Answer at the bottom of the page
3.1 Multiple-Choice Questions
1) When the following equation is balanced, the coefficients are __________.
C8H18 + O2 → CO2 + H2O
A) 2, 3, 4, 4
B) 1, 4, 8, 9
C) 2, 12, 8, 9
D) 4, 4, 32, 36
E) 2, 25, 16, 18
2) Of the reactions below, which one is not a combination reaction?
A) C + O2 → CO2
B) 2Mg + O2 → 2MgO
C) 2N2 + 3H2 → 2NH3
D) CaO + H2O → Ca(OH)2
E) 2CH4 + 4O2 → 2CO2 + 4H2O
3) When a hydrocarbon burns in air, what component of air reacts?
A) oxygen
B) nitrogen
C) carbon dioxide
D) water
E) argon
4) When a hydrocarbon burns in air, a component produced is?
A) oxygen
B) nitrogen
C) carbon
D) water
E) argon
5) Of the reactions below, which one is a decomposition reaction?
A) NH4Cl → NH3 + HCl
B) 2Mg + O2 → 2MgO
C) 2N2 + 3 H2 → 2NH3
D) 2CH4 + 4O2 → 2CO2 + 4H2O
E) Cd(NO3)O2 + Na2S → CdS + 2NaNO3
6) Which one of the following substances is the product of this combination reaction?
Al (s) + I2 (s) → __________
A) AlI2
B) AlI
C) AlI3
D) Al2I3
E) Al3I2
7) Which one of the following is not true concerning automotive air bags?
A) They are inflated as a result of a decomposition reaction
B) They are loaded with sodium azide initially
C) The gas used for inflating them is oxygen
D) The two products of the decomposition reaction are sodium and nitrogen
E) A gas is produced when the air bag activates.
8) The reaction used to inflate automobile airbags __________.
A) produces sodium gas
B) is a combustion reaction
C) is a combination reaction
D) violates the law of conservation of mass
E) is a decomposition reaction
9) Which of the following are combination reactions?
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, and 3
B) 2 and 3
C) 1, 2, 3, and 4
D) 4 only
E) 2, 3, and 4
10) Which of the following are combustion reactions?
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) 1 and 4
B) 1, 2, 3, and 4
C) 1, 3, and 4
D) 2, 3, and 4
E) 3 and 4
11) Which of the following are decomposition reactions?
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, and 3
B) 4 only
C) 1, 2, 3, and 4
D) 2 and 3
E) 2, 3, and 4
12) The formula of nitrobenzene is C6H5N O2. The molecular weight of this compound is __________ amu.
A) 107.11
B) 43.03
C) 109.10
D) 123.11
E) 3.06
13) The formula weight of potassium dichromate (K2Cr2O7) is __________ amu.
A) 107.09
B) 255.08
C) 242.18
D) 294.18
E) 333.08
14) The formula weight of lead (II) carbonate (PbCO3) is __________ amu.
A) 207.2
B) 219.2
C) 235.2
D) 267.2
E) 273.2
15) The formula weight of potassium phosphate (K3PO4) is __________ amu.
A) 173.17
B) 251.37
C) 212.27
D) 196.27
E) 86.07
16) The formula weight of aluminum sulfate (Al2(SO4)3) is __________ amu.
A) 342.15
B) 123.04
C) 59.04
D) 150.14
E) 273.06
17) The formula weight of silver chromate (Ag2CrO4) is __________ amu.
A) 159.87
B) 223.87
C) 331.73
D) 339.86
E) 175.87
18) The formula weight of ammonium sulfate ((NH4)O2SO4), rounded to the nearest integer, is __________ amu.
A) 100
B) 118
C) 116
D) 132
E) 264
19) The molecular weight of the acetic acid (CH3CO2H), rounded to the nearest integer, is __________ amu.
A) 60
B) 48
C) 44
D) 32
20) The molecular weight of the ethanol (C2H5OH), rounded to the nearest integer, is __________ amu.
A) 34
B) 41
C) 30
D) 46
E) 92
21) The molecular weight of glucose (C6H12O6), rounded to the nearest integer, is __________ amu.
A) 24
B) 96
C) 136
D) 180
E) 224
22) What is the mass % of carbon in dimethylsulfoxide (C2H6SO) rounded to three significant figures?
A) 60.0
B) 20.6
C) 30.7
D) 7.74
E) 79.8
23) The mass % of H in methane (CH4) is __________.
A) 25.13
B) 4.032
C) 74.87
D) 92.26
E) 7.743
24) The mass % of Al in aluminum sulfate (Al2(SO4)3) is __________.
A) 7.886
B) 15.77
C) 21.93
D) 45.70
E) 35.94
25) The formula weight of a substance is __________.
