Chem 101 Fall 2012 Practice Final Exam
1. Water has a density of 1.0 g/mL. Will object I float in water?
Object I: mass = 80.0 g; volume = 60.8 mL
A) Yes
B) No
C) Not enough information to tell
2. Carbon dioxide is an example of
A) a homogeneous mixture
B) a heterogeneous mixture
C) a compound or molecule
D) an element
3. Which is the weakest force? dipole-dipole, London dispersion, covalent bonding, or
hydrogen bonding
A) dipole-dipole
B) London dispersion
C) hydrogen bonding
D) covalent bonding
4. When the following equation is balanced using the smallest possible integers, what is
the number in front of the underlined substance?
FeCl2(aq) + Ag3PO4(aq) Fe3(PO4)2(aq) + AgCl(s)
A) 1
B) 3
C) 4
D) 6
E) 12
5. Calculate the mass of carbon dioxide produced from 39.4 g of octane, C8H18, in the
following reaction.
2C8H18 (g) 25O2 (g)
A)
B)
C)
D)
E)
16CO2 (g) 18H2O(g)
60.7 g CO2
121 g CO2
68.3 g CO2
0.949 g CO2
1.380 g CO2
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6. A 1.6-mol sample of KClO3 was decomposed according to the equation
2KClO3 (s)
2KCl(s) 3O2 (g)
How many moles of KCl are formed assuming 100% yield?
A) 1.1 mol
B) 1.3 mol
C) 1.6 mol
D) 0.8 mol
E) 2.4 mol
7. What is the percent (by mass) of carbon in CH2O?
A) 40.0 %
B) 6.67 %
C) 25.0 %
D) 47.9 %
8. The reaction AgNO3(aq) + KCl(aq)
reaction.
A) double-displacement
B) acid-base
C) oxidation-reduction
D) single-displacement
AgCl(s) + KNO3(aq) is a(n) ______________
9. The correct formula for sodium carbonate is
A) Na2CO3
B) NaCO3
C) Na3CO3
D) Na2(CO3)3
E) Na4C
10. How many moles of Ar atoms are in 162.2 g Ar?
A) 6.022 x 1023 mol
B) 4.060 mol
C) 9.768 1025 mol
D) 162.2 mol
E) 9.011 mol
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11. Classify the following reaction:
Zn(s) + 2HCl(aq) H2(g) + ZnCl2(aq)
A) combination or synthesis
B) precipitation
C) decomposition
D) single displacement
E) double displacement
12. (Limiting Reactant Problem) Reacting 1.10 mol nitrogen gas with 3.58 mol of hydrogen
gas will produce how many moles of ammonia (NH3) according to the following
balanced chemical equation?
N2 (g) 3H2 (g)
A)
B)
C)
D)
E)
2NH3 (g)
3.58 mol NH3
2.20 mol NH3
2.39 mol NH3
7.16 mol NH3
6.00 mol NH3
13. How many neutrons are there in one atom of
A) 22
B) 26
C) 44
D) 66
44
22
Ti?
14. How many total electrons are present in a sodium, Na, atom?
A) 9
B) 10
C) 11
D) 18
E) 19
15. The electron configuration for the phosphorus atom is
A) 1s22s22p63s23p2
B) 1s22s22p63s23p3
C) 1s22s22p63s5
D) 1s22s22p63s23p5
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16. Which element has 8 valence electrons?
A) Calcium, Ca
B) Magnesium, Mg
C) Krypton, Kr
D) Oxygen, O
17. Which of the following atoms has the largest atomic radius?
A) Na
B) Mg
C) Si
D) P
E) Al
18. Non-metal atoms tend to ______________ electrons and form ______________ ions.
A) lose; positive
B) lose; negative
C) gain; negative
D) gain; positive
E) share; neutral
19. Chemical bonds formed by the attraction of oppositely charged ions are called
A) covalent bonds
B) magnetic bonds
C) coordinate bonds
D) ionic bonds
20. What is the correct formula for the product of the reaction B + O2?
A) BO
B) BO2
C) BO3
D) B3O2
E) B2O3
21. Which element or ion listed below has the electron configuration 1s22s22p6 ?
A) Na+
B) Mg2+
C) FD) Ne
E) all of these
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22. Equal masses of nitrogen gas and oxygen gas are reacted to form NO2. Which
substance is the limiting reactant?
