Sample Chapter

 

INSTANT DOWNLOAD COMPLETE TEST BANK WITH ANSWERS

 

Test Bank For Chemistry  The Central Science 10th Edition by Theodore E. Brown, H. Eugene LeMay , Bruce E Bursten

 

 

 

SAMPLE QUESTIONS

 

Exam

 

Name___________________________________

 

 

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

1) The mass % of H in methane (CH4) is __________. 1)
A) 74.87 B) 4.032 C) 25.13 D) 92.26 E) 7.743
Answer: C
Explanation: A)
B)
C)
D)
E)
2) What is the mass % of carbon in dimethylsulfoxide (C2H6SO)? 2)
A) 79.8 B) 60.0 C) 20.6 D) 7.74 E) 30.7
Answer: E
Explanation: A)
B)
C)
D)
E)
3) The formula weight of ammonium sulfate ((NH4)2SO4) is __________ amu. 3)
A) 264 B) 100 C) 132 D) 116 E) 118
Answer: C
Explanation: A)
B)
C)
D)
E)
4) How many grams of sodium carbonate contain 1.773 × 1017 carbon atoms? 4)
A) 3.121 × 105
B) 1.011 × 105
C) 6.066 × 105
D) 1.517 × 105
E) 9.100 × 105
Answer: A
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

1

 

5) When a hydrocarbon burns in air, what component of air reacts? 5)
A) nitrogen
B) water
C) oxygen
D) carbon dioxide
E) argon
Answer: C
Explanation: A)
B)
C)
D)
E)
6) The mass % of Al in aluminum sulfate (Al2(SO4)3) is __________. 6)
A) 45.70 B) 21.93 C) 35.94 D) 7.886 E) 15.77
Answer: E
Explanation: A)
B)
C)
D)
E)
7) Which of the following are decomposition reactions? 7)
1) CH4 (g) + O2 (g)CO2 (g) + H2O (l)
2) CaO (s) + CO2 (g)CaCO3 (s)
3) Mg (s) + O2 (g)MgO (s)
4) PbCO3 (s)PbO (s) + CO2 (g)
A) 1, 2, 3, and 4
B) 4 only
C) 2, 3, and 4
D) 1, 2, and 3
E) 2 and 3
Answer: B
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

2

 

8) Which hydrocarbon pair below have identical mass percentage of C? 8)
  1. A) C2H4 and C4H2
  2. B) C2H4 and C3H4
  3. C) C3H4 and C3H6
  4. D) C2H4 and C3H6

 

  1. E) none of the above

 

Answer: D

Explanation:      A)

B)

C)

D)

E)

 

  • Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 9) 2NaN3 (s) 2Na (s) + 3N2 (g)

 

How many grams of sodium azide are required to produce 18.0 g of nitrogen?
A) 62.7 B) 0.964 C) 0.428 D) 41.8 E) 27.9
Answer: E
Explanation: A)
B)
C)
D)
E)

 

10) Lithium and nitrogen react in a combination reaction to produce lithium nitride: 10)
6Li (s) + N2 (g)    2Li3N (s)
How many moles of N2 are needed to react with 0.500 mol of lithium?
A) 1.50 B) 0.0833 C) 3.00 D) 0.167 E) 0.500
Answer: B
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

3

 

11) How many sulfur dioxide molecules are there in 0.180 mol of sulfur dioxide? 11)
A) 1.08 × 1024
B) 6.02 × 1024
C) 6.02 × 1023
D) 1.80 × 1023
E) 1.08 × 1023

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

12) How many oxygen atoms are there in 52.06 g of carbon dioxide? 12)
A) 1.018 × 1024
B) 1.424 × 1024
C) 6.022 × 1023
D) 5.088 × 1023
E) 1.204 × 1024

Answer: B

Explanation:      A)

B)

C)

D)

E)

 

  • Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements: 13) 2NaN3 (s) 2Na (s) + 3N2 (g)

 

How many moles of N2 are produced by the decomposition of 2.88 mol of sodium azide?

 

A) 4.32 B) 1.92 C) 0.960 D) 1.44 E) 8.64
Answer: A
Explanation: A)
B)
C)
D)
E)
14) Calculate the percentage by mass of nitrogen in PtCl2(NH3)2. 14)
A) 4.67 B) 9.34 C) 4.95 D) 12.67 E) 9.90
Answer: B
Explanation: A)
B)

C)

D)

E)

 

 

 

 

4

 

15) How many oxygen atoms are contained in 2.74 g of Al2(SO4)3? 15)
A) 12
B) 6.02 × 1023
C) 5.79 × 1022
D) 8.01 × 103
E) 7.22 × 1024

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

16) Lithium and nitrogen react in a combination reaction to produce lithium nitride: 16)

 

6Li (s) + N2 (g)      2Li3N (s)

 

How many moles of lithium are needed to produce 0.60 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?

  1. A) 0.20 B) 3.6 C) 1.8                            D) 0.40                           E) 0.30

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

17) Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 17)

 

2Mg (s) + O2 (g)      2MgO (s)

 

How many moles of O2 are consumed when 0.770 mol of magnesium burns?

 

A) 1.54 B) 0.385 C) 2.60 D) 0.770 E) 0.0317
Answer: B
Explanation: A)
B)
C)
D)
E)
18) The formula weight of magnesium fluoride (MgF2) is __________ amu. 18)
A) 92.9 B) 62.3 C) 86.6 D) 67.6 E) 43.3
Answer: B
Explanation: A)
B)
C)
D)
E)

 

 

 

 

5

 

19) The mass % of C in methane (CH4) is __________. 19)
A) 7.743 B) 74.87 C) 92.26 D) 25.13 E) 133.6
Answer: B
Explanation: A)
B)
C)
D)
E)
20) The formula weight of aluminum sulfate (Al2(SO4)3) is __________ amu. 20)
A) 123.04 B) 342.14 C) 273.06 D) 59.04 E) 150.14
Answer: B
Explanation: A)
B)
C)
D)
E)
21) What is the empirical formula of a compound that is 64.8% C, 13.6% H, and 21.6% O by mass? 21)
A) C5HO2 B) C4HO1 C) C8H20O2 D) C5H14O1 E) C4H10O1
Answer: E
Explanation: A)
B)
C)
D)
E)
22) Calculate the percentage by mass of chlorine in PtCl2(NH3)2. 22)
A) 23.63 B) 12.53 C) 25.05 D) 11.82 E) 18.09
Answer: A
Explanation: A)
B)
C)
D)
E)
23) A sulfur oxide is 50.0% by mass sulfur. This molecular formula could be __________. 23)
  1. S2O4
  2. SO2
  3. S2O

 

  1. SO
  2. either SO2 or S2O4

 

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

6

 

24) The formula weight of a substance is __________. 24)
  1. the weight of a sample of the substance
  2. identical to the molar mass
  3. the same as the percent by mass weight
  4. the sum of the atomic weights of each atom in its chemical formula
  5. determined by combustion analysis

 

Answer: D

Explanation:      A)

B)

C)

D)

E)

 

25) A sample of CH4O with a mass of 32.0 g contains __________ molecules of CH4O. 25)
A) 32.0
B) 1.00 × 10-23
C) 5.32
D) 1.88 × 1022
E) 6.02 × 1023
Answer: E
Explanation:    A)
B)
C)
D)
E)
26) The molecular weight of the ethanol (C2H5OH) is __________ amu. 26)
A) 30 B) 92 C) 34 D) 41 E) 46

 

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

27) Magnesium burns in air with a dazzling brilliance to produce magnesium oxide: 27)

 

2Mg (s) + O2 (g)       2MgO (s)

 

When 4.00 g of magnesium burns, the theoretical yield of magnesium oxide is __________ g.

  1. A) 13.3 B) 4.00 C) 3.32                          D) 6.63                           E) 0.165

 

Answer: D

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

7

 

28) Calculate the percentage by mass of hydrogen in PtCl2(NH3)2. 28)
A) 1.008 B) 0.034 C) 2.016 D) 0.672 E) 1.558
Answer: C
Explanation: A)
B)
C)
D)
E)
29) One million argon atoms is __________ mol of argon atoms. 29)
A) 3
B) 1.0 × 106
C) 1.7 × 1018
D) 1.0 × 10+6
E) 6.0 × 1023
Answer: C
Explanation: A)
B)
C)
D)
E)
30) The formula of nitrobenzene is C6H5NO2. The molecular weight of this compound is __________ 30)
amu.
A) 109.10 B) 43.03 C) 123.11 D) 107.11 E) 3.06
Answer: C
Explanation: A)
B)
C)
D)
E)
31) How many atoms of nitrogen are in 10 g of NH4NO3? 31)
A) 2 B) 3.0 × 1023 C) 1.8 D) 3.5 E) 1.5 × 1023
Answer: E
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

8

 

32) Lithium and nitrogen react in a combination reaction to produce lithium nitride: 32)

 

6Li (s) + N2 (g)      2Li3N (s)

 

In a particular experiment, 3.50-g samples of each reagent are reacted. The theoretical yield of lithium nitride is __________ g.

A) 3.52 B) 5.85 C) 8.7 D) 2.93 E) 17.6
Answer: B
Explanation: A)
B)
C)
D)
E)
33) The formula weight of potassium phosphate (K3PO4) is __________ amu. 33)
A) 212.27 B) 86.07 C) 251.37 D) 173.17 E) 196.27
Answer: A
Explanation: A)
B)
C)
D)
E)
34) Of the reactions below, which one is a decomposition reaction? 34)
A) 2CH4 + 4O22CO2 + 4H2O
B) 2Mg + O22MgO
C) Cd(NO3)2 + Na2SCdS + 2NaNO3
D) 2N2 + 3H22NH3
E) NH4ClNH3 + HCl
Answer: E
Explanation: A)
B)
C)
D)
E)
35) Lithium and nitrogen react in a combination reaction to produce lithium nitride: 35)

 

6Li (s) + N2 (g)      2Li3N (s)

 

How many moles of lithium nitride are produced when 0.450 mol of lithium react in this fashion?

