CHEM 101 WINTER 09-10 FINAL EXAM
On the answer sheet (Scantron) write you name, student ID number, and recitation section
number. Choose the best (most correct) answer for each question and enter it on your answer
sheet.
Avogadro’s Number: 6.022 × 1023 mol-1
P1V1 / n1T1 = P2V2 / n2T2
Speed of Light: c = 3.00 x 108 m s-1
PV = nRT
Planck’s Constant: h = 6.626 x 10-34 J s
d = PM / RT
Rydberg Constant: R = 2.179 x 10-18 J
R = 0.0821 L atm mol-1 K-1
E = hc/λ = hυ
1 atm = 760 Torr = 760 mm Hg
Specific Heat of Water = 4.184 J g-1 °C-1
q = mcΔT
h1d1 = h2d2
C1V1 = C2V2
1. Please chose the letter “a” as your answer for this question.
2. Which of the following represents either a chemical property or a change in a chemical property?
a. Br2 (l) → Br2 (g)
b. Gold is both very malleable and very ductile.
c. High purity water has a resistance ≥ 18.2 MΩ·cm
d. A metal more easily conducts electricty at a low temperature.
e. 2 H2O (l) → 2 Η2 (g) + Ο2 (g)
3. Which of the following compounds can be dissolved in water to give a solution that conducts electricity?
a. C8H18 (2,2,4,-trimethylpentane)
b. C6H12O6 (glucose)
c. CHCl3 (chloroform)
d. KClO4 (potassium perchlorate)
e. (CH3)2CHOH (isopropyl alcohol)
4. Which of the following is not a metal?
a. cobalt (Co, atomic number 27)
b. indium (In, atomic number 49)
c. selenium (Se, atomic number 34)
d. lithium (Li, atomic number 3)
e. beryllium (Be, atomic number 4)
1 5. When neutral atoms gain one or more electrons, ____ are formed.
a. hadrions
b. cations
c. fermions
d. deuterions
e. anions
6. Which two of the following represent a pair of isotopes?
P
P
P
S
I.
II.
III.
IV.
a.
b.
c.
d.
e.
S
V.
I and IV
III and IV
I and III
I and II
II and V
7. Which of the following consists of a pair of allotropes?
a. air and oxygen
b. phosgene, O=C–(Cl)2 and phosphine, PH3
c. red phosphorus and white phosphorus
d. carbon tetrachloride and carbon tetrabromide
e. yellow sulfur and yellow phosphorus
8. An element that has 24 protons, 24 electrons, and 28 neutrons has a molar mass of ______.
a. 76 amu.
b. 56 amu.
c. 52 amu.
d. 48 amu.
e. 84 amu.
9. Three elements that are likely to have similar chemical and physical properties are:
a. Ca, Co, Cr
b. H, He, Ne
c. Pb, Bi, Po
d. B, C, Si
e. Na, K, Li
10. Which formula and name combination is incorrect?
a. SF6 and sulfur hexafluoride
b. N2O3 and dinitrogen tetraoxide
c. P4O10 and tetraphosphorus decaoxide
d. AsBr5 and arsenic pentabromide
e. SeF4 and selenium tetrafluoride
2 11. What is the correct general formula for a straight-chain alkene?
a. CnH2n+2
b. CnHn+2
c. CnHn
d. CnH2n−2
e. CnH2n
12. Determince the correct combination of protons and electrons for the phosphide ion, P3–.
a. 18 protons and 10 electrons
b. 16 protons and 12 electrons
c. 15 protons and 18 electrons
d. 15 protons and 12 electrons
e. 12 protons and 24 electrons
13. Determine the number of moles of water in a liter of water (density = 1000. g / L), and the Molarity of
water, respectively
a. 56 and 74
b. 18 and 56
c. 18 and 18
d. 18 and 74
e. 56 and 56
14. Which statement regarding the complete combustion of a hydrocarbon is incorrect?
a. The hydrocarbon is consumed in the reaction and must be shown in the balanced chemical
equation.
b. Heat is produced in the reaction but does not need to be shown in the balanced chemical
equation.
c. Balancing the chemical equation requires knowledge of the physical state of each reactant
and each product.
d. Oxygen is the oxidizing agent and must be shown in the balanced chemical equation.
e. Carbon dioxide and water are produced in the reaction and must be shown in the balanced
chemical equation.
