Chapter 10 Matching



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Chapter 10

Matching

Match each item with the correct statement below.

a.

molar volume

b.

molar mass

c.

atomic mass

____ 1. the number of grams of an element that is numerically equal to the atomic mass of the element in amu

____ 2. the mass of a mole of any element or compound

____ 3. the volume occupied by a mole of any gas at STP



Match each item with the correct statement below.

a.

representative particle

d.

percent composition

b.

mole

e.

standard temperature and pressure

c.

Avogadro's number

f.

empirical formula

____ 4. the number of representative particles of a substance present in 1 mole of that substance

____ 5. an atom, an ion, or a molecule, depending upon the way a substance commonly exists

____ 6. the SI unit used to measure amount of substance

____ 7. 0C and 1 atm

____ 8. the percent by mass of each element in a compound

____ 9. the smallest whole number ratio of the atoms in a compound

Multiple Choice

Identify the letter of the choice that best completes the statement or answers the question.

____ 10. What SI unit is used to measure the number of representative particles in a substance?



a.

kilogram

c.

kelvin

b.

ampere

d.

mole

____ 11. How many hydrogen atoms are in 5 molecules of isopropyl alcohol, CHO?



a.

5 (6.02 10)

c.

35

b.

5

d.

35 (6.02 10)

____ 12. Which of the following is NOT a representative particle?



a.

atom

c.

anion

b.

cation

d.

all of the above

____ 13. Which of the following elements exists as a diatomic molecule?



a.

neon

c.

nitrogen

b.

lithium

d.

sulfur

____ 14. Avogadro's number of representative particles is equal to one ____.



a.

kilogram

c.

kelvin

b.

gram

d.

mole

____ 15. All of the following are equal to Avogadro's number EXCEPT ____.



a.

the number of atoms of bromine in 1 mol Br

b.

the number of atoms of gold in 1 mol Au

c.

the number of molecules of nitrogen in 1 mol N

d.

the number of molecules of carbon monoxide in 1 mol CO

____ 16. How many moles of tungsten atoms are in 4.8 10 atoms of tungsten?



a.

8.0 10 moles

c.

1.3 10 moles

b.

8.0 10 moles

d.

1.3 10 moles

____ 17. How many moles of silver atoms are in 1.8 10 atoms of silver?



a.

3.0 10

c.

3.0 10

b.

3.3 10

d.

1.1 10

____ 18. How many atoms are in 0.075 mol of titanium?



a.

1.2 10-25

c.

6.4 10

b.

2.2 10

d.

4.5 10

____ 19. How many molecules are in 2.10 mol CO?



a.

2.53 10 molecules

c.

3.49 10 molecules

b.

3.79 10 molecules

d.

1.26 10 molecules

____ 20. How many atoms are in 3.5 moles of arsenic atoms?



a.

5.8 10 atoms

c.

2.1 10 atoms

b.

7.5 10 atoms

d.

1.7 10 atoms

____ 21. Butanol is composed of carbon, hydrogen, and oxygen. If 1.0 mol of butanol contains 6.0 10 atoms of hydrogen, what is the subscript for the hydrogen atom in CHO?



a.

1

c.

6

b.

10

d.

8

____ 22. The atomic masses of any two elements contain the same number of ____.



a.

atoms

c.

ions

b.

grams

d.

milliliters

____ 23. Which of the following is NOT a true about atomic mass?



a.

The atomic mass is 12 g for magnesium.

b.

The atomic mass is the mass of one mole of atoms.

c.

The atomic mass is found by checking the periodic table.

d.

The atomic mass is the number of grams of an element that is numerically equal to the mass in amu.

____ 24. What is true about the molar mass of chlorine gas?



a.

The molar mass is 35.5 g.

b.

The molar mass is 71.0 g.

c.

The molar mass is equal to the mass of one mole of chlorine atoms.

d.

none of the above

____ 25. The mass of a mole of NaCl is the ____.



a.

molar mass

c.

molecular mass

b.

atomic mass

d.

gram atomic mass

____ 26. What is the molar mass of AuCl3?



a.

96 g

c.

232.5 g

b.

130 g

d.

303.6 g

____ 27. What is the molar mass of (NH)CO?



a.

144 g

c.

96 g

b.

138 g

d.

78 g

____ 28. The molar mass of CH and the molar mass of CaCO contain approximately the same number of ____.



a.

carbon atoms

c.

cations

b.

anions

d.

grams

____ 29. What is the mass in grams of 5.90 mol CH?



a.