A) 1.35 B) 0.0750 C) 0.150 D) 0.225 E) 0.900
Answer: C
Explanation: A)

B)

C)

D)

E)

 

 

 

 

9

 

36) How many sulfur dioxide molecules are there in 1.80 mol of sulfur dioxide? 36)
A) 1.80 × 1024
B) 6.02 × 1024
C) 6.02 × 1023
D) 1.08 × 1023
E) 1.08 × 1024

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

 

  • One mole of
    1. C10H8

 

Answer: A Explanation:

__________ contains the largest number of atoms.                                                                           37)

  1. B) Na3PO4 C) Cl2 D) S8                               E) Al2(SO4)3

 

A)

B)

C)

D)

E)

 

 

38) A nitrogen oxide is 63.65% by mass nitrogen. The molecular formula could be __________. 38)
A) N2O4
B) N2O
C) NO2
D) NO
E) either NO2 or N2O4
Answer: B
Explanation: A)
B)
C)
D)
E)
39) The molecular weight of the acetic acid (CH3CO2H) is __________ amu. 39)
A) 60 B) 48 C) 32 D) 44
Answer: A
Explanation: A)
B)

C)

D)

 

 

 

 

 

 

 

 

 

 

 

10

 

40) The compound responsible for the characteristic smell of garlic is allicin, C6H10OS2. The mass of 40)
1.00 mol of allicin is __________ g.
A) 34 B) 162 C) 61 D) 19 E) 86
Answer: B
Explanation: A)
B)
C)
D)
E)
41) Which of the following are combination reactions? 41)
1) CH4 (g) + O2 (g)CO2 (g) + H2O (l)
2) CaO (s) + CO2 (g)CaCO3 (s)
3) Mg (s) + O2 (g)MgO (s)
4) PbCO3 (s)PbO (s) + CO2 (g)
A) 4 only
B) 1, 2, and 3
C) 2, 3, and 4
D) 2 and 3
E) 1, 2, 3, and 4
Answer: D
Explanation: A)
B)
C)
D)
E)
42) What is the mass in grams of 9.76 × 1012 atoms of naturally occurring sodium? 42)
A) 1.62 × 1011
B) 7.05 × 1013
C) 2.24 × 1014
D) 22.99
E) 3.73 × 1010
Answer: E
Explanation: A)
B)
C)
D)
E)
43) A sample of CH2F2 with a mass of 19 g contains __________ atoms of F. 43)
A) 38 B) 9.5 C) 2.2 × 1023 D) 4.4 × 1023 E) 3.3 × 1024
Answer: D
Explanation: A)
B)
C)
D)
E)

 

 

 

11

 

44) Gaseous argon has a density of 1.40 g/L at standard conditions. How many argon atoms are in 1.00 44)
L of argon gas at standard conditions?
A) 4.7 × 1022
B) 2.1 × 1022
C) 3.4 × 1025
D) 1.5 × 1025
E) 6.02 × 1023
Answer: B
Explanation: A)
B)
C)
D)
E)
45) There are __________ atoms of oxygen are in 300 molecules of CH3CO2H. 45)
A) 600
B) 3.01 × 1024
C) 1.80 × 1026
D) 300
E) 3.61 × 1026
Answer: A
Explanation: A)
B)
C)
D)
E)
46) The molecular formula of aspartame, the generic name of NutraSweet®, is C H 18 N 2 O . The 46)
molar mass of aspartame is __________ g. 14 5
A) 156 B) 24 C) 294 D) 39 E) 43
Answer: C
Explanation: A)
B)
C)
D)
E)
47) The mass % of F in the binary compound KrF2 is __________. 47)
A) 45.38 B) 68.80 C) 18.48 D) 81.52 E) 31.20
Answer: E
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

12

 

48) Of the reactions below, which one is not a combination reaction? 48)
A) 2CH4 + 4O22CO2 + 4H2O
B) CaO + H2OCa(OH)2
C) 2Mg + O22MgO
D) C + O2CO2
E) 2N2 + 3H22NH3
Answer: A
Explanation:    A)
B)
C)
D)
E)
49) Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: 49)
CaO (s) + H2O (l)Ca(OH)2 (s)

 

In a particular experiment, a 5.00-g sample of CaO is reacted with excess water and 6.11 g of Ca(OH)2 is recovered. What is the percent yield in this experiment?

 

A) 7.19 B) 122 C) 81.9 D) 1.22 E) 92.4
Answer: E
Explanation: A)
B)
C)
D)
E)
50) The formula weight of potassium dichromate (K2Cr2O7) is __________ amu. 50)
A) 242.18 B) 107.09 C) 333.08 D) 255.08 E) 294.18
Answer: E
Explanation: A)
B)
C)
D)
E)
51) The formula weight of calcium nitrate (Ca(NO3)2) is __________ amu. 51)
A) 150.1 B) 204.2 C) 102.1 D) 116.1 E) 164.0
Answer: E
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

13

 

52) The total number of atoms in 0.111 mol of Fe(CO)3(PH3)2 is __________. 52)
A) 15
B) 1.67
C) 1.07 × 1024
D) 2.76 × 1024
E) 4.46 × 1021
Answer: C
Explanation: A)
B)
C)
D)
E)
53) How many molecules of CH4 are in 48.2 g of this compound? 53)
A) 5.00 × 1024
B) 4.00
C) 3.00
D) 2.90 × 1025
E) 1.81 × 1024
Answer: E
Explanation: A)
B)
C)
D)
E)
54) The molecular weight of urea ( (NH2)2CO ), a compound used as a nitrogen fertilizer, is 54)
__________ amu.
A) 43.0 B) 8.0 C) 44.0 D) 32.0 E) 60.1
Answer: E
Explanation: A)
B)
C)
D)
E)
55) The reaction used to inflate automobile airbags __________. 55)
  1. is a decomposition reaction
  2. produces sodium gas
  3. violates the law of conservation of mass
  4. is a combination reaction
  5. is a combustion reaction

 

Answer: A

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

14

 

56) How many moles of pyridine (C5H5N) are contained in 3.13 g of pyridine? 56)
A) 0.00404 B) 0.0396 C) 25.3 D) 4.04 × 103 E) 0.319
Answer: B
Explanation: A)
B)
C)
D)
E)
57) Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide: 57)

 

CaO (s) + H2O (l)      Ca(OH)2 (s)

 

A 1.50-g sample of CaO is reacted with 1.45 g of H2O. How many grams of water remains after completion of reaction?

  1. A) 0.00 B) 0.0536 C) 0.966                        D) 1.04                           E) 0.00297

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

58) Which one of the following is not true concerning automotive air bags? 58)

 

  1. The gas used for inflating them is oxygen
  2. A gas is produced when the air bag activates.
  3. They are loaded with sodium azide initially
  4. The two products of the decomposition reaction are sodium and nitrogen
  5. They are inflated as a result of a decomposition reaction

 

Answer: A

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

15

 

59) Which of the following are combustion reactions? 59)
1) CH4 (g) + O2 (g)CO2 (g) + H2O (l)
2) CaO (s) + CO2 (g)CaCO3 (s)
3) PbCO3 (s)PbO (s) + CO2 (g)
4) CH3OH (l) + O2 (g)CO2 (g) + H2O (l)
A) 2, 3, and 4
  1. B) 3 and 4
  2. C) 1 and 4
  3. D) 1, 3, and 4
  4. E) 1, 2, 3, and 4

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

60) Which one of the following substances is the product of this combination reaction? 60)
Al (s) + I2 (s)    __________
A) AlI B) AlI3 C) Al2I3 D) Al3I2 E) AlI2
Answer: B
Explanation: A)
B)
C)
D)
E)
61) How many moles of sodium carbonate contain 1.773 × 1017 carbon atoms? 61)
A) 2.945 × 107
B) 8.836 × 107
C) 5.890 × 107
D) 9.817 × 108
E) 1.473 × 107
Answer: A
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

16

 

62) How many carbon atoms are there in 52.06 g of carbon dioxide? 62)
A) 3.134 × 1025
B) 1.424 × 1024
C) 7.122 × 1023
D) 5.206 × 1024
E) 8.648 × 10-23
Answer: C
Explanation: A)
B)
C)
D)
E)
63) The formula weight of silver chromate (Ag2CrO4) is __________ amu. 63)
A) 159.87 B) 175.87 C) 223.87 D) 331.73 E) 339.86
Answer: D
Explanation: A)
B)
C)
D)
E)

 

SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question.

64) The combustion of propane (C3H8 ) in the presence of excess oxygen yields CO2 and H2O: 64)
C3H8 (g) + 5O2 (g)   3CO2 (g) + 4H2O (g)
When 7.3 g of C3H8 burns in the presence of excess O2, __________ g of CO2 is produced.
Answer: 22
Explanation:
65) A compound was found to contain 90.6% lead (Pb) and 9.4% oxygen. The empirical 65)
formula for this compound is __________.
Answer: Pb3O4
Explanation:
66) Water can be formed from the stoichiometric reaction of hydrogen with oxygen: 66)
2H2 (g) + O2 (g)2H2O (g)

 

A complete reaction of 5.0 g of O2 with excess hydrogen produces __________ g of H2O.

 

Answer: 5.6

Explanation:

 

 

 

 

 

 

 

 

 

17

 

67) If 294 grams of FeS2 is allowed to react with 176 grams of O2 according to the following 67)
equation, how many grams of Fe2O3 are produced?
FeS2 + O2Fe2O3 + SO2
Answer: 160
Explanation:
68) Complete and balance the following reaction, given that elemental rubidium reacts with 68)
elemental sulfur to form Rb2S (s).
Na (s) + S (s)__________
Answer:    Na2S (s)
Explanation:
69) Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to 69)
yield ammonia:
N2 (g) + 3H2 (g)2NH3 (g)
A 9.3-g sample of hydrogen requires __________ g of N2 for a complete reaction.
Answer: 43
Explanation:
70) A certain alcohol contains only three elements, carbon, hydrogen, and oxygen. Combustion 70)
of a 50.00 gram sample of the alcohol produced 95.50 grams of CO2 and 58.70 grams of
H2O. What is the empirical formula of the alcohol?
Answer: C2H6O
Explanation:
71) Determine the mass percent (to the hundredth’s place) of H in sodium bicarbonate 71)
(NaHCO3).
Answer: 1.20
Explanation:
72) The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide 72)

and sulfur dioxide:

 

CS2 (g) + 3O2 (g)        CO2 (g) + 2SO2 (g)

 

The combustion of 15 g of CS2 in the presence of excess oxygen yields __________ g of SO2.