15. Assuming an excess of aluminum, how many moles of aluminum tribromide can be produced from 111
moles of bromine?
2 Al + 3 Br2
2 AlBr3
a. 167
b. 56
c. 111
d. 148
e. 74
16. Classify the following reaction.
Ni(ClO4)2 (aq) + K2S (aq)
a. decomposition
b. exchange
c. combustion
d. displacement
e. combination
2 KClO4 (aq) + NiS (s)
3 17. The Roman numerals in the reaction given represent the coefficients in the balanced chemical equation.
What are the values of the coefficients?
I Al (s) + II CuSO4 (aq)
III Al2(SO4)3 (aq) + IV Cu (s)
a.
b.
c.
d.
e.
I
3
2
2
1
2
II
1
1
1
3
3
III
1
3
1
3
1
IV
3
2
2
1
3
18. What is the net ionic equation for the the following reaction?
3 Ca(NO3)2 (aq) + 2 H3PO4 (aq)
Ca3(PO4)2 (s) + 6 HNO3 (aq)
a.
b.
c.
d.
e.
N+ + NO3−
NNO3
P2+ + 2NO3−
P(NO3)2
3 Ca2+ (aq) + 2 PO43− (aq)
Ca3(PO4)2 (s)
−
+
2 H + NO6
2 HNO3
2 H3PO4 (aq)
6 HNO3 (aq)
19. Which of the following would be expected to be present in a 1. M aqueous solution of perchloric acid,
HClO4 ?
a. Cl−
b. PO43–
c. HCl
d. H−
e. H3O+
20. What is the reducing agent in the reaction below?
MnO4– (aq) + 8 H+ (aq) + 5 e–
Mn2+ (aq) + 4 H2O
+
a. H
b. e–
c. Mn2+
d. H2O
e. MnO4–
21. Using high purity water, to what final volume would 100.0 mL of a 1.00 x 107 ppb (parts per billion)
solution of arsenic need to be diluted to be useable as a Federal drinking water testing standard at an
arsenic concentration of 10.00 ppb?
a. 1.00 x 108 mL
b. 50.00 mL
c. 18,000 mL
d. 22,400 mL
e. 1.00 x 105 mL
4 22. Determine the specific heat of uranium (atomic number 92, molar heat capacity = 28.56 J mol−1 °C−1).
a. 6797 J g−1 °C−1
b. 2799 J g−1 °C−1
c. 2628 J g−1 °C−1
d. 0.31 J g−1 °C−1
e. 0.12 J g−1 °C−1
23. What is the enthalpy change if 28 moles of carbon dioxide are formed by the following reaction?
C4H10(g) + 13/2 O2(g)
4 CO2(g) + 5 H2O(g)
H° = −1895 kJ
a. −7580 kJ
b. −28,000 kJ
c. −13,265 kJ
d. −68000 kJ
e. −190 kJ
24. A chemical reaction is exothermic when
a. the strength of bonds broken is greater than the strength of bonds formed.
b. weak bonds are broken and stronger bonds are formed
c. no bonds are formed.
d. strong bonds are broken and weaker bonds are formed.
e. the strengths of all bonds broken and formed are the same.
25. Calculate the standard enthalpy change, H°, for the following reaction
PbCl4 (l)
Pb(Cl)2 (s) + Cl2 (g)
using the information given below:
Pb (s) + Cl2 (g)
PbCl2 (s)
H° = -359.4 kJ
Pb (s) + 2 Cl2 (g)
a.
b.
c.
d.
e.