A) identical to the molar mass
B) the same as the percent by mass weight
C) determined by combustion analysis
D) the sum of the atomic weights of each atom in its chemical formula
E) the weight of a sample of the substance
26) The formula weight of calcium nitrate (Ca(NO3)2), rounded to one decimal place, is __________ amu.
A) 102.1
B) 164.0
C) 204.2
D) 150.1
E) 116.1
27) The formula weight of magnesium fluoride (MgF2), rounded to one decimal place, is __________ amu.
A) 86.6
B) 43.3
C) 62.3
D) 67.6
E) 92.9
28) The formula weight of lead nitrate (Pb(NO3)2) is __________ amu.
A) 269.2
B) 285.2
C) 317.2
D) 331.2
E) 538.4
29) The mass % of C in methane (CH4) is __________.
A) 25.13
B) 133.6
C) 74.87
D) 92.26
E) 7.743
30) The mass % of F in the binary compound KrF2 is __________.
A) 18.48
B) 45.38
C) 68.80
D) 81.52
E) 31.20
31) Calculate the percentage by mass of nitrogen in PtCl2(NH3)2.
A) 4.67
B) 9.34
C) 9.90
D) 4.95
E) 12.67
32) Calculate the percentage by mass of lead in Pb(NO3)2.
A) 38.6
B) 44.5
C) 62.6
D) 65.3
E) 71.2
33) Calculate the percentage by mass of nitrogen in Pb(NO3)2.
A) 4.2
B) 5.2
C) 8.5
D) 10.4
E) 12.6
34) Calculate the percentage by mass of lead in PbCO3.
A) 17.96
B) 22.46
C) 73.05
D) 77.54
E) 89.22
35) Calculate the percentage by mass of oxygen in Pb(NO3)2.
A) 9.7
B) 14.5
C) 19.3
D) 29.0
E) 33.4
36) Calculate the percentage by mass of chlorine in PtCl2(NH3)2.
A) 23.63
B) 11.82
C) 25.05
D) 12.53
E) 18.09
37) Calculate the percentage by mass of hydrogen in PtCl2(N H3)2
A) 1.558
B) 1.008
C) 0.672
D) 0.034
E) 2.016
38) One mole of __________ contains the largest number of atoms.
A) S8
B) C10H8
C) Al2(SO4)3
D) Na3PO4
E) Cl2
39) One mole of __________ contains the smallest number of atoms.
A) S8
B) C10H8
C) Al2(SO4)3
D) Na3PO4
E) NaCl
40) One million argon atoms is __________ mol (rounded to two significant figures) of argon atoms.
A) 3.0
B) 1.7 × 10-18
C) 6.0 × 1023
D) 1.0 × 10-6
E) 1.0 × 10+6
41) There are __________ atoms of oxygen are in 300 molecules of CH3CO2H.
A) 300
B) 600
C) 3.01 × 1024
D) 3.61 × 1026
E) 1.80 × 1026
42) How many molecules of CH4 are in 48.2 g of this compound?
A) 5.00 × 1024
B) 3.00
C) 2.90 × 1025
D) 1.81 × 1024
E) 4.00
43) A 30.5 gram sample of glucose (C6H12O6) contains __________ mol of glucose.
A) 0.424
B) 0.169
C) 5.90
D) 2.36
E) 0.136
44) A 30.5 gram sample of glucose (C6H12O6) contains __________ atoms of carbon.
A) 1.02 x 1023
B) 6.12 x 1023
C) 6.02 x 1023
D) 2.04 x 1023
E) 1.22 x 1024
45) A sample of CH2F2 with a mass of 19 g contains __________ atoms of F.
A) 2.2 × 1023
B) 38
C) 3.3 × 1024
D) 4.4 × 1023
E) 9.5
46) A sample of CH4O with a mass of 32.0 g contains __________ molecules of CH4O.
A) 5.32 × 10-23
B) 1.00
C) 1.88 × 1022
D) 6.02 × 1023
E) 32.0
47) How many atoms of nitrogen are in 10 g of NH4NO3?
A) 3.5
B) 1.5 × 1023
C) 3.0 × 1023
D) 1.8
E) 2
48) Gaseous argon has a density of 1.40 g/L at standard conditions. How many argon atoms are in 1.00 L of argon gas at standard conditions?
A) 4.76 × 1022
B) 3.43 × 1026
C) 2.11 × 1022
D) 1.59 × 1025
E) 6.02 × 1023
49) What is the mass in grams of 9.76 × 1012 atoms of naturally occurring sodium?
A) 22.99
B) 1.62 × 10-11
C) 3.73 × 10-10
D) 7.05 × 10-13
E) 2.24 × 1014
50) How many moles of pyridine (C5H5N) are contained in 3.13 g of pyridine?
