Solutions Chapter.13 Full Test Bank

Student name:__________

MULTIPLE CHOICE - Choose the one alternative that best completes the statement or answers the question.
1) How many atoms are in 0.534 mol of nickel, Ni?

A) 1.13 × 10 ²⁴ atoms
B) 1.48 × 10 ²⁵ atoms
C) 2.44 × 10 ²² atoms
D) 3.22 × 10 ²³ atoms
E) 6.98 × 10 ²¹ atoms

2) How many atoms are in 7.12 mol of gold, Au?

A) 1.18 × 10⁻²³ atoms
B) 4.29 × 10 ²⁴ atoms
C) 8.46 × 10 ²² atoms
D) 4.70 × 10 ²⁴ atoms
E) 3.34 × 10 ²⁶ atoms

3) How many moles are in 8.73 × 10²⁵ atoms of boron, B?

A) 145 moles
B) 3.84 × 10²⁷ moles
C) 1.45 moles
D) 5.04 × 10⁻²⁵ moles
E) 6.90 × 10⁻³ moles

4) How many moles are present in 17.4 g of lead?

A) 0.0994 moles
B) 1.05 × 10 ²⁵ moles
C) 0.0840 moles
D) 10.06 moles
E) 11.9 moles

5) How many grams are present in 0.885 moles of manganese?

A) 62.1 g
B) 48.6 g
C) 21.5 g
D) 27.5 g
E) 0.016 g

6) Determine the mass of hydrogen (in grams) that contains 5.08 × 10 ¹⁵ hydrogen atoms.

A) 5.12 × 10 ¹⁵ g
B) 3.06 × 10 ³⁹ g
C) 3.06 × 10⁻⁹ g
D) 8.50 × 10⁻⁹ g
E) 8.5 × 10¹⁵ g

7) A rock contains an element with a molar mass of 40.08 g/mol. If 9.28 × 10²⁴ atoms of this element were found in the rock, how many grams of the unknown element are present in the rock?

A) 618 g
B) 1.49 × 10 ²⁸ g
C) 2.24 × 10 ⁵⁰ g
D) 0.38 g
E) 3.80 g

8) Five vials each contain 12 grams of a solid metal sample. The samples include calcium, platinum, barium, gold, and silver. Which vial has the most metal atoms?

A) Calcium
B) Barium
C) Gold
D) Silver
E) Platinum

9) Five vials each contain 12 grams of a solid metal sample. The samples include calcium, platinum, barium, gold, and silver. Which vial has the fewest moles of metal atoms?

A) Calcium
B) Barium
C) Gold
D) Silver
E) Platinum

10) Calcium fluoride, CaF2, is a source of fluorine and is used to fluoridate drinking water. Calculate its formula mass.

A) 118.15 g/mol
B) 99.15 g/mol
C) 78.08 g/mol
D) 59.08 g/mol
E) 50.01 g/mol

11) Calculate the molecular mass of tetraphosphorus decaoxide, P4O10, a corrosive substance that can be used as a drying agent.

A) 469.73 amu
B) 283.88 amu
C) 190.97 amu
D) 139.88 amu
E) 94.97 amu

12) Calculate the formula mass of rubidium carbonate, Rb2CO3.

A) 340.43 amu
B) 255.00 amu
C) 230.95 amu
D) 145.47 amu
E) 113.48 amu

13) Calculate the formula mass of (NH4)3AsO4.

A) 417.80 amu
B) 193.05 amu
C) 165.02 amu
D) 156.96 amu
E) 108.96 amu

14) Aluminum sulfate, Al2(SO4)3, is used in tanning leather, purifying water, and the manufacture of antiperspirants. Calculate its molecular or formula mass.

A) 450.06 amu
B) 342.17 amu
C) 315.15 amu
D) 278.02 amu
E) 74.98 amu

15) Calculate the molar mass of Ca(BO2)2·6H2O.

A) 273.87 g/mol
B) 233.80 g/mol
C) 183.79 g/mol
D) 174.89 g/mol
E) 143.71 g/mol

16) Calculate the formula mass of potassium permanganate, KMnO4.