 

Answer: 25

Explanation:

 

 

 

 

 

 

 

 

 

18

 

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

 

73) A compound is composed of only C, H, and O. The combustion of a 0.519-g sample of the 73)
compound yields 1.24 g of CO2 and 0.255 g of H2O. What is the empirical formula of the
compound?
A) C6H6O B) CH3O C) C3H3O D) C2H6O2 E) C2H6O5
Answer: C
Explanation: A)
B)
C)
D)
E)
74) A 2.25-g sample of magnesium nitrate, Mg(NO3)2, contains __________ mol of this compound. 74)
A) 0.0261 B) 65.8 C) 0.0152 D) 148.3 E) 38.4
Answer: C
Explanation: A)
B)
C)
D)
E)
75) What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by 75)
mass?
A) SOCl2 B) S2OCl C) SOCl D) SO2Cl E) ClSO4
Answer: A
Explanation: A)
B)
C)
D)
E)
76) A compound that is composed of only carbon and hydrogen contains 80.0% C and 20.0% H by 76)
mass. What is the empirical formula of the compound?
A) C2H6 B) C20H60 C) CH4 D) C7H20 E) CH3
Answer: E
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

19

 

77) When the following equation is balanced, the coefficient of H2SO4 is __________. 77)
H2SO4 (aq) + NaOH (aq)Na2SO4 (aq) + H2O (l)
A) 2 B) 3 C) 0.5 D) 1 E) 4
Answer: D
Explanation: A)
B)
C)
D)
E)
78) There are __________ mol of carbon atoms in 4 mol of dimethylsulfoxide (C2H6SO). 78)
A) 2 B) 8 C) 4 D) 6 E) 3
Answer: B
Explanation: A)
B)
C)
D)
E)
79) Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 79)
4Al (s) + 3O2 (g)    2Al2O3 (s)
The maximum amount of Al2O3 that can be produced from 2.5 g of Al and 2.5 g of O2 is
__________ g.
A) 5.0 B) 9.4 C) 5.3 D) 7.4 E) 4.7
Answer: E
Explanation: A)
B)
C)
D)
E)
80) How many moles of magnesium oxide are produced by the reaction of 3.82 g of magnesium nitride 80)
with 7.73 g of water?
Mg3N2 + 3H2O2NH3 + 3MgO
A) 0.0378 B) 0.113 C) 0.429 D) 4.57 E) 0.0756
Answer: B
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

20

 

81) When the following equation is balanced, the coefficient of Al is __________. 81)
Al (s) + H2O (l)Al(OH)3 (s) + H2 (g)
A) 3 B) 1 C) 5 D) 4 E) 2
Answer: E
Explanation: A)
B)
C)
D)
E)
82) When the following equation is balanced, the coefficient of HCl is __________. 82)
CaCO3 (s) + HCl (aq)CaCl2 (aq) + CO2 (g) + H2O (l)
A) 2 B) 1 C) 0 D) 4 E) 3
Answer: A
Explanation: A)
B)
C)
D)
E)
83) Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in 83)
air. What is the coefficient of methanol in the balanced equation?
A) 1 B) 2 C) 3 D) 4 E) 3/2
Answer: B
Explanation: A)
B)
C)
D)
E)
84) Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide: 84)
PbCO3 (s)PbO (s) + CO2 (g)
How many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II)
carbonate?
A) 0.00936 B) 0.41 C) 2.61 D) 2.09 E) 2.50
Answer: D
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

21

 

85) When the following equation is balanced, the coefficient of H2O is __________. 85)
Ca (s) + H2O (l)Ca(OH)2 (aq) + H2 (g)
A) 4 B) 1 C) 5 D) 3 E) 2
Answer: E
Explanation: A)
B)
C)
D)
E)
86) The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 86)
4 NH3 (g) + 7 O2 (g)4 NO2 (g) + 6 H2O (g)
The combustion of 28.8 g of ammonia consumes __________ g of oxygen.
A) 108 B) 94.9 C) 28.8 D) 54.1 E) 15.3
Answer: B
Explanation: A)
B)
C)
D)
E)
87) A compound contains 40.0% C, 6.71% H, and 53.29% O by mass. The molecular weight of the 87)
compound is 60.05 amu. The molecular formula of this compound is __________.
A) C2H3O4 B) CHO2 C) C2H4O2 D) C2H2O4 E) CH2O
Answer: C
Explanation: A)
B)
C)
D)
E)
88) When the following equation is balanced, the coefficient of H3PO4 is __________. 88)
H3PO4 (aq) + NaOH (aq)   Na3PO4 (aq) + H2O (l)
A) 2 B) 0 C) 1 D) 3 E) 4
Answer: C
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

22

 

89) What is the maximum amount in grams of SO3 that can be produced by the reaction of 1.0 g of S 89)
with 1.0 g of O2 via the equation below?
S (s) + O2 (g)SO3 (g) (not balanced)
A) 2.0 B) 2.5 C) 1.7 D) 0.27 E) 3.8
Answer: C
Explanation: A)
B)
C)
D)
E)
90) Silver nitrate and aluminum chloride react with each other by exchanging anions: 90)

 

3AgNO3 (aq)+ AlCl3 (aq)      Al(NO3)3 (aq) + 3AgCl (s)

 

What mass in grams of AgCl is produced when 4.22 g of AgNO3 react with 7.73 g of AlCl3?

 

A) 11.9 B) 17.6 C) 24.9 D) 3.56 E) 4.22
Answer: D
Explanation: A)
B)
C)
D)
E)
91) The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O: 91)
4 NH3 (g) + 7 O2 (g)4 NO2 (g) + 6 H2O (g)

 

The combustion of 43.9 g of ammonia produces __________ g of NO2.

 

A) 2.58 B) 178 C) 43.9 D) 0.954 E) 119
Answer: E
Explanation: A)
B)
C)
D)
E)
92) What is the empirical formula of a compound that contains 49.4% K, 20.3% S, and 30.3% O by 92)
mass?
A) K2SO3 B) K2SO4 C) KSO3 D) KSO2 E) KSO4
Answer: A
Explanation: A)
B)
C)
D)
E)

 

 

 

 

23

 

93) When the following equation is balanced, the coefficient of water is __________. 93)
K (s) + H2O (l)KOH (aq) + H2 (g)
A) 5 B) 4 C) 1 D) 2 E) 3
Answer: D
Explanation: A)
B)
C)
D)
E)
94) Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2): 94)
CaC2 (s) + 2H2O (g)Ca(OH)2 (s) + C2H2 (g)
Production of 13g of C2H2 requires consumption of __________ g of H2O.
A) 9.0 B) 18 C) 4.8 × 102 D) 4.8 × 102 E) 4.5
Answer: B
Explanation: A)
B)
C)
D)
E)
95) A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water. 95)
Mg3N2 + 3H2O2NH3 + 3MgO
The yield of MgO is 3.60 g. What is the percent yield in the reaction?
A) 46.6 B) 78.8 C) 99.9 D) 94.5 E) 49.4
Answer: B
Explanation: A)
B)
C)
D)
E)
96) When the following equation is balanced, the coefficient of H2 is __________. 96)
K (s) + H2O (l)KOH (aq) + H2 (g)
A) 4 B) 2 C) 5 D) 1 E) 3
Answer: D
Explanation: A)
B)
C)

D)

E)

 

 

 

24

 

97) The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O: 97)
C3H8 (g) + 5O2 (g)3CO2 (g) + 4H2O (g)
When 2.5 mol of O2 are consumed in their reaction, __________ mol of CO2 are produced.
A) 2.5 B) 5.0 C) 3.0 D) 1.5 E) 6.0
Answer: D
Explanation: A)
B)
C)
D)
E)
98) How many grams of oxygen are in 65 g of C2H2O2? 98)
A) 18 B) 130 C) 29 D) 9.0 E) 36
Answer: E
Explanation: A)
B)
C)
D)
E)
99) When the following equation is balanced, the coefficient of H2S is __________. 99)
FeCl3 (aq) + H2S (g)   Fe2S3 (s) + HCl (aq)
A) 1 B) 4 C) 2 D) 3 E) 5
Answer: D
Explanation: A)
B)
C)
D)
E)
100) When the following equation is balanced, the coefficient of sulfur dioxide is __________. 100)
PbS (s) + O2 (g)PbO (s) + SO2 (g)
A) 2 B) 5 C) 1 D) 4 E) 3
Answer: A
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

25

 

101) Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield 101)
ammonia:
N2 (g) + 3H2 (g)2NH3 (g)
A 7.1-g sample of N2 requires __________ g of H2 for complete reaction.
A) 17.2 B) 0.76 C) 1.2 D) 1.5 E) 0.51
Answer: D
Explanation: A)
B)
C)
D)
E)
102) Combustion of a 1.031-g sample of a compound containing only carbon, hydrogen, and oxygen 102)
produced 2.265 g of CO2 and 1.236 g of H2O. What is the empirical formula of the compound?
A) C3H5O B) C3H8O C) C3H9O3 D) C6H16O2 E) C3H6O3
Answer: B
Explanation: A)
B)
C)
D)
E)
103) There are __________ hydrogen atoms in 25 molecules of C4H4S2. 103)
A) 3.8 × 1024 B) 6.0 × 1025 C) 100 D) 1.5 × 1025 E) 25
Answer: C
Explanation: A)
B)
C)
D)
E)
104) When the following equation is balanced, the coefficient of oxygen is __________. 104)
PbS (s) + O2 (g)PbO (s) + SO2 (g)
A) 3 B) 4 C) 2 D) 5 E) 1
Answer: A
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

 

26

 

105) A compound contains 38.7% K, 13.9% N, and 47.4% O by mass. What is the empirical formula of 105)
the compound?
A) KNO2 B) K4NO5 C) KNO3 D) K2NO3 E) K2N2O3
Answer: C
Explanation: A)
B)
C)
D)
E)
106) Predict the product in the combination reaction below. 106)
Al (s) + N2 (g)__________
A) Al3N2 B) AlN2 C) Al3N D) AlN3 E) AlN
Answer: E
Explanation: A)
B)
C)
D)
E)
107) When the following equation is balanced, the coefficient of C3H8O3 is __________. 107)
C3H8O3 (g) + O2 (g)   CO2 (g) + H2O (g)
A) 7 B) 5 C) 1 D) 2 E) 3
Answer: D
Explanation: A)
B)
C)
D)
E)
108) A compound that is composed of only carbon and hydrogen contains 85.7% C and 14.3% H by 108)
mass. What is the empirical formula of the compound?
A) CH4 B) C2H4 C) CH2 D) C86H14 E) C4H8
Answer: C
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

27

 

109) How many moles of carbon dioxide are there in 52.06 g of carbon dioxide? 109)
A) 0.8452
B) 1.183 × 1023
C) 6.022
D) 3.134 × 1025
E) 8.648 × 1023

Answer: B

Explanation:      A)

B)

C)

D)

E)

 

110) Magnesium and nitrogen react in a combination reaction to produce magnesium nitride: 110)

 

3 Mg + N2        Mg3N2

 

In a particular experiment, a 9.27-g sample of N2 reacts completely. The mass of Mg consumed is __________ g.