A) 0.0396
B) 25.3
C) 0.319
D) 0.00404
E) 4.04 × 103
51) How many oxygen atoms are contained in 2.74 g of Al2(SO4)3?
A) 12
B) 6.02 × 1023
C) 7.22 × 1024
D) 5.79 × 1022
E) 8.01 × 10-3
52) The total number of atoms in 0.111 mol of Fe(CO)3(PH3)2 is __________.
A) 15.0
B) 1.00 × 1024
C) 4.46 × 1021
D) 1.67
E) 2.76 × 10-24
53) How many sulfur dioxide molecules are there in 1.80 mol of sulfur dioxide?
A) 1.08 × 1023
B) 6.02 × 1024
C) 1.80 × 1024
D) 1.08 × 1024
E) 6.02 × 1023
54) How many sulfur dioxide molecules are there in 0.180 mol of sulfur dioxide?
A) 1.80 × 1023
B) 6.02 × 1024
C) 6.02 × 1023
D) 1.08 × 1024
E) 1.08 × 1023
55) How many carbon atoms are there in 52.06 g of carbon dioxide?
A) 5.206 × 1024
B) 3.134 × 1025
C) 7.122 × 1023
D) 8.648 × 10-23
E) 1.424 × 1024
56) How many oxygen atoms are there in 52.06 g of carbon dioxide?
A) 1.424 × 1024
B) 6.022 × 1023
C) 1.204 × 1024
D) 5.088 × 1023
E) 1.018 × 1024
57) How many moles of sodium carbonate contain 1.773 × 1017 carbon atoms?
A) 5.890 × 10-7
B) 2.945 × 10-7
C) 1.473 × 10-7
D) 8.836 × 10-7
E) 9.817 × 10-8
58) How many grams of sodium carbonate contain 1.773 × 1017 carbon atoms?
A) 3.121 × 10-5
B) 1.011 × 10-5
C) 1.517 × 10-5
D) 9.100 × 10-5
E) 6.066 × 10-5
59) The compound responsible for the characteristic smell of garlic is allicin, C6H10OS2. The mass of 1.00 mol of allicin, rounded to the nearest integer, is __________ g.
A) 34
B) 162
C) 86
D) 61
E) 19
60) The molecular formula of aspartame, the generic name of NutraSweet®, is C14H18N2O5. The molar mass of aspartame, rounded to the nearest integer, is __________ g.
A) 24
B) 156
C) 294
D) 43
E) 39
61) There are ________ oxygen atoms in 30 molecules of C20H42S3O2.
A) 6.0 x 1023
B) 1.8 x 1025
C) 3.6 x 1025
D) 1.2 x 1024
E) 60
62) A nitrogen oxide is 63.65% by mass nitrogen. The molecular formula could be __________.
A) NO
B) NO2
C) N2O
D) N2O4
E) either NO2 or N2O4
63) A sulfur oxide is 50.0% by mass sulfur. This molecular formula could be __________.
A) SO
B) SO2
C) S2O
D) S2O4
E) either SO2 or S2O4
64) Which hydrocarbon pair below have identical mass percentage of C?
A) C3H4 and C3H6
B) C2H4 and C3H4
C) C2H4 and C4H2
D) C2H4 and C3H6
E) none of the above
65) Sulfur and oxygen react to produce sulfur trioxide. In a particular experiment, 7.9 grams of SO3 are produced by the reaction of 5.0 grams of O2 with 6.0 grams of S. What is the % yield of SO3 in this experiment?
S (s) + O2 (g) → SO3 (g) (not balanced)
A) 32
B) 63
C) 75
D) 95
E) 99
66) Propane (C3H8) reacts with oxygen in the air to produce carbon dioxide and water. In a particular experiment, 38.0 grams of carbon dioxide are produced from the reaction of 22.05 grams of propane with excess oxygen. What is the % yield in this reaction?
A) 38.0
B) 57.6
C) 66.0
D) 86.4
E) 94.5
3.2 Bimodal Questions
1) When the following equation is balanced, the coefficients are __________.
NH3 (g) + O2 (g) → NO2 (g) + H2O (g)
A) 1, 1, 1, 1
B) 4, 7, 4, 6
C) 2, 3, 2, 3
D) 1, 3, 1, 2
E) 4, 3, 4, 3
2) When the following equation is balanced, the coefficients are __________.
Al(NO3)3 + Na2S → Al2S3 + NaNO3
A) 2, 3, 1, 6
B) 2, 1, 3, 2
C) 1, 1, 1, 1
D) 4, 6, 3, 2
E) 2, 3, 2, 3
3) When the following equation is balanced, the coefficient of H2 is __________.
K (s) + H2O (l) → KOH (aq) + H2 (g)
A) 1
B) 2
C) 3
D) 4
E) 5
4) When the following equation is balanced, the coefficient of Al is __________.
