Quantitative Composition – Ch7 Test Bank | 15th - Test Bank | Foundations of College Chemistry 15e by Hein Arena by Hein Arena, Willard. DOCX document preview.
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Hein Test Bank
Course title: Hein 15e
Chapter Number: 7
Question type: Multiple Choice
1) What is the mass of 1.000 mol of HCl?
a) 1.01 g
b) 6 
1023 g
c) 35.45 g
d) 36.46 g
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
2) What is the mass of 0.360 mol of HCl?
a) 0.360 g
b) 13.1 g
c) 101 g
d) 2.17 
1023 g
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
3) What is the mass of 3.61 mol of Ca2O?
a) 3.61 g
b) 26.6 g
c) 21.7 
1023 g
d) 347 g
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
4) What is the mass of 1.80 mol of Al(NO3)3?
a) 383 g
b) 272 g
c) 257 g
d) 161 g
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
5) What is the molar mass of NaCl?
a) 58.5 g
b) 6.023 1023 g
c) 23 g
d) 35.5 g
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
6) How many total atoms are present in 1.00 mol of Al2(SO4)3?
a) 6.02 × 1023 atoms
b) 1.20 × 1024 atoms
c) 9.03 × 1024 atoms
d) 1.02 × 1025 atoms
Difficulty; hard
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
7) How many O atoms are present in 1.04 mol of MgSO4?
a) 1.04 
1023 atoms
b) 4.16 
1023 atoms
c) 2.51 
1024 atoms
d) 6.26 
1023 atoms
Difficulty: hard
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
8) How many moles are present in a sample of HCl with a mass of 3.65 g?
a) 3.46 mol
b) 0.100 mol
c) 2.19 
1024 mol
d) 10.0 mol
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
9) How many moles are present in 140. g of CaCl2?
a) 15500 mol
b) 1.46 mol
c) 1.26 mol
d) 0.793 mol
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
10) How many moles of fluoride ions are present in 10.4 g of NaF?
a) 0.247 mol
b) 6.26 1024 mol
c) 6.26 mol
d) 437 mol
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
11) How many total atoms are present in 0.140 g of HCl?
a) 2.31 1021 atoms
b) 4.62 1021 atoms
c) 4.57 1022 atoms
d) 1.20 1024 atoms
Difficulty: hard
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
12) How many moles of silver ions are present in 32.46 g of AgNO3?
a) 0.191 mol
b) 5520 mol
c) 5.23 mol
d) 32.5 mol
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
13) How many moles of magnesium ions are present in 1.64 g of MgSO4?
a) 0.734 mol
b) 1.64 mol
c) 120. mol
d) 0.0136 mol
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
14) How many moles of chloride ions are present in 18.4 g of CaCl2?
a) 0.332 mol
b) 0.166 mol
c) 6.03 mol
d) 184 mol
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
15) How many formula units of MgSO4 are present in 18.0 g of this compound?
a) 6.02 
1023 formula units
b) 3.60 
10–21 formula units
c) 4.03 
1024 formula units
d) 9.00 
1022 formula units
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
16) How many formula units of AgNO3 are present in 1.36 g of this compound?
a) 3.84 × 10–22 formula units
b) 4.82 × 1021 formula units
c) 1.36 × 1023 formula units
d) 7.52 × 1025 formula units
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
17) How many total ions are present in 347 g of CaCl2?
a) 1.88 × 1024 ions
b) 5.65 × 1024 ions
c) 3.77 × 1024 ions
d) 4.87 × 1024 ions
Difficulty: hard
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
18) How many molecules are present in 0.340 g of HCl?
a) 1.78 
10–22 molecules
b) 6.46 
1025 molecules
c) 5.61 
1021 molecules
d) 2.06 
10–23 molecules
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
19) How many formula units of AgNO3 are present in 147 g of this compound?
a) 4.15 
10–20 formula units
b) 5.21 
1023 formula units
c) 1.47 
1021 formula units
d) 6.96 
1023 formula units
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
20) How many moles of atoms are present in 154 g of HCl?
a) 4.22 mol
b) 8.45 mol
c) 2.00 mol
d) 0.0270 mol
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
21) How many formula units of NaCl are present in 351 g of this compound?