A) Neither gas is limiting.
B) Oxygen gas (O2)
C) Nitrogen gas (N2)
23. Which of the following compounds contains one or more covalent bonds?
A) NaCl
B) CaO
C) SO2
D) K2O
E) BaBr2
24. 2.00 moles of carbon dioxide has a mass of
A) 9.34 g
B) 14.7 g
C) 88.0 g
D) 132 g
E) 264 g
25. When the equation Si(s) + HF(aq)
for HF?
A) 0
B) 1
C) 2
D) 3
E) 4
SiF4(g) + H2(g) is balanced, what is the coefficient
26. The correct name for an aqueous solution of HF is
A) fluoric acid
B) hydrofluoric acid
C) hydrogen fluoride
D) hydrogen monofluoride
E) perfluoric acid
27. Based on the solubility rules AgNO3 is
A) soluble
B) insoluble
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28. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of
lead(II) nitrate.
The net ionic equation would contain which of the following species? (With correct
coefficient from balanced equation.)
A) K (aq)
B) SO24 (aq)
C) 2NO3 (aq)
D) 2Pb2 (aq)
E) NO3 (aq)
29. The empirical formula for sugar is CH2O. Its molar mass is 90 g/mol. The molecular
formula is
A) CH2O
B) C2H4O2
C) C3H6O3
D) C6H12O6
30. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of
lead(II) nitrate.
Which species would be a spectator ion in this reaction? (With correct coefficient from
balanced equation.)
A) PbSO4 (s)
B) SO24 (aq)
C) 2NO3 (aq)
D) Pb2 (aq)
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31. The pressure in a weather balloon is 1.00 atm at 25.0°C. What is the pressure at 30.0°C?
A) 1.00 atm
B) 1.02 atm
C) 1.20 atm
D) 0.833 atm
E) 0.983 atm
32. A sample of helium gas occupies 11.9 L at 23.0°C and 0.956 atm. What volume will it
occupy at 20.0°C and 0.956 atm?
A) 20.7 L
B) 0.0795 L
C) 11.8 L
D) 12.6 L
33. The air in the inner tube of the tire of a racing bike has a pressure of 15.24 psi. Convert
this pressure to atm.
A) 0.1382 atm
B) 7.143 atm
C) 1544 atm
D) 1.037 atm
E) 105.0 atm
34. How many protons are in the nucleus of a Mn atom?
A) 54.938
B) 24
C) 25
D) 30
E) variable
35. A 2.0 L piston containing nitrogen gas had a pressure of 3.3 atm. When the piston was
compressed to 1.50 L, what was the pressure?
A) 2.0 atm
B) 2.5 atm
C) 3.3 atm
D) 4.4 atm
E) 6.6 atm
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36. Classify the following reaction:
2Mg(s) + O2(g)
2MgO(s)
A) combination or synthesis
B) precipitation
C) decomposition
D) single displacement
E) double displacement
37. How many atoms of carbon are present in 3728.2 g of carbon? Select the closest answer.
A) 310.40 atoms
B) 5.6019 1025 atoms
C) 6.0221 1023 atoms
D) 1.8692 1026 atoms
38. When an electron in an excited state returns to its ground state in the atom
A) Energy is absorbed
B) The electron becomes a spectator electron
C) The wavelength changes from red to blue
D) A photon of light is released
E) The atom changes phase from gas to solid
39. What type of bonding occurs when a nonmetal reacts with a nonmetal?
A) Ionic bonding
B) Covalent bonding
40. The compound MgF2 is named
A) magnesium difluoride
B) magnesium II fluoride
C) monomagnesium difluoride
D) magnesium fluoride
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Answer Key Chem 101 Fall 2012 Practice Final Exam
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