Al (s) + H2O (l) → Al(OH)3 (s) + H2 (g)
A) 1
B) 2
C) 3
D) 5
E) 4
5) When the following equation is balanced, the coefficient of H2O is __________.
Ca (s) + H2O (l) → Ca(OH)2 (aq) + H2 (g)
A) 1
B) 2
C) 3
D) 5
E) 4
6) When the following equation is balanced, the coefficient of Al2O3 is __________.
Al2O3 (s) + C (s) + Cl2 (g) → AlCl3 (s) + CO (g)
A) 1
B) 2
C) 3
D) 4
E) 5
7) When the following equation is balanced, the coefficient of H2S is __________.
FeCl3 (aq) + H2S (g) → Fe2S3 (s) + HCl (aq)
A) 1
B) 2
C) 3
D) 5
E) 4
8) When the following equation is balanced, the coefficient of HCl is __________.
CaCO3 (s) + HCl (aq) → CaCl2 (aq) + CO2 (g) + H2O (l)
A) 1
B) 2
C) 3
D) 4
E) 0
9) When the following equation is balanced, the coefficient of HNO3 is __________.
HNO3 (aq) + CaCO3 (s) → Ca(NO3)2 (aq) + CO2 (g) + H2O (l)
A) 1
B) 2
C) 3
D) 5
E) 4
10) When the following equation is balanced, the coefficient of H3PO4 is __________.
H3PO4 (aq) + NaOH (aq) → Na3PO4 (aq) + H2O (l)
A) 1
B) 2
C) 3
D) 4
E) 0
11) When the following equation is balanced, the coefficient of C3H8O3 is __________.
C3H8O3 (g) + O2 (g) → CO2 (g) + H2O (g)
A) 1
B) 2
C) 3
D) 7
E) 5
12) When the following equation is balanced, the coefficient of O2 is __________.
C2H4O (g) + O2 (g) → CO2 (g) + H2O (g)
A) 2
B) 3
C) 4
D) 5
E) 1
13) When the following equation is balanced, the coefficient of H2 is __________.
CO (g) + H2 (g) → H2O (g) + CH4 (g)
A) 1
B) 2
C) 3
D) 4
E) 0
14) When the following equation is balanced, the coefficient of H2SO4 is __________.
H2SO4 (aq) + NaOH (aq) → Na2SO4 (aq) + H2O (l)
A) 1
B) 2
C) 3
D) 4
E) 0.5
15) When the following equation is balanced, the coefficient of water is __________.
K (s) + H2O (l) → KOH (aq) + H2 (g)
A) 1
B) 2
C) 3
D) 4
E) 5
16) When the following equation is balanced, the coefficient of hydrogen is __________.
K (s) + H2O (l) → KOH (aq) + H2 (g)
A) 1
B) 2
C) 3
D) 4
E) 5
17) When the following equation is balanced, the coefficient of oxygen is __________.
PbS (s) + O2 (g) → PbO (s) + SO2 (g)
A) 1
B) 3
C) 2
D) 4
E) 5
18) When the following equation is balanced, the coefficient of sulfur dioxide is __________.
PbS (s) + O2 (g) → PbO (s) + SO2 (g)
A) 5
B) 1
C) 3
D) 2
E) 4
19) When the following equation is balanced, the coefficient of dinitrogen pentoxide is __________.
N2O5 (g) + H2O (l) → HNO3 (aq)
A) 1
B) 2
C) 3
D) 4
E) 5
20) When the following equation is balanced, the coefficient of water is __________.
N2O5 (g) + H2O (l) → HNO3 (aq)
A) 5
B) 2
C) 3
D) 4
E) 1
21) When the following equation is balanced, the coefficient of nitric acid is __________.
N2O5 (g) + H2O (l) → HNO3 (aq)
A) 5
B) 2
C) 3
D) 4
E) 1
22) Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in air. What is the coefficient of methanol in the balanced equation?
A) 1
B) 2
C) 3
D) 4
E) 3/2
23) Write the balanced equation for the reaction that occurs when methanol, CH3OH (l), is burned in air. What is the coefficient of oxygen in the balanced equation?
A) 1
B) 2
C) 3
D) 4
E) 3/2
24) What is the coefficient of O2 when the following equation is completed and balanced?
C4H8O2 + O2 → __________
A) 2
B) 3
C) 5
D) 6
E) 1
25) Predict the product in the combination reaction below.
Al (s) + N2 (g) → __________
A) AlN
B) Al3N
C) Al N2
D) Al3N2
E) AlN3
26) The balanced equation for the decomposition of sodium azide is __________.
