Chem 101 Exam 3 Fall 2012 Section 001
1. Based on the solubility rules Mg3(PO4)2 is
A) soluble
B) insoluble
2. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of
lead(II) nitrate.
What is one of the spectator ions (with correct coefficient)?
A) SO24 (aq)
B) Pb(NO3 )(aq)
C) 3Pb2 (aq)
D) 2NO3 (aq)
E) Pb2 (aq)
3. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of
lead(II) nitrate.
The complete ionic equation contains which of the following species (with correct
coefficient)?
A) 2SO24 (aq)
B) 2K (aq)
C) 3Pb2 (aq)
D) NO3 (aq)
E) P (aq)
4. Based on the solubility rules KOH is
A) soluble
B) insoluble
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5. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of
lead(II) nitrate.
The net ionic equation contains which of the following species (with correct
coefficient)?
A) 2NH4 (aq)
B) 2SO24 (aq)
C) 2NO3 (aq)
D) Pb2 (aq)
E) NO3 (aq)
6. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of
lead(II) nitrate.
What is the coefficient of the solid in the balanced equation?
A) 1
B) 2
C) 3
D) 4
E) 6
7. When the following equation is balanced in standard form, what is the coefficient in
front of the underlined substance?
C2H6(g) + O2(g) CO2(g) + H2O(l)
A) 1
B) 2
C) 3
D) 4
E) 5
8. An aqueous solution of potassium sulfate is allowed to react with an aqueous solution of
lead(II) nitrate.
Identify the solid in the balanced equation.
A) K2SO4
B) Pb(NO3)2
C) PbSO4
D) KNO3
E) There is no solid formed when the two solutions are mixed.
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9. What is the mass in grams of 33.66 moles of iron?
A) 55.85 g
B) 126.9 g
C) 1880. g
D) 4038 g
10. The reaction HCl(aq) + KOH(aq)
reaction.
A) precipitation
B) acid-base or neutralization
C) combination or synthesis
D) single-replacement
E) none of these
H2O(l) + KCl(aq) is a(n) ______________
11. Based on the solubility rules PbCl2 is
A) soluble
B) insoluble
12. Based on the solubility rules LiNO3 is
A) soluble
B) insoluble
13. What is the molar mass of calcium carbonate, MgCO3?
A) 24.305 g
B) 52.315 g
C) 84.313 g
D) 99.803 g
Use the following to answer questions 14-18:
Use the following choices to classify each reaction given below .
A. single replacement
B. double replacement
C. synthesis
D. decomposition
E. combustion
14. 2HgO(s)
2Hg(l) + O2(g)
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15. 2Na(s) + H2(g)
2NaH(s)
16. C3H8(g) + 5O2(g)
3CO2(g) + 4H2O(g)
17. Zn(s) + 2HCl(aq)
H2(g) + ZnCl2(aq)
18. AgNO3(aq) + NaCl(aq)
AgCl(s) + NaNO3(aq)
19. Tin(II) fluoride is added to some dental products to help prevent cavities. Manufacturers
have to make the tin(II) fluoride first, though, before they can add it to their products.
Sn(s) + 2HF(aq)
SnF2(aq) + H2(g)
How many moles of tin(II) fluoride can be made from 3.70 moles of hydrogen fluoride
if there is plenty of tin available to react?
A) 7.40 moles
B) 1.85 moles
C) 3.70 moles
D) 3.70 x 1023 moles
E) 1.00 moles
20. Which of the following is not an indication that a reaction may be happening?
A) Permanent color change
B) Volume decreases
C) Precipitate forms
D) Gas given off
E) Heat or light given off
21. Considering the activity series Ca, Mg, Zn, Fe, Cu where Ca is the most reactive metal
and Cu is the least reactive metal would the following reaction take place?
Zn(s) + CuSO4(aq) Cu(s) + ZnSO4(aq)
A) yes
B) no
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22. Considering the activity series Ca, Mg, Zn, Fe, Cu where Ca is the most reactive metal
and Cu is the least reactive metal would the following reaction take place?
Cu(s) + MgSO4(aq)
Mg(s) + CuSO4(aq)
A) yes
B) no
23. 4.5 mol of Al and an excess of Br2 are reacted according to the equation
2Al 3Br2
2AlBr3
How many moles of Br2 are consumed in the reaction assuming 100% yield?
A) 1.5 mol
B) 2.3 mol
C) 3.0 mol
D) 4.5 mol
E) 6.8 mol
24. True or false? The equation N2(g) + 3H2(g) 2NH3(g) can be interpreted by saying
that 1 mol of N2 reacts with 3 mol of H2 to form 2 mol of NH3.
A) True
B) False
25. Refer to the following equation:
4NH3(g) + 7O2(g)
4NO2(g) + 6H2O(g)
How many moles of oxygen gas (O2) will be required to produce 15.8 mol of NO2?
A) 9.03 moles
B) 15.8 moles
C) 13.9 moles
D) 27.7 moles
E) 23.7 moles
26. 1.00 moles of hydrogen gas are reacted with oxygen gas to form water. How much
oxygen gas (O2) is used up in the reaction?
A) 0.500 moles
B) 1.00 moles
C) 1.50 moles
D) 2.00 moles
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27. Consider the reaction of magnesium metal with hydrochloric acid to produce
magnesium chloride and hydrogen gas.
Mg + 2HCl → MgCl2 + H2
If 3.72 mol of hydrochloric acid are reacted, how many moles of hydrogen gas are
produced?
A) 1.86 mol
B) 3.72 mol
C) 7.44 mol
D) 5.72 mol
28. The rusting of iron is represented by the equation 4Fe + 3O2
2Fe2O3. If you have a
2.40-mol sample of iron, how many moles of Fe2O3 will there be after the iron has
rusted completely?
A) 0.600 mol
B) 0.900 mol
C) 1.20 mol
D) 1.80 mol
E) 2.70 mol
29. True or false? When solutions of barium hydroxide and potassium sulfate are mixed,
the net ionic equation is Ba2+(aq) + SO42-(aq)
BaSO4(s) because only the species
involved in making the precipitate are included.
A) True
B) False
30. In neutralization reactions water is one of the products.
A) True
B) False
31. Predict the identity of the precipitate that forms when an aqueous solution of lithium
hydroxide reacts with an aqueous solution of copper II chloride.
A) LiCl
B) CuCl
C) Li2OH
D) Cu2OH
E) Cu(OH)2
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32. When a precipitation reaction occurs, the ions that do not form the precipitate
A) evaporate
B) are cations only
C) form a second insoluble compound in the solution
D) are left as ions in the solution
33. A 0.87 mol sample of KClO3 was decomposed according to the equation
2KClO3 (s)
2KCl(s) 3O2 (g)
How many moles of O2 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
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Answer Key
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B
D
B
A
D
A
B
C
C
B
B
A
C
D
C
E
A
B
B
B
A
B
E
A
D
A
A
C
A
A
E
D
B
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