A) 149.91 amu
B) 79.41 amu
C) 127.41 amu
D) 158.04 amu
E) 174.04 amu

17) Calculate the molecular mass of menthol, C10H20O.

A) 156 amu
B) 140 amu
C) 29 amu
D) 146 amu
E) 136 amu

18) What is the molecular mass of acetaminophen, C8H9NO2?

A) 43 amu
B) 76 amu
C) 151 amu
D) 162 amu
E) 125 amu

19) What is the molar mass of nicotine, C10H14N2?

A) 134 g/mol
B) 148 g/mol
C) 158 g/mol
D) 210 g/mol
E) 162 g/mol

20) Calculate the number of moles in 17.8 g of the antacid magnesium hydroxide, Mg(OH)2.

A) 3.28 mol
B) 2.32 mol
C) 0.431 mol
D) 0.305 mol
E) 0.200 mol

21) How many moles are present in 17.4 g of lead?

A) 0.0994 moles
B) 1.05 × 10²⁵ moles
C) 0.0840 moles
D) 10.06 moles
E) 11.9 moles

22) How many grams are present in 0.885 moles of manganese?

A) 62.1 g
B) 48.6 g
C) 21.5 g
D) 27.5 g
E) 0.016 g

23) How many moles of aspirin, C9H8O4, are in a tablet that contains 325 mg of aspirin?

A) 0.00180 moles
B) 0.555 moles
C) 0.467 moles
D) 0.357 moles
E) 2.80 moles

24) How many grams are contained in a 0.893 mol sample of methane, CH4?

A) 1.48 × 10⁻²⁴ g
B) 5.38 × 10²³ g
C) 8.64 × 10²⁴ g
D) 14.3 g
E) 18.0 g

25) How many moles of ammonia, NH3, are in 13.81 g of NH3?

A) 1.234 moles
B) 0.8107 moles
C) 8.316 × 10²⁴ moles
D) 4.881 × 10²³ moles
E) 235.3 moles

26) How many grams are contained in a 0.183 mol sample of ammonium phosphate?

A) 1.23 × 10⁻³ g
B) 617 g
C) 20.7 g
D) 27.3 g
E) 815.1 g

27) Phosphorus pentachloride, a white solid that has a pungent, unpleasant odor, is used as a catalyst for certain organic reactions. Calculate the number of moles in 38.7 g of phosphorus pentachloride.

A) 5.38 mol
B) 3.55 mol
C) 0.583 mol
D) 0.282 mol
E) 0.186 mol

28) Aluminum oxide, Al2O3, is used as a filler for paints and varnishes as well as in the manufacture of electrical insulators. Calculate the number of moles in 47.51 g of Al2O3.

A) 2.377 mol
B) 2.146 mol
C) 1.105 mol
D) 0.4660 mol
E) 0.4207 mol

29) What is the mass in grams of 0.250 mol of the common antacid calcium carbonate?

A) 4.00 × 10² g
B) 25.0 g
C) 17.0 g
D) 4.00 × 10⁻² g
E) 2.50 × 10⁻³ g

30) What is the mass of 0.0250 mol of P2O5?

A) 35.5 g
B) 5676 g
C) 0.0250 g
D) 1.51 × 10²² g
E) 3.55 g

31) Calculate the mass of 3.00 moles of CF2Cl2.

A) 3.00 g
B) 174 g
C) 363 g
D) 1.81 × 10²⁴ g
E) 40.3

32) Determine the number of ammonia molecules in 4.85 g of ammonia. (NA = 6.022 × 1023 mol−1)

A) 2.92 × 10²³ molecules
B) 4.73 × 10⁻²⁵ molecules
C) 1.24 × 10²³ molecules
D) 5.83 × 10⁻²⁴ molecules
E) 1.71 × 10²³ molecules

33) What is the average mass, in grams, of one atom of iron? (NA = 6.022 × 1023 mol−1)

A) 6.02 × 10²³ g
B) 1.66 × 10⁻²⁴ g
C) 9.27 × 10⁻²³ g
D) 55.85 g
E) 55.85 × 10⁻²³ g