A) 2NaN3 (s) → 2Na (s) + 3 N2 (g)
B) 2NaN3 (s) → Na2 (s) + 3 N2 (g)
C) NaN3 (s) → Na (s) + N2 (g)
D) NaN3 (s) → Na (s) + N2 (g) + N (g)
E) 2NaN3 (s) → 2Na (s) + 2 N2 (g)
27) There are __________ mol of carbon atoms in 4 mol C4H8O2.
A) 4
B) 8
C) 16
D) 20
E) 32
28) There are __________ sulfur atoms in 25 molecules of C4H4S2.
A) 1.5 × 1025
B) 4.8 × 1025
C) 3.0 × 1025
D) 50
E) 6.02 × 1023
29) There are __________ hydrogen atoms in 25 molecules of C4H4S2.
A) 25
B) 3.8 × 1024
C) 6.0 × 1025
D) 100
E) 1.5 × 1025
30) A sample of C3H8O that contains 200 molecules contains __________ carbon atoms.
A) 600
B) 200
C) 3.61 × 1026
D) 1.20 × 1026
E) 4.01 × 1025
31) How many moles of carbon monoxide are there in 36.55 g of carbon monoxide?
A) 0.8452
B) 1.305
C) 0.9291
D) 2.589
E) 3.046
32) How many moles of carbon dioxide are there in 52.06 g of carbon dioxide?
A) 0.8452
B) 1.183
C) 6.022 × 1023
D) 8.648 × 1023
E) 3.134 × 1025
33) There are __________ molecules of methane in 0.123 mol of methane (CH4).
A) 5
B) 2.46 × 10-2
C) 2.04 × 10-25
D) 7.40 × 1022
E) 0.615
34) What is the empirical formula of a compound that contains 27.0% S, 13.4% O, and 59.6% Cl by mass?
A) SOCl
B) SOCl2
C) S2OCl
D) SO2Cl
E) ClSO4
35) What is the empirical formula of a compound that contains 29% Na, 41% S, and 30% O by mass?
A) Na2S2O3
B) NaSO2
C) NaSO
D) NaSO34
E) Na2S2O6
36) What is the empirical formula of a compound that contains 49.4% K, 20.3% S, and 30.3% O by mass?
A) KSO2
B) KSO3
C) K2SO4
D) K2O3
E) KSO4
37) A compound contains 40.0% C, 6.71% H, and 53.29% O by mass. The molecular weight of the compound is 60.05 amu. The molecular formula of this compound is __________.
A) C2H4O2
B) C H2O
C) C2H3O4
D) C2H2O4
E) CHO2
38) A compound that is composed of carbon, hydrogen, and oxygen contains 70.6% C, 5.9% H, and 23.5% O by mass. The molecular weight of the compound is 136 amu. What is the molecular formula?
A) C8H8O2
B) C8H4O
C) C4H4O
D) C9H12O
E) C5H6O2
39) A compound that is composed of only carbon and hydrogen contains 85.7% C and 14.3% H by mass. What is the empirical formula of the compound?
A) CH2
B) C2H4
C) C H42
D) C4H8
E) C86H14
40) A compound that is composed of only carbon and hydrogen contains 80.0% C and 20.0% H by mass. What is the empirical formula of the compound?
A) C20H60
B) C7H20
C) C H3
D) C2H6
E) CH4
41) A compound contains 38.7% K, 13.9% N, and 47.4% O by mass. What is the empirical formula of the compound?
A) KNO3
B) K2N2O3
C) KNO2
D) K2NO3
E) K4NO5
42) A compound is composed of only C, H, and O. The combustion of a 0.519-g sample of the compound yields 1.24 g of CO2 and 0.255 g of H2O. What is the empirical formula of the compound?
A) C6H6O
B) C3H3O
C) CH3O
D) C2H6O5
E) C2H6O2
43) Combustion of a 1.031-g sample of a compound containing only carbon, hydrogen, and oxygen produced 2.265 g of CO2 and 1.236 g of H2O. What is the empirical formula of the compound?
A) C3H8O
B) C3H5O
C) C6H16O2
D) C3H9O3
E) C3H6O3
44) Combustion of a 0.9835-g sample of a compound containing only carbon, hydrogen, and oxygen produced 1.900 g of CO2 and 1.070 g of H2O. What is the empirical formula of the compound?
A) C2 H5O
B) C4 H10O2
C) C4 H11O2
D) C4 H10O
E) C2 H5O2
45) The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O:
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) 119
D) 0.954
E) 43.9
46) The combustion of propane (C3H8) in the presence of excess oxygen yields CO2 and H2O:
C3H8 (g) + 5 O2 (g) → 3CO2 (g) + 4 H2O (g)
When 2.5 mol of O2 are consumed in their reaction, __________ mol of CO2 are produced.
