl2 iii. XeF4
A)
B)
C)
D)
E)
All of them
i and ii only
i and iii only
ii and iii only
none of them
2
38. For which of the following molecules and or ions does the central atom have sp hybridization?
(The central atom is underlined in each formula below; for I3 one of the I is in centre)
A)
B)
C)
D)
E)
NOBr
SO42–
SBr2
I3CO2
39. Which of the following statements are correct for the molecular orbital theory?
i. Hund's rule is obeyed.
ii. electrons are assigned to orbitals of successively higher energy.
iii. a bonding molecular orbital is lower in energy than its parent atomic orbitals.
iv combination of two atomic orbitals creates one molecular orbital.
A)
B)
C)
D)
E)
i, ii and iii only
i, ii and iv only
i and iv only
ii, iii and iv only
all of them
40. Consider the molecules B2, C2, N2 and F2. Which two molecules have the same bond
order?
A)
B)
C)
D)
E)
B2 and F2
C2 and N2
N2 and F2
C2 and F2
B2 and C2
Page 10
Answer Key
1.
2.
3.
4.
5.
6.
7.
8.
9.
10.
11.
12.
13.
14.
15.
16.
17.
18.
19.
20.
21.
22.
23.
24.
25.
26.
27.
28.
29.
30.
31.
32.
33.
34.
35.
36.
37.
38.
39.
40.
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
A
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