A) 16.1 B) 0.92 C) 8.04 D) 24.1 E) 13.9
Answer: D
Explanation: A)
B)
C)
D)
E)
111) When the following equation is balanced, the coefficient of nitric acid is __________. 111)
N2O5 (g) + H2O (l)HNO3 (aq)
A) 5 B) 4 C) 1 D) 3 E) 2
Answer: E
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

28

 

112) The combustion of propane (C3H8) produces CO2 and H2O: 112)
C3H8 (g) + 5O2 (g)3CO2 (g) + 4H2O (g)
The reaction of 2.5 mol of O2 will produce __________ mol of H2O.
A) 4.0 B) 3.0 C) 2.5 D) 2.0 E) 1.0
Answer: D
Explanation: A)
B)
C)
D)
E)
113) Combustion of a 0.9835-g sample of a compound containing only carbon, hydrogen, and oxygen 113)
produced 1.900 g of CO2 and 1.070 g of H2O. What is the empirical formula of the compound?
A) C4H10O B) C2H5O2 C) C4H10O2 D) C2H5O E) C4H11O2
Answer: E
Explanation: A)
B)
C)
D)
E)
114) GeF3H is formed from GeH4 and GeF4 in the combination reaction: 114)

 

GeH4 + 3GeF4        4GeF3H

 

If the reaction yield is 92.6%, how many moles of GeF4 are needed to produce 8.00 mol of GeF3H?

 

  1. A) 5.56 B) 2.16 C) 6.48                          D) 2.78                           E) 3.24

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

29

 

115) Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental 115)

pollutant:

 

2S (s) + 3O2 (g)      2SO3 (g)

 

In a particular experiment, the reaction of 1.0 g S with 1.0 g O2 produced 0.80 g of SO3. The %

yield in this experiment is __________.
A) 88 B) 29 C) 21 D) 48 E) 30
Answer: D
Explanation: A)
B)
C)
D)
E)
116) When the following equation is balanced, the coefficient of water is __________. 116)
N2O5 (g) + H2O (l)HNO3 (aq)
A) 4 B) 3 C) 2 D) 1 E) 5
Answer: D
Explanation: A)
B)
C)
D)
E)
117) Pentacarbonyliron (Fe(CO)5) reacts with phosphorous trifluoride (PF3) and hydrogen, releasing 117)
carbon monoxide:

 

Fe(CO)5 + PF3 + H2          Fe(CO)2(PF3)2(H)2 + CO (not balanced)

 

The reaction of 5.0 mol of Fe(CO)5, 8.0 mol of PF3 and 6.0 mol of H2 will release __________ mol of CO.

  1. A) 24 B) 12 C) 6.0                             D) 15                              E) 5.0

 

Answer: B

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

30

 

118) There are __________ sulfur atoms in 25 molecules of C4H4S2. 118)
A) 3.0 × 1025
B) 50
C) 6.02 × 1023
D) 1.5 × 1025
E) 4.8 × 1025

Answer: B

Explanation:      A)

B)

C)

D)

E)

 

119) What is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass? 119)
A) NaSO2 B) Na2S2O6 C) NaSO3 D) Na2S2O3 E) NaSO
Answer: D
Explanation: A)
B)
C)
D)
E)
120) When the following equation is balanced, the coefficient of H2 is __________. 120)
CO (g) + H2 (g)H2O (g) + CH4 (g)
A) 4 B) 3 C) 2 D) 0 E) 1
Answer: B
Explanation: A)
B)
C)
D)
E)
121) There are __________ molecules of methane in 0.123 mol of methane (CH4). 121)
A) 7.40 × 1022
B) 0.615
C) 5
D) 2.04 × 1025
E) 2.46 × 102
Answer: A
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

31

 

122) What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of 122)
water?
Mg (s) + 2H2O (l)Mg(OH)2 (s) + H2 (g)
A) 0.0485 B) 0.219 C) 0.102 D) 0.0162 E) 0.204
Answer: C
Explanation: A)
B)
C)
D)
E)
123) What is the maximum mass in grams of NH3 that can be produced by the reaction of 1.0 g of N2 123)
with 3.0 g of H2 via the equation below?
N2 (g) + H2 (g)NH3 (g) (not balanced)
A) 0.61 B) 2.0 C) 17 D) 1.2 E) 4.0
Answer: D
Explanation: A)
B)
C)
D)
E)
124) A compound that is composed of carbon, hydrogen, and oxygen contains 70.6% C, 5.9% H, and 124)
23.5% O by mass. The molecular weight of the compound is 136 amu. What is the molecular
formula?
A) C8H8O2 B) C4H4O C) C5H6O2 D) C9H12O E) C8H4O
Answer: A
Explanation: A)
B)
C)
D)
E)
125) How many grams of hydrogen are in 46 g of CH4O? 125)
A) 1.5 B) 5.8 C) 184 D) 2.8 E) 0.36
Answer: B
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

32

 

126) A sample of C3H8O that contains 200 molecules contains __________ carbon atoms. 126)
A) 4.01 × 1025
B) 1.20 × 1026
C) 600
D) 200
E) 3.61 × 1026
Answer: C
Explanation: A)
B)
C)
D)
E)
127) A 22.5-g sample of ammonium carbonate contains __________ mol of ammonium ions. 127)
A) 2.14 B) 0.234 C) 0.468 D) 3.47 E) 0.288
Answer: C
Explanation: A)
B)
C)
D)
E)
128) What is the coefficient of O2 when the following equation is completed and balanced? 128)
C4H8O2 + O2__________
A) 3 B) 1 C) 2 D) 6 E) 5
Answer: E
Explanation: A)
B)
C)
D)
E)
129) When the following equation is balanced, the coefficient of Al2O3 is __________. 129)
Al2O3 (s) + C (s) + Cl2 (g)AlCl3 (s) + CO (g)
A) 5 B) 3 C) 4 D) 1 E) 2
Answer: D
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

33

 

130) Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide: 130)

 

4Al (s) + 3O2 (g)        2Al2O3 (s)

 

In a particular experiment, the reaction of 2.5 g of Al with 2.5 g of O2 produced 3.5 g of Al2O3. The

% yield of the reaction is __________.
A) 47 B) 66 C) 74 D) 26 E) 37
Answer: C
Explanation: A)
B)
C)
D)
E)
131) When the following equation is balanced, the coefficient of dinitrogen pentoxide is __________. 131)
N2O5 (g) + H2O (l)HNO3 (aq)
A) 2 B) 1 C) 5 D) 3 E) 4
Answer: B
Explanation: A)
B)
C)
D)
E)
132) Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: 132)
S (s) + 3F2 (g)    SF6 (g)

 

In a particular experiment, the percent yield is 79.0%. This means that a 7.90-g sample of fluorine yields __________ g of SF6 in the presence of excess sulfur.

 

  1. A) 0.110 B) 24.0 C) 7.99                          D) 10.1                           E) 30.3

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

34

 

133) When the following equation is balanced, the coefficients are __________. 133)
Al(NO3)3 + Na2S    Al2S3 + NaNO3
A) 2, 3, 2, 3 B) 4, 6, 3, 2 C) 2, 1, 3, 2 D) 1, 1, 1, 1 E) 2, 3, 1, 6
Answer: E
Explanation: A)
B)
C)
D)
E)
134) Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride: 134)
S (s) + 3F2 (g)    SF6(g)
The maximum amount of SF6 that can be produced from the reaction of 3.5 g of sulfur with 4.5 g of
fluorine is __________ g.
A) 16 B) 8.0 C) 5.8 D) 12 E) 3.2
Answer: C
Explanation: A)
B)
C)
D)
E)
135) When the following equation is balanced, the coefficient of HNO3 is __________. 135)
HNO3 (aq) + CaCO3 (s)   Ca(NO3)2 (aq) + CO2 (g) + H2O (l)
A) 4 B) 1 C) 2 D) 5 E) 3
Answer: C
Explanation: A)
B)
C)
D)
E)
136) Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in 136)
air. What is the coefficient of oxygen in the balanced equation?
A) 1 B) 2 C) 3 D) 4 E) 3/2
Answer: C
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

35

 

137) When the following equation is balanced, the coefficients are __________. 137)
NH3 (g) + O2 (g)   NO2 (g) + H2O (g)
A) 2, 3, 2, 3 B) 1, 3, 1, 2 C) 4, 3, 4, 3 D) 4, 7, 4, 6 E) 1, 1, 1, 1
Answer: D
Explanation: A)
B)
C)
D)
E)
138) When the following equation is balanced, the coefficient of O2 is __________. 138)
C2H4O (g) + O2 (g)   CO2 (g) + H2O (g)
A) 4 B) 3 C) 2 D) 1 E) 5
Answer: E
Explanation: A)
B)
C)
D)
E)
139) When the following equation is balanced, the coefficient of hydrogen is __________. 139)
K (s) + H2O (l)KOH (aq) + H2 (g)
A) 2 B) 5 C) 3 D) 4 E) 1
Answer: E
Explanation: A)
B)
C)
D)
E)
140) The balanced equation for the decomposition of sodium azide is __________. 140)
A) 2NaN3 (s)2Na (s) + 2N2 (g)
B) 2NaN3 (s)Na2 (s)  + 3N2 (g)
C) NaN3 (s)Na (s) + N2 (g) + N (g)
D) 2NaN3 (s)2Na (s) + 3N2 (g)
E) NaN3 (s)Na (s) + N2 (g)
Answer: D
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

36

 

TRUE/FALSE. Write ‘T’ if the statement is true and ‘F’ if the statement is false.

