BirZeit University
Chemistry Department
Chem 141 Equivalent Exam
2014/2015
Student Name:________________________
Student No:___________________________
Application No:_______________________
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Chem 141 Equivalent Exam
2014/2015
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Please read each question carefully before you answer and choose the correct answer:
1. Which of the following is an example of a physical property?
A) corrosiveness of sulfuric acid
B) toxicity of cyanide
C) flammability of gasoline
D) neutralization of stomach acid with an antacid
E) lead becomes a liquid when heated to 601oC
2. Which of the following represents the largest mass?
A) 2.0  102 mg
D) 2.0  102 cg
B) 0.0010 kg
E) 10.0 dg
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C) 1.0  10 ng
3. Lead melts at 601.0oC. What temperature is this in oF?
A) 302 F
B) 365 F
C) 1,050 F
D) 1,082 F
E) 1,114 F
4. How many significant figures does the result of the following operation contain?
8.52010  7.9
A) 2
B) 3
C) 4
D) 5
E) 6
5. Rutherford's experiment with alpha particle scattering by gold foil established that
A) protons are not evenly distributed throughout an atom.
B) electrons have a negative charge.
C) electrons have a positive charge.
D) atoms are made of protons, neutrons, and electrons.
E) protons are 1840 times heavier than electrons.
6. An oxide ion, O2–, has:
A) 8 protons and 10 electrons
B) 10 protons and 8 electrons
C) 8 protons and 9 electrons
D)
E)
8 protons and 7 electrons
10 protons and 7 electrons
7. Name the binary compound formed between barium and phosphorus.
A) barium phosphorus
D) barium diphosphate
B) barium phosphide
E) barium triphosphide
C) barium phosphate
8. Which is the correct formula for copper(II) phosphate?
A) Cu2PO4
B) Cu3(PO4)2
D) Cu(PO4)2
E) Cu(PO3)2
3
C) Cu2PO3
9.The chemical name for ClO2– is chlorite ion. Therefore, the name of HClO2 is
A) hydrochloric acid
D) chlorous acid
B) chloroform
E) chloric acid
C) hydrogen dioxychloride
10.Which of the following elements is chemically similar to magnesium?
A) sulfur B) calcium C) iron D) nickel E) potassium
11.What is the average mass, in grams, of one potassium atom?
A) 5.14  10–23 g
D) 31.0 g
–23
B) 6.49  10 g
E) 39.1 g
–18
C) 6.02  10 g
12. The mass of 1.21 × 1020 atoms of sulfur is
A) 3.88  1021 g. B) 2.00 mg. C) 32.06 g. D) 6.44 mg.
13. How many atoms are in 5.54 g of F2?
A) 6.02  1023 atoms
B) 0.146 atoms
C) 0.292 atoms
D)
E)
E) 2.00  10–4 g.
8.78  1022 atoms
1.76  1023 atoms
14. What is the coefficient of H2O when the following equation is properly balanced with
smallest set of whole numbers?
---- Al4C3 + --- H2O  --- Al(OH)3 + --- CH4
A) 3
B) 4
C) 6
D) 12
E) 24
15. Vanadium(V) oxide reacts with calcium according to the chemical equation below.
When 10.0 mol of V2O5 are mixed with 10.0 mol of Ca, which is the limiting reagent?
V2O5(s) + 5Ca(l)  2V(l) + 5CaO(s)
A) V2O5
B) Ca
C) V
D) CaO
E) No reagent is limiting.
16. Calculate the mass of FeS formed when 9.42 g of iron reacts with 8.50 g of sulfur
according to the following reaction.
Fe(s) + S(s)  FeS(s)
A) 17.9 g
B) 87.9 g
C) 26.0 g
D) 14.8 g E) 1.91  10–3 g
17. In the reaction
4NH3(g) + 5O2(g)  4NO(g) + 6H2O(g).
If the reaction of 150. g of ammonia with 150. g of oxygen gas yields 87. g of nitric oxide
(NO), what is the percent yield of this reaction?
A) 100%
B) 49%
C) 77%
D) 33%
E) 62%
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18.Which of the following compounds is a nonelectrolyte?
A) NaF
D) NaOH
B) HNO3
E) C6H12O6 (glucose)
C) CH3COOH (acetic acid)
19. Based on the solubility rules, which one of the following compounds should be insoluble
in water?
A) NaCl
B) MgBr2
C) FeCl2
D) AgBr
E) ZnCl2
20.What is the chemical formula of the salt produced by the complete neutralization of
sodium hydroxide with sulfuric acid?
A) Na2SO4 B) Na2(SO4)3 C) Na(SO4)2 D) NaSO3
E) Na3SO4
21.The oxidation number of N in NaNO3 is
A) +6
B) +5
C) +3
D) –3
E) None of the above.