a) 2.15 10–20 formula units
b) 3.61 1024 formula units
c) 1.00 1023 formula units
d) 1.96 1024 formula units
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
22) What is the mass of 4.36 
1023 molecules of carbon tetrachloride?
a) 312 g
b) 212 g
c) 111 g
d) 154 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
23) What is the mass of 1.36 
1022 molecules of HCl?
a) 0.824 g
b) 1610 g
c) 36.5 g
d) 136 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
24) How many moles of atoms are present in 154 g of Na2O?
a) 2.48 mol
b) 7.45 mol
c) 51.3 mol
d) 0.827 mol
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
25) What is the mass of 1.20 
1023 molecules of CH3OH?
a) 161 g
b) 38.5 g
c) 6.39 g
d) 32.1 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
26) What is the mass of 4.23 × 1024 molecules of oxygen?
a) 225 g
b) 7.02 g
c) 112 g
d) 448 g
Difficulty: hard
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
27) What is the mass of 2.00 
1023 molecules of H2O?
a) 5.99 g
b) 54.2 g
c) 18.0 g
d) 36.0 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
28) What is the mass of 3.01 
1024 molecules of Cl2?
a) 137 g
b) 14.2 g
c) 213 g
d) 355 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
29) How many molecules are present in 0.500 mol of CH4?
a) 3.01 
1023 molecules
b) 6.02 
1023 molecules
c) 8.00 
1023 molecules
d) 5.00 
1022 molecules
Difficulty: medium
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
30) How many molecules of CH3OH will contain 3.20 × 1023 H atoms?
a) 3.20 
1023 molecules
b) 1.07 
1023 molecules
c) 8.00 
1022 molecules
d) 1.28 
1024 molecules
Difficulty: hard
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
31) How many molecules are present in 4.21 mol of oxygen gas?
a) 1.53 
1025 molecules
b) 2.53 
1025 molecules
c) 4.21 
1023 molecules
d) 2.53 
1024 molecules
Difficulty: medium
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
32) How many molecules are present in 0.300 mol of HI?
a) 2.43 
1024 molecules
b) 1.81 
1023 molecules
c) 2.01 
1024 molecules
d) 3.00 
1022 molecules
Difficulty: easy
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
33) How many molecules are present in 4.00 mol of Cl2?
a) 1.51 
1023 molecules
b) 2.41 
1024 molecules
c) 7.09 
1024 molecules
d) 2.84 
1025 molecules
Difficulty: easy
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
34) How many chlorine atoms are present in 0.778 mol of Cl2?
a) 4.69 
1023 atoms
b) 9.37 
1023 atoms
c) 2.34 
1023 atoms
d) 1.56 atoms
Difficulty: medium
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
35) How many oxygen atoms are present in 2.35 mol of calcium phosphate?
a) 1.42 × 1024 atoms
b) 5.67 × 1024 atoms
c) 1.13 × 1025 atoms
d) 1.70 × 1025 atoms
Difficulty: hard
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
36) How many atoms are present in 0.0350 mol of barium phosphate?
a) 2.74 x 1023
b) 2.11 x 1022
c) 1.68 x 1023
d) 1.87 x 1022
Difficulty: hard
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
37) How many moles are present in 1.51 
1023 molecules of HCl?
a) 9.12 mol
b) 0.251 mol
c) 3.99 mol
d) 146 mol
Difficulty: easy
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
38) How many sulfur atoms are present in 1.50 mol of sodium sulfate?
a) 3.61 × 1024 atoms
b) 5.67 × 1024 atoms
c) 9.03 × 1023 atoms
d) 1.70 × 1025 atoms
Difficulty: medium
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
39) How many moles of HBr are present in 1.21 
1024 molecules of HBr?
a) 7.28 mol
b) 0.500 mol
c) 2.01 mol
d) 0.201 mol
Difficulty: easy
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
40) How many moles of hydrogen atoms are present in 2.41 
1024 molecules of CH3OH?
a) 0.250 mol
b) 4.00 mol
c) 1.00 mol
d) 16.0 mol
Difficulty: hard
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
41) How many moles are present in 6.02 
1024 molecules of I2?