 

141) Carbon dioxide called a greenhouse gas because bacterial degradation of fertilizers in a greenhouse 141)
environment produce large quantities of carbon dioxide.
Answer: True False
Explanation:
142) The mass of a single atom of an element (in amu) is numerically EQUAL to the mass in grams of 1 142)
mole of that element.
Answer: True False
Explanation:
143) The molecular weight is ALWAYS a whole-number multiple of the empirical formula weight. 143)
Answer: True False
Explanation:
144) The quantity of product that is calculated to form when all of the limiting reagent reacts is called 144)
the actual yield.
Answer: True False
Explanation:
145) A great deal of the carbon dioxide produced by the combustion of fossil fuels is absorbed into the 145)
oceans.
Answer: True False

Explanation:

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

37

 

Answer Key

 

Testname: C3

 

 

 

  • C
  • E
  • C
  • A
  • C
  • E
  • B
  • D
  • E
  • B
  • E
  • B
  • A
  • B
  • C
  • C
  • B
  • B
  • B
  • B
  • E
  • A
  • E
  • D
  • E
  • E
  • D
  • C
  • C
  • C
  • E
  • B
  • A
  • E
  • C
  • E
  • A
  • B
  • A
  • B
  • D
  • E
  • D
  • B
  • A
  • C
  • E
  • A
  • E
  • E

 

 

38

 

Answer Key

 

Testname: C3

 

 

 

  • E
  • C
  • E
  • E
  • A
  • B
  • C
  • A
  • C
  • B
  • A
  • C
  • D
  • 22
  • Pb3O4

 

  • 6
  • 160
  • Na2S (s)

 

  • 43
  • C2H6O

 

  • 20
  • 25
  • C
  • C

 

 

Exam

 

Name___________________________________

 

 

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

1) Which one of the following is most soluble in hexane (C6H14)? 1)
A) CH3CH2CH2OH
B) CH3OH
C) CH3CH2CH2CH2CH2OH
D) CH3CH2CH2CH2OH
E) CH3CH2OH
Answer: C
Explanation: A)
B)
C)
D)
E)
2) When solutions of strong electrolytes in water are formed, the ions are surrounded by water 2)
molecules. These interactions are best described as a case of __________.
A) hydration
B) crystallization
C) supersaturation
D) dehydration
E) solvation
Answer: A
Explanation: A)
B)
C)
D)
E)
3) An unsaturated solution is one that __________. 3)
A) contains the maximum concentration of solute possible, and is in equilibrium with
undissolved solute
B) has a concentration lower than the solubility
C) contains no solute
D) has no double bonds
E) contains more dissolved solute than the solubility allows
Answer: B
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

1

 

4) Calculate the freezing point of a solution containing 40.0 grams of KCl and 4400.0 grams of water. 4)
The molal-freezing-point-depression constant (Kf) for water is 1.86 ° C/m.
A) +0.45 oC B) -0.45 oC C) -0.23 oC D) 1.23 oC E) +0.23 oC
Answer: B
Explanation: A)
B)
C)
D)
E)
5) A 0.100 m solution of which one of the following solutes will have the lowest vapor pressure? 5)
A) Ca(ClO4)2 B) Al(ClO4)3 C) KClO4 D) sucrose E) NaCl
Answer: B
Explanation: A)
B)
C)
D)
E)
6) When argon is placed in a container of neon, the argon spontaneously disperses throughout the 6)
neon because __________.
A) of solvent-solute interactions
B) the dispersion of argon atoms produces an increase in disorder
C) of hydrogen bonding
D) of the large attractive forces between argon and neon atoms
E) a decrease in energy occurs when the two mix
Answer: B
Explanation: A)
B)
C)
D)
E)
7) A solution is prepared by adding 30.00 g of lactose (milk sugar) to 110.0 g of water at 55 °C. The 7)
partial pressure of water above the solution is __________ torr. The vapor pressure of pure water at
55 °C is 118 torr. The MW of lactose is 342.3 g/mol.
A) 169.4 B) 1.670 C) 92.7 D) 94.1 E) 116.3
Answer: E
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

2

 

8) In a saturated solution of a salt in water, __________. 8)
  1. seed crystal addition may cause massive crystallization
  2. the rate of crystallization > the rate of dissolution
  3. addition of more water causes massive crystallization
  4. the rate of dissolution > the rate of crystallization
  5. the rate of crystallization = the rate of dissolution

 

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

9) Which of the following is not a colloid? 9)
  1. A) whipped cream
  2. B) smoke
  3. C) air
  4. D) homogenized milk
  5. E) fog

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

10) The phrase “like dissolves like” refers to the fact that __________. 10)
  1. gases can only dissolve other gases
  2. condensed phases can only dissolve other condensed phases
  3. polar solvents dissolve polar solutes and nonpolar solvents dissolve nonpolar solutes
  4. polar solvents dissolve nonpolar solutes and vice versa
  5. solvents can only dissolve solutes of similar molar mass

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

11) A solution contains 28% phosphoric acid by mass. This means that __________. 11)
  1. A) 1 mL of this solution contains 28 g of phosphoric acid
  2. B) the density of this solution is 2.8 g/mL
  3. C) 1 L of this solution has a mass of 28 g
  4. D) 100 g of this solution contains 28 g of phosphoric acid
  5. E) 1 L of this solution contains 28 mL of phosphoric acid

 

Answer: D

Explanation:      A)

B)

C)

D)

E)

 

 

 

3

 

12) The Henry’s law constant for helium gas in water at 30 °C is 3.70 × 104 M/atm. When the partial 12)
pressure of helium above a sample of water is 0.650 atm, the concentration of helium in the water is
__________ M.
A) 1.76 × 103
B) 2.41 × 104
C) 5.69 × 104
D) 3.70 × 104
E) 1.30
Answer: B
Explanation: A)
B)
C)
D)
E)
13) Ammonium nitrate (NH4NO3) dissolves readily in water even though the dissolution is 13)
endothermic by 26.4 kJ/mol. The solution process is spontaneous because __________.
A) of the increase in disorder upon dissolution of this strong electrolyte
B) the vapor pressure of the water decreases upon addition of the solute
C) of the increase in enthalpy upon dissolution of this strong electrolyte
D) of the decrease in enthalpy upon addition of the solute
E) osmotic properties predict this behavior
Answer: A
Explanation: A)
B)
C)
D)
E)
14) A solution is prepared by dissolving calcium chloride in water and diluting to 500.0 mL. If this 14)
solution contains 44 ppm chloride ions, the concentration of calcium ions is __________ ppm.
A) 11 B) 44 C) 88 D) 500 E) 22
Answer: E
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

4

 

15) A saturated solution __________. 15)
  1. contains as much solvent as it can hold
  2. cannot be attained
  3. contains dissolved solute in equilibrium with undissolved solid
  4. will rapidly precipitate if a seed crystal is added
  5. contains no double bonds

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

16) A supersaturated solution __________. 16)
  1. is one with a higher concentration than the solubility
  2. exists only in theory and cannot actually be prepared
  3. is one that has been heated
  4. must be in contact with undissolved solid
  5. is one with more than one solute

 

Answer: A

Explanation:      A)

B)

C)

D)

E)

 

17) The dissolution of gases in water is virtually always exothermic because __________. 17)
  1. neither of the two endothermic steps in the solution-formation process is necessary
  2. one of the two endothermic steps (separation of solute particles) in the solution-formation process is unnecessary
  3. gases react exothermically with water
  4. the exothermic step in the solution-formation process is unnecessary
  5. all three steps in the solution-formation process are exothermic

 

Answer: B

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

5

 

18) Which of the following liquids will have the lowest freezing point? 18)
A) pure H2O
B) aqueous CoI2 (0.030 m)
C) aqueous FeI3 (0.030 m)
D) aqueous glucose (0.050 m)
E) aqueous NaI (0.030 m)
Answer: C
Explanation: A)
B)
C)
D)
E)
19) Which of the following cannot be a colloid? 19)
A) a foam
B) an aerosol
C) an emulsion
D) a homogenous mixture
E) All of the above are colloids.
Answer: D
Explanation: A)
B)
C)
D)
E)
20) The dissolution of water in octane (C8H18) is prevented by __________. 20)
A) hydrogen bonding between water molecules
B) repulsion between like-charged water and octane molecules
C) dipole-dipole attraction between octane molecules
D) London dispersion forces between octane molecules
E) ion-dipole attraction between water and octane molecules
Answer: A
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

6

 

21) Which one of the following substances is more likely to dissolve in CCl4? 21)
A) CBr4
B) NaCl
C) HBr
D) HCl
E) CH3CH2OH
Answer: A
Explanation: A)
B)
C)
D)
E)
22) Of the concentration units below, only __________ is temperature dependent. 22)
A) mass % B) ppb C) ppm D) molality E) molarity
Answer: E
Explanation: A)
B)
C)
D)
E)
23) Hydrophobic colloids __________. 23)
  1. can be stabilized by coagulation
  2. can be stabilized by adsorption of ions
  3. will separate into two phases if they are stabilized
  4. are those that do not contain water
  5. are those that contain water

 

Answer: B

Explanation:      A)

B)

C)

D)

E)

 

24) A solution is prepared by adding 1.43 mol of KCl to 889 g of water. The concentration of KCl is 24)
__________ molal.
A) 622
B) 0.622
C) 1.61 × 103
D) 1.27 × 103
E) 1.61

 

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

7

 

25) Which one of the following substances is more likely to dissolve in benzene (C6H6)? 25)
A) CCl4
B) CH3CH2OH
C) HBr
D) NH3
E) NaCl
Answer: A
Explanation: A)
B)
C)
D)
E)
26) The osmotic pressure of a solution formed by dissolving 25.0 mg of aspirin (C9H8O4) in 0.250 L of 26)
water at 25 °C is __________ atm.
A) 1.14 × 103
B) 0.0136
C) 1.38
D) 13.6
E) 2.45
Answer: B
Explanation: A)
B)
C)
D)
E)
27) A solution is prepared by dissolving 7.00 g of glycerin (C3H8O3) in 201 g of ethanol (C2H5OH). 27)
The freezing point of the solution is _______°C. The freezing point of pure ethanol is -114.6 °C at 1
atm. The molal-freezing-point-depression constant (Kf) for ethanol is 1.99 ° C/m. The molar masses
of glycerin and of ethanol are 92.1 g/mol and 46.1 g/mol, respectively.
A) -121.3 B) -107.9 C) -113.8 D) 0.752 E) -115.4
Answer: E
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