34) What is the mass, in grams, of one arsenic atom? (NA = 6.022 × 1023 mol−1)

A) 5.48 × 10⁻²³ g
B) 33.0 g
C) 74.9 g
D) 1.24 × 10⁻²² g
E) 8.04 × 10²¹ g

35) What is the mass of one copper atom? (NA = 6.022 × 1023 mol−1)

A) 1.055 × 10⁻²² g
B) 63.55 g
C) 1 amu
D) 1.66 × 10⁻²⁴ g
E) 9.476 × 10²¹ g

36) What is the mass of 1.21 × 1020 atoms of sulfur? (NA = 6.022 × 1023 mol−1)

A) 3.88 × 10²¹ g
B) 2.00 mg
C) 32.06 g
D) 6.44 mg
E) 2.00 × 10⁻⁴ g

37) What is the mass of 1.63 × 1021 atoms of silicon? (NA = 6.022 × 1023 mol−1)

A) 2.71 × 10⁻²³ g
B) 4.58 × 10 ²² g
C) 28.08 g
D) 1.04 × 10⁴ g
E) 7.60 × 10⁻² g

38) What is the mass of 7.80 × 1018 carbon atoms? (NA = 6.022 × 1023 mol−1)

A) 1.30 × 10⁻⁵ g
B) 6.43 × 10³ g
C) 7.80 × 10¹⁸ g
D) 1.56 × 10⁻⁴ g
E) 12.01 g

39) The density of water is 1.00 g/mL at 4°C. How many water molecules are present in 6.25 mL of water at this temperature? (NA = 6.022 × 1023 mol−1)

A) 6.27 × 10²³ molecules
B) 3.76 × 10²⁴ molecules
C) 2.09 × 10²³ molecules
D) 6.02 × 10²³ molecules
E) 0.347 molecules

40) Sulfur trioxide can react with atmospheric water vapor to form sulfuric acid that falls as acid rain. Calculate the mass in grams of 3.65 × 1020 molecules of sulfur trioxide.

A) 6.06 × 10⁻⁴ g
B) 2.91 × 10⁻² g
C) 4.85 × 10⁻² g
D) 20.6 g
E) 1650 g

41) Calculate the mass in grams of 8.35 × 1022 molecules of CBr4.

A) 0.0217 g
B) 0.139 g
C) 7.21 g
D) 12.7 g
E) 46.0 g

42) Which of the following substances contains the greatest mass of carbon?

A) 100 g CH₄
B) 100 g C₂H₄
C) 100 g CCl₄
D) 100 g CH₂Cl₂
E) 100 g CO₂

43) Proteins found in humans are polymers that consist of different combinations of 20 amino acids. Proline, one of the 20 amino acids, has the molecular formula, C5H9NO2. If a human protein has 25 proline monomers, how many carbon atoms from proline are present in the protein?

A) 4 C atoms
B) 25 C atoms
C) 40 C atoms
D) 100 C atoms
E) 125 C atoms

44) Smooth muscle myosin is a motor protein that plays a crucial role in the contraction of smooth muscle. If this protein has a molar mass of 480,000 grams/mol, what is the mass, in grams, of 27 moles of smooth muscle myosin?

A) 1.8 × 10⁴ g
B) 1.3 × 10⁷ g
C) 1.8 × 10² g
D) 2.8 × 10²⁹ g
E) None of the answers is correct.

45) Determine the mass of Sr(C₂H₃O₂)₂ that contains 2.780 ×10²³ atoms of carbon.

A) 205.7 g
B) 57.19 g
C) 46.16 g
D) 94.96 g
E) 23.74 g

46) Determine the mass of Al(C₂H₃O₂)₃ that contains 2.63 ×10²⁴ atoms of oxygen.

A) 652 g
B) 891 g
C) 149 g
D) 89.5 g
E) 26.2 g

47) Determine the number of oxygen atoms contained in 29.7 grams of Al₂(CO₃)₃.

A) 6.88 × 10²³ O atoms
B) 7.64 × 10²² O atoms
C) 1.27 × 10²² O atoms
D) 9.44 × 10²³ O atoms
E) 4.37 × 10²³ O atoms

48) How many nitrate ions are in 24.4 grams of Ca(NO₃)₂?