a) 0.100 mol
b) 1.00 mol
c) 10.0 mol
d) 100. mol
Difficulty: easy
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
42) What is the total number of atoms in a 400. g sample of P2O5?
a) 1.70 x 1024 atoms
b) 1.19 x 1025 atoms
c) 8.50 x 1024 atoms
d) 6.02 x 1023 atoms
Difficulty: hard
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
43) What is the molar mass of P4?
a) 6.02 
1023 g
b) 31.00 g
c) 60.53 g
d) 124 g
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
44) What is the molar mass of oxygen gas?
a) 6.02 1023 g
b) 16.00 g
c) 12.04 1024 g
d) 32.00 g
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
45) What is the molar mass of sodium chloride?
a) 6.02 1023 g
b) 1.00 g
c) 67.53 g
d) 58.44 g
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
46) What is the molar mass of potassium chlorate?
a) 90.55 g
b) 122.55 g
c) 161.45 g
d) 6.02 
1023 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
47) What is the molar mass of magnesium perchlorate?
a) 223.21 g
b) 1.00 g
c) 301.01 g
d) 187.76 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
48) What is the molar mass of strontium nitrate?
a) 117.63 g
b) 181.63 g
c) 237.67 g
d) 211.64 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
49) What is the molar mass of calcium sulfate?
a) 88.14 g
b) 136.14 g
c) 184.30 g
d) 232.32 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
50) What is the molar mass of carbon tetrachloride?
a) 47.46 g
b) 82.91 g
c) 118.36 g
d) 153.81 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
51) What is the percent by mass of chlorine in Ca(ClO3)2?
a) 20.7%
b) 34.3%
c) 38.7%
d) 22.8%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
52) What is the percent by mass of oxygen in carbon dioxide?
a) 42.86%
b) 366.6%
c) 72.72%
d) 27.27%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
53) What is the percent by mass of oxygen in water?
a) 11.2%
b) 88.8%
c) 5.94%
d) 94.1%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
54) What is the percent by mass of hydrogen in sulfuric acid?
a) 1.04%
b) 2.06%
c) 4.03%
d) 5.93%
Difficulty: medium
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
55) What is the percent by mass of hydrogen in HC2H3O2?
a) 1.68%
b) 5.05%
c) 6.73%
d) 53.3%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
56) What is the percent by mass of hydrogen in NaHCO3?
a) 27.4%
b) 1.20%
c) 24.7%
d) 44.2%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
57) How many grams of carbon are present in 45.0 g of CCl4?
a) 0.293 g
b) 3.51 g
c) 5.76 g
d) 41.49 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
58) How many grams of oxygen are present in 76.8 g of CO2?
a) 1.75 g
b) 55.8 g
c) 27.9 g
d) 48.9 g
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
59) A compound is found to consist of 2.89 g of calcium and 5.11 g of chlorine. What is the percent by mass of calcium in the compound?
a) 56.6%
b) 36.1%
c) 63.9%
d) 100%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
60) A compound is found to consist of 1.37g of iron and 2.62g of chlorine. What is the percent by mass of chlorine in the compound?
a) 34.3%
b) 65.7%
c) 52.3%
d) 87.6%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
61) A 5.00 g sample of potassium chloride is found to contain 2.62 g of potassium. What is the percent by mass of potassium in the compound?
a) 90.8%
b) 47.6%
c) 52.4%
d) 34.4%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
62) A 6.00 g sample of calcium sulfide is found to contain 3.33 g of sulfur. What is the percent by mass of calcium in the compound?
a) 80.2%
b) 35.7%
c) 44.5%
d) 28.6%
Difficulty: medium
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
63) A substance is found to consist of 1.900 g of silver, 0.250 g of nitrogen, and 0.850 g of oxygen. What is the percent by mass of oxygen in the compound?
a) 28.3%
b) 8.33%
c) 63.3%
d) 85.0%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
64) A 10.00 g sample of a substance is found to contain 5.12 g of water. What is the percent by mass of water in the compound?
a) 5.12%
b) 4.88%
c) 48.8%
d) 51.2%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
65) What is the percent composition by mass of carbon in the chloroform CHCl3?