8

 

28) The concentration of chloride ion in a solution that contains 35.0 ppm chloride is __________% by 28)
mass. × 101
A) 3.50
B) 3.50 × 103
C) 3.50 × 106
D) 3.50 × 102
E) 3.50 × 102

Answer: B

Explanation:      A)

B)

C)

D)

E)

 

29) At 20°C, a 3.54 M aqueous solution of ammonium chloride has a density of 1.0512 g/mL. What is 29)
the mass % of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.
A) 6.95 B) 4.10 C) 3.36 D) 18.00 E) 0.297
Answer: D
Explanation: A)
B)
C)
D)
E)
30) A 1.35 m aqueous solution of compound X had a boiling point of 101.4°C. Which one of the 30)
following could be compound X? The boiling point elevation constant for water is 0.52°C/m.
A) Na3PO4
B) CH3CH2OH
C) KCl
D) CaCl2
E) C6H12O6
Answer: C
Explanation: A)
B)
C)
D)
E)
31) At 20°C, a 2.32 M aqueous solution of ammonium chloride has a density of 1.0344 g/mL. What is 31)
the molality of ammonium chloride in the solution? The formula weight of NH4Cl is 53.50 g/mol.
A) 0.0449 B) 2.55 C) 12.00 D) 0.446 E) 2.32
Answer: B
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

9

 

32) The most likely van’t Hoff factor for an 0.01 m CaI2 solution is __________. 32)
A) 1.27 B) 1.00 C) 3.29 D) 2.69 E) 3.00
Answer: D
Explanation: A)
B)
C)
D)
E)
33) The ideal value of i (van’t Hoff factor) for (NH4)3PO4. 33)
A) 5 B) 1 C) 4 D) 3 E) 2
Answer: C
Explanation: A)
B)
C)
D)
E)
34) A solution is prepared by dissolving 16.2 g of benzene (C6H6) in 282 g of carbon tetrachloride 34)
(CCl4). The concentration of benzene in this solution is __________ molal. The molar masses of
C6H6 and CCl4 are 78.1 g/mol and 154 g/mol, respectively.
  1. 102
  2. 36 × 104
  3. 43
  4. 736
  5. 0543

 

Answer: D

Explanation:      A)

B)

C)

D)

E)

 

35) A solution contains 11% by mass of sodium chloride. This means that __________. 35)
  1. A) 100 mL of the solution contains 11 g of sodium chloride
  2. B) the molality of the solution is 11
  3. C) there are 11 g of sodium chloride in in 1.0 mL of this solution
  4. D) the density of the solution is 11 g/mL
  5. E) 100 g of the solution contains 11 g of sodium chloride

 

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

10

 

36) Of the following, a 0.1 M aqueous solution of __________ will have the lowest freezing point. 36)
A) Al(NO3)3 B) NaCl C) K2CrO4 D) Na2SO4 E) sucrose
Answer: A
Explanation: A)
B)
C)
D)
E)
37) Molality is defined as the __________. 37)
A) moles solute/kg solution
B) moles solute/Liters solution
C) moles solute/moles solvent
D) moles solute/kg solvent
E) none (dimensionless)
Answer: D
Explanation: A)
B)
C)
D)
E)
38) Colligative properties of solutions include all of the following except __________. 38)
  1. the increase of reaction rates with increase in temperature
  2. depression of vapor pressure upon addition of a solute to a solvent
  3. depression of the freezing point of a solution upon addition of a solute to a solvent
  4. an increase in the osmotic pressure of a solution upon the addition of more solute
  5. elevation of the boiling point of a solution upon addition of a solute to a solvent

 

Answer: A

Explanation:      A)

B)

C)

D)

E)

 

39) If the partial pressure of oxygen in the air a diver breathes is too great, __________. 39)
  1. respiratory tissue is damaged by oxidation
  2. hyperventilation results
  3. the urge to breathe is reduced and not enough CO2 is removed from the body
  4. the urge to breathe is increased and excessive CO2 is removed from the body

 

  1. No problems result from this situation.

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

 

11

 

40) Which of the following choices has the compounds correctly arranged in order of increasing 40)
solubility in water? (least soluble to most soluble)
A) LiF < NaNO3 < CHCl3
B) CH4 < NaNO3 < CHCl3
C) CH3OH < CH4 < LiF
D) CCl4 < CHCl3 < NaNO3
E) CH3OH < Cl4 < CHCl3
Answer: D
Explanation: A)
B)
C)
D)
E)
41) The process of a substance sticking to the surface of another is called 41)
A) coagulation
B) adsorption
C) absorption
D) diffusion
E) effusion
Answer: B
Explanation: A)
B)
C)
D)
E)
42) Which produces the greatest number of ions when one mole dissolves in water? 42)
A) NH4NO3 B) NH4Cl C) Na2SO4 D) NaCl E) sucrose
Answer: C
Explanation: A)
B)
C)
D)
E)
43) Which one of the following concentration units varies with temperature? 43)
A) mole fraction
B) mass percent
C) molarity
D) molality
E) all of the above
Answer: C
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

12

 

44) Hydration is a specific example of the phenomenon known generally as __________. 44)
A) condensation
B) disordering
C) dilution
D) salutation
E) solvation
Answer: E
Explanation: A)
B)
C)
D)
E)
45) At 20°C, an aqueous solution that is 24.00% by mass in ammonium chloride has a density of 45)
1.0674 g/mL. What is the molarity of ammonium chloride in the solution? The formula weight of
NH4Cl is 53.50 g/mol.
A) 22.5 B) 4.79 C) 0.479 D) 5.90 E) 0.0445
Answer: B
Explanation: A)
B)
C)
D)
E)
46) The principal reason for the extremely low solubility of NaCl in benzene (C6H6) is the __________. 46)
A) strong solvent-solvent interactions
B) increased disorder due to mixing of solute and solvent
C) hydrogen bonding in C6H6
D) strength of the covalent bond in NaCl
E) weak solvation of Na+ and Cl by C H 6
6
Answer: E
Explanation: A)
B)
C)
D)
E)
47) The Procter & Gamble Company product called olestraTM is formed by combining a sugar 47)
molecule with __________.
A) alcohols
B) cholesterol
C) vitamin A
D) fatty acids
E) protein
Answer: D
Explanation: A)
B)
C)
D)
E)

 

 

 

13

 

48) Which one of the following substances would be the most soluble in CCl4? 48)
A) C10H22
B) CH3CH2OH
C) H2O
D) NaCl
E) NH3
Answer: A
Explanation: A)
B)
C)
D)
E)
49) Which of the following aqueous solutions will have the highest boiling point? 49)
A) 0.10 m SrSO4
B) 0.20 m glucose
C) 0.25 m sucrose
D) 0.10 m NaCl
E) 0.10 m Na2SO4
Answer: E
Explanation: A)
B)
C)
D)
E)
50) The largest value of the Henry’s Law constant for the liquid solvent H2O will be obtained with 50)
__________ gas as the solute and a temperature of __________°C.
A) Ar, 11 B) C2H4, 45 C) CO2, 32 D) HCl, 49 E) N2, 15
Answer: D
Explanation: A)
B)
C)
D)
E)
51) A solution with a concentration higher than the solubility is __________. 51)
A) is unsaturated
B) is supercritical
C) is saturated
D) is supersaturated
E) is not possible
Answer: D
Explanation: A)
B)
C)
D)
E)

 

 

 

 

14

 

52) Formation of solutions where the process is endothermic can be spontaneous provided that 52)
__________.
A) they are accompanied by an increase in order
B) the solvent is a gas and the solute is a solid
C) they are accompanied by an increase in disorder
D) the solvent is water and the solute is a gas
E) they are accompanied by another process that is exothermic
Answer: C
Explanation: A)
B)
C)
D)
E)
53) As the concentration of a solute in a solution increases, the freezing point of the solution 53)
__________ and the vapor pressure of the solution __________.
A) decreases, increases
B) decreases, is unaffected
C) increases, increases
D) decreases, decreases
E) increases, decreases
Answer: D
Explanation: A)
B)
C)
D)
E)
54) Which of the following liquids will have the lowest freezing point? 54)
A) pure H2O
B) aqueous FeI3 (0.24 m)
C) aqueous sucrose (0.60 m)
D) aqueous glucose (0.60 m)
E) aqueous KF (0.50 m)
Answer: E
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

15

 

55) Which of the following substances is more likely to dissolve in water? 55)
A) HOCH2CH2OH
B) CH3(CH2)8CH2OH
C) CCl4
D) CHCl3
E) O
CH3(CH2)9CH
Answer: A
Explanation: A)
B)
C)
D)
E)
56) Which of the following substances is more likely to dissolve in CH3OH? 56)
A) N2
B) Kr
C) CCl4
D) H2
E) CH3CH2OH
Answer: E
Explanation: A)
B)
C)
D)
E)
57) A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that 57)
__________.
A) there are 15 mg of benzene in 1.0 L of this solution
B) 100 g of the solution contains 15 g of benzene
C) 100 g of the solution contains 15 mg of benzene
D) the molarity of the solution is 15
E) the solution is 15% by mass of benzene
Answer: A
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

 

 

 

 

16

 

58) Which one of the following is most soluble in water? 58)
A) CH3CH2OH
B) CH3CH2CH2CH2OH
C) CH3OH
D) CH3CH2CH2OH
E) CH3CH2CH2CH2CH2OH
Answer: C
Explanation: A)
B)
C)
D)
E)
59) A solution contains 15 ppm of benzene. The density of the solution is 1.00 g/mL. This means that 59)
__________.
A) there are 15 mg of benzene in 1.0 g of this solution
B) 1.0 L of the solution contains 15 g of benzene
C) the solution is 15% by mass of benzene
D) 1.0 g of the solution contains 15 × 106 g of benzene
E) 100 g of the solution contains 15 g of benzene
Answer: D
Explanation: A)
B)
C)
D)
E)
60) The magnitudes of Kf and of Kb depend on the identity of the __________. 60)
A) solvent and on temperature
B) solute and solvent
C) solvent
D) solute
E) solution
Answer: C
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

17

 

61) Pressure has an appreciable effect on the solubility of __________ in liquids. 61)
  1. A) solids
  2. B) solids and liquids
  3. C) liquids
  4. D) salts
  5. E) gases

 

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

62) The concentration of KCl in a solution prepared by adding 0.0660 mol of KCl to 1.00 mol of water is     62)

__________ % by mass.

  1. 733
  2. 0130
  3. 0519
  4. 33 × 104
  5. 19

 

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

63) Which component of air is the primary problem in a condition known as “the bends?” 63)
A) N2 B) He C) CO2 D) CO E) O2
Answer: A
Explanation: A)
B)
C)
D)
E)
64) When two nonpolar organic liquids are mixed, a solution forms and the enthalpy of solution is 64)
quite small. Label the two organic liquids as A (solvent) and B (solute). The formation of solution
is favored by __________.
A) the highly negative enthalpy of the solution process
B) an increase in disorder, since A-A, B-B, and A-B interactions are similar
C) solvation of the solvent, A
D) hydration of the solute, B
E) the equal enthalpy of the solvent and solute
Answer: B
Explanation: A)
B)
C)
D)
E)

 

 

 

 

18

 

65) Which one of the following solutes has a limiting van’t Hoff factor (i) of 3 when dissolved in water?     65)

  1. A) CCl4 B) Na2SO4 C) sucrose                    D) KNO3                        E) CH3OH

 

Answer: B

Explanation:      A)

B)

C)

D)

E)

 

SHORT ANSWER. Write the word or phrase that best completes each statement or answers the question.