PbCl4 (l)
H° = -329.3 kJ
+ 398.4 kJ
−30.1 kJ
+30.1 kJ
−131.1 kJ
+ 131.1kJ
26. The standard enthalpies of formation for several substances are given below:
CO (g)
CO2 (g)
−110.5 kJ/mol
−393.5 kJ/mol
H2O (l)
H2O (g)
−241.8 kJ/mol
−285.8 kJ/mol
CH
OH
(g)
H2O2(l)
−187.8 kJ/mol
−200.7 kJ/mol
3
C3H8 (g)
CH3OH (l)
−103.8 kJ/mol
−238.7 kJ/mol
Determine the H° for the reverse of the reaction shown below.
C3H8 (g) + 5 O2 (g)
3 CO2 (g) + 4 H2O (l)
a. −2220 kJ
b. +2220 kJ
c. −782. kJ
d. +575 kJ
e. −575 kJ
5 27. A 10.0 mole sample of CH4 reacts completely with excess oxygen in a calorimeter having a heat capacity
of 3915 J/°C. The calorimeter contains 1270 g of water. Determine the total amount of energy produced
by the combustion.
CH4(g) + 2 O2(g)
2 H2O(g) + CO2(g)
H° = −802.3 kJ
a.
b.
c.
d.
e.
4.35 kJ
127 kJ
8023 kJ
392 kJ
8.02 kJ
28. Light has a wavelength of 280 nm. What is its frequency?
a. 1.07 × 1015 Hz
b. 1.48 × 10−6 Hz
c. 6.76 × 10−4 Hz
d. 1.48 × 102 Hz
e. 5.64 × 1014 Hz
29. Determine the energy of a photon that has a wavelength of 280 nm.
a. 1.16 × 10−27 J
b. 1.04 × 10−10 J
c. 7.09 × 10−19 J
d. 1.27 × 10−48 J
e. 7.87 × 1047 J
30. Which values for the fourth (spin) quantum number are allowed for n = 1?
a. ms = + −
b. ms = 0, 1, 2
c. ms = −1, 0, +1
d. ms = 0, 1, 2, 3, 4
e. ms = 0, 1, 2, 3
31. How many orbitals and electrons, respectively, can be contained in each p subshell?
a. 3
6
b. 20 10
c. 10 20
d. 14 7
e. 5 10
32. Which of the following corresponds to the electron configuration of a noble gas?
a. 1s22s22p63s23p5
b. 1s22s2
c. 1s22s22p63s23p63d104s24p3
d. 1s22s22p63s23p6
e. 1s22s22p4
6 33. Atoms and ions that have identical electron configurations are referred to as being
a. isoelectronic.
b. isopiestronic.
c. ferromagnetic.
d. diamagnetic.
e. paratronic.
34. How many electrons will be in the correctly drawn Lewis Structure for the acetate anion, CH3COO– ?
a. 22
b. 23
c. 17
d. 24
e. 20
35. Assume that all of the following are straight-chain hydrocarbons. Which compound will contain a triple
bond?
a. C2H6
b. C8H16
c. C13H28
d. C9H16
e. C6H14
36. In straight-chain organic molecules, cis-trans isomerism is a possibility only if the molecule contains at
least one
a. carbon-carbon single bond
b. carbon-oxygen single bond
c. carbon-carbon double bond
d. carbon-oxygen double bond
e. carbon-carbon triple bond
37. Of the elements shown, which is the most electronegative?
a. calcium, Ca, atomic no. 20
b. nitrogen, N, atomic no. 7
c. gallium, Ga, atomic no. 31
d. selenium, Se, atomic no. 34
e. strontium, Sr, atomic no. 38
38. Which properly shows the formal charges on the atoms in phosgene, O=C–(Cl)2 ?
a. +1 on oxygen, −3 on carbon, +1 on chlorine
b. −1 on oxygen, +4 on carbon, −4 on chlorine
c. 0 on oxygen, 0 on carbon, 0 on chlorine
d. −1 on oxygen, +1 on carbon, −2 on chlorine
e. −2 on oxygen, +4 on carbon, −1 on chlorine
7 39. Construct correct Lewis dot structures for the three molecules below. Which compound(s) exceed(s) the
octet rule?