A) 1.5
B) 3.0
C) 5.0
D) 6.0
E) 2.5
47) Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2):
CaC2 (s) + 2 H2O (g) → Ca(OH)2 (s) + C2H2 (g)
Production of 13 g of C2H2 requires consumption of __________ g of H2O.
A) 4.5
B) 9.0
C) 18
D) 4.8 × 102
E) 4.8 × 10-2
48) Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2):
CaC2 (s) + 2 H2O (g) → Ca(OH)2 (s) + C2H2 (g)
The complete reaction of 57.4 g of CaC2 requires consumption of __________ g of H2O.
A) 0.895
B) 64.1
C) 32.3
D) 1.79
E) 18.0
49) Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia:
N2 (g) + 3 H2 (g) → 2NH3 (g)
A 7.1-g sample of N2 requires __________ g of H2 for complete reaction.
A) 0.51
B) 0.76
C) 1.2
D) 1.5
E) 17.2
50) Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia:
N2 (g) + 3 H2 (g) → 2NH3 (g)
A __________ g sample of N2 requires 3.0 g of H2 for complete reaction.
A) 0.51
B) 0.76
C) 1.2
D) 14.0
E) 17.2
51) Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide:
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) 0.41
B) 2.50
C) 0.00936
D) 2.09
E) 2.61
52) The combustion of propane (C3H8) produces CO2 and H2O:
C3H8 (g) + 5 O2 (g) → 3CO2 (g) + 4 H2O (g)
The reaction of 2.5 mol of O2 with 4.6 mol of C3H8 will produce __________ mol of H2O.
A) 4.0
B) 3.0
C) 2.5
D) 2.0
E) 1.0
53) GeF3H is formed from GeH4 and GeF4 in the combination reaction:
GeH4 + 3Ge F4 → 4GeF3H
If the reaction yield is 92.6%, how many moles of GeF4 are needed to produce 8.00 mol of GeF3H?
A) 3.24
B) 5.56
C) 6.48
D) 2.78
E) 2.16
54) Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia:
N2 (g) + 3 H2 (g) → 2NH3 (g)
If the reaction yield is 87.5%, how many moles of N2 are needed to produce 3.00 mol of NH3?.
A) 0.166
B) 1.00
C) 1.5
D) 1.71
E) 2.32
55) Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide:
PbCO3 (s) → PbO (s) + CO2 (g)
If the reaction yield is 95.7%, how many grams of lead (II) oxide will be produced by the decomposition of 2.50 g of lead (II) carbonate?
A) 1.04
B) 1.55
C) 2.09
D) 4.00
E) 5.55
56) The combustion of ammonia in the presence of oxygen yields NO2 and H2O:
4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g)
The combustion of 43.9 g of ammonia with 258 g of oxygen produces __________ g of NO2.
A) 212
B) 178
C) 119
D) 0.954
E) 43.9
57) What mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water?
Mg (s) + 2 H2O (l) → Mg(OH)2 (s) + H2 (g)
A) 0.102
B) 0.0162
C) 0.0485
D) 0.219
E) 0.204
58) If the reaction yield is 94.4%, what mass in grams of hydrogen is produced by the reaction of 4.73 g of magnesium with 1.83 g of water?
Mg (s) + 2 H2O (l) → Mg(OH)2 (s) + H2 (g)
A) 0.0962
B) 0.0162
C) 0.0485
D) 0.219
E) 0.204
59) Silver nitrate and aluminum chloride react with each other by exchanging anions:
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) 17.6
B) 4.22
C) 24.9
D) 3.56
E) 11.9
60) How many moles of magnesium oxide are produced by the reaction of 3.82 g of magnesium nitride with 7.73 g of water?
Mg3N2 + 3 H2O → 2NH3 + 3MgO
A) 0.114
B) 0.0378
C) 0.429
D) 0.0756
E) 4.57
61) A 3.82-g sample of magnesium nitride is reacted with 7.73 g of water.
Mg3N2 + 3 H2O → 2NH3 + 3MgO
The yield of MgO is 3.60 g. What is the percent yield in the reaction?
A) 94.5
B) 78.4
C) 46.6
D) 49.4
E) 99.9
62) Pentacarbonyliron (Fe(CO)5) reacts with phosphorous trifluoride (PF3) and hydrogen, releasing 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 PF3and 6.0 mol of H2 will release __________ mol of CO.
A) 15
B) 5.0
C) 24
D) 6.0
E) 12
63) What is the maximum mass in grams of NH3 that can be produced by the reaction of 1.0 g of N2 with 3.0 g of H2 via the equation below?
N2 (g) + H2 (g) → NH3 (g) (not balanced)
A) 2.0
B) 1.2
C) 0.61
D) 17
E) 4.0
64) What is the maximum amount in grams of SO3 that can be produced by the reaction of 1.0 g of S with 1.0 g of O2 via the equation below?
