Question 1

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

Question 2

Lead(II)sulfide was once used in glazing earthenware.It will also react with hydrogen peroxide to form lead(II)sulfate and water.How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II)sulfide?

Accepted Answer

A) 151 g 
B) 123 g 
C) 50.3 g 
D) 37.7 g 
E) 9.41 g 
A) 151 g 
B) 123 g 
C) 50.3 g 
D) 37.7 g 
E) 9.41 g

Question 3

What is the percent carbon in CH3CH2OH?

Accepted Answer

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

Question 4

How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?

Accepted Answer

A) 90.g 
B) 36 g 
C) 42 g 
D) 45 g 
E) 108 g 
A) 90.g 
B) 36 g 
C) 42 g 
D) 45 g 
E) 108 g

Question 5

Which is a representation of a balanced chemical equation for the reaction of nitrogen gas and chlorine gas to form nitrogen trichloride?

Accepted Answer

A)    
B)    
C)    
D)    
E)    
A)    
B)    
C)    
D)    
E)

Question 6

Once the following equation is balanced with the smallest set of whole number coefficients,what is the sum of the coefficients? (Don't forget to include coefficients of one.) __ SF4 + __ H2O → __ H2SO3 + __ HF

Accepted Answer

A) 4 
B) 6 
C) 7 
D) 9 
E) None of these answers is correct. 
A) 4 
B) 6 
C) 7 
D) 9 
E) None of these answers is correct.

Question 7

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride.What mass of chlorine gas is required to react completely with 163 g of aluminum?

Accepted Answer

A) 214 g 
B) 286 g 
C) 321 g 
D) 428 g 
E) 643 g 
A) 214 g 
B) 286 g 
C) 321 g 
D) 428 g 
E) 643 g

Question 8

The ____ is the amount of product physically collected from a chemical reaction and is typically less than the theoretical yield.

Accepted Answer

The answer of The ____ is the amount of product...

Question 9

Calculate the molar mass of sulfuric acid.

Accepted Answer

A) 98.086 g/mol 
B) 81.078 g/mol 
C) 49 g/mol 
D) 41 g/mol 
E) None of the answers are correct. 
A) 98.086 g/mol 
B) 81.078 g/mol 
C) 49 g/mol 
D) 41 g/mol 
E) None of the answers are correct.

Question 10

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

Accepted Answer

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 
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

Question 11

What mass of oxygen is required to react with calcium to produce 44.8 g calcium oxide?

Accepted Answer

A) 12.8 g 
B) 25.6 g 
C) 6.39 g 
D) 0.399 g 
E) 51.1 g 
A) 12.8 g 
B) 25.6 g 
C) 6.39 g 
D) 0.399 g 
E) 51.1 g

Question 12

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 13

How many moles are present in 17.4 g of lead?

Accepted Answer

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

Question 14

Many compounds can be represented with the same empirical formula.

Accepted Answer

A) True 
 B)False

Question 15

What is the theoretical yield of vanadium,in moles,that can be produced by the reaction of 2.0 mole of V2O5 with 6.0 mole of calcium based on the following chemical equation? V2O5(s)+ 5Ca(l)→ 2V(l)+ 5CaO(s)

Accepted Answer

A) 1.0 mol 
B) 1.6 mol 
C) 2.0 mol 
D) 2.4 mol 
E) 4.0 mol 
A) 1.0 mol 
B) 1.6 mol 
C) 2.0 mol 
D) 2.4 mol 
E) 4.0 mol

Question 16

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 17

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 18

How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO2 and 30.0 g of HCl according to the following balanced chemical equation? MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

Accepted Answer

A) 6.52 g 
B) 7.29 g 
C) 13.0 g 
D) 14.6 g 
E) 58.4 g 
A) 6.52 g 
B) 7.29 g 
C) 13.0 g 
D) 14.6 g 
E) 58.4 g

Question 19

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 20

Calculate the molecular mass of menthol,C10H20O.

Accepted Answer

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

Exam 3: Stoichiometry Ratios of Combination

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

Lead(II)sulfide was once used in glazing earthenware.It will also react with hydrogen peroxide to form lead(II)sulfate and water.How many grams of hydrogen peroxide are needed to react completely with 265 g of lead(II)sulfide?

What is the percent carbon in CH3CH2OH?

How many grams of water could be made from 5.0 mol H2 and 3.0 mol O2?

Which is a representation of a balanced chemical equation for the reaction of nitrogen gas and chlorine gas to form nitrogen trichloride?

Once the following equation is balanced with the smallest set of whole number coefficients,what is the sum of the coefficients? (Don't forget to include coefficients of one.) __ SF4 + __ H2O → __ H2SO3 + __ HF

Aluminum metal reacts with chlorine gas to form solid aluminum trichloride.What mass of chlorine gas is required to react completely with 163 g of aluminum?

The ____ is the amount of product physically collected from a chemical reaction and is typically less than the theoretical yield.

Calculate the molar mass of sulfuric acid.

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

What mass of oxygen is required to react with calcium to produce 44.8 g calcium oxide?

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?

How many moles are present in 17.4 g of lead?

Many compounds can be represented with the same empirical formula.

What is the theoretical yield of vanadium,in moles,that can be produced by the reaction of 2.0 mole of V2O5 with 6.0 mole of calcium based on the following chemical equation? V2O5(s)+ 5Ca(l)→ 2V(l)+ 5CaO(s)

What is the molecular mass of acetaminophen,C8H9NO2?

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

How many grams of Cl2 can be prepared from the reaction of 16.0 g of MnO2 and 30.0 g of HCl according to the following balanced chemical equation? MnO2 + 4HCl → MnCl2 + Cl2 + 2H2O

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?

Calculate the molecular mass of menthol,C10H20O.

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 mass of 1.21 × 10²⁰atoms of sulfur? (N_A = 6.022 × 10²³ mol^-1)

What is the percent carbon in CH₃CH₂OH?

How many grams of water could be made from 5.0 mol H₂ and 3.0 mol O₂?

Once the following equation is balanced with the smallest set of whole number coefficients,what is the sum of the coefficients? (Don't forget to include coefficients of one.) SF₄ + H₂O → H₂SO₃ + HF

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

What is the theoretical yield of vanadium,in moles,that can be produced by the reaction of 2.0 mole of V2O5 with 6.0 mole of calcium based on the following chemical equation? V₂O₅(s)+ 5Ca(l)→ 2V(l)+ 5CaO(s)

What is the molecular mass of acetaminophen,C₈H₉NO₂?

How many grams of Cl₂ can be prepared from the reaction of 16.0 g of MnO₂ and 30.0 g of HCl according to the following balanced chemical equation? MnO₂ + 4HCl → MnCl₂ + Cl₂ + 2H₂O

Calculate the molecular mass of menthol,C₁₀H₂₀O.