22.In the following chemical reaction the oxidizing agent is
5S + 6KNO3 + 2CaCO3  3K2SO4 + 2CaSO4 + CO2 + 3N2
A) S
B) N2
C) KNO3
D) CaSO4
E) CaCO3
23.Which of the following represents an acid-base neutralization reaction?
A) 2Al(s) + 3H2SO4(aq)  Al2(SO4)3(aq) + 3H2(g)
B) SO2(g) + H2O(l)  H2SO3(g)
C) LiOH(aq) + HNO3(aq)  LiNO3(aq) + H2O(l)
D) 2KBr(aq) + Cl2(g)  2KCl(aq) + Br2(l)
E) CaBr2(aq) + H2SO4(aq)  CaSO4(s) + 2HBr(g)
24. A 20.00 mL sample of 0.1015 M nitric acid is introduced into a flask, and water is
added until the volume of the solution reaches 250. mL. What is the concentration of
nitric acid in the final solution?
A) 1.27 M
D) 3.25  10–2 M
B) 8.12  10–3 M
E) 5.08  10–4 M
C) 0.406 M
25.
25.0 mL of a 0.2450 M NH4Cl solution is added to 55.5 mL of 0.1655 M FeCl3. What
is the concentration of chloride ion in the final solution?
A) 0.607 M
B) 0.418 M
C) 1.35 M
D) 0.190 M
E) 0.276 M
26. A sample of nitrogen gas has a volume of 32.4 L at 20 °C. The gas is heated to 220 ºC at
constant pressure. What is the final volume of nitrogen?
A) 2.94 L
B) 19.3 L
C) 31.4 L
D) 54.5 L
E) 356 L
27. Which of these gases will have the greatest density at the same specified temperature
and pressure?
A) H2
B) CClF3
C) CO2
D) C2H6
E) CF4
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28.A 1.07 g sample of a Noble gas occupies a volume of 363 mL at 35 °C and 678 mmHg.
Identify the Noble gas in this sample? (R = 0.08206 Latm/Kmol)
A) He
B) Ne
C) Ar
D) Kr
E) Xe
29.1.000 atm of dry nitrogen, placed in a container having a pinhole opening in its side,
leaks from the container 3.55 times faster than does 1.000 atm of an unknown gas
placed in this same apparatus. Which of these species could be the unknown gas?
A) NH3
B) C4H10
C) SF6
D) UF6
E) Rn
30.Which one of the following sets of quantum numbers is not possible?
31.Which ground-state atom has an electron configuration described by the following
orbital diagram?
A) phosphorus
B) germanium C) selenium D) tellurium
E) none of these
32.Which element has the following ground-state electron configuration?
[Kr]5s24d105p3
A) Sn
B) Sb
C) Pb
D) Bi
E) Te
33.A ground-state atom of manganese has ___ unpaired electrons and is _____.
A) 0, diamagnetic
D) 5, paramagnetic
B) 2, diamagnetic
E) 7, paramagnetic
C) 3, paramagnetic
34.The general electron configuration for atoms of all elements in Group 5A is
A) ns2np6 B) ns2np5 C) ns2np4 D) ns2np3 E) ns2np1
35. Comparing the energies of the following intermolecular forces on a kJ/mol basis, which
would normally have the highest energy (i.e., be the strongest force)?
A) ion-induced dipole
D) dipole-dipole
B) dipole-induced dipole
E) dispersion
C)
ion-dipole
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36.Consider the species O2–, O2, and O2+. Which of these species will be paramagnetic?
A) O2 and O2–
D) only O2
+
B) O2 and O2
E) all three are paramagnetic
C) O2+ and O2–
37.Which of the atoms listed below has the smallest radius?
A) Al
B) P
C) As
D) Te
E) Na
38. Based on the phase diagram shown below, how will the melting point of the substance
change if the pressure is increased above 1 atm?
A)
B)
C)
D)
The melting point will decrease.
The melting point will remain the same.
The melting point will increase.
The substance will not melt at pressures of 1 atm and above; instead, the solid
sublimes to form the gas phase.
39.A system that does no work but which transfers heat to the surroundings has
A) q < 0, E > 0
D) q > 0, E < 0
B) q < 0, E < 0
E) q < 0, E = 0
C) q > 0, E > 0
40.Arrange the following ions in order of decreasing ionic radius: Al3+, Mg2+, Na+, O2–.
decreasing radius 
A) Al3+ > Mg2+ > O2– > Na+
D) O2– > Al3+ > Mg2+ > Na+
3+
2+
+
2–
B) Al > Mg > Na > O
E) O2– > Na+ > Mg2+ > Al3+
C) Na+ > Mg2+ > Al3+ > O2–
Avogadro’s number = 6.022×1023
R = 0.0821 atm L/mol K
R = 8.314 J/mol K
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Chem 141 Equivalent Exam
2014/2015
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