Question 1

What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?

Accepted Answer

A)  28.1 g 
B)  14.04 g 
C)  4.96 g 
D)  7.02 g 
E)  400.0 g 
A)  28.1 g 
B)  14.04 g 
C)  4.96 g 
D)  7.02 g 
E)  400.0 g

Question 2

What is the coefficient of O2 when the following equation is properly balanced with the smallest set of whole numbers? ________ CH3OH + ________ O2 → ________ CO2 + ________ H2O

Accepted Answer

A)  1 
B)  2 
C)  3 
D)  7 
E)  None of these answers is correct. 
A)  1 
B)  2 
C)  3 
D)  7 
E)  None of these answers is correct.

Question 3

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

Accepted Answer

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

Question 4

What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V2O5 with 40.0 g of calcium based on the following chemical equation? V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)

Accepted Answer

A)  11.2 g 
B)  5.6 g 
C)  22.4 g 
D)  40.0 g 
E)  20.3 g 
A)  11.2 g 
B)  5.6 g 
C)  22.4 g 
D)  40.0 g 
E)  20.3 g

Question 5

Hydroxylammonium nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. What is its empirical formula?

Accepted Answer

A)  HNO 
B)  H2NO2 
C)  HN6O16 
D)  HN16O7 
E)  H2NO3 
A)  HNO 
B)  H2NO2 
C)  HN6O16 
D)  HN16O7 
E)  H2NO3

Question 6

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%

Question 7

What is the coefficient of O2 when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers?
________ C18H36O2 + ________ O2 → ________ CO2 + ________ H2 O

Accepted Answer

Question 8

One way of obtaining pure sodium carbonate is through the decomposition of the mineral trona, Na3(CO3)(HCO3)·2H2O. 2Na3(CO3)(HCO3)·2H2O(s) → 3Na2CO3(s) + CO2(g) + 5H2O(g)
When 1.00 metric ton (1.00 × 103 kg) of trona is decomposed, 0.650 metric ton of Na2CO3 is recovered. What is the percent yield of this reaction?

Accepted Answer

A)  92.4% 
B)  72.1% 
C)  65.0% 
D)  48.1% 
E)  35.0% 
A)  92.4% 
B)  72.1% 
C)  65.0% 
D)  48.1% 
E)  35.0%

Question 9

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 10

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

Accepted Answer

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

Question 11

What is the empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium and 32.4% fluorine by mass?

Accepted Answer

A)  U2F 
B)  U3F4 
C)  UF4 
D)  UF6 
E)  UF8 
A)  U2F 
B)  U3F4 
C)  UF4 
D)  UF6 
E)  UF8

Question 12

How many grams of lead(II) chloride is produced if 13.87 g lead(II) nitrate combines with excess hydrochloric acid to produce lead(II) chloride and nitric acid?

Accepted Answer

A)  5.82 g 
B)  14.33 g 
C)  0.086 g 
D)  11.64 g 
E)  16.52 g 
A)  5.82 g 
B)  14.33 g 
C)  0.086 g 
D)  11.64 g 
E)  16.52 g

Question 13

The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule.

Accepted Answer

A) True 
 B)False

Question 14

What is the empirical formula for a sample containing 81.70% carbon and 18.29% hydrogen?

Accepted Answer

A)  CH 
B)  CH3 
C)  C2H6 
D)  CH4 
E)  C3H8 
A)  CH 
B)  CH3 
C)  C2H6 
D)  CH4 
E)  C3H8

Question 15

Ammonia reacts with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in the production of aluminum, in uranium processing, and in the frosting of light bulbs). 2NH3(g) + 5F2(g) → N2F4(g) + 6HF(g)
How many moles of NH3 are needed to react completely with 13.6 mol of F2?

Accepted Answer

A)  34.0 mol 
B)  27.2 mol 
C)  6.80 mol 
D)  5.44 mol 
E)  2.27 mol 
A)  34.0 mol 
B)  27.2 mol 
C)  6.80 mol 
D)  5.44 mol 
E)  2.27 mol

Question 16

Balance the following equation: Ca3(PO4)2(s) + SiO2(s) + C(s) → CaSiO3(s) + CO(g) + P4(s)