0.0512 g

c.

389 g

b.

19.4 g

d.

673 g

____ 30. What is the number of moles in 432 g Ba(NO)?



a.

0.237 mol

c.

1.65 mol

b.

0.605 mol

d.

3.66 mol

____ 31. What is the number of moles of beryllium atoms in 36 g of Be?



a.

0.25 mol

c.

45.0 mol

b.

4.0 mol

d.

320 mol

____ 32. How many moles of CaBr are in 5.0 grams of CaBr?



a.

2.5 10 mol

c.

4.0 10 mol

b.

4.2 10 mol

d.

1.0 10 mol

____ 33. For which of the following conversions does the value of the conversion factor depend upon the formula of the substance?



a.

volume of gas (STP) to moles

b.

density of gas (STP) to molar mass

c.

mass of any substance to moles

d.

moles of any substance to number of particles

____ 34. What is the mass of silver in 3.4 g AgNO?



a.

0.025 g

c.

2.2 g

b.

0.64 g

d.

3.0 g

____ 35. What is the mass of oxygen in 250 g of sulfuric acid, HSO?



a.

0.65 g

c.

16 g

b.

3.9 g

d.

160 g

____ 36. The volume of one mole of a substance is 22.4 L at STP for all ____.



a.

gases

c.

solids

b.

liquids

d.

compounds

____ 37. The molar volume of a gas at STP occupies ____.



a.

22.4 L

c.

1 kilopascal

b.

0C

d.

12 grams

____ 38. Which combination of temperature and pressure correctly describes standard temperature and pressure, STP?



a.

0C and 101 kPa

c.

0C and 22.4 kPa

b.

1C and 0 kPa

d.

100C and 100 kPa

____ 39. The molar mass of a substance can be calculated from its density alone, if that substance is a(n) ____.



a.

element

c.

liquid

b.

gas at STP

d.

solid

____ 40. The molar mass of a gas can be determined from which of the following?



a.

the density of the gas at STP

c.

Avogadro's number

b.

the volume of a mole of the gas

d.

none of the above

____ 41. What is the volume, in liters, of 0.500 mol of CH gas at STP?



a.

0.0335 L

c.

16.8 L

b.

11.2 L

d.

22.4 L

____ 42. What is the number of moles in 500 L of He gas at STP?



a.

0.05 mol

c.

22 mol

b.

0.2 mol

d.

90 mol

____ 43. What is the number of moles in 9.63 L of HS gas at STP?



a.

0.104 mol

c.

3.54 mol

b.

0.430 mol

d.

14.7 mol

____ 44. What is the density at STP of the gas sulfur hexafluoride, SF?



a.

0.153 g/L

c.

3270 g/L

b.

6.52 g/L

d.

3.93 10 g/L

____ 45. The molar mass of a certain gas is 49 g. What is the density of the gas in g/L at STP?



a.

3.6 10 g/L

c.

2.2 g/L

b.

0.46 g/L

d.

71 g/L

____ 46. A 22.4-L sample of which of the following substances, at STP, would contain 6.02 10 representative particles?



a.

oxygen

c.

cesium iodide

b.

gold

d.

sulfur

____ 47. If the density of an unknown gas Z is 4.50 g/L at STP, what is the molar mass of gas Z?



a.

0.201 g/mol

c.

26.9 g/mol

b.

5.00 g/mol

d.

101 g/mol

____ 48. Which of the following gas samples would have the largest number of representative particles at STP?



a.

12.0 L He

c.

0.10 L Xe

b.

7.0 L O

d.

0.007 L SO

____ 49. Given 1.00 mole of each of the following gases at STP, which gas would have the greatest volume?



a.

He

c.

SO

b.

O

d.

All would have the same volume.

____ 50. If the density of a noble gas is 1.783 g/L at STP, that gas is ____.



a.

Kr

c.

Ar

b.

Xe

d.

He

____ 51. To determine the formula of a new substance, one of the first steps is to find the ____.



a.

molar mass

c.

volume at STP

b.

percent composition

d.

number of particles per mole

____ 52. What information is needed to calculate the percent composition of a compound?



a.

the weight of the sample to be analyzed and its density

b.

the weight of the sample to be analyzed and its molar volume

c.

the formula of the compound and the atomic mass of its elements

d.

the formula of the compound and its density

____ 53. If 60.2 grams of Hg combines completely with 24.0 grams of Br to form a compound, what is the percent composition of Hg in the compound?



a.

28.5%

c.

71.5%

b.

39.9%

d.

60.1%

____ 54. What is the percent composition of chromium in BaCrO?



a.

4.87%

c.

20.5%

b.

9.47%

d.

25.2%

____ 55. If 20.0 grams of Ca combines completely with 16.0 grams of S to form a compound, what is the percent composition of Ca in the compound?



a.

1.25%

c.

44.4%

b.

20.0%

d.

55.6%

____ 56. What is the percent composition of carbon, in heptane, CH?



a.

12%

c.

68%

b.

19%

d.

84%

____ 57. What is the percent by mass of carbon in acetone, CHO?



a.

20.7%

c.

1.61%

b.

62.1%

d.

30.0%

____ 58. Which expression represents the percent by mass of nitrogen in NH4NO3?



a.

14 g N/80 g NHNO 100%

c.

80 g NHNO/14 g N 100%

b.

28 g N/80 g NHNO 100%

d.

80 g NHNO/28 g N 100%

____ 59. Which of the following compounds has the lowest percent gold content by weight?



a.

AuOH

c.

AuCl

b.

Au(OH)

d.

AuI

____ 60. Which of the following compounds has the highest oxygen content, by weight?



a.

NaO

c.

BaO

b.

CO

d.

HO

____ 61. The lowest whole-number ratio of the elements in a compound is called the ____.



a.

empirical formula

c.

binary formula

b.

molecular formula

d.

representative formula

____ 62. Which of the following is NOT an empirical formula?



a.

CNH

c.

BeCrO

b.

CHO

d.

SbS

____ 63. Which of the following compounds have the same empirical formula?



a.

CO and SO

c.

CH and CH

b.

CH and CH

d.

CH and CH

____ 64. What is the empirical formula of a compound that is 40% sulfur and 60% oxygen by weight?



a.

SO

c.

SO

b.

SO

d.

SO

____ 65. What is the empirical formula of a substance that is 53.5% C, 15.5% H, and 31.1% N by weight?



a.

CHN

c.

CHN

b.

CHN

d.

CHN

____ 66. The ratio of carbon atoms to hydrogen atoms to oxygen atoms in a molecule of dicyclohexyl maleate is 4 to 6 to 1. What is its molecular formula if its molar mass is 280 g?



a.

CHO

c.

CHO

b.

CHO

d.

CHO

____ 67. Which of the following is NOT true about empirical and molecular formulas?



a.

The molecular formula of a compound can be the same as its empirical formula.

b.

The molecular formula of a compound can be some whole-number multiple of its empirical formula.

c.

Several compounds can have the same empirical formula, but have different molecular formulas.

d.

The empirical formula of a compound can be triple its molecular formula.

____ 68. Which of the following sets of empirical formula, molar mass, and molecular formula is correct?



a.

CH, 78 g, CH

c.

CaO, 56 g, CaO

b.

CHN, 90 g, CHN

d.

CHO, 120 g, CHO


Short Answer

69. How many representative particles are in 1.45 g of a molecular compound with a molar mass of 237 g?

70. Find the mass in grams of 3.10 10 molecules of F.

71. Find the number of moles of argon in 607 g of argon.

72. Find the mass, in grams, of 1.40 10 molecules of N.

73. What is the percent composition of NiO, if a sample of NiO with a mass of 41.9 g contains 33.1 g Ni and 8.8 g O?

74. What is the percent by mass of hydrogen in aspirin, CHO?

75. Calculate the molecular formulas of the compounds having the following empirical formulas and molar masses: CH, 58 g/mol; CH, 78 g/mol; and HgCl, 236.1 g/mol.



Essay

76. Give three examples of methods of measuring the amount of something, and give an example of how one of these quantities can be converted to another type of quantity.

77. When determining the moles of a gas from the volume of that gas, why is it important that the volume be measured at STP?

78. Why is it possible to calculate the density of a gas at STP, knowing only its molar mass, but it is not possible to make the same calculation for a solid or a liquid?



79. The percentage composition of a polymer used for the non-stick surfaces of cooking utensils is 24% C and 76% F by mass. Explain the steps in determining the empirical formula of the polymer.

80. The density of acetylene at STP is 1.17 g/L. The empirical formula of acetylene is CH. Describe how you can determine the molar mass of acetylene and its molecular formula if you know only its density at STP and its empirical formula.

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