a) 10.04%
b) 99.58%
c) 29.71%
d) 0.830%
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
66) A substance is known to contain 2.00 g of carbon for every 5.33 g of oxygen. How many grams of carbon will be present in 55.0 g of this substance?
a) 15.0 g
b) 27.5 g
c) 20.6 g
d) 10.3 g
Difficulty: hard
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
67) A compound is known to consist of 19.36% carbon, 3.25% hydrogen, and the rest is oxygen. How many grams of this compound will be needed in order to have 23.5 g of oxygen?
a) 30.4 g
b) 104 g
c) 80.4 g
d) 53.1 g
Difficulty: hard
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
68) What is the empirical formula of a substance that consists of 92.15% carbon and 7.85% hydrogen?
a) CH
b) CH2
c) CH3
d) CH4
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
69) What is the empirical formula of a compound that consists of 39.99% carbon, 6.73% hydrogen, and 53.28% oxygen?
a) CHO
b) C2HO
c) CH2O
d) CHO2
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
70) What is the empirical formula of a substance that contains 3.09% hydrogen, 31.60% phosphorous, and 65.31% oxygen?
a) HPO4
b) H2PO
c) H3PO3
d) H3PO4
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
71) What is the empirical formula of a substance that contains 60.0% carbon, 4.48% hydrogen, and 35.52% oxygen?
a) C2H2O
b) C3H2O
c) C4H6O2
d) C9H8O4
Difficulty: hard
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
72) What is the empirical formula of a substance that consists of 0.910 g calcium, 0.636 g nitrogen, and 1.453 g oxygen?
a) CaNO
b) Ca2NO7
c) CaN2O4
d) CaN2O6
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
73) What is the empirical formula of a substance that consists of 3.704 g aluminum and 3.295 g oxygen?
a) AlO
b) AlO2
c) Al2O3
d) Al3O2
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
74) What is the empirical formula of a substance that consists of 5.687 g copper and 1.305 g oxygen?
a) CuO
b) CuO2
c) Cu2O
d) Cu2O2
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
75) A 30.5 g sample of a compound contains 9.29 g of nitrogen and the rest is oxygen. What is the empirical formula of the compound?
a) N2O3
b) N2O
c) NO
d) NO2
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
76) A 65.2 g sample of a compound contains 32.1 g of phosphorus and the rest is oxygen. What is the empirical formula of the compound?
a) P3O2
b) PO2
c) PO
d) P2O3
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
77) What is the molecular formula of a compound with the empirical formula CH and molar mass of 26.04 g?
a) CH
b) C2H
c) CH2
d) C2H2
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Section 7.5
78) What is the molecular formula of a compound with the empirical formula CH2O and molar mass of 180.18 g?
a) CH2O
b) C2H4O2
c) C4H8O4
d) C6H12O6
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Section 7.5
79) What is the molecular formula of a compound with the empirical formula CH2Cl and molar mass of 98.96 g?
a) CH2Cl
b) C2H4Cl2
c) C3H6Cl3
d) C4H8Cl4
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Section 7.5
80) What is the molecular formula of a compound with the empirical formula CH2O and molar mass of 60.06 g?
a) CH2O
b) C2H4O2
c) C3H6O3
d) C4H8O4
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Section 7.5
81) What is the molecular formula of a compound with the empirical formula CH2O and molar mass of 150. g?
a) CH2O
b) C6H12O6
c) C5H10O5
d) C2H4O2
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Section 7.5
82) What is the molecular formula of a compound with the empirical formula C13H19O2 and molar mass of 414.64 g?
a) CHO
b) C13H19O2
c) C26H38O4
d) C39H57O6
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Section 7.5
83) A compound consists of 4.50 g of nitrogen for every 7.71 g of oxygen and has the same empirical and molecular formula. Identify the compound.
a) NO2
b) N2O
c) N2O3
d) NO3
Difficulty: hard
Learning Objective 1: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Section 7.5
84) Which statement is incorrect?
a) one mole contains 6.02 
1023 molecules.
b) one molar mass equals one mole.
c) one mole equals 6.02 
1023 g of a compound.
d) one mole of water contains the same number of molecules as one mole of carbon dioxide.