CF4
SeF4
SiF4
I
II
III
a.
b.
c.
d.
e.
III
II and III
I, II, and II
II
I
40. VSEPR Theory attempts to ____ electron-pair ____.
a. minimize, repulsions
b. eliminate, attractions
c. minimize, collisions
d. maximize, attractions
e. maximize, repulsions
41. Assuming that there are no lone pairs of electrons on the central atom, using VSEPR Theory predict the
molecular geometry consistent with one, three, and five bonded electron pairs, respectively.
a. linear, trigonal planar, trigonal bipyramidal
b. tetrahedral, trigonal bipyramidal, octahedral
c. linear, tetrahedral, hexagonal
d. angular, trigonal pyramidal,octahedral
e. linear, trigonal pyramidal, pentahedral
42. Draw the Lewis dot structure for trimethylamine, N(CH3)3 , and then use VSEPR Theory to predict the
electron-pair geometry, the molecular geometry, and to estimate the C-N-C bond angle, respectively.
a. tetrahedral, trigonal pyramidal, 109.5°
b. tetrahedral, tetrahedral, 109.5°
c. tetrahedral, trigonal square planar, 109.5°
d. square planar, square planar, 90°
e. trigonal bipyramidal, tetrahedral, 90°
43. Which of the following molecules is/are non-polar?
I.
SiH3F
II.
SiHF3
III.
SiH2F2
IV.
SiF4
a.
b.
c.
d.
e.
I and II
I, II, and III
II, III, and IV
IV only
II only
8 44. What is the major type of force that must be overcome to allow each of the processes below, in the order I
to IV?
I.
the evaporation of liquid CH3CH2OH
II.
the vaporization of liquid CHCl3
III.
the sublimation of solid I2
IV.
the boiling of liquid C5H12
a.
b.
c.
d.
hydrogen bonding, dipole-dipole, London (dispersion) forces, London (dispersion) forces
hydrogen bonding, London (dispersion) forces, dipole-dipole, dipole-dipole
London (dispersion) forces, covalent bonding, dipole-dipole, dipole-dipole
London (dispersion) forces, London (dispersion) forces, London (dispersion) forces,
London (dispersion) forces
e. dipole-dipole, dipole-dipole, London (dispersion) forces, London (dispersion) forces
45. Determine the height (in mm) of a column of toluene in a barometer at a pressure of 790 mm Hg. The
densities of mercury and toluene are 13.546 and 0.865 g/cm3, respectively.
a. 1.75 × 102
b. 4.34
c. 1.24 × 104
d. 0.00571
e. 50.45
46. Assuming ideal gas behavior, calculate the number of moles of phosphine gas, PH3 , that occupy 8.2 L at
STP.
a. 3.30 × 102
b. 3.10
c. 0.37
d. 2.40 × 104
e. 0.125
47. Assuming ideal gas behavior, what is the density (in g/L) of arsine gas, AsH3 , at 60°C and 0.25 atm of
pressure?
a. 9.9
b. 0.71
c. 1.87 × 10–4
d. 4.9 × 10−2
e. 1.2
48. A mixture of He and O2 exerts a total pressure of 2.24 atm. The partial pressure of oxygen is 1.40 atm.
What is the mole fraction of helium?
a.
b.
c.
d.
e.
0.38
0.20
0.63
0.44
0.09
9 49. Under what conditions do real gases most closely approximate the behavior of ideal gases?
a. low pressure and high temperature
b. high pressure and low temperature
c. all real gases behave like ideal gases at all temperatures and pressures
d. high pressure and high temperature
e. low pressure and low temperature
50. Which of the following is the correct sequence for the three principle types of reactions which make up a
free-radical process?
a. substitution, elimination, termination
b. initiation, propagation, termination
c. initiation, elimination, termination
d. elimination, termination, substitution
e. initiation, substitution, termination
51. Which of the following greenhouse gases is considered to be the principal global warming gas
generated by the combustion of fossil fuels in electric power plants and internal combustion engines?
a. water vapor
b. carbon dioxide
c. ozone
d. methane
e. all of the above
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