A) 1.79 × 10²³ nitrate ions
B) 0.149 nitrate ions
C) 1.47 × 10²⁵ nitrate ions
D) 8.95 × 10²² nitrate ions
E) 0.297 nitrate ions

49) Household sugar, sucrose, has the molecular formula C12H22O11. What is the % of carbon in sucrose, by mass?

A) 26.7%
B) 33.3%
C) 41.4%
D) 42.1%
E) 51.4%

50) What is the percent carbon in CH3CH2OH?

A) 13%
B) 26%
C) 35%
D) 46%
E) 52%

51) What is the percent sodium in sodium carbonate?

A) 43.4%
B) 11.3%
C) 45.3%
D) 27.7%
E) 21.7%

52) What is the mass percent of oxygen in barium perchlorate?

A) 4.7%
B) 8.5%
C) 23.4%
D) 38.1%
E) 19.0%

53) What is the percent sulfur in iron(III) sulfate?

A) 28%
B) 32%
C) 24%
D) 48%
E) 42%

54) Which of the following is the empirical formula for hexane, C6H14?

A) C₁₂H₂₈
B) C₆H₁₄
C) C₃H₇
D) CH_2.3
E) C_0.43H

55) Which of the following is a molecular formula for a compound with an empirical formula of CH?

A) C₂H₆
B) C₃H₉
C) C₄H₁₀
D) C₆H₆
E) None of the answers is correct.

56) Which of the following is a molecular formula for a compound with an empirical formula of CH2O and a molar mass of 150. g/mol?

A) C₇H₁₈O₃
B) C₅H₁₀O₅
C) C₃H₆O₃
D) CH₂O
E) None of the answers is correct.

57) Which of the following is an empirical formula of a compound that is 52.15 percent C, 13.13 percent H, and 34.73 percent O?

A) C₄H₁₂O₂
B) CH₆O₂
C) C₃HO₆
D) C₂H₆O
E) None of the answers is correct.

58) Determine the empirical formula of a compound that contains 1.409 moles of P and 3.52 moles of O in a particular sample.

A) PO₂
B) PO₃
C) P₂O₆
D) P₂O₅
E) P₂O₃

59) A compound is found to be 15.65% H and 31.07% N, with the remainder from carbon, by mass. Determine the empirical formula of the compound.

A) N₄C₇H₂
B) NC₂H₇
C) NC₂H₈
D) N₂CH₃
E) NCH₅

60) Determine the empirical formula for a compound that is composed of 0.953 mol Na, 0.322 mol Al, and 1.93 mol F.

A) AlNaF₂
B) AlNa₃F₆
C) AlNaF
D) Al₄Na₁₀F₁₇
E) AlNa₂F₅

61) A compound is found to be 73.03% C, 6.13% H, and 20.84% O by mass. What is the empirical formula of the compound?

A) C₆H₆O
B) CHO
C) C₂H₂O
D) C₁₄H₁₄O₃
E) C₁₁HO₃

62) Determine the mass (in g) of Al ₂(CO ³) ³ that contains 3.65 × 10 ²⁴ Al atoms.

A) 6.06 g
B) 711 g
C) 1420 g
D) 70.3 g
E) 474 g

63) Determine the mass (in g) of Al ₂(CO ₃) ₃ that contains 8.99 × 10 ²³ carbonate ions.

A) 175 g
B) 70.0 g
C) 14.9 g
D) 448 g
E) 117 g

64) Determine the number of carbonate ions present in 4.76 × 10 ²⁴ formula units of Al ₂(CO ₃) ₃.

A) 1.43 × 10 ²⁵
B) 790
C) 2.37 × 10 ²³
D) 4.76 × 10 ²⁴
E) 7.90 × 10 ²³

65) Determine the number of lithium ions present in 7.32 × 10 ²⁴ formula units of Li ₃PO ₄.

A) 7.32 × 10 ²⁴
B) 122
C) 1.22 × 10 ²³
D) 6.45× 10 ²⁴
E) 2.20 × 10 ²⁵