Difficulty: medium
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
85) In which pair would both compounds have the same empirical formula?
a) C2H4 and C3H6
b) K2CrO4 and K2Cr2O7
c) NaHCO3 and Na2CO3
d) FeCl3 and FeCl2
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Learning Objective 2: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Sections 7.4 and 7.5
86) In which pair would both compounds have the same empirical formula?
a) H2O and H2O2
b) BaSO4 and BaSO3
c) FeO and Fe2O3
d) C6H12O6 and HC2H3O2
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Learning Objective 2: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Sections 7.4 and 7.5
87) In which pair would both compounds have the same empirical formula? Nearly same as the previous one
a) H2O and Na2O
b) MgSO4 and MgSO3
c) CuO and Cu2O
d) C3H6O3 and C2H4O2
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Learning Objective 2: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Sections 7.4 and 7.5
88) One atom of magnesium has a mass of
a) 24.31 g.
b) 4.04 
10-23 g.
c) 2.48 
1022 g.
d) 6.02 
1023 g.
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
89) One mole of sulfur molecules have a mass of
a) 5.33 
10-23 g.
b) 32.06 g.
c) 16.01 g.
d) 1.93 
1025 g.
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
90) All the following contain the same number of molecules except which one?
a) 64.06 g of sulfur dioxide molecules
b) One mole of water molecules
c) 88.02 g of carbon dioxide molecules
d) 2.02g of hydrogen molecules
Difficulty: hard
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
91) Which statement is correct?
a) one mole of SO2 contains 6.02 1023 atoms of oxygen.
b) Molar mass of SO2 is same as molar mass of oxygen gas.
c) one mole of SO2 equals 6.02 1023 g of a compound.
d) one mole of SO2 contains the same number of molecules as one mole of oxygen gas.
Difficulty: hard
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1 and section 7.2
92) All of the following contain the same number of molecules except which one?
a) 1.20 × 1024 molecules of water
b) 36.04 g of water molecules
c) 141.8 g of chlorine molecules
d) 32.0 g of oxygen molecules
Difficulty: hard
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.1 and 7.2
93) Which of the following contains the largest number of moles?
a) 1.0 g of lithium
b) 1.0 g of sodium
c) 1.0 g of aluminum
d) 1.0 g of silver
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
94) Which of the following contains the greatest number of atoms?
a) 1.0 g of lithium
b) 1.0 g of sodium
c) 1.0 g of aluminum
d) 1.0 g of silver
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
Question type: True/False
95) One mole of acetic acid, HC2H3O2, contains 4 moles of hydrogen atoms.
Difficulty: easy
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
96) 6.02 
1023 g of hydrogen is one mole of hydrogen.
Difficulty: easy
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1 and 7.2
97) One mole of oxygen has a mass of 8.00 g.
Difficulty: easy
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
98) One mole of glucose, C6H12O6, contains 24 atoms.
Difficulty: easy
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
99) One mole of magnesium and one mole of magnesium sulfate contain the same number of magnesium atoms.
Difficulty: medium
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
100) A compound with the empirical formula CH2O can have a molar mass of 150.15 g.
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Section 7.5
101) C12H22O11 is an empirical formula.
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
102) The compounds FeO and Fe2O3 have the same empirical formula.
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
103) The mole is a unit for counting.
Difficulty: easy
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
104) Two moles of O3 contain the same number of oxygen atoms as three moles of O2.
Difficulty: medium
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
105) O3 is an empirical formula.
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
106) One mole of magnesium has the same number of atoms but a smaller mass than one mole of sulfur.
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.1 and 7.2
107) The compounds C2H2 and C6H6 have the same percent composition by mass.
Difficulty: medium
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
108) If you analyze two unknown substances and find that they have the same empirical formula, then these two unknown substances are the same compound.
Difficulty: hard
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
109) H2O2 is an empirical formula.
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4
110) Molecular formula represents the actual number of atoms of each element present in the molecule.
Difficulty: easy
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Section Reference 1: Section 7.4 and 7.5
Question type: Essay
111) A 2.489 g sample of a compound is found to contain water. When heated, the water is driven off. The mass of the remaining compound is 1.591g.
a) What is the mass of the water that was lost?
b) What is the percent by mass of the water in the original compound?