S (s) + O2 (g) → SO3 (g) (not balanced)
A) 0.27
B) 1.7
C) 2.5
D) 3.8
E) 2.0
65) Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide:
4Al (s) + 3 O2 (g) → 2 Al2O3 (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) 9.4
B) 7.4
C) 4.7
D) 5.3
E) 5.0
66) Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride:
S (s) + 3 F3 (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) 12
B) 3.2
C) 5.8
D) 16
E) 8.0
67) Solid aluminum and gaseous oxygen react in a combination reaction to produce aluminum oxide:
4Al (s) + 3 O2 (g) → 2 Al2O3 (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) 74
B) 37
C) 47
D) 66
E) 26
68) Sulfur and oxygen react in a combination reaction to produce sulfur trioxide, an environmental 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) 30
B) 29
C) 21
D) 88
E) 48
69) Sulfur and fluorine react in a combination reaction to produce sulfur hexafluoride:
S (s) + 3F2 (g) → SF6 (g)
In a particular experiment, the percent yield is 79.0%. This means that in this experiment, a 7.90-g sample of fluorine yields __________ g of SF6.
A) 30.3
B) 10.1
C) 7.99
D) 24.0
E) 0.110
3.3 Algorithmic Questions
1) The molecular weight of acetic acid ( HC2H3O2), the acid in vinegar, is __________ amu (rounded to one decimal place).
A) 59.0
B) 29.0
C) 60.1
D) 8.0
E) 32.0
2) Determine the mass percent (to the hundredths place) of Na in sodium bicarbonate (NaHCO3).
3) There are __________ mol of carbon atoms in 3 mol of dimethylsulfoxide (C2H6SO).
A) 2
B) 4
C) 6
D) 8
E) 10
4) How many grams of hydrogen are in 23 g of CH4O?
A) 2.9
B) 4.6
C) 2.3
D) 4.0
E) 5.8
5) How many grams of oxygen are in 45 g of C2H2O2?
A) 8.3
B) 9.3
C) 17
D) 25
E) 31
6) A 3.92-g sample of magnesium nitrate, Mg(NO3)2, contains __________ mol of this compound.
A) 2.32
B) 1.65
C) 0.111
D) 0.0529
E) 0.0264
7) A 17.6-g sample of ammonium carbonate contains __________ mol of ammonium ions.
A) 0.366
B) 0.183
C) 0.176
D) 2.14
E) 3.47
8) What is the empirical formula of a compound that is 52.1% C, 13.1% H, and 34.7% O by mass?
A) C2HO
B) C2HO3
C) C4H12O2
D) C4H13O2
E) C2H6O
9) A certain alcohol contains only three elements, carbon, hydrogen, and oxygen. Combustion of a 30.00 gram sample of the alcohol produced 57.30 grams of CO2 and 35.22 grams of H2O. What is the empirical formula of the alcohol?
10) Lithium and nitrogen react to produce lithium nitride:
6Li (s) + N2 (g) → 2Li3N (s)
How many moles of N2 are needed to react with 0.710 mol of lithium?
A) 4.26
B) 0.710
C) 0.237
D) 2.13
E) 0.118
11) The combustion of propane (C3H8) produces CO2 and H2O:
C3H8 (g) + 5 O2 (g) → 3CO2 (g) + 4 H2O (g)
The reaction of 5.5 mol of O2 will produce __________ mol of H2O.
A) 5.5
B) 5.0
C) 2.0
D) 4.4
E) 1.0
12) Magnesium and nitrogen react in a combination reaction to produce magnesium nitride:
3 Mg + N2 → Mg3N2
In a particular experiment, a 10.1-g sample of N2 reacts completely. The mass of Mg consumed is __________ g.
A) 8.76
B) 26.3
C) 35.1
D) 0.92
E) 13.9
13) The combustion of ammonia in the presence of excess oxygen yields NO2 and H2O:
4 NH3 (g) + 7 O2 (g) → 4 NO2 (g) + 6 H2O (g)
The combustion of 57.6 g of ammonia consumes __________ g of oxygen.
A) 27.0
B) 28.8
C) 54.1
D) 189
E) 94.6
14) Lithium and nitrogen react to produce lithium nitride:
6Li (s) + N2 (g) → 2Li3N (s)
How many moles of lithium nitride are produced when 0.400 mol of lithium react in this fashion?
A) 0.133
B) 0.800
C) 0.0667
D) 1.20
E) 0.200
15) Lithium and nitrogen react in a combination reaction to produce lithium nitride:
6Li (s) + N2 (g) → 2Li3N (s)
How many moles of lithium are needed to produce 0.20 mol of Li3N when the reaction is carried out in the presence of excess nitrogen?