Accepted Answer

A)  Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) → 3CaSiO3(s) + 8CO(g) + P4(s) 
B)  Ca3(PO4)2(s) + 3SiO2(s) + 14C(s) → 3CaSiO3(s) + 14CO(g) + P4(s) 
C)  Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) → 3CaSiO3(s) + 8CO(g) + 2P4(s) 
D)  2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) → 6CaSiO3(s) + 10CO(g) + P4(s) 
E)  2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) → 6CaSiO3(s) + 10CO(g) + 4P4(s) 
A)  Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) → 3CaSiO3(s) + 8CO(g) + P4(s) 
B)  Ca3(PO4)2(s) + 3SiO2(s) + 14C(s) → 3CaSiO3(s) + 14CO(g) + P4(s) 
C)  Ca3(PO4)2(s) + 3SiO2(s) + 8C(s) → 3CaSiO3(s) + 8CO(g) + 2P4(s) 
D)  2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) → 6CaSiO3(s) + 10CO(g) + P4(s) 
E)  2Ca3(PO4)2(s) + 6SiO2(s) + 10C(s) → 6CaSiO3(s) + 10CO(g) + 4P4(s)

Question 17

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 18

A compound was discovered whose composition by mass is 85.6% C and 14.4% H. Which of these formulas could be the molecular formula of this compound?

Accepted Answer

A)  CH4 
B)  C2H4 
C)  C3H4 
D)  C2H6 
E)  C3H8 
A)  CH4 
B)  C2H4 
C)  C3H4 
D)  C2H6 
E)  C3H8

Question 19

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

Accepted Answer

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

Question 20

What is the average 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

Exam 3: Stoichiometry: Ratios of Combination

What mass of sodium carbonate is required for complete reaction with 8.35 g of nitric acid to produce sodium nitrate, carbon dioxide, and water?

What is the coefficient of O2 when the following equation is properly balanced with the smallest set of whole numbers? ________ CH3OH + ________ O2 → ________ CO2 + ________ H2O

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

What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V2O5 with 40.0 g of calcium based on the following chemical equation? V2O5(s) + 5Ca(l) → 2V(l) + 5CaO(s)

Hydroxylammonium nitrate contains 29.17 mass % N, 4.20 mass % H, and 66.63 mass % O. What is its empirical formula?

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

What is the coefficient of O2 when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? ________ C18H36O2 + ________ O2 → ________ CO2 + ________ H2 O

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

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

What is the empirical formula of a compound of uranium and fluorine that is composed of 67.6% uranium and 32.4% fluorine by mass?

How many grams of lead(II) chloride is produced if 13.87 g lead(II) nitrate combines with excess hydrochloric acid to produce lead(II) chloride and nitric acid?

The empirical formula is the simplest whole number ratio of atoms representing a chemical formula of a molecule.

What is the empirical formula for a sample containing 81.70% carbon and 18.29% hydrogen?

Ammonia reacts with fluorine to produce dinitrogen tetrafluoride and hydrogen fluoride (used in the production of aluminum, in uranium processing, and in the frosting of light bulbs). 2NH3(g) + 5F2(g) → N2F4(g) + 6HF(g) How many moles of NH3 are needed to react completely with 13.6 mol of F2?

Balance the following equation: Ca3(PO4)2(s) + SiO2(s) + C(s) → CaSiO3(s) + CO(g) + P4(s)

What is the molar mass of nicotine, C10H14N2?

A compound was discovered whose composition by mass is 85.6% C and 14.4% H. Which of these formulas could be the molecular formula of this compound?

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

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

Chemistry: the Central Science

Atoms, Molecules, and Ions

Reactions in Aqueous Solutions

Thermochemistry

Quantum Theory and the Electronic Structure of Atoms

Electron Configuration and the Periodic Table

Chemical Bonding I: Basic Concepts

Chemical Bonding II: Molecular Geometry and Bonding Theories

Gases

Intermolecular Forces and the Physical Properties of Liquids and Solids

Modern Materials

Physical Properties of Solutions

Chemical Kinetics

Chemical Equilibrium

Acids and Bases

Acid-Base Equilibria and Solubility Equilibria

Entropy, Free Energy, and Equilibrium

Electrochemistry

Nuclear Chemistry

Environmental Chemistry

Coordination Chemistry

Metallurgy and the Chemistry of Metals

Nonmetallic Elements and Their Compounds

Organic Chemistry

Filters

What is the coefficient of O₂ when the following equation is properly balanced with the smallest set of whole numbers? CH₃OH + O₂→ CO₂ + H₂O

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

What is the theoretical yield of vanadium that can be produced by the reaction of 40.0 g of V₂O₅ with 40.0 g of calcium based on the following chemical equation? V₂O₅(s) + 5Ca(l) → 2V(l) + 5CaO(s)

What is the coefficient of O₂ when the following combustion reaction of a fatty acid is properly balanced using the smallest set of whole numbers? C₁₈H₃₆O₂ + O₂→ CO₂ + H₂ O

Balance the following equation: Ca₃(PO₄)₂(s) + SiO₂(s) + C(s) → CaSiO₃(s) + CO(g) + P₄(s)

What is the molar mass of nicotine, C₁₀H₁₄N₂?

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

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