 

66) What is the osmotic pressure (in atm) of a 0.040 M solution of a non-electrolyte at 30.0 oC? 66)
Answer: 1.0
Explanation:
67) Water (H2O) and the alcohol methanol (CH3OH) are infinitely soluble in each other. The 67)
primary intermolecular force responsible for this is __________.
Answer: hydrogen bonding
Explanation:
68) A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor 68)
pressure of water (in torr) over the solution at 25.0 oC. (Note: the vapor pressure of pure
water at 25.0 oC is 23.76 torr.)
Answer: 20.91
Explanation:
69) A solution contains 150.8 grams of NaCl in 678.3 grams of water. Calculate the vapor 69)
pressure lowering (in torr) of the solution at 25.0 oC. (Note: the vapor pressure of pure
water at 25.0 oC is 23.76 torr.)
Answer: 2.85
Explanation:
70) Physical properties of a solution that depend on the quantity of the solute particles present, 70)
but not the kind or identity of the particles, are termed __________ properties.
Answer: colligative
Explanation:
71) The phenomenon used to differentiate colloids and true solutions is called the __________ 71)
effect.

 

Answer: Tyndall

Explanation:

 

 

 

 

 

 

 

 

 

 

 

 

 

 

19

 

MULTIPLE CHOICE. Choose the one alternative that best completes the statement or answers the question.

 

72) A solution is prepared by dissolving 0.60 g of nicotine (a nonelectrolyte) in water to make 12 mL of 72)
solution. The osmotic pressure of the solution is 7.55 atm at 25 °C. The molecular weight of nicotine
is __________ g/mol.
A) 43 B) 0.60 C) 160 D) 28 E) 50
Answer: C
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

73) A sample of potassium chlorate (15.0 g) is dissolved in 201 g of water at 70 °C, with precautions 73)

taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no precipitate is observed. This solution is __________.

  1. A) unsaturated
  2. B) saturated
  3. C) miscible
  4. D) supersaturated
  5. E) hydrated

 

Answer: A

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

20

 

74) The vapor pressure of pure water at 25 °C is 23.8 torr. What is the vapor pressure (torr) of water 74)
above a solution prepared by dissolving 18.0 g of glucose (a nonelectrolyte, MW = 180.0 g/mol) in
95.0 g of water?
A) 0.443 B) 23.8 C) 24.3 D) 0.451 E) 23.4
Answer: E
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

75) A sample of potassium nitrate (49.0 g) is dissolved in 101 g of water at 100 °C, with precautions 75)

taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and no precipitate is observed. This solution is __________.

  1. A) saturated
  2. B) unsaturated
  3. C) hydrated
  4. D) placated
  5. E) supersaturated

 

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

21

 

76) Calculate the freezing point (0°C) of a 0.05500 m aqueous solution of NaNO3. The molal 76)
freezing-point-depression constant of water is 1.86 °C/m.
A) 0.1023 B) 0.0286 C) -0.05627 D) -0.1023 E) -0.2046
Answer: E
Explanation: A)
B)
C)

D)

E)

 

77) A solution is prepared by dissolving 6.00 g of an unknown nonelectrolyte in enough water to make      77)

1.00 L of solution. The osmotic pressure of this solution is 0.750 atm at 25.0 °C. What is the

molecular weight (g/mol) of the unknown solute?

  1. 4
  2. 110
  3. 12 × 103
  4. 6
  5. 195

 

Answer: E

Explanation:      A)

B)

C)

D)

E)

 

78) The mole fraction of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 78)
39 g of H2O is __________.
A) 0.37 B) 0.58 C) 9.1 D) 0.13 E) 0.11
Answer: E
Explanation: A)
B)
C)
D)
E)
79) The concentration of HCl in a solution that is prepared by dissolving 5.5 g of HCl in 200 g of 79)
C2H6O is __________ molal.
A) 1.3 B) 0.75 C) 27.5 D) 7.5 × 104 E) 3.3 × 102
Answer: B
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

22

 

80) Determine the fraction of ionization of HX if a solution prepared by dissolving 0.020 mol of HX in 80)
  • g of water freezes at -47 °C. The molal freezing-point-depression constant of water is
  • 86 °C/m.
A) 1.45 B) 0.45 C) 0.044 D) 0.348 E) 0.30
Answer: B
Explanation: A)
B)
C)
D)
E)

 

81) The solubility of MnSO4 monohydrate in water at 20 °C is 70.0 g per 100.0 mL of water. A solution 81)
at 20 °C that is 4.22 M in MnSO4 monohydrate is best described as a(n) __________ solution. The
formula weight of MnSO4 monohydrate is 168.97 g/mol.
A) solvated
B) supersaturated
C) hydrated
D) unsaturated
E) saturated
Answer: B
Explanation: A)
B)
C)
D)
E)
82) A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting 82)
solution is 1.05 g/mL. The concentration of CaCl2 is __________% by mass.
A) 6.24 B) 0.0632 C) 0.0594 D) 5.94 E) 6.32
Answer: D
Explanation: A)
B)
C)
D)
E)
83) The concentration of urea in a solution prepared by dissolving 16 g of urea in 39 g of H2O is 83)
__________% by mass. The molar mass of urea is 60.0 g/mol.
A) 0.29 B) 0.41 C) 29 D) 0.48 E) 41
Answer: C
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

23

 

84) The concentration of a benzene solution prepared by mixing 12.0 g C6H6 with 38.0 g CCl4 is 84)
__________ molal.
A) 0.240 B) 4.04 C) 0.508 D) 0.622 E) 0.316
Answer: B
Explanation: A)
B)
C)
D)
E)
85) The vapor pressure of pure water at 25 °C is 23.8 torr. Determine the vapor pressure (torr) of water 85)
at 25 °C above a solution prepared by dissolving 35 g of urea (a nonvolatile, non-electrolyte, MW =
60.0 g/mol) in 75 g of water.
A) 0.88 B) 27 C) 21 D) 3.3 E) 2.9
Answer: C
Explanation: A)
B)
C)
D)
E)
86) A solution is prepared by dissolving 15.0 g of NH3 in 250 g of water. The density of the resulting 86)
solution is 0.974 g/mL. The molarity of NH3 in the solution is __________.
A) 3.53 B) 3.24 C) 0.882 D) 60.0 E) 0.00353
Answer: B
Explanation: A)
B)
C)
D)
E)
87) A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting 87)
solution is 1.05 g/mL. The concentration of Cl in this solution is __________ M.
A) 1.20
B) 6.64 × 102
C) 1.12
D) 0.214
E) 0.562
Answer: C
Explanation: A)
B)

C)

D)

E)

 

 

 

 

 

 

 

 

 

 

24

 

88) Determine the freezing point (°C) of a 0.015 molal aqueous solution of MgSO4. Assume i = 2.0 for 88)
MgSO4. The molal freezing-point-depression constant of water is 1.86 °C/m.
A) 0.000 B) -0.056 C) -0.028 D) -0.084 E) -0.17
Answer: B
Explanation: A)
B)
C)

D)

E)

 

89) The solubility of Ar in water at 25 °C is 1.6 × 103 M when the pressure of the Ar above the solution 89) is 1.0 atm. The solubility of Ar at a pressure of 2.5 atm is __________ M.

A) 4.0 × 103 B) 7.5 × 102 C) 1.6 × 103 D) 6.4 × 104 E) 1.6 × 103
Answer: A
Explanation: A)
B)
C)
D)
E)
90) The concentration of KBr in a solution prepared by dissolving 2.21 g of KBr in 897 g of water is 90)
__________ molal.
A) 0.0207
B) 0.0167
C) 2.46
D) 0.0186
E) 2.07 × 105
Answer: A
Explanation: A)
B)
C)

D)

E)

 

91) The concentration of lead nitrate (Pb(NO3)2) in a 0.726 M solution is __________ molal. The density   91)

of the solution is 1.202 g/mL.
A) 1.928 B) 0.650 C) 0.755 D) 0.819 E) 0.476
Answer: C
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

25

 

92) A solution is prepared by dissolving 2.60 g of a strong electrolyte (formula weight = 101 g/mol) in 92)
enough water to make 1.00 L of solution. The osmotic pressure of the solution is 1.25 atm at 25.0 °C.
What is the van’t Hoff factor (i) for the unknown solute?
A) 0 B) 0.99 C) 1.98 D) 2.98 E) 0.630
Answer: C
Explanation: A)
B)
C)
D)
E)

 

93) On a clear day at sea level, with a temperature of 25 °C, the partial pressure of N2 in air is 0.78 atm 93) and the concentration of nitrogen in water is 5.3 × 104 M. When the partial pressure of N2 is

 

__________ atm, the concentration in water is 1.1 × 103 M.

A) 1.6 atm B) 0.78 atm C) 2.1 atm D) 0.63 atm E) 1.0 atm
Answer: A
Explanation: A)
B)
C)
D)
E)
94) Which one of the following vitamins is water soluble? 94)
A
B
K
D
E
A) A B) B C) K D) D E) E
Answer: B
Explanation: A)
B)
C)
D)
E)
95) George is making spaghetti for dinner. He places 4.01 kg of water in a pan and brings it to a boil. 95)
Before adding the pasta, he adds 58 g of table salt to the water and again brings it to a boil. The
temperature of the salty, boiling water is __________°C.
It is a nice day at sea level so that pressure is 1.00 atm. Assume negligible evaporation of water. Kb
for water is 0.52°C/m.
A) 100.13 B) 100.00 C) 100.26 D) 99.74 E) 99.87
Answer: C
Explanation: A)
B)
C)
D)
E)

 

 

 

26

 

96) The concentration of urea (MW = 60.0 g/mol) in a solution prepared by dissolving 16 g of urea in 39     96)

g of H2O is __________ molal.
A) 0.68 B) 0.11 C) 6.9 D) 96 E) 6.3
Answer: C
Explanation: A)
B)
C)
D)
E)

 

97) Pairs of liquids that will mix in all proportions are called __________ liquids. 97)
  1. A) miscible
  2. B) saturated
  3. C) unsaturated
  4. D) polar liquids
  5. E) supersaturated

 

Answer: A

Explanation:      A)

B)

C)

D)

E)

 

98) What is the molarity of sodium chloride in solution that is 13.0% by mass sodium chloride and that 98) has a density of 1.10 g/mL?