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
Solution: a) 0.898 g of water was lost; b) 36.1% water by mass
112) A 3.000 g sample of a compound is found to contain water. When heated the water is driven off. The mass of the remaining compound is 1.465 g.
a) What is the mass of the water that was lost?
b) What is the percent by mass of the water in the original compound?
Difficulty: easy
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
Solution: a) 1.535g of water was lost; b) 51.17% water by mass
113) A sample of glucose, C6H12O6, has a mass of 300.0 g.
a) What mass of carbon atoms is in the sample?
b) What mass of hydrogen atoms is in the sample?
c) What mass of oxygen atoms is in the sample?
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
Solution: a) 120.0 g of carbon atoms; b) 20.18 g of hydrogen atoms; c) 159.8 g of oxygen atoms
114) A sample of glucose, C6H12O6, has a mass of 300.0g.
a) How many moles of carbon atoms are in the sample?
b) How many moles of hydrogen atoms are in the sample?
c) How many moles of oxygen atoms are in the sample?
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
Solution: a) 9.990 mol of carbon atoms; b) 19.98 mol of hydrogen atoms; c) 9.990 mol of oxygen atoms
115) You receive a gift of one mole of dollars, the only condition is that you spend it at the rate of one million dollars per second. How many years will it take you to spend the mole of dollars?
Difficulty: hard
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
Solution: 1.91 
1010 years
116) A compound is composed of 24.27% carbon, 4.08% hydrogen, and 71.65% chlorine. The compound has a molar mass of 98.96 g.
a) What is the empirical formula of the compound?
b) What is the molecular formula of the compound?
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Learning Objective 2: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Sections 7.4 and 7.5
Solution: a) The empirical formula is CH2Cl; b) The molecular formula is C2H4Cl2
117) A compound is composed of 49.292% carbon, 2.764% hydrogen, and 47.945% chlorine. The compound has a molar mass of 146.19 g.
a) What is the empirical formula of the compound?
b) What is the molecular formula of the compound?
Difficulty: medium
Learning Objective 1: Compare an empirical formula to a molecular formula and determine the empirical formula for a compound from its percent composition.
Learning Objective 2: Compare an empirical formula to a molecular formula and calculate a molecular formula from the empirical formula of a compound and its molar mass
Section Reference 1: Sections 7.4 and 7.5
Solution: a) The empirical formula is C3H2Cl ; b) The molecular formula is C6H4Cl2
118) Which of these samples:
1) 0.76 mol of titanium
2) 70.06 g of calcium chloride
3) 3.62 
1022 mol of water
a) has the greatest mass?
b) has the fewest atoms?
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.1 and 7.2
Solution: a) The sample with the greatest mass is 3) 3.62 × 1022 mol of water; b) The sample with the fewest atoms is 1) 0.76 moles of titanium
119) How many carbon atoms have about the same mass as one mole of titanium atoms?
Difficulty: hard
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.1 and 7.2
Solution: The number of carbon atoms is 2.40 
1024
120) What is the percent composition by mass of the substance shown below?
Difficulty: medium
Learning Objective 1: Calculate the percent composition of a compound from its chemical formula and from experimental data
Section Reference 1: Section 7.3
Solution: 0.57% H, 72.14% I, 27.29% O
121) Calculate the number of molecules present in 122 g of the compound shown below.
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
Solution: 2.16 
1024 molecules
122) A sample of sodium sulfate (Na2SO4) contains 2.3 
1023 sodium cations. How many moles of sulfate anions will be present in the sample?
Difficulty: medium
Learning Objective 1: Apply the concepts of the mole, molar mass and Avogadro’s number to solve chemistry problems.
Section Reference 1: Section 7.1
Solution: 0.191 mol
123) An x-gram sample of P4O6 contains 455 g of phosphorus. Calculate x.
Difficulty: hard
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
Solution: 807 g
124) A 205 g sample of H2Se contains x-moles of hydrogen atoms. Calculate x.
Difficulty: medium
Learning Objective 1: Calculate the molar mass of a compound.
Section Reference 1: Section 7.2
Solution: 5.06 mol
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Test Bank | Foundations of College Chemistry 15e by Hein Arena
By Hein Arena, Willard