A) 0.10
B) 0.60
C) 0.067
D) 0.13
E) 1.2
16) Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements:
2NaN3 (s) → 2Na (s) + 3N2 (g)
How many moles of H2 are produced by the decomposition of 3.55 mol of sodium azide?
A) 2.37
B) 10.7
C) 5.33
D) 1.18
E) 1.78
17) Automotive air bags inflate when sodium azide decomposes explosively to its constituent elements:
2NaN3 (s) → 2Na (s) + 3N2 (g)
How many grams of sodium azide are required to produce 30.5 g of nitrogen?
A) 1.63
B) 0.726
C) 70.8
D) 47.2
E) 106.2
18) Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:
2Mg (s) + O2 (g) → 2MgO (s)
How many moles of O2 are consumed when 4.11 mol of magnesium burns?
A) 0.169
B) 0.487
C) 4.11
D) 8.22
E) 2.06
19) Calcium carbide (CaC2) reacts with water to produce acetylene (C2H2):
CaC2 (s) + 2 H2O (g) → Ca(OH)2 (s) + C2H2 (g)
Production of 3.3 g of C2H2 requires consumption of __________ g of H2O.
A) 1.2
B) 2.3
C) 4.6
D) 480
E) 0.048
20) Lead (II) carbonate decomposes to give lead (II) oxide and carbon dioxide:
PbCO3 (s) → PbO (s) + CO2 (g)
__________ grams of lead (II) oxide will be produced by the decomposition of 7.50 g of lead (II) carbonate?
A) 0.41
B) 2.50
C) 0.00936
D) 6.26
E) 7.83
21) Lithium and nitrogen react in a combination reaction to produce lithium nitride:
6Li (s) + N2 (g) → 2Li3N (s)
In a particular experiment, 5.50-g samples of each reagent are reacted. The theoretical yield of lithium nitride is __________ g.
A) 5.53
B) 4.60
C) 27.6
D) 9.20
E) 13.7
22) Magnesium burns in air with a dazzling brilliance to produce magnesium oxide:
2Mg (s) + O2 (g) → 2MgO (s)
When 2.00 g of magnesium burns, the theoretical yield of magnesium oxide is __________ g.
A) 2.00
B) 3.32
C) 0.0823
D) 1.66
E) 6.63
23) Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:
CaO (s) + H2O (l) → Ca(OH)2 (s)
A 4.00-g sample of CaO is reacted with 3.86 g of H2O. How many grams of water remains after completion of reaction?
A) 0.00
B) 0.00793
C) 2.57
D) 1.04
E) 0.143
24) If 2352 grams of FeS2 is allowed to react with 1408 grams of O2 according to the following equation, how many grams of Fe2O3 are produced?
FeS2 + O2 → Fe2O3 + SO2
25) Calcium oxide reacts with water in a combination reaction to produce calcium hydroxide:
CaO (s) + H2O (l) → Ca(OH)2 (s)
In a particular experiment, a 1.50-g sample of CaO is reacted with excess water and 1.48 g of Ca(OH)2 is recovered. What is the percent yield in this experiment?
A) 99
B) 0.99
C) 2.16
D) 74.8
E) 101.2
3.4 Short Answer Questions
1) Complete and balance the following reaction, given that elemental rubidium reacts with elemental sulfur to form Rb2S (s).
Na (s) + S (s) → __________
2) A compound was found to contain 90.6% lead (Pb) and 9.4% oxygen. The empirical formula for this compound is __________.
3) The combustion of propane (C3H8 ) in the presence of excess oxygen yields CO2 and H2O:
C3H8 (g) + 5O2 (g) → 3CO2 (g) + 4 H2O (g)
When 7.3 g of C3H8 burns in the presence of excess O2, __________ g of CO2 is produced.
4) Under appropriate conditions, nitrogen and hydrogen undergo a combination reaction to yield ammonia:
N2 (g) + 3 H2 (g) → 2NH3 (g)
A 9.3-g sample of hydrogen requires __________ g of N2 for a complete reaction.
5) Water can be formed from the stoichiometric reaction of hydrogen with oxygen:
2 H2 (g) + O2 (g) → 2 H2O (g)
A complete reaction of 5.0 g of O2 with excess hydrogen produces __________ g of H2O.
6) The combustion of carbon disulfide in the presence of excess oxygen yields carbon dioxide 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.
3.5 True/False Questions
1) The mass of a single atom of an element (in amu) is numerically EQUAL to the mass in grams of 1 mole of that element.
2) The molecular weight is ALWAYS a whole-number multiple of the empirical formula weight.
3) A great deal of the carbon dioxide produced by the combustion of fossil fuels is absorbed into the oceans.
4) The quantity of product that is calculated to form when all of the limiting reagent reacts is called the actual yield.
Answer:
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