 

  1. 23
  2. 143
  3. 45
  4. 56
  5. 43 × 102

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

99) The molarity of urea in a solution prepared by dissolving 16 g of urea (MW = 60.0 g/mol) in 39 g of 99)
H2O is __________ M. The density of the solution is 1.3 g/mL.
A) 3.7 B) 6.8 C) 0.11 D) 6.3 E) 0.16
Answer: D
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

27

 

100) The solubility of oxygen gas in water at 25 °C and 1.0 atm pressure of oxygen is 0.041 g/L. The 100)
solubility of oxygen in water at 3.0 atm and 25 °C is __________ g/L.
A) 3.0 B) 0.12 C) 0.31 D) 0.014 E) 0.041
Answer: B
Explanation: A)
B)
C)
D)
E)
101) A solution is prepared by dissolving 15.0 g of NH3 in 250 g of water. The density of the resulting 101)
solution is 0.974 g/mL. The mole fraction of NH3 in the solution is __________.
A) 0.0597 B) 0.922 C) 0.940 D) 0.0640 E) 16.8
Answer: A
Explanation: A)
B)
C)
D)
E)
102) A 0.15 m aqueous solution of a weak acid has a freezing point of -0.31 °C. What is the percent 102)
ionization of this weak acid at this concentration? The molal freezing-point-depression constant of
water is 1.86 °C/m.
A) 35 B) 31 C) 89 D) 17 E) 11
Answer: E
Explanation: A)
B)
C)
D)
E)
103) Calculate the freezing point (0°C) of a 0.05500 m aqueous solution of glucose. The molal 103)
freezing-point-depression constant of water is 1.86 °C/m.
A) -0.05627 B) -0.2046 C) 0.1023 D) 0.0286 E) -0.1023
Answer: E
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

28

 

104) The process of solute particles being surrounded by solvent particles is known as __________. 104)
  1. A) agglomeration
  2. B) agglutination
  3. C) solvation
  4. D) dehydration
  5. E) salutation

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

 

  • The solubility of nitrogen gas in water at 25 °C and a nitrogen pressure of 1.0 atm is 6.9 × 104 The solubility of nitrogen in water at a nitrogen pressure of 0.80 atm is __________ M.
  1. A) 5 × 104 B) 1.2 × 103 C) 8.6 × 104               D) 0.80                           E) 3.7 × 103

Answer: A

Explanation:      A)

B)

C)

D)

E)

 

  • The concentration (M) of HCl in a solution prepared by dissolving 5.5 g of HCl in 200 g of C2H6O is __________ M. The density of the solution is 0.79 g/mL.
  1. A) 0.58 B) 21 C) 0.93                          D) 0 × 104               E) 1.72

Answer: A

Explanation:      A)

B)

C)

D)

E)

105)

 

 

 

 

 

 

 

 

 

 

 

 

106)

 

 

107) The concentration of sodium chloride in an aqueous solution that is 2.23 M and that has a density of   107)

1.01 g/mL is __________% by mass.
A) 45.3 B) 7.83 C) 12.9 D) 10.1 E) 2.21
Answer: C
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

 

 

 

 

29

 

  • An aqueous solution of a soluble compound (a nonelectrolyte) is prepared by dissolving 33.2 g of the compound in sufficient water to form 250 mL of solution. The solution has an osmotic pressure of 1.2 atm at 25 °C. What is the molar mass (g/mL) of the compound?
  1. A) 3 × 102 B) 1.0 × 103 C) 2.7 × 103                 D) 6.8 × 102                 E) 28

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

  • What is the freezing point (°C) of a solution prepared by dissolving 11.3 g of Ca(NO3)2

 

(formula weight = 164 g/mol) in 115 g of water? The molal freezing point depression constant for

 

water is 1.86 °C/m.

  1. A) -34 B) -1.11 C) 3.34                          D) 1.11                           E) 0.00

 

Answer: A

Explanation:      A)

B)

C)

D)

E)

108)

 

 

 

 

 

 

 

 

 

 

 

 

 

109)

 

 

110) The concentration of nitrate ion in a solution that contains 0.900 M aluminum nitrate is __________ 110)
M.
A) 1.80 B) 0.450 C) 0.300 D) 0.900 E) 2.70
Answer: E
Explanation: A)
B)
C)
D)
E)
111) The freezing point of ethanol (C2H5OH) is -114.6 °C. The molal freezing point depression constant 111)
for ethanol is 2.00 °C/m. What is the freezing point (°C) of a solution prepared by dissolving 50.0 g
of glycerin (C3H8O3, a nonelectrolyte) in 200 g of ethanol?
A) -5.42 B) -120.0 C) -115 D) -114.6 E) -132.3
Answer: B
Explanation: A)
B)
C)
D)
E)

 

 

 

 

 

 

 

 

 

 

 

 

 

30

 

  • A solution containing 10.0 g of an unknown liquid and 90.0 g water has a freezing point of -33 °C. 112) Given Kf = 1.86 °C/m for water, the molar mass of the unknown liquid is __________ g/mol.
A) 69.0 B) 161 C) 333 D) 619 E) 62.1
Answer: E
Explanation: A)
B)
C)
D)
E)
113) A solution is prepared by dissolving 23.7 g of CaCl2 in 375 g of water. The density of the resulting 113)
solution is 1.05 g/mL. The concentration of CaCl2 in this solution is __________ molal.
A) 5.70 B) 63.2 C) 1.76 D) 0.214 E) 0.569
Answer: E
Explanation: A)
B)
C)
D)
E)
114) The mole fraction of He in a gaseous solution prepared from 4.0 g of He, 6.5 g of Ar, and 10.0 g of 114)
Ne is __________.
A) 1.5 B) 0.61 C) 0.86 D) 0.11 E) 0.20
Answer: B
Explanation: A)
B)
C)
D)
E)
115) The vapor pressure of pure ethanol at 60 °C is 0.459 atm. Raoult’s Law predicts that a solution 115)
prepared by dissolving 10.0 mmol naphthalene (nonvolatile) in 90.0 mmol ethanol will have a
vapor pressure of __________ atm.
A) 0.367 B) 0.0918 C) 0.498 D) 0.790 E) 0.413
Answer: E
Explanation: A)
B)
C)

D)

E)

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

31

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

116) A sample of potassium nitrate (49.0 g) is dissolved in 101 g of water at 100 °C, with precautions 116)

taken to avoid evaporation of any water. The solution is cooled to 30.0 °C and a small amount of precipitate is observed. This solution is __________.

  1. A) hydrated
  2. B) unsaturated
  3. C) saturated
  4. D) placated
  5. E) supersaturated

 

Answer: C

Explanation:      A)

B)

C)

D)

E)

 

TRUE/FALSE. Write ‘T’ if the statement is true and ‘F’ if the statement is false.

117) The value of the boiling-point-elevation constant (Kb) depends on the identity of the solvent. 117)
Answer: True False
Explanation:
118) Adding solute to a solution decreases the vapor pressure of the solution. 118)
Answer: True False
Explanation:
119) After swimming in the ocean for several hours, swimmers noticed that their fingers appeared to be 119)
very wrinkled. This is an indication that seawater is supertonic relative to the fluid in cells.
Answer: True False

Explanation:

 

 

 

 

 

32

 

120) A solution with a solute concentration greater than the solubility is called a supercritical solution. 120)
Answer: True False
Explanation:
121) Emulsifying agents typically have a hydrophobic end and a hydrophilic end. 121)
Answer: True False

Explanation:

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

33

 

Answer Key

 

Testname: C13

 

 

 

  • C
  • A
  • B
  • B
  • B
  • B
  • E
  • E
  • C
  • C
  • D
  • B
  • A
  • E
  • C
  • A
  • B
  • C
  • D
  • A
  • A
  • E
  • B
  • E
  • A
  • B
  • E
  • B
  • D
  • C
  • B
  • D
  • C
  • D
  • E
  • A
  • D
  • A
  • C
  • D
  • B
  • C
  • C
  • E
  • B
  • E
  • D
  • A
  • E
  • D

 

 

34

 

Answer Key

 

Testname: C13

 

 

 

  • D
  • C
  • D
  • E
  • A
  • E
  • A
  • C
  • D
  • C
  • E
  • E
  • A
  • B
  • B
  • 0
  • hydrogen bonding

 

  • 91
  • 85
  • colligative
  • Tyndall
  • C
  • A
  • E
  • E
  • E
  • E
  • E
  • B
  • B
  • B
  • D
  • C
  • B
  • C
  • B
  • C
  • B
  • A
  • A
  • C
  • C
  • A
  • B
  • C
  • C
  • A
  • C
  • D
  • B

 

 

35

 

Answer Key

 

Testname: C13

 

 

 

  • A
  • E
  • E
  • C
  • A
  • A
  • C
  • C
  • A
  • E
  • B
  • E
  • E
  • B
  • E
  • C
  • TRUE
  • TRUE
  • FALSE
  • FALSE
  • TRUE

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

 

36

 

 

 

40