Question 1

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

Accepted Answer

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 
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 D

Question 2

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?

Accepted Answer

A) 618 g 
B) 1.49 × 1028 g 
C) 2.24 × 1050 g 
D) 0.38 g 
E) 3.80 g 
A) 618 g 
B) 1.49 × 1028 g 
C) 2.24 × 1050 g 
D) 0.38 g 
E) 3.80 g A

Question 3

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

Accepted Answer

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 
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 B

Question 4

What is the molecular mass of acetaminophen, C8H9NO2?

Accepted Answer

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

Question 5

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

Accepted Answer

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 
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

Question 6

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

Accepted Answer

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

Question 7

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

Accepted Answer

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 
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

Question 8

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

Accepted Answer

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

Question 9

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

Accepted Answer

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

Question 10

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

Accepted Answer

A) 3.88 × 1021 g 
B) 2.0 mg 
C) 32.06 g 
D) 6.44 mg 
E) 2.00 × 10−4 g 
A) 3.88 × 1021 g 
B) 2.0 mg 
C) 32.06 g 
D) 6.44 mg 
E) 2.00 × 10−4 g

Question 11

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

Accepted Answer

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 
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

Question 12

How many atoms are in 0.534 mol of nickel, Ni?

Accepted Answer

A) 1.13 × 1024 atoms 
B) 1.48 × 1025 atoms 
C) 2.44 × 1022 atoms 
D) 3.22 × 1023 atoms 
E) 6.98 × 1021 atoms 
A) 1.13 × 1024 atoms 
B) 1.48 × 1025 atoms 
C) 2.44 × 1022 atoms 
D) 3.22 × 1023 atoms 
E) 6.98 × 1021 atoms

Question 13

What is the molar mass of nicotine, C10H14N2?

Accepted Answer

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

Question 14

How many grams are present in 0.885 moles of manganese?

Accepted Answer

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

Question 15

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?

Accepted Answer

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

Question 16

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

Accepted Answer

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

Question 17

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

Accepted Answer

A) 2.71× 10−23 g 
B) 4.58 × 1022 g 
C) 28.08 g 
D) 1.04 × 104 g 
E) 7.60 × 10−2 g 
A) 2.71× 10−23 g 
B) 4.58 × 1022 g 
C) 28.08 g 
D) 1.04 × 104 g 
E) 7.60 × 10−2 g

Question 18

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

Accepted Answer

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

Question 19

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.

Accepted Answer

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

Question 20

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

Accepted Answer

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

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

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?

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

What is the molecular mass of acetaminophen, C₈H₉NO₂?

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

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

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

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

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

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

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

How many atoms are in 0.534 mol of nickel, Ni?

What is the molar mass of nicotine, C₁₀H₁₄N₂?

How many grams are present in 0.885 moles of manganese?

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?

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

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

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

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.

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

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Exam 5: The Mole and Chemical Formulas

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

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?

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

What is the molecular mass of acetaminophen, C8H9NO2?

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

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

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

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

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

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

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

How many atoms are in 0.534 mol of nickel, Ni?

What is the molar mass of nicotine, C10H14N2?

How many grams are present in 0.885 moles of manganese?

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?

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

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

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

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.

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

Atoms and Elements

Electrons and the Periodic Table

Compounds and Chemical Bonds

How Chemists Use Numbers

Molecular Shape

Solids, Liquids, and Phase Changes

Gases

Physical Properties of Solutions

Chemical Reactions and Chemical Equations

Using Balanced Chemical Equations

Acids and Bases

Equilibrium

Organic Chemistry

Biochemistry

Nuclear Chemistry

Electrochemistry

Filters

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

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?

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

What is the molecular mass of acetaminophen, C₈H₉NO₂?

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

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

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

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

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

What is the molar mass of nicotine, C₁₀H₁₄N₂